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Chemistry 30S Crystal Growing Project
Objective (What will I accomplish?)Work independently and apply the principles of solution chemistry to grow a crystal athome.
Rationale (Why am I doing this?)To develop a working understanding of the following terms.
• Solute
• Soluble
• Mixture
e Unsaturated• Solvent
• Insoluble
• Heterogeneous • Saturated• Solution
• Homogeneous • Precipitate
• Supersaturated• Concentrated • Dilute
• Aqueous
• Crystal
Procedure1. Research and develop a procedure for growing a crystal at home.2. Conference with the teacher to articulate your method and have it approved.3. Display your crystal in a three dimensional exhibit.
Due Date(s)
Wednesday, November 5,2008
Wednesday, November 5,
Thursday, November 6,2008Thursday, November2008Monday, November 24,2008
Bragging Rights Bonus CategoriesOne bonus mark will be awarded to each student that wins a bragging rights category, asdetermined by a class vote (silent auction method). No student may win more than onebragging rights title. No student may be awarded a bonus mark where the project mark
would exceed 100%. The bonus mark in tied votes in any category will be split betweenno more than two winners, with each winner receiving one bonus mark. In the case of athree or more person tie in a single category winners will not be awarded a bonus mark..NOTE: in case of disagreement, the final decision to award a bonus mark rests with theteacher.
Timeline
Project Stage
Experimental Method
2.
3.
DueStudent & TeacherPlanning Conferences
Begin Growing Crystal
2008
4. Crystal Exhibit
• Biggest crystal
• Best decorated
• Most functionallooking
• Most perfectlooking
• Smallest crystal
• Most colourful• Greatest number of detached
crystals
• Coolest shape or design
• Best display
Chemistry 30S Crystal Growing Project
PLANNING CONVERSATIONIntermediateExpert
4 points)
(3-2 points
CRYSTAL GROWING PROJECT ASSESSMENT RUBRIC
Novice1-0 point
Name:
Criteria
Articulates amethod
Student articulates amethod personalized
to their homeenvironment to
successfully grow acrystal that requires
no revisions
Student articulates amethod to
successfully grow acrystal that requiresminor revisions (3)
or the studentrequires furtherinformation toarticulate their
method (2)
Student is unable toarticulate a method
(0) or presents amethod that clearly
has not been thought Iout and/or is not
personalized to theirenvironment (1)
CRYSTAL EXHIBITMinimum of threepictures illustratingdiverse stages of
One (3) or two (2)Pictures of growing
growth including
aspects of expertstages displayed
some method of
level criteriameasurement clearly
missingvisible with date
stampsInformation aboutthe chemical used,the growing time,
the biggestchallenge, and the
Crystal Display
most rewarding
Two (2) or three (3)Information
experience
criteria metassociated with
growing the crystali is communicated in
the display
' attractive, three- Two (2) or three (3)dimensional display
criteria metincluding crystal j
Colourful,
Crystal Display
More than twoaspects of expert
level criteriamissing (1) or no
pictures displayedof growing stages
(0)
Less than twocriteria met (1) or
no displayinformation present
(0)
Only one criteriamet (1) or no crystal
displayed (0)
/16
Chemistry 30S Silent Auction Ballots
Voting InstructionsCut out each ticket. Cast your ballot by placing each ticket in the appropriate container.
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for
and
rem
ove
cont
act
lens
es. F
lush
tho
roug
hly
wit
h w
ater
for
at le
ast 1
5 m
inut
es, l
ifti
ng u
pper
and
low
er e
yeli
ds o
ccas
iona
lly.
Get
imm
edia
te m
edic
al a
tten
tion
.SK
ftR
emov
eco
ntam
inat
ed c
loth
ing.
Flu
sh th
orou
ghly
wit
h m
ild
soap
and
wat
er I
f ir
rita
tion
occ
urs,
get
med
ical
att
enti
on. 1
Rem
ove
to f
resh
or,
. If
not b
reat
hing
, giv
e ar
t' ci
al r
espi
rati
on. I
f br
eath
ing
isdi
ffic
ult,
give
oxy
gen.
Get
med
ical
att
enti
on.
)SEC
TIO
0-
IRE
AC
,TIV
>DA
TAS
tab
ilit
Uns
tabl
eC
on
dit
ion
s t
o A
vo
id
Exc
essi
ve te
mer
atur
e an
d he
aty
Sta
ble
p.
X
Inco
mp
atib
ility
( Mat
eria
ls t
oA
void
) )
Avo
id c
onta
ct w
ith
hydr
oxyl
amin
e, m
agne
sium
and
red
ucin
g ag
ents
. Thi
s pr
oduc
tco
rrod
e st
eel a
nd ir
on
Inco
mpa
tibl
e w
ith
alka
lise
s, p
hosp
hate
s, a
cety
lene
,h
dras
ine
and
nitr
omet
hane
.
Haz
ard
ous
Dec
om
posi
tion
Pro
du
cts
Oxi
des
of s
ulfu
r, c
oppe
r fu
mes
.
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ardo
us P
olym
eriz
atio
nC
ond
itio
ns
to A
void
May
Occ
urW
ill N
ot O
ccur
Not
app
licab
le.
X1, av
U-4
7-S
.1.
,ilf,
q
•
Ven
tIfa
te th
e ar
ea. S
prin
kle
lim
e or
sod
a as
h on
spi
ll to
for
min
solu
ble
copp
er s
alt.
Sw
eep
up a
nd p
lace
in a
sui
tabl
e co
ntai
ner
for d
i€sp
osal
,W
ash
spil
l are
a w
ith
soap
and
wat
er. P
reve
ntm
ater
ial f
rom
ent
erin
g se
wer
s an
d w
ater
way
s
0is.c
gha
r a.
tre
ats
renl
, or
efts
pasa
I tr
ay b
e su
bjec
t to
Fed
eral
, Sta
le o
r L
ocal
law
s.Ti
rane
dis
posa
l 5ui
dalin
as a
re in
tend
ed ta
r the
dis
;zel
sal o
f cat
alog
Siz
e gi
iarr
dtlr'
sonly
.
Dis
pose
of
in a
n ap
prov
ed c
hem
ical
land
fill
or
cont
ract
wit
h a
was
tedi
spos
al a
genc
y.
SPE
CI"
A` P
I RO
TEC
T[O
NIN
FOR
MA
TIO
1R
espi
ratio
n Pr
otec
tion
(Spe
cify
Typ
e)N
one
shou
ld b
e re
quir
ed in
nor
mal
labo
rato
ry u
se. I
f du
sty
cond
itio
ns p
reva
il,
wor
k in
a v
enti
lati
on h
ood
or w
ear
a N
IOS
H/M
SH
A-a
ppro
ved
dust
mas
k.V
til
Loca
l Exh
avst
Rec
omm
ende
d.sp
ecia
l
No.
ta
en
ion
Mec
hani
cal (
Gen
eral
)R
ecom
men
ded,
Oth
er
No.
Pro
tecti
ve G
loves
Rub
ber.
Eye P
rote
cti
on
Che
mic
al s
afet
y go
ggle
s.
Saf
ety
2 ss
es, s
moc
k, a
pron
, ven
ted
hood
, pro
per
glov
es, a
nd e
ye w
ash
stat
ion
SEC
TID
N`1
-
^S
:pE
CIA
PR
EC
AiJ
'I I
©N
Pre
cau
tion
s to
be
Tak
enin
Han
dli
ng
&S
tori
ng
Keep c
o+
+ta
tmr
N] ht y
c-narr
f w
t,^«
„cr
d, Lam
Oth
er P
recau
tion
sR
ead
idbo
lnn
co+
rlai
nar
bafo
reus
ing.
bo
not
woa
+co
oc
lr-^
sao
wh
n on
g u
€e e
he n
.i0.
Far'a
boid
iPry
u.5
a on
ly, N
at fo
r 6: +
g, rr
:L,f
f hnn
se,h
o!1
use-
Kry
t..q
Put d
t rsa
ch n
i ch7
l+i u
n.
Avo
id c
onta
ct w
ith
skin
, eye
s an
d cl
othi
ngA
void
bre
athi
ng d
ust
Use
wit
h ad
equa
te v
enti
lati
on. R
emov
e an
d w
ash
cont
amin
ated
clo
thin
g.
Rev
isio
n N
o.
9D
ate
0410
4705
Ap
pro
ved
Mir
haf:
Ras
zeja
MR
rr,
rr»
i
e
r hn c
le k
r
W w
e -
r y o
f any
ON
CC
O53
5M
SD
S N
o.:
CC
O545 C
CO
550
Eff
ecti
ve D
ata:
Apri
l 4, 2005
24 H
OU
R E
ME
RG
EN
CY
ASS
IST
AN
CE
Fla
sh P
oin
t(M
etho
d U
sed)
Exti
nguis
her
Med
ia
Non
-fla
mm
able
,Fl
,imm
abie
e L
imits
in A
/2 b
y V
olum
e
N/A
owe
_ .a_
Ste
ps
to b
e ta
ken
in c
ase
mate
rial
is r
ele
ase
d o
r sp
ille
d
Was
te D
isp
osa
l Met
ho
d
SE
CT
ION
Vfl
Sto
re in
a c
ool,
dry
plac
e.W
ash
thor
ough
ly a
fter
han
dlin
g.
MA
TE
RIA
L S
AF
ET
Y D
AT
A S
HE
ET
AL
DO
N
221
Roc
hest
er S
ireet
Avo
n N
ew Y
ork
1441
4-94
93
Pro
duct
Sod
ium
Bic
arbo
nate
, Anh
ydro
usC
HE
MT
RE
CC
hem
ical
8004
24-8
300
Hea
lthp
Syno
nym
sb
Bic
aron
ate
of S
oda;
Fla
king
Sod
apa
y 58
5226
-617
7F1
rep
Form
ula
NaH
CO
3NFPA
Rea
ctiv
ity1
Unit
Siz
eup
to 2
.5 K
gH
AZ
AR
D R
AT
IO 'H
MIS
*G
.A.S
. N
o,
144-
55-8
MIN
IMAL
5..
