1.1 Lab Safety Highlights

#1 Don't know what you're doing? Check the pre

ask your partners, and then ask me.

alone in lab!

#2 No food / drink in lab. We use toxic chemicals daily

and the tables are never truly "safe".

#3 Goggles and tennis shoes are worn for ALL labs.

Aprons and gloves are sometimes required.

#4 Accident? Inform me immediately,

no matter how big or small.

#5

1.1 Lab Safety Highlights

~ 1 ~

know what you're doing? Check the pre

ask your partners, and then ask me. Never work

No food / drink in lab. We use toxic chemicals daily

tables are never truly "safe".

Goggles and tennis shoes are worn for ALL labs.

Aprons and gloves are sometimes required.

Inform me immediately,

no matter how big or small.

Follow lab procedures for

chemical disposal. Not everything

can safely (or legally) be trashed

or washed down the drain.

Safety Highlights

know what you're doing? Check the pre-lab,

Never work

No food / drink in lab. We use toxic chemicals daily

Goggles and tennis shoes are worn for ALL labs.

Not everything

an safely (or legally) be trashed

#6 Hot and cold don't mix in lab (esp. in glass!)

#7 Acid into water = ok // Water into acid = boom!

#8 Pretend test tubes are bazookas,

point away from people and

towards cabinets.

#9 Don't return "used" chemicals into clean containers.

A chemical is contaminated the moment it leaves its

storage bottle.

#10 Got chemicals (on you?)

water, especially if in your eyes! Failure to do so

could result in a life of piracy or your assimilation

into the collective.

Yarrr! Resistance be futile!

~ 2 ~

Hot and cold don't mix in lab (esp. in glass!)

into water = ok // Water into acid = boom!

Pretend test tubes are bazookas,

point away from people and

towards cabinets.

Don't return "used" chemicals into clean containers.


Got chemicals (on you?) Wash for 20 min with cold



into the collective.

Yarrr! Resistance be futile!

into water = ok // Water into acid = boom!

Don't return "used" chemicals into clean containers.


with cold



#11

and clear the area of both people and

materials. Refer to #12 and #13

#12 Don't assume that water will put out a fire, it might

make it worse. Sand is great for smaller fires, but

the CO2 fire extinguishers in the lab are best overall.

Pull the pin, aim at the base of the fire,

trigger (hang on tight!)

#13 Fire blankets are for people! Fire extinguishers are

for everything else!

~ 3 ~

Don't panic! Fires in

lab occur frequently,

often intentionally.

Should an accidental

fire occur, inform me

area of both people and flammable

Refer to #12 and #13 below.

Don't assume that water will put out a fire, it might

Sand is great for smaller fires, but

fire extinguishers in the lab are best overall.

Pull the pin, aim at the base of the fire, squeeze the

trigger (hang on tight!) and sweep from side to side.

Fire blankets are for people! Fire extinguishers are

for everything else!

Don't panic! Fires in

occur frequently,

often intentionally.

ccidental

, inform me

flammable

Don't assume that water will put out a fire, it might

Sand is great for smaller fires, but

fire extinguishers in the lab are best overall.

squeeze the

and sweep from side to side.

Fire blankets are for people! Fire extinguishers are

Common Hazard

Hazard - something harmful or dangerous

Acute Toxicity - immediately poisonous, avoid all

direct contact.

Oxidizing - will react violently with fuel sources such

as organic materials (paper, sugar, skin) and metals.

Corrosive - literally means "having little teeth". Eats

away at other materials.

examples of corrosive materials.

~ 4 ~

Common Hazard Symbols and their Meanings:

something harmful or dangerous.

immediately poisonous, avoid all

will react violently with fuel sources such


literally means "having little teeth". Eats

away at other materials. Acids and bases are good

examples of corrosive materials.

and their Meanings:

immediately poisonous, avoid all

will react violently with fuel sources such


literally means "having little teeth". Eats

Acids and bases are good

~ 5 ~

~ 6 ~

Directions: using the diagram on the previous page,

briefly correct 10 of the mistakes shown.

Ex.1) Use a ladder or taller person to reach high shelves.

Ex.2)

Ex.3)

Ex.4)

Ex.5)

Ex.6)

Ex.7)

Ex.8)

Ex.9)

Ex.10)

~ 7 ~

Identify and sketch each of the following:

Beaker Erlenmeyer Flask

Heating Storing

Storage Mixing

Mixing

Graduated Cylinder ` Crucible

Measuring High temp,

volume Heating

(Coarse)

Mortar/Pestle Wire Gauze/Mesh

Mixing Support,

Grinding Distribute

heat

Beaker Tongs Crucible Tongs

Insulated, High temp,

Transfer Transfer

beakers materials

1.2 Lab Equipment and Glassware

~ 8 ~

Tirrill Burner Forceps

Heating Transfer

(High) (Solids)

Scoopula Burette

Transfer Measuring

(Solids) volume

(Fine)

Pipette Watch Glass

Transfer Splatter

(Liquids) shield

Iron Ring Volumetric Flask

Support Precise mixing

(High heat) (chem + H2O)

~ 9 ~

Pre-Labs:

• You will notified of labs 2-3 days in advance and the

details will be posted online at least 24 hours prior.