OCT
MO
DiP
Aft
0
1
2SE
RIOU
S
:
VERE
3
I•
•
Pri
ncip
al C
ompo
nent
(s)
TL
V U
nits
Sod
ium
bic
arbo
nate
100%
Non
e es
tabl
ishe
d
CA
UT
ION
!
MA
Y C
AU
SE I
RR
ITA
TIO
N T
o SK
IN A
ND
EY
ES.
Mel
tin
g P
oin
t (°
F)
10!
C (
228°
F): a
ravl
ry(H
,O =
1)
2.16
at
20'C
Boi
ling
Poin
t ('
F)
Dec
ompo
ses
to r
elea
se C
OPH
rcen
ty,:a
tr,e
byV
r,!.
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/A
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or P
ress
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m H
g)N
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ible
as
solid
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InAG6
gAte_tl
N/A
Vap
or D
ensi
ty(A
ir-1
)N
IA
Solu
bilit
y in
Wat
er9,
6 gr
ams
per
100
mL
. at
20"C
.
Ap
peara
nce
&O
do
rW
h
, cry
stal
line
po
wd
er;
no
od
or,
1r
Fla
sh P
oin
t!M
etho
d U
sed}
Non
-fla
mm
ab
Exti
nguis
her
Med
ia
"SE
C TIO
NV
.,ej$u
HE
AI:
:"C
H H
AZ
AR
D
Eff
ects
of
Over
ex o
sure
p
tN8&
1AJ1
N L
ow h
azar
d fo
r us
ual
labo
rato
ry h
andl
ing
F_Y
E N
o sp
ecif
icha
zard
kno
wn
to u
s. H
owev
er, a
ny m
ater
ial t
hat c
onta
cts
the
eye
may
be
irri
tati
ng. S
K1N
; Low
hac
ari
l for
usu
alla
bora
tory
han
dlin
g. I
NG
ES
TIQ
j Non
-haz
ard
clas
sifi
cati
onG
ross
inge
stio
n m
ay p
rodu
ce a
lkal
osis
: how
ever
as
ana
tura
l mat
eria
l in
the
body
, it i
s w
ell t
oler
ated
and
nor
mal
Tar
get
orga
ns:
Non
e kn
own.
IllR
EA
CT
IVIT
Y,,'O
77
Sta
bil
ity
Un
stab
leC
on
dit
ion
s to
Avoid
Hlg
h te
mpe
r ^
ure
caus
es d
ecom
posi
tion
toS
tab
leX
Sod
ium
car
bona
te, w
ater
and
car
bon
diox
ide.
Inco
mp
atib
ility
(Mat
eria
ls t
o A
void
)R
eact
s w
ith
acid
s to
yie
ld a
crid
sal
ts, w
ater
and
car
bon
diox
ide
Haz
ard
ou
sD
eco
mp
osi
tio
n P
rod
uct
sG
ase
ous
carb
on d
ioxi
de
Haza
rdou
s P
oly
mer
izati
on
Con
dit
ion
s to
Avoid
May
Occ
urW
ill N
ot O
ccur
Not
app
lira
ble
X
MU
LMS
teps
to b
e ta
ken
in c
ase
mat
eria
l is
rel
ease
d o
r sp
ille
d
Waste
Dis
posal
Meth
od
Dis
char
ge, t
reat
men
t, o
r di
spos
al m
ay b
e su
hlee
l to
Fr
or
tor
rr:
,ial l
aws.
Tha
mo
disp
osal
gui
delt
yen
are
Inte
nded
for
the
disp
asnl
of
I
afee
tlt
art1
tos
only
.
Dis
pose
of
in a
ccor
danc
e w
ith
fede
ral,
stoi
c an
d lo
cal r
egul
atio
ns
'A Res
pira
tion
Pro
tect
ion
® C
OR
PO
RA
TIO
N
226
6177
24 H
OU
R E
ME
RG
EN
CY
ASS
IST
AN
CE
MS
DS
No:
SS
0270
Effe
ct.v
e D
ate:
Apr
il 4,
200
5
RD
SD
AT
A)
Upp
er
Non
e ne
eded
.T
his
mat
eria
lis
use
d in
fire
ext
ingu
ishe
rs
IN_4
3E T
I N
: C
all p
hysi
cian
or
Poi
son
Con
trol
Cen
ter
imm
edia
tely
. Ind
uce
vom
itin
g on
ly if
adv
ised
by
appr
opri
ate
med
ical
per
sonn
elN
ever
giv
e
5IN
; R
emov
e co
ntam
inat
ed c
loth
ing.
Flu
sh t
horo
ughl
y w
ith
mil
d so
ap a
nd w
ater
. If
irri
tati
on o
ccur
s, g
et
anyt
hing
by
mou
th t
o an
unc
onsc
ious
per
son
.Esm
Che
ck f
or a
nd r
emov
e co
ntac
t le
nses
. Flu
sh t
horo
ughl
yw
ith
wat
er fo
r at
leas
t 15
min
utes
, lif
ting
upp
er a
nd lo
wer
eye
lids
occa
sion
ally
. Get
imm
edia
te m
edic
al a
tten
tion
.
med
ical
att
enti
on.
INF!
A.L
&T
iO,I
j Rem
ove
to fr
esh
air.
If n
ot b
reat
hing
, giv
e ar
tifi
cial
res
pira
tion
. If b
reat
hing
isdi
ffic
ult,
give
oxy
gen.
Get
med
ical
att
enti
on.
Em
erge
ncy
and
Fir
st A
id P
roce
dure
s
N "
:161
414
b
Sw
eep
up a
nd p
lace
in
a su
itab
le c
onta
iner
for
c l
oW
ash
spit
s ar
ea w
ith
soap
and
wat
er.
(Spe
cify
Typ
e)N
one
shou
ld b
e ne
eded
in n
orm
al la
bora
tory
use
If
du
sty
cond
i tion
s pr
evai
l, w
ear
aN
IOSH
/ MSH
Aap
prov
eddu
st m
ask
or r
espi
rato
r
Ventila
tion
Pro
tect
ive G
I
ocal Exhaust
one
shou
ld b
e ne
eded
Mec
hani
cal
(Genera
l) I R
eco
mm
ended
oves
Non
e re
quir
ed.
Eye P
rote
ction
No 0
Che
mic
al s
afet
y gl
asse
s
Sp
ecia
l
Oth
SP
EC
IAL
FIR
EF
IGH
TIN
GP
RO
CE
DU
RE
S
In f
ire
cond
itio
ns, w
ear
a N
IOSH
/MSH
A-a
ppro
ved
self
-con
tain
edbr
eath
ing
appa
ratu
s an
d fu
ll p
rote
ctiv
e cl
othi
ng.
UN
US
UA
L F
IRE
AN
DE
XP
LO
SIO
N H
AZ
AR
DS
No k
now
n h
aza
rds,
Can r
eact
vig
oro
usl
y w
ith a
cids
and
aci
d fum
es.
D.O.T. I
NON-REGULATED,
App
rove
d by
U E
7 D
epar
tmen
t of
Lab
or °
asae
i t .i
lly s
itni
?af"
to f
orm
OSH
A-2
0
Pre
cauti
ons
to b
e T
aken
in H
and
lin
g &
Sto
rin
g
Stor
ein
a c
lean
, coo
l, dr
y pl
ace
away
from
aci
ds a
nd a
c f
fum
es.
Wash
thoro
ughly
after
handlin
g
Qtt
Eer
Pre
caut
ions
tro
-ad
apei
n'ao-r lyarw
2 usire ba net w
ear corrtaa rnnscr. w
kr_n aura? t^.ru.^m
tcauv.
fur
ia4ara
Fgry
we o
nt,
Nat!
dr
ty f
ang
nr
M,^
uvsh,^
aus
r'-K
eep n
W o
f nra
!o
f tl
i.drt
xt.
Rem
ove
and
was
h co
ntam
inat
edcl
othi
ng.
Rev
isio
rtN
o.6
pate
04/0
4105
App
rove
dT
he
ibon ^
^t •:
ahe
:
r..•h
•R
K-p
r^a
nta
inor
i5htiy c
tasm
d w
hen n
ot k, u,
/^^
MA
TE
RIA
LS
AF
ET
Y D
AT
A S
HE
ET
AL
DO
N
227
€tor
hest
er S
tree
tta
at4
-sac
s
Pro
du
ctS
odiu
m F
erro
cyan
lde
Che
mic
alS
ynon
yms
Yel
low
Pru
ssia
te o
f S
oda
Fo
rmu
laC
6F
eN
5N
a4.1
0H
2O
Un
it S
ize
up to 1
80 K
g.
C.A
.S, N
o. F
1360
1-19
-9
NT
LOIS
Pri
ncip
al C
om
ponent(
s)
Sod
ium
fer
rocy
anid
e, d
ecah
ydra
te
CA
UT
ION
!
LO
W H
EA
LT
H H
AZ
AR
D F
OR
USU
AL
LA
BO
RA
TO
RY
H
Mel
tin
g P
oin
t ("
F)
Not
app
licab
le.
cnav
ty (H
2O
1)1 4
58
Bo
ilin
g P
oin
t ('
F)
Dec
om
Pose
sr 4
35'C
(8141F
)R
llm
;by
tot
app
€ica
ble.
Vap
or
Pre
ssure
(m
m H
g)
Not
app
licab
le.
Era
para
lian
Rat
e
-t)
Not
app
licab
le.
Vap
or
Den
sity
(A
ir-1
)N
ot a
pplic
able
.
Sol
ubil
ity
in W
ater
Cal
cula
ted
as t
he a
nhyd
rous
sal
t cr
25"
C:
17.6
1
Ap
pea
rance
& O
dor
Pale
yel
low
mor
loc€
inic
slig
htly
eff
lore
scen
t cry
stal
s.
SEC
TIO
N V
:
Fxs
HE
AL
TH
HA
ZA
RD
DA
TA
M1',""
`.'
z"s
sa53
^T
hres
hold
Lim
ited
Val
ueN
one
esta
blis
hed
Eff
ects
of
Ov
erex
po
sure ]
Low
leve
l of
toxi
city
alth
ough
arty
chem
ical
may
be
harm
ful b
y in
hala
tion
,in
gest
ion
or s
kin
abso
rpti
onM
ay c
ause
irri
tati
on. T
o th
e be
st o
f ou
rkn
owle
dge,
the
chem
ical
, phy
sica
l and
toxi
colo
gica
l pro
pert
ies
have
not
bee
nth
orou
ghly
inve
stig
ated
. Spe
cifi
c. d
ata
is n
ot a
vail
able
Exe
rcis
e ap
prop
riat
epr
oced
ures
to
min
imiz
e po
tent
ial h
azar
ds. T
arge
t or
gans
: N
one
know
n.E
mer
gen
cy a
nd
Fir
st A
id P
roced
ures
ING
ES
TIO
N: C
all p
hysi
cian
or
Poi
son
Con
trol
Cen
ter
imm
edia
tely
. Ind
uce
vom
itin
g on
ly if
adv
ised
by
appr
opri
ate
med
ical
pet
sonn
el N
ever
giv
ean
ythi
ng b
y m
outh
to
an u
ncon
scio
us p
erso
n. E
YE
S:
Che
ck f
or a
nd r
emov
e co
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.N
ot a
pplic
able
.
Vap
or P
ress
ure
(mn-
i F
ig)
Not
app
iicab
ie.
rv4r
ateN
ot a
pplic
able
.V
apor
Den
sity
(A
ir=
1)N
ot a
pplic
able
.
Sol
ubil
ity
inW
ater
Mod
erat
e.
Ap
pea
ran
ce &
Od
or
Whi
te c
ryst
als
or p
owde
r, n
o od
or.
SE
CT
ION
:V 4
WI.
,.HE
AL
TH
; HA
ZA
RD
: 'D
AT
A
AM
01ss
10 m
g/rn
3 a
s A
lum
inum
met
al d
ust
(AC
GIF
I 200
1).
Eff
ects
of
Overe
xp
osu
rTIN
HA
LA
TI_
0 , R
ust m
ay c
ause
upp
er r
espi
rato
ry tr
act i
rrit
atio
n.}f
NA
ND
EY
ES:
May
cau
se ir
rita
tion
, red
ness
, pai
n. if
1GE
^TIO
N:
Tox
ic in
larg
e do
ses.
May
cau
se li
ver
and
kidn
eyda
mag
eE
xerc
ise
appr
opri
ate
proc
edur
es t
o m
inim
ize
pote
ntia
l haz
ards
. Tar
get
orga
ns:
live
r, k
idne
ys.
Sta
bilit
yU
nst
able
Co
nd
itio
ns t
o A
vo
id
Lose
s S
O3
at h
igh
tem
pera
ture
s.St
able
XE
xces
sive
tem
pera
ture
and
hea
tIn
com
pati
bilit
y(M
ater
ials
to
Avo
id)
Avo
id c
onta
ct w
ith
alka
lies
. Cor
rosi
ve to
alu
min
um, s
teel
, cop
per,
zin
can
d m
any
othe
rm
etal
s.
Hazard
ou
sD
eco
mp
osi
tio
n P
ro
du
cts
The
rmal
dec
ompo
siti
on o
r bu
rnin
g m
ay p
rodu
ce s
ulfu
r tr
ioxi
de a
nd s
ulfu
rdi
oxid
e.
Ha
zard
ou
s P
oly
mer
iza
tio
nC
ond
itio
ns
to A
void
May
Occ
urW
ill N
ot O
ccur
Not
app
licab
le.
X
Waste
Dis
posal
Meth
od
©is
char
ge, I
roat
nten
t, or
dis
paxn
f m
ay b
e su
bjec
t to
Fed
eral
, Sta
te o
r L
oral
lam
p.T
hese
dis
posa
l gui
deli
nes
are
inte
nded
far
the
dis
posa
l of
cata
log
srzr
. qua
ntit
ies
only
.
Dis
solv
e in
wat
er a
nd f
lush
to s
ewer
wit
h co
piou
s am
ount
sof
wat
er.
A L D O N
CO
RP
OR
AT
ION
(585
22£
-e177
MSD
S N
o.:
AA
0195
AA
0196
Effe
ctiv
eD
ate:
Apr
il 4,
200
5
PIR
IAN
DD
EX
PL
QS
ION
HA
AR
D:U
AT
AF
lash P
oin
t(M
eth
od U
sed)
Non
-flar
nF
lam
mable
Lim
its in
Air
by V
olum
eN/A
owe
Uppe
Em
erge
ncy
an
dF
irst
Aid
Pro
ced
ure
sIN
GE
STIO
N;,
Cal
l phy
sici
an o
r P
oiso
n C
ontr
ol C
ente
r im
med
iate
ly I
nduc
evo
mit
ing
only
if a
dvis
ed b
y ap
prop
riat
e m
edic
al p
erso
nnel
Nev
er g
ive
anyt
hing
by
mou
th t
o an
unc
onsc
ious
per
son.
EY
ES:
Che
ck f
or a
nd r
emov
e co
ntac
t le
nses
. Flu
sh t
horo
ughl
yw
ith
wat
er f
or a
t le
ast
15 m
inut
es, l
ifti
ng u
pper
and
low
er e
yelid
s oc
casi
onal
ly. G
et im
med
iate
med
ical
att
enti
on.
IN:
Rem
ove
cont
amin
ated
clo
thin
g. F
lush
tho
roug
hly
wit
h m
ild s
oap
and
wat
er, I
fir
rita
tion
occ
urs,
get
med
ical
att
enti
on. I
NH
AI .
AT
I^ R
em
ove
to fr
esh
air.
If n
ot b
reat
hing
, giv
e a
rtif
icia
l res
pira
tion
. If b
reat
hing
isdi
ffic
ult,
give
oxy
gen
Get
mer
tl'S
l att
enti
on.
Ste
ps
to b
e ta
ken
in
cas
em
ater
ial
is r
elea
sed
or
spil
led
Neu
tral
ize
wit
h A
lkal
i, L
ime,
Cau
stic
Sod
a, S
odiu
m C
arbo
nate
Sw
eep
up a
nd p
lace
in a
sui
tabl
e co
ntai
ner.
Was
h sp
ill a
rea
wel
lw
ith
soap
and
wat
er.
Ext
ingu
ish
erM
edia
Use
any
med
ia s
uita
ble
for
exti
ngui
shin
g su
ppor
ting
fir
e.
In f
ire
cond
itio
ns, w
ear
a N
IOSH
/MSH
A-a
ppro
ved
self
-con
tain
edbr
eath
ing
appa
ratu
s
,"SE
CTI
ON
",.,V
II
SP
EC
IAR
OT
EC
TIO
N:I
IN O
RM
AT
IfJ
Res
pira
tion
Prot
ectio
n1
Non
e sn
ould
be
need
ed in
nor
mal
labo
rato
ry h
andl
ing.
If
dust
y co
ndit
ions
pre
vail
,(S
peci
fy T
ype)
wor
k in
a v
enti
lati
on h
ood
or w
ear
a N
IOS
H/M
SH
A-a
ppro
ved
dust
mas
k.S
PE
CIA
L F
IRE
FIG
HT
ING
PR
OC
ED
UR
ES
Ventila
tion
Pro
tective G
lO
ther
Pro
tective
Equip
ment
oves
Local Exhaust
Mechanical (General)
Gog
gles
, sm
ock,
apr
on, p
rope
r gl
oves
, eye
was
h st
afio
n, a
nd
Rub
ber.
Rec
omm
ende
d.Recommended.
Sp
ecia
l
Oth
er
Eye
Pro
tect
ion
Che
mic
al s
afet
y gl
asse
s
a ve
ntiti
on h
ood.
No No
aSE
C'T
IOU
NU
SU
AL
FIR
E A
ND
EX
PL
OS
ION
HA
ZA
RD
SP
reca
utio
ns
to b
in H
andlin
u &
Sto
ring
Kee
p m
axi e
* dg
ht!y
c;o
;ad
whe
n m
iin w
aSt
ore
in a
coo
l, dr
y pl
ace
Was
h th
orou
-ly
aft
er h
andl
ing.
Can
giv
e of
f su
lfur
trio
xide
and
lor
sulf
ur d
ioxi
de g
as u
nder
hig
hhe
at 7
60'C
(14
00-F
).
Oth
er P
recau
tion
sR
¢ad€
ahcl
onam
txaa
rtetv
e
x.
cm
wri
cn
sew
h
wih
1311
wal
sr.
.^ i
b..
Wry
oae c
^n1y
-N
t tu
rd u
g. h
loxf
.hie
^es
ho,d
use
Kam
p ou
t o9
Rem
ove
and
was
h co
ntam
inat
ed c
loth
ing.
Rev
isio
n N
o.
8
Dat
e04
/041
05JA
ppro
ved
Mic
has
!R
asze
jaT
he in n
..S
ill
"h
er
fm
w:.
^^
•^.
ni
ht?nlth Sd
simila
r" to
form
OSH
A-2
11
D.O.T.
NO
N-R
EG
UL
AT
ED
,A
pprr
wed
by U
-S. D
epar
tmsr
il ci
f La4
rm "
ease
nt'r
all
/^
MA
TE
RIA
L S
AF
ET
Y D
AT
A S
HE
ET
AL
DO
N
221
Rac
hesl
er S
trae
iA
von,
New
Yor
k 14
4 14
,940
9
Pro
du
ct.....
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dium
Bor
a'
Dec
ahyd
rate
CH
EM
TR
EC
Che
mic
etB0
0-42
4.93
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alth
1S
ynon
yms
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etra
bora
te;
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xpa
y 58
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77
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eF
orm
ula
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NF
PA
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cti i
ty0
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it S
ize
upto
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Kg.
HAZA
RDRA
TING '
HM
IS "
C.A
-S. N
o.
1303
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INIM
AL
5 0
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MO
LL A
TE0
1
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R01-
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RE3
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ncip
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ompo
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%T
LV
Uni
tsS
odiu
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orat
e, d
ecah
ydra
te10
0"/
See
Sec
tion
V.
CA
UT
ION
( MA
Y B
E H
AR
MF
UL
IF
SW
AL
LO
WE
D. M
AY
CA
USE
YE
IRR
iTA
ION
.
SE
CT
IM
elti
ng P
oin
t (°
F)
62`C
(14
3°F
)SIN
sue,
,(H
,O W
1)
1.73
6oiii
ngP
oin
t('F
)N
ot d
eter
min
ed.
f^txV
"!
Vol
yi!e
by v
ol" r
ne ry
^lN
ot d
eter
min
ed.
Vapor
Pre
ssure
(m
m H
g)
Not
det
erm
ined
.Ew
po w
or, R
ifeN
ot d
eter
min
ed.
Vap
or
Den
sity
(A
irw
l)N
ot d
eter
min
ed.
Solu
bili
ty in
Wate
r51
% @
20°
C ,
65.6
3% (
rD 1
00=C
.
Appea
rance
& O
dor
Whi
te c
ryst
allin
e or
pow
der;
no
odor
. Eff
lore
scen
t in
war
m, d
ry a
ir.
Fla
sh P
oin
t(M
etho
d U
sed)
Non- c
omL.
....ib
le.
Flam
mab
le L
imits
in A
ir
Low
er
uppe
r%
by
Vol
ume
N/A
- -
- -
- -
- -
- -
- -
- -
- -
Ext
ingu
ishe
rM
edia
Non
e re
quir
ed. P
rodu
ct in
here
nt f
ire
reta
rdan
t.
SP
EC
IAL
FIR
EF
IGH
TIN
GP
RO
CE
DU
RE
S
In f
ire
cond
itio
ns, w
ear
a N
IOSH
/MSH
A-a
ppro
ved
self
-con
tain
edbr
eath
ing
appa
ratu
sN
o sp
ecia
l fir
efig
htin
g pr
oced
ures
req
uire
d.
SE
CT
ION
V`:
'.i
'HE
AL
»TH
^HA
ZA
RD
,_DA
TA
`T
hre
shol
d L
imit
ed V
alu
eT
LV-T
WA
5 m
glm
3 (A
GG
If-i 2
001)
Ora
l-rat
: LC
350:
613
rng
fkg.
Eff
ects
of
Over
exposu
res
YE
S:
May
cau
se i
rrit
atio
n r
ednes
s, p
ain
N. M
ay c
ause
irri
tati
on.
iN.T
.[.Q
&, M
ay b
e ha
rmfu
l if
swa€
low
€sd.
May
cau
se g
astr
oint
esti
nal
irri
tati
on, k
idne
y in
jury
, cen
tral
ner
vous
sys
tem
dep
ress
ion
or c
ircu
lato
ry f
ailu
re.
!NH
AL
AT
tON
N: M
ay c
ause
res
pira
tory
trac
t irr
itat
ion,
cou
ghin
g, n
ause
a,vo
mit
ing.
Tar
get
orga
ns:
Non
e kn
own
Em
ergen
cy a
nd
Fir
st A
id P
roced
ures
]it
t f
ST
IQN
_.. C
al p
hysi
cian
or
Poi
son
Con
trol
Cen
ter
imm
edia
tely
Ind
uce
vom
itin
g on
ly if
adv
ised
by
appr
opri
ate
med
ical
per
sonn
el N
ever
giv
ean
ythi
ng b
y m
outh
to
an u
ncon
scio
us p
erso
n. E
YE
S:
Che
ck f
or a
nd r
emov
e co
ntac
t le
nses
. Flu
sh t
horo
ughl
yw
ith
wat
er f
or a
t lea
st 1
5 m
inut
es, l
ifti
ng u
pper
and
low
er e
yeli
ds o
ccas
iona
lly.
Get
imm
edia
te m
edic
al a
tten
tion
.1N
:R
emov
e co
ntam
inat
ed c
loth
ing.
Flu
sh th
orou
ghly
wit
h m
ild
soap
and
wat
er. I
f ir
rita
tion
occ
urs,
get
med
ical
att
enti
on. j
NH
AL
AT
)O'•,
- R
emov
e to
fre
sh a
ir. I
f no
t bre
athi
ng, g
ive
arti
fici
al r
espi
rati
on. I
f br
eath
ing
isdi
ffic
ult,
give
oxy
gen.
(-e
f m
edic
al a
tten
tion
Sta
bili
tyU
nsta
ble
Co
nd
itio
ns
to A
void
Sta
ble
X!
cces
sive
tem
pera
ture
and
hea
t
Inco
mp
ati
bilit
y(M
ate
rials
to
Avo
id)
Ele
men
tal Z
irco
nium
, str
ong
acid
s an
d ox
idiz
ing
agen
ts.
Hazard
ou
sD
ecom
posi
tion
Prod
ucts
Bar
an o
xide
and
sod
ium
oxi
de.
Haz
ardo
us P
olym
eriz
atio
nC
on
dit
ion
s to
Avo
idM
ay O
ccur
Will
Not
Occ
urN
ot a
pplic
able
.X
Ste
ps
to b
e ta
ken
in c
ase
mat
eria
l is
rele
ased
or
spill
ed sch2
rge,
[re
etm
ao, o
r di
spas
7l m
ay b
e su
bjec
t to
Fed
ora]
, Sta
le o
r L
ocal
Im
wS
.W
aste
Dis
pos
alM
eth
od
p,_
-T
hese
dis
posa
l gut
deli
nea
are
it€e
nded
for
lye
diap
osa3
of
cafa
leg-
size
gr+
anti
iies
onl
y.
Dis
solv
e in
wat
er a
nd f
lush
to s
ewer
wit
h co
piou
s am
ount
s of
wat
er.
SE
G lO
N V
II
SPE
C A
L:z
PR
OT
EC
TI O
N"I
NF
OR
MA
TIO
Res
pira
tion
Prot
ectio
n
Non
esh
ould
be
requ
ired
in n
orm
al la
bora
tory
use
. If
dust
y co
ndit
ions
pre
vail
, use
a(s
pecif
yTy
pe)
N I
OSH
/MSH
A-a
ppro
ved
resp
irat
or.
A L D O N®
CO
RP
OR
AT
ION
1585
1226
-617
7MSDS No..
SS0320
Effe
ctiv
eD
ate:
Apr
il 4,
200
5
SE
CT
ION
°^l'
24 H
OU
R E
ME
RG
EN
CY
ASS
IST
AN
CE
Sw
eep
up a
nd p
lace
in
a su
itab
le c
onta
iner
Dis
solv
e in
wat
er a
nd f
lush
to s
ewer
wit
h co
piou
s am
ount
s of
wat
er.
Ven
tila
tio
n
Loca
lE
xhau
st
Reco
mm
ended.
spec
ial
Mec
hani
ca;G
enera
l
Reco
mm
ended
Oth
erN
one
need
ed u
nles
ssk
in is
abr
aded
.
jE
ye P
rote
c#io
n
Sm
ock,
apr
on, g
oggl
es,
eye
was
h st
atio
n, v
enti
lati
on h
ood
Pro
tect
ive
Glo
ves
No.
No-
Che
mic
al s
afet
ygl
asse
s
7777
7777
77-^T
11
UN
US
UA
L F
IRE
AN
DE
XP
LO
SIO
N H
AZ
AR
DS
Pre
cau
tion
sto
be
Tak
ers
in H
and
lin
g &
Sto
rin
g
IK
een
mtn =r
ter t
ipht
y cln
s®d
act
Sto
re in
a c
ool,
dry
plac
eW
ash
thor
ough
ly a
fter
han
dlin
g
WA
RN
tNnl
, Thi
s pr
oduc
t co
ntai
ns t
race
am
ount
s of
ars
enic
, a c
hem
ical
know
n to
cau
se c
ance
r,F
ire
or e
xces
sive
hea
t may
pro
duce
haza
rdou
sde
com
posi
tion
prod
ucts
. Pro
duct
is a
n in
here
ntfir
e re
tard
ant.
No
unus
ual f
ire
and
expl
osio
nha
zard
Oth
er P
recau
tion
sR
osa
Lab
e, o
n co
n;at
nrvb
Enjn
o n
ot
i
tvv
wh
en o
rh
1,c
leas
;rn
reb
nW
a y
usu
oil
y N
r! 0
f O
rug
,f
J
-p-1
0 -
0ntc
fv4,e
r,
Glo
ves
are
usua
lly n
ot n
eces
sary
unl
ess
open
ski
n is
pre
sent
.R
emov
e an
d w
ash
cont
amin
ated
clo
thin
g.
Revi
sion N
o.
7J D
ate
04/0
4/0
5MR
D.O
.T. I
NO
N-R
EG
ULA
TE
D.
A;p
prov
e4 b
y U
.S. O
ep^3
rtm
ent o
f L
ahor
'ess
enti
a€I
sim
itotr"
to fa
rm O
SH
A-2
011re
n'o
rmrt
ron d
inla
lned h
em
farm
-ed
Ihem
on
o m
uid
make
,edo
anco
=:^,
-liN
:= ..
,iii
IL o
f em
pid
yeos. `
Huro
n,u
-. M
,!-i
Defining a SolutionMisleading Labelling
Pvtili; is sometimes labelled as "honoae-nized," meaning that the cream: is equal 'ydistributed throughout the milk. This use ofthe word does not match the chemistry defi-nition of homogeneous. Using the strictchemistry deuniton, milk is not a hor<;eae-
neous mixture, but a heterogeneo s mixture.WK is not a solution.
a homogeneous mixture of sub-stances composed of at least one solute andone solvent
a uniform mix-tore of only one phase
a substance that is dissolved in asolvent {e.g., salt, NaCl)
the medium in which a solute isdissolved; often the liquid component of asolution )e.g., water)
Figure 1Gasoline, shown here in a spill on asphalt, isa nonaqueous solution containing many dif-ferent solutes (mostly hydrocarbons such asbenzene and paraffin) in an octane solvent.The composition of gasoline is not fixed: itvaries with the source of the raw material,the manufacturer, and the season.
Many of the substances that we use every day come packaged with water, We buyother substances with little or no water, but then mix water with them before use.For example, we may purchase syrup, household ammonia, and pop with wateralready added, but we mix baking soda, salt, sugar, and powdered drinks withwater, Most of the chemical reactions that you see in high school occur in a waterenvironment. Indeed, most of the chemical reactions necessary for life on ourplanet occur in water.
Because so many substances dissolve in it, water is often referred to as theuniversal solvent. Of course, this is an exaggeration. Not all things dissolve inwater. Imagine if they did; we would not be able to find a container for water.
Before restricting our study to mixtures involving water, we will review themore general definition and types of a solution.
Solutions
Solutions are homogeneous mixtures of substances composed of at least onesolute and one solvent. Liquid-state and gas-state solutions are clear (trans-parent)-you can see through them; they are not cloudy or murky in appear-ance. Solutions may be coloured or colourless. Opaque or translucent (cloudy)mixtures, such as milk, contain undissolved particles large enough to block orscatter light waves. These mixtures are considered to be heterogeneous.
It is not immediately obvious whether a clear substance is pure or is a mix-
ture, but it is certainly homogeneous. Homogeneous mixtures in the liquid stateand the gas state are always clear with only one phase present. If you were to doa chemical analysis of a sample of a homogeneous mixture (i.e., a solution), youwould find that the proportion of each chemical in the sample remains the same,regardless of how small the sample is. This is explained by the idea that there is auniform mixture of particles (atoms, ions, and/or molecules) in a solution.
Empirically, a solution is homogeneous; theoretically, it is uniform at the atomicand molecular level,
Both solutes and solvents may
be gases, liquids, or solids, pro-
Table 1: Classification of Solutionsducing a number of different com-binations (Table 1). In metal alloys,
such as bronze or the mercuryamalgam used in tooth fillings, thedissolving has taken place in liquid
form before the solution is used insolid form. Common liquid solu-
tions that have a solvent other thanwater include varnish, spray furni-ture polish, and gasoline. Gasoline,
for example, is a mixture of as manyas 400 different hydrocarbons andother compounds (Figure I.). Thesesubstances form a solution-a
homogeneous mixture at the molecular level. There are many such hydrocarbon
solutions, including kerosene (a Canadian-invented fuel for lamps and stoves),and turpentine (used for cleaning paintbrushes). Most greases and oils will dis-solve in hydrocarbon solvents.
Solutein solvent Example of solution
gas in gas oxygen in nitrogen (in air)
gas in liquid oxygen in water (in most water)
gas in solid oxygen in solid water (in ice)
liquid in gas water in air (humidity)
liquid in liquid methanol in water (in antifreeze)
liquid in solid mercury in silver (in toothfillings)
solid in liquid sugar jr) water (in syrup)
solid in solid tin in copper in bronze)
266 Chapter 6
6.1
Other examples of liquids and solids dissolving in solvents other than waterinclude the many chemicals that dissolve in alcohols. For example, solid iodinedissolved in ethanol (an alcohol) is used as an antiseptic (Figure 2), Aspirin(acetylsalicylic acid, ASA) dissolves better in methanol (a poisonous alcohol)than it does in water, for example, when doing chemical analyses. Of course, itshould never be mixed with alcohol when ingested. Some glues and sealantsmake use of other solvents: acetic acid is used as a solvent of the components ofsilicone sealants. You can smell the vinegar odour of acetic acid when sealingaround tubs and fish tanks.
The chemical formula representing a solution specifies the solute by using itschemical formula and shows the solvent by using a subscript. For example,
Nil3(.3„
ammonia gas (solute) dissolved in water (solvent)
NaCl(,q)
solid sodium chloride (solute) dissolved in water (solvent)
I2(at)
solid iodine (solute) dissolved in alcohol (solvent)
CnHSOH(aq)
liquid ethanol (solute) dissolved in water (solvent)
By far the most numerous and versatile solutions are those in which water isthe solvent (Figure 3). Water can dissolve many substances, forming manyunique solutions. All aqueous solutions have water as the solvent and are clear(transparent). They may be either coloured or colourless. Although water solu-tions are all different, they have some similarities and can be classified ordescribed in a number of ways. This chapter deals primarily with the character-istics of aqueous solutions.
Properties of Aqueous Solutions
Compounds can be classified as either electrolytes or nonelectrolytes.Electrolytes are solutes that form solutions that conduct electricity. At this pointwe will restrict ourselves to compounds in aqueous solutions. Compounds areelectrolytes if their aqueous solutions conduct electricity. Compounds are non-electrolytes if their aqueous solu-
tions do not conduct electricity.Most household aqueous solutions,such as fruit juices and cleaningsolutions, contain electrolytes. Theconductivity of a solution is easilytested with a simple conductivityapparatus (Figure 4) or an ohm-meter. This evidence also provides adiagnostic test to determine theclass of a solute---electrolyte ornonelectrolyte. This very broadclassification of compounds intoelectrolyte and nonelectrolyte cate-gories can be related to the maintypes of compounds classified inChapter 2. Electrolytes are mostlyhighly soluble ionic compounds
(e.g., KBr,agl), including bases such as
Figure 4ionic hydroxides (e.g., sodium hyd.rox-
The bulb in this conductivity apparatus lights
ide, NaOH(;pct}). Most molecular
up if the solute is an electrolyte.
Figure 2tincture of iodine is a solution of the element
iodine and the compound potassium or sodiumiodide dissolved in ethanol. It is used to pre -
vent the infection of minor cuts and scrapes.
a solute dissolved inwater
Figure 3Concentrated hydrochloric acid soften sold
under its common name, muriatic acid) con-
taints hydrogen chloride gas dissolved in
water. It is used to etch concrete before
painting it, clean rusted metal, and adjust
acidity in swimming peals,
a compound that, in anaqueou utio,n, conducts el ectricity
compound that, in anaqueous solution, does not conduct electricity
Ilse Nature afad Properties of Solutions 267
6.1
1. Carry out your Procedure, recording your observations in a suitableformat.
(d) Using the evidence you have collected in your experiment, answer theQuestion: Which of the white solids labelled 1, 2, 3, and 4 is calcium chlo-ride, citric acid, glucose, and calcium hydroxide?
(e) Evaluate the evidence by critiquing the Experimental Design, Materials,and Procedure. Look for any flaws, sources of error, and possible improve-ments. Overall, how certain are you about your answer to the Question?
Understanding Concepts
1. Classify the following mixtures as heterogeneous or homogeneous.Justify your answers.(a) fresh-squeezed orange juice(b)
(e)
(d)
(e)
(f)
(g)
(h)
(i)
white vinegarred winean antique bronze daggera stainless steel knifean old lead water pipehumid aira clouda dirty puddle
2. Which of the following are solutions and which are not solutions?(a) milk(b) apple juice(c) the gas in a helium-filled balloon(d) pop(e) pure water
(f) smoke-filled air(g) silt-filled water
(h) rainwater(i) 14K gold in jewellery
3. State at least three ways of classifying solutions.
4. (a) What is an aqueous solution?(b) Give at least five examples of aqueous solutions that you can
find at home.
5. Using the information in Table 3, classify each of the compounds aseither an electrolyte or a nonelectrolyte. Provide your reasoning.
6. (a) What types of salutes are electrolytes?(b) Write a definition of an electrolyte.
7. Describe the salutes in the following types of solutions:(a) acidic(b) basic(c) neutral
8. Electrolytes are lost during physical activity and in hot weatherthrough sweating. The body sweats in order to keep cool-cooling by
Table 3
Compound Classmethanol molecular
sodium chloride highly soluble ionic
hydrochloric acid acid (molecular)
potassium hydroxide base (ionic hydroxide)
The Nature and Properties of Solutions 269
GRADE 11 CHEMISTRY • Topic 4: Solutions
SK]LLS AND ATriTUDES OUTCOMES
C11-0-U1: Use appropriate strategies and skills to develop an understanding of chemical concepts.
Exam!es: analogies, concept frames, concept maps, manipulotives, particulate representations, rote-plays, simulations, sort,or.d-predict frames, ward cycles...
C11--R1: Synthesize information obtained from a variety of sources.
In lode: print and electronic spec€atsts, orther resource people
with a small crystal seed placed at the bottom. The crystal solid that results willform a tall column in the beaker if poured slowly. The column. is fragile.
TEACHER NOTES
Most chemical reactions occur in an aqueous medium, and not in the solid, liquid,or gaseous phase. Students should be familiar with the nine types of solutionspresented below and should be able to provide an example for each. Emphasize thatthe smaller amount in a solution is usually classified as the solute and the largeramount the solvent. Ask students to provide examples other than those presentedbelow.
Types of Solutions
Solution Example
solid in solid copper in silver (sterling silver)•
zinc in copper (brass)
solid in liquid salt in water (ocean water)•
iodine in alcohol (tincture)solid in gas microscopic particulates in air
mothball particles in air
liquid in solid mercury in silver amalgams (tooth fillings)*
liquid in liquid •
ethylene glycol in water (engine antifreeze)•
methanol in water (gas line antifreeze)
liquid in gas •
water vapour in air
gas in solid •
hydrogen in palladium** (purification of hydrogen)•
poisonous gases adsorbed in carbon (charcoal filter)
gas in liquid •
carbon dioxide in beverages (carbonated beverages)•
oxygen in water (supporting aquatic life)
gas in gas oxygen in nitrogen (air)
Have students ask their dentists to explain the use of a known carcinogen in an amalgam fororal/dental use.
** At room temperature, palladium will absorb 900 times its own volume of hydrogen.
Journal Writing
Have students relate the demonstration/discrepant event in their journals. Students
could also include their dentists' explanation of the use of a known carcinogen in anamalgam for oral/dental use (as a follow-Lip).
Topic 4: Solutions - 5
Dissolving of Molecular and Ionic Compounds
Sucrose dissolved in water
The dissociation of
sodium chloride
into positive and
negative ions
CQ Copyright 2002 Nelson Thomson Learning
29
Intermolecular Forces and Dissolving
Polar solute molecules (in red) are surrounded by polarsolvent molecules (in green).
H-0:------- H---N-H------- :0-H
H
H
H
:0-H
H
Multiple hydrogen bonds between ammonia and water result ina very high solubility for ammonia.
o Copyright 2002 Ne'son Thomson Learning
28
SOLUTIONS: TYPES OF SOLUTIONS
Objective: Differentiate among unsaturated, saturated, and supersaturated solutions.
Equipment and Chemicals:
Lab Setup:
1. Burner
2. 250 mlbeaker
3. Test tube holder 4. Dropper pipet5. Small test tubes
(3)6. 1- lint striker
7. sodium thiosulfate pentahydratecrystals
Safety:1. Wear safety goggles over your eyes2. Observe all glassware precautions3. Observe all fire precautions4. Clean up all spills immediately5. Rinse affected areas with lots of running water6. Sodium thiosulfate pentahydrate may be harmful if swallowed and may cause
irritation to skin, eyes, and mucous membranes.7. Wash your hands with soap and water after conducting the experiment.
Procedure:
1. Obtain all materials.
2. Label three test tubes A, B. and C.3. Half fill test tube A with sodium thiosulfate pentahydrate crystals. Return to your
lab station.4. Remove 5 crystals and set aside. Pour half of the remaining sodium thiosulfate
pentahydrate into test tube B.5. Place two of the 5 reserved crystals into test tube C.6. Add one half complete dropper pipet of water to each test tube. Drum test tubes
B and C with your fingers to dissolve each solution.7. Clamp test tube A with test tube holders and gently heat in a burner flame for 3 to
5 seconds at a time. Use the proper technique for heating and mixing as describedto you by the instructor.
S. Fill a 250 mL beaker with about 175 mL of cold tap water. Gently place each testtube into the cold water to cool. Wait three minutes. Do not agitate any of thesolutions.
9. One at a time, remove each test tube from the water bath, dry the outside withpaper towel, and insert a single crystal into the solution. Hold the bottom of eachtest tube in your hand. Record your observations.
10. Drum test tubes B and C on your fingers in an attempt to dissolve the crystal.11. Dissolve any solids remaining in the test tubes and rinse down the sink with lots
of water.12. Rinse all remaining glassware with lots of tap water and put all equipment away.
SOLUTIONS: TYPES OF SOLUTIONS
Observations:Test Tube A
Test Tube B
Test Tube C
Questions:1. Identify which solutions are unsaturated, saturated, and supersaturated.
2. Describe the differences between unsaturated, saturated, and supersaturated solutions.
TYPES OF SOLUTIONS LAB RUBRICCriteria Novice Intermediate Exert
Student observes Student does not Student is naggedAll aspects of the
proper safety wear their safety once or more aboutlab are conducted in
precautions goggles or has a lab not following propera safe manneraccident safety precautions
Student follows Evidence that theEvidence that the
written and student has notstudent has not Student follows all
verbal followed more thanfollowed one written
written or verbal
instructions one written or verbalor verbal instruction instructions
instruction
Evidence of Little or no evidence Some evidence hat--a Evidence that all
equitable of equitable group member group members
participation participation by a participated more participatedgroup member than another equitably
More than one pieceEvidence of Entire station is
Lab station is of evidence remainschemicals or a piece cleaned up with no
cleaned up after of chemicals orof equipment remains evidence remaining
lab equipment afterafter cleanup of equipment or
I Cleanup chemicals
I
Solubility Curve of K 03
ObjectiveConstruct a solubility curve of potassium nitra
ChemicalsKNO3
• Tap water
SafetyDo not bum yourself on the hotplate. Be careful with glassware and thermometres.
Equipment•
Test tube
Temperature probe
•
Hotplate•
Test tube
•
10 mL graduated
•
250mL beakersholder
cylinder
(2)•
Dropper pipet
Procedure
1. Set up a water bath by filling a 250 mL beaker with approximately 175 mL of tapwater and carefully placing it on a hotplate. Set the hot plate to high. One groupmember should be consciously monitoring the water bath at all times.
2. Obtain all materials. Boot the computer, launch the software package, and set upthe temperature probe. Press the MON button to activate the sensor.
3. Place clean dry test tube in a clean 250 mL beaker.4. Label the test tube with an indelible marker if you are sharing a water bath.5. Obtain the appropriate mass of potassium nitrate in your test tube, as instructed by
your teacher.6. Fill a clean 10 mL graduated cylinder with 10.0 mL of tap water. Using a dropper
pipet, suction out 2.0 mL of water and add it to the test tube. Be sure to read themeniscus properly as directed by your instructor.
7. Insert the clean dry temperature probe into the test tube.8. Place the test tube with the probe in it into the hot water bath to dissolve the
KNO3. Monitor your solution and the cord to prevent any lab accidents.9. Once your solution has completely dissolved, using a test tube holder remove the
test tube from the water bath with the temperature probe still in it and place in theempty 250 mL beaker. Turn off the hotplate and unplug it. Carefully transportthe beaker and test tube to your lab station.
10. Continuously observe your solution with stirring as it cools, recording thetemperature at which crystals first begin to appear. Record the temperature in thetable below beside your corresponding mass of KNO3.
11. Repeat steps 7 to 9 as many times as possible in order to obtain precise results.12. To clean up, return your test tube and thermometer to the hot water bath. Allow
solutions to dissolve and empty them into the appropriate beaker for recycling.13. Rinse all equipment with lots of water and put it away,
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Solubility Curve of KN03
Quantitative DataMass and Temperature Data or Saturated Potassium Nitrate Solutions
Mass of KNO3 (g) Volume of water (mL) Crystallization Temperature (°C)
Trial 1 Trial 2 Trial 3 Average
1.00
1.50
2.00
2.50
3.00
3.50
4.00
CalculationsShow a sample calculation of the conversion of grams KNO3 per volume of water tograms KNO3 per 100 mL water.
SOLUBILITY CURVE OF KNO 3 LAB RUBRICCriteria Novice Intermediate Expert
Student observes Student does not Student is naggedAll aspects of the
proper safety wear their safety once or more aboutlab are conducted in
precautionsgoggles or has a lab not following proper
a safe manneraccident safety
recautions
Student follows Evidence that thestudent has not Evidence that the
Student follows allwritten andfollowed more than student has not
written or verbalverbalone written or verbal
followed one writtenI
instructionsinstructions or verbal instructioninstruction
Evidence of Little or no evidence Some evidence that a Evidence that all
equitableof equitable group member group members
participation participation by a participated more participatedgroup member than another e uitably
More than one pieceEvidence of Entire station is
Lab station is of evidence remainschemicals or a plea,
cleaned up with nocleaned up after i of chemicals or
of equipment remainsevidence remaining
lab equipment afterafter cleanup of equipment or
cleanup
j 1 chemicals
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Solubility Curve of KNO3
Conclusion1) Construct and hand in a graph of mass of K-N,03 per 100 mL H2O on the y -- axis
versus temperature on the x - axis.2) Draw the curve of best fit.
Questions:
1) Describe the relationship between the solubility of KNO3 and the temperature ofthe solvent.
2) Using your graph, determine how many gram of KNO3 can be dissolved in 100grams of water at the following temperatures:
a) 35°C
b) 60°Cc) 70°C
Predict whether the following solutions of KNO3 would be considered saturated,unsaturated or supersaturated.
a) 75 g of KNO3 in 100 ml waterb) 60 g of KNO3 in 100 ml of water.
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GRADE, 11 CHEMISTRY • Topic 4 Appendices
Solubility Curve
150
140
130
120
0 110T-
a, 100CC7
900)
80C3
° 70
60
0CO
a,
30
20
10
0
50
40
Solubility vs. Temperature for Several Substances
I
IT If}I
NaNO3
7-7I
NH C ,4
.......... ......[I
3
I
VNaCI
KCIO3
Ce2(S 4)3
10 20 30 40 50 60 70 80 90 100
Temperature (°C)
Topic 4 Appendices - 17
SVLUDILIJ-T %;UWVLSAnswer the following questions basedon the s'c blllty curve below.
1. Which salt Is least soluble in water
Name
5a40
30
20
10
0
at 20° C?
2, How many grams of potassiumchloride can be dissolved in 200 gof water at 80° C?
3. At 40° C, how much potassium
nitrate can be d tvedJn 3010. g of
water?
4. Which salt shows the least changeIn solubility from 0° - 100° C?
At 30° C, 90 g of sodium nitrate Is
dissolved in 100 g of water. Is this
solution saturated, unsaturated or
supersaturated?
:1::±^l -] I __M
20 30 40 50 60 70 80 90 100Temperature (0°C)
so
140
6. A saturated-solution-ofpotassium chlorate Is formed from one hundred grams ofwater. If the saturated solution Is cooled from 80° C to 50° C, how many grams ofprecipitate are formed?
7. What compound shows a decrease In solubility from 0° to 100° C?
8. Which salt Is most soluble at 10° C?
9. Which salt is least soluble at 50° C?
Which salt Is feast soluble at 900 C?
hemtstry IF8766
67
Clnstructloncal For. Inc.
Date
Class
Text Reference: Section 16.4
Name
CHAPTER 16 REVIEW ACTIVITY
solubility Curves
Study the solubility curves in the figure, and thenanswer the questions that follow.
1. What relationship exists between solubility
and temperature for most of the substancesshown?
2. a. What is the exception?
b. What general principle accounts for this ex-ception?
3. a. Approximately how many grams of NaNO3will dissolve in 100 g of water at 20°C?
b. How many grams will dissolve at 60°C?
4. How many grams of NH4CI will dissolve in1 dm3 of H2O at 50°C?
5. Ninety grams of NaNO3 is added to 100 g of H2Oat 0°C. With constant stirring, to what temperaturemust the solution be raised to produce a saturatedsolution with no solid NaNO3 remaining?
6. A saturated solution of KC103 was made with300 g of H2O at 40°C. How much KCIO3 could berecovered by evaporating the solution to dryness?
7. Five hundred grams of water is used to make asaturated solution of KCI at 10°C. How many moregrams of KCI could be dissolved if the tem-perature were raised to 100°C?
8. A saturated solution of KNO3 in 200 g of H2O at50°C is cooled to 20°C. How much KNO3 will pre-cipitate out of solution?
COPYRIGHT by Prentice Hill. Inc.Reproduction of this master is restricted to duplication for classroom use only.
CHEMISTRY: The Study of Matter
1&11
1.
2.a.
b.
240
I- 1 11 F" ^. ^ ^ ^ ^. ^ ^, 14-1 1::F;1-1 v
I 1111L.14-11- IAit 111 1111111 11 FVT-111
Poul1tojm Mrs
220
t
S 120
t 1. 1 L t. I f Lorl R
A
= I I I 1 1-1 f-I
I I I H^
k
!0 20 30 40 50 00 70 80 90 ro0
TTrrowa urI ("C)
poeaetiutn SUMAC
Temperature ('C)
,ON
SCIENCE
1. Calculate the maximum number of grams of each solute that can be dissolved:
J) potassium nitrate in 300 cm3
b) sodium chloride in 1250 arts
c) sodium nitrate in 50 cmm
of water at $0` C.
of water at 40' C.
of water at 00 C.
2. Calculate the minimum volume of water needed to dissolve;
'
a) 500 g of sodium chloride
b) 10.0 g of potassium nitrate
c) 1.001cg of sodium nitrate
in water at 100° C.
in water at 0' C.
I
in water at 50° C
3. Calculate the temperature the water must be to just dissolve;
a) $0.0 g of potassium nitrate
b) 60.0 g of potassium nitrate
in 200 cm3 of water.
in 50 cma of water.It
4. Calculate the mass of precipitate in each case below;
a) a saturated solution of sodium nitrate
in 400 cros of water at 100' C is made.The temperature is then changed to 13' C.
Solubility Calculations ........................•.............................................«............
C) 500.0 g of sodium nitratein 500 ems of water.
b) a saturated solution of pota ssium nitrate
in 250 cm3 of water at $0" C is made.The temperature is then changed to 8' C.
Soiubiiiy Chart
Negative Ions Positive Ions Solubility
Essentially All Alkali ions (Li+, Na', K+, Rb+, Cs) Soluble, (aq)
Essentially Al. Hydrogen ion, H+ Soluble, (aq)
Essentially All Ammonium ion, NI-14" Soluble, (aq)
Nitrate, NO3- Essentially All Soluble, (aq)
Acetate,CH3000 Essentially All, EXCEPT Ag Soluble, (aq)
Chloride, Cl" 2+
2+Ag-,Pb
,Hg2
,Cu,TlLow Solubility,
Bromide, Br (s)iodide, I Alt others Soluble, (aq)
Sulfate, SO42-^-
Cat+, Sr2+, Ba2, Pb2+, Ra2+ Low Solubility,(s)
All others
Soluble, (aq)Alkali ions and H+, NH4+, Be +, Mg
Ca2+2+ SL3luble
(a q)( q)s2-lfidRaSr
Ba'
,S e,u
AU others Low Solubility,(s)
Alkali ions and H+, NH4, Sr +, Ba
Ra +, Tl+ Soluble, (aq)Hydroxide, OH-
All others Low Solubility,(s)
Phosphate, Alkali ions and H+, NH4+ Soluble, (aq)P043Carbonate,
All others
I Low Solubility,C03 (s)Sulfite, S032
Chromate, Ba2+, Sr2+, Pb2+, A Low Solubility,
0 2C r 4 f All others Soluble, (aq)
Solubility Rules Worksheet
1. Name or give the chemical formula for each of the followingcompounds.
2. State whether they are soluble (will dissolve) or insoluble (will notdissolve) in solution. Use solubility rules.
Chemical Formula Name Solubility1. NH4CH3COO2. Ba(OH)23. Iron (I1) Carbonate4. NaOH5. RbNO36. Cesium Sulfate7.MSO48. ZnC129. Zinc HydroxideI O.Zn3(P04)211.AgBr12.KNO313.A12S314. Silver Acetate15.S r2C rO416. Alunninur Phosphate
17.BaSO418.Ca(OH)219.BaCO320.MgCrO421. Iron (111) sulfide22.NH4CN23. Silver Iodide24.Hg2SO425. Lithium Chloride
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Writing Balanced Ionic Equations for Precipitate Reactions
Write the balanced dissolving ionic (DIE), overall ionic (OIE), and the net ionicequations (NIE) when:
I. a solution of silver nitrate is mixed with sodium iodide solution.
2. solutions of potassium chromate and strontium bromide combine.
3. an ammonium hydroxide solution is mixed with a solution of copper (I) chromate.
4. aqueous lithium sulphate combines with dissolved calcium iodide.
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Solubility Rules Lab
Objectives1. Examine the solubilities of pairs of ionic solutions in double displacement
reactions.2. Write balanced dissociation., overall ionic, and net ionic equations for precipitate
reactions.3. Verify the solubility rules.
Lab Setup
1. Paper towel
2. Aqueous solution of ions3. Watch glass 4. Tap water5. Glass stir rod
Chemicals1. 0.1 M AgNO3(aq)
4. 0.1 M Fe(N03)3(aq)
2. 0.5 M Pb(N03)2(aq) 3. 0.5 M K2Cr04(aq)5. 6.0 M NaOH(aq)
6. 0.5 M NaI(aq)
Safety• Wear safety goggles over your eyes at all times during the experiment• Clean up all spills immediately with copious quantities of tap water• Rinse affected areas with copious quantities of running tap water• All solutions are poisonous, AgNTO3 permanently stains skin and clothing dark brown,
and NaOH is corrosive, so observe appropriate precautions
Procedure1. Into a clean, dry watchglass, add two drops of your solution.2. Combine your solution with two drops of another solution. Mix with a clean, dry
stir rod. Record your observations.3. repeat steps I and 2 until you have combined your solution with every other
solution.4. Rinse all glassware with copious quantities of tap water, dry all equipment, and
return it to its original location.
Solubility Rules Lab
Data & Observations
Solution &Observation
BalancedDissociation
Eq uation
I Cations do NOTdissolve withthese Anions
Anions do NOTdissolve withthese Cations
12.
3
4.
5.f
[
3
6.
Balanced DIE, OIE, NIE
ConclusionExplain how the results of the experiment verify the solubility rules.
Molarity Practice Problems1) How many grams of potassium carbonate are needed to make 200 mL of a
2.5 M solution?
2) How many liters of 4 M solution can be made using 100 grams of lithiumbromide?
3) What is the concentration of a 450 mL solution that contains 200 grams of iron(Il) chloride?
4) How many liters of 0.88 M solution can be made with 25.5 grams of lithiumfluoride?
5) What is the concentration of a solution that has a volume of 2.5 L andcontains 660 grams of calcium phosphate?
6) How many grams of copper (II) fluoride are needed to make 6.7 liters of a 1.2M solution?
Making Solutions Practice Problems
Explain how you would make the following solutions. Your answer should be astatement, not just a number.
7) 2Lof6MHC1
8) 0.75 L of 0.25 M Na2SO4
9) 250 mL of 0.75 M lithium nitrite
10) 4.5 mL of 0.05 M magnesium sulfate
11) 90 mL of 1.2 M BF3
.Making a Solution Lab
Before you begin to obtain glassware and chemicals,know that EACH member of the group must check inwith Mr. Deakin 3 times during this experiment.
1. Show me your complete answer, including yourstatement - to the prompt:Explain how to make a 100.00 mL solution of 0.20
mol/L potassium nitrate.
2. Show me your dissolved solution BEFORE youpour it into the volumetric flask.
3. Show me how you lined the meniscus up with thegraduation mark on the neck of the volumetricflask BEFORE you invert and mix your solution.
Dilutions Practice Problems
12) if I have 340 mL of a 0.5 M NaBr solution, what will the concentration be if Iadd 560 mL more water to it?
13) If I dilute 250 mL of 0.10 M lithium acetate solution to a volume of 750 mL,what will the concentration of this solution be?
14) If I leave 750 mL of 0.50 M sodium chloride solution uncovered on awindowsill and 150 mL of the solvent evaporates, what will the newconcentration of the sodium chloride solution be?
15) To what volume would I need to add water to the evaporated solution inproblem 3 to get a solution with a concentration of 0.25 M?
DILUTING A SOLUTION LAB
Purpose:Prepare a 0.016 mol'L solution from 100.00 mL of 0.20 mol/L stocksolution of potassium nitrate.
Chemicals & Equipment:• 100.00 mL of 0.20 mol/L potassium nitrate
• Droppersolution
pipet• 150 mL beaker
• 50 mL beaker• Distilled water
• Funnel• 10 mL graduated cylinder
Procedure:1. Obtain all chemicals and equipment.2. Empty all of 0.20 mol /L stock solution into a 150 mL beaker.3. Rinse the volumetric flask 3 times with very small amounts of
distilled water. Fill 1/3 full with distilled water and set aside.4. Fill a 10.0 mL graduated cylinder with the correct amount of stock
solution. Use a dropper pipet to obtain a precise amount.5. Check your work with the instructor before moving on to the next
step.6. Pour the solution from the graduated cylinder into the volumetric
flask.7. Fill to just under the calibration mark.8. Put a very small amount of distilled water into a 50 mL beaker and
use the dropper pipet to rill the volumetric flask to the calibrationmark.
9. Stopper your solution and check with your instructor.10.Invert the solution 3 times to mix.11. Rinse all remaining solutions down the drain with lots of running
water, rinse remaining and put everything away.
DILUTING A SOLUTION LAB
Before you begin to obtain glassware and chemicals, EACHmember of the group must check in with Mr. Deakin 3 timesduring this experiment.
1. Show me your complete answer, including your statement-- to the prompt:Explain how to make a 100. 00 mL solution of 0.016 mol1L
potassium nitratefrom a 0.20 mol/L stock solution.
2. Show me a volumetric flask 1/3 full of water and agraduated cylinder filled with 10.0 mL of 0.20 mol/Lstock solution.
3. Show me how you lined the meniscus up with thegraduation mark on the neck of the volumetric flaskBEFORE you invert and mix your solution.
LUTING A SOLUTION LAB RumCriteria Novice Intermediate Expert
Student observes Student does not wear Student is nagged onceAll aspects of the lab
proper safety their safety goggles or or more about notfollowing proper safety are conducted in a safe
precautions has a lab accident mannerprecautions
Student follows Evidence that theEvidence that the
written and student has notstudent has not Student follows all
verbal followed more than onefollowed one written or written or verbal
[
instructions written or verbalverbal instruction instructions
iinstruction
Evidence of Little or no evidence of Some evidence that aEvidence that all
equitable equitable participation (Yroup membergroup members
participation by a group member participated more thanparticipated equitably
another[
M th i Entire station isLab station is
fore an one p ece oevidence remains of Evidence of chemicals cleaned up with no
cleaned up afterchemicals or equipment or a piece of equipment evidence remaining of
labafter cleanup remains after cleanup
? equipment orchemicals
Answers
2. 7.5% WV
3. 32% WN
4. 4.8% W;'W
5.8 mg
6. 5.4 ppm
7. (a) 1/1000
(c) 30µg
8. 1.8 mol/L
Understanding Concepts
1. What are three different ways of expressing the concentration of asolution?
2. Gasohol, which is a solution of ethanol and gasoline, is considered tobe a cleaner fuel than just gasoline alone. A typical gasohol mixtureavailable across Canada contains 4.1 L of ethanol in a 55-L tank offuel. Calculate the percentage by volume concentration of ethanol.
3. Solder flux, available at hardware and craft stores, contains 16 g ofzinc chloride in 50 mL of solution. The solvent is aqueous hydrochloricacid. What is the percentage weight by volume of zinc chloride in thesolution?
4. Brass is a copper-zinc alloy. If the concentration of zinc is relativelylow, the brass has a golden colour and is often used for inexpensivejewellery. If a 35.0 g pendant contains 13 g of zinc, what is the per-centage weight by weight of zinc in this brass?
5. If the concentration of oxygen in water is 8 ppm, what mass ofoxygen is present in 1 L of water?
6. Formaldehyde, CH2Orgi, is an indoor air pollutant that comes fromsynthetic materials and cigarette smoke. Formaldehyde is controver-sial because it is a probable carcinogen. If a 500-L indoor air samplewith a mass of 0.59 kg contained 3.2 mg of formaldehyde, this wouldbe considered a dangerous level. What would be the concentration offormaldehyde in parts per million?
7. Very low concentrations of toxic substances sometimes require theuse of the parts per billion (ppb) concentration.(a) How much smaller is 1 ppb than 1 ppm?(b) Use the list of equivalent units for parts per million to make a
new list for parts per billion.(c) Copper is an essential trace element for animal life. An average
adult requires the equivalent of a litre of water containing 30 ppbof copper a day. What mass of copper is this per kilogram ofsolution?
8. A plastic dropper bottle for a chemical analysis contains 0.11 mol ofcalcium chloride in 60 mL of solution. Calculate the molar concentra-tion of calcium chloride.
Making Connections
9. Toxicity of substances for animals is usually expressed by a quantitydesignated as "LDse." Use the Internet to research the use of thisquantity. What does LDS0 mean? What is the concentration in ppm fora substance considered "extremely toxic" and one considered"slightly toxic"?Follow the links for Nelson Chemistry 11, 6.3.
Reflecting
10. How is your report card mark in a subject like a concentration? Whatother ratios have you used that are similar to concentration ratios?
Calculations Involving ConcentrationsSolutions are so commonly used in chemistry that calculating concentrationsmight be the primary reason why chemists pull out their calculators. In associ-ated calculations, chemists and chemical technicians also frequently need to cal-
284 Chapter 6
6.3
Figure 5Aqueous ammonia is purchased for sciencelaboratories as a concentrated solution. Whatis the concentration of the solute?
14.8 viol
IL
2,5 L
2.5x 14.8 motI l
?z%" n = 37 mcl
The amount of ammonia present in the bottle is 37 mol.
You should always check that your answer makes sense. For example, inSample Problem 8, 14.8 mol/L means that there is 14.8 mol of ammonia in 1 Lof solution. Therefore, 2.5 L, which is greater than I L, must produce an amountgreater than 14.8 mol.
In some situations you may know the molar concentration and need to findeither the volume of solution or amount (in moles) of solute. In these situationsuse either the volume /amount or amount /volume ratio. Notice that the units ofthe quantity you want to find should be the units in the numerator of the con-version factor ratio.
What volume of a 0.25 mot/L salt solution in a laboratory contains 0.10 mol ofsodium chloride?
0,25 molI L
CN
nhaC1 = 0.10 mal
VNaCl ° 0.10IL
.25 pibtX
VivaCl ^ 0.40 L
You need 0.40 L of salt solution to provide 0.10 mol of sodium chloride.
Understanding Concepts11. Rubbing alcohol, C3H7QH,,), is sold as a 70.0% V/V solution for
external use only. What volume of pure C3H70HM is present in a 500-mL (assume three significant digits) bottle?
12. Suppose your company makes hydrogen peroxide solution with ageneric label for drugstores in your area. What mass of purehydrogen peroxide is needed to make 1000 bottles each containing250 mL of 3.0% WA' H202^agr?
13. The maximum acceptable concentration of fluoride ions in municipalwater supplies is 1.5 ppm. What is the maximum mass of fluorideions you would get from a 0.250-L glass of water?
Answers
11. 0.350 L
12. 7.5 kg
13. 0.38 mg
The Nature arnd Properties of Solt{ tions 287
CONCENTRATION QUESTIONS
1, Toothpaste contains 0.24 % w/ww, of sodium fluoride. If 0.50 g of toothpaste issqueezed onto a toothbrush, what mass of sodium fluoride is used'? (0.0012 g)
2. Zinc oxide is the main ingredient in sunscreen. A premium brand advertises itssunscreen contains 10 % w/v of zinc oxide. What size bottle contains 23 grams ofzinc oxide? (230 mL)
3. The maximum contaminant level of lead in drinking water is 15 ppb. Assuming awater source has 15 ppb of lead, what mass of lead are you drinking if youconsume 2 L of water a day? If lead accumulates in the fat cells of your body,how many grams of lead are in your body after 1 year? (3 x 10-5 g, 0.01095 g)
4. Tincture of iodine is used as a disinfectant for boo-boos. If 25 mg/mL ofpotassium iodide is dissolved in a bottle of iodine tincture, what percent by massis the solution? (2.5 % w/v)
5. Joanne drinks water containing 0.08 g of dissolved minerals. What concentrationin parts per million of minerals is present in a 500 mL bottle of water? (160 ppm)
DILUTION QUESTIONS
6. Natalie likes to feed the humming birds in her garden. If she dissolves 12 g of
fructose - chemical formula CoHi2O6 - in 250 mL of water, what is theconcentration of her sucrose solution? (0.27 moUL)
7. If humming birds are partial to a O.10 M solution of fructose and Natalie's birdfeeder only holds 100 mL of solution, how much of her original solution must shedilute to make a new 0.10 M solution? (37 mL)
Limiting Factor Questions
For each of the following pairs of solutions,a) write the balanced dissolving equations
b) write the balanced overall ionic equationc) write the balanced net ionic equation
d) calculate the concentrations of all ions in solutione) calculate the mass of the precipitate
125 mL of 0.25 M barium iodide solution and 75 mL of 0.10 M sodium sulfatesolution are mixed.
2. Two solutions containing 200 mL of 0.15 M strontium chloride and 150 mL of 0.09 Mpotassium chromate are mixed.
3. 225 mL of 0.5 M silver nitrate solution and 275 mL of 0.12 M lithium iodide solutionare mixed.
4. Two solutions containing 150 mL of 0.15 M lithium chloride and 150 mL of 0.10 Mlead (II) acetate are mixed.
5. A 50 mL solution of magnesium nitrate with a concentration of 0.20 M is combinedwith 100 mL of 0.15 M rubidium hydroxide.
6. 100 mL of 0.10 M ammonium phosphate solution is mixed with 200 mL of 0.12 Msilver nitrate solution.
7. A 150 mL solution of potassium hydroxide with a concentration of 0.40 M iscombined with 100 mL of 0.15 M aluminum acetate.
Two solutions containing 100 mL of 0.10 M sodium carbonate and 200 mL of 0.10 Maluminum chloride are mixed.
www.pembinatrails.ca/shaftesbury/mrdeakin -J adeakin(gpembinatrails.ca2 (204) 888-5898
Shaftesbury High School, 2240 Grant Ave, Winnipeg, MB, R3P 0P7