• Take the time to read through the procedure.

In-Labs:

• Goggles and closed-toe shoes (tennis shoes) are

required in the lab area at all times.

Inform me and step out if you need to adjust/clean.

• Tie back long hair, remove jewelry on wrists, roll

long sleeves back to elbows.

• Record data and observations as you work, not after

the lab. This prevents massive errors later!

Post-Labs:

• Clean, dry, and return all equipment. Tuck in stools.

Leave the area clean and organized- always!

1.3 Lab Investigation and Measurement

Measuring Volume:

half-moon shape known as a

containers. This effect becomes more powerful in

narrow glassware (ex. water in straws):

Volume is always measured from the bottom of the

meniscus, not the edges.

eyes up if you want accurate results!

Ex.1) Estimate the volume of fluid in each of the following

graduated cylinders:

_______ mL

~ 10 ~

Measuring Volume: most liquids naturally form a

moon shape known as a meniscus in their


narrow glassware (ex. water in straws):


meniscus, not the edges. Take a knee and line your

eyes up if you want accurate results!

the volume of fluid in each of the following

graduated cylinders:

_______ mL _______ mL

liquids naturally form a

in their



Take a knee and line your

the volume of fluid in each of the following

_______ mL

~ 11 ~

Ex.2)

________ mL ________ mL

Accuracy vs. Precision

In science, accuracy is used to describe how close to

the actual answer (truth) a result may be, while

precision describes how close your results are to

one another. Precision measures whether results

are reproducible, accuracy measures correctness:

~ 12 ~

Ex.3) Describe the following data sets as accurate,

precise, both, or neither:

4.5 3.4 2.9 12.0 11.8 12.2

3.6 5.0 3.8 11.9 12.1 12.3

Average = 3.86 Average = 12.1

Actual = 3.90 Actual = 12.0

Ex.4) How would you classify each of the following data

sets? Accurate, precise, both, or neither?

1202 g 980 g Average: 1081

1400 g 740 g Actual: 670

0.98 mL 1.00 mL Average: 0.988 mL

1.01 mL 0.96 mL Actual: 1.40 mL

0.011 kg 0.020 kg Average: 0.016 kg

0.014 kg 0.017 kg Actual: 0.0155 kg

~ 13 ~

Ex.5) In glassware, more graduations (lines) tends to

equal greater precision. Knowing this, compare a

beaker, buret, and graduated cylinder in terms of

precision. Which is highest? Lowest?

Ex.6) In lab, you use several different balances to

measure the mass of a sample of gold metal. You

record the results as 4.91 g, 5 g, and 4.9065 g.

Which result is more precise, and why?

~ 14 ~

SDS, or safety data sheets, contain detailed

information on how to safety use and dispose of

chemicals in the lab. Specific dangers, or hazards,

are found here and will be included in your pre-labs.

Pay close attention!

Safety Diamonds (also known as NFPA codes)

summarize the risks associated with the substances

we use and can be found in SDS as well as on the

labels of most chemical containers.

Hazard Level:

0 - None

1 - Low / Slight

2 - Hazardous

3 - High / Danger

4 - Lethal/Extreme

(Above: Color the NFPA Code / Safety Diamond)

1.4 SDS and Safety Diamonds

~ 15 ~

Each section of a safety diamond is color-coded by

the type of hazard:

• Blue: Health (Poison / Toxicity)

• Red: Fire (Flammability)

• Yellow: Reactivity (Unstable / Explosive)

• White: Special hazards (Radioactive, etc)

Ex.1) So, the safety diamond on the previous page

indicates that this substance is ....

Ex.2) Gasoline is a relatively stable chemical and is mildy

toxic by exposure. Predict and draw the safety

diamond below:

Ex.3) Pure nicotine ( the addictive component of tobacco)

is coded as H-4, F-1, R-0. Interpret this code:

Ex.4) Pure sodium metal reacts powerfully with water,

creating an intense flame and can make you ill if

consumed in moderate quantities. Predict the

hazard ratings for this substance and sketch a

possible safety diamond:

~ 16 ~

Pure sodium metal reacts powerfully with water,




possible safety diamond:

Pure sodium metal reacts powerfully with water,




Ex.5) Nitric acid has the fire code shown

at right. Name two precautions

(preventive measures) necessary to

handle this substance:

Ex.6) When working with open flames and heat, which 2

color codes are most important / relevant?

Blue / Red / White / Yellow

Ex.7) Diborane has the safety diamond shown below.

Suggest 5 precautions which should be taken or

"things to avoid" when handling this chemical:

~ 17 ~

Nitric acid has the fire code shown

at right. Name two precautions

(preventive measures) necessary to

handle this substance:

When working with open flames and heat, which 2

color codes are most important / relevant?


Diborane has the safety diamond shown below.



When working with open flames and heat, which 2


Diborane has the safety diamond shown below.



~ 18 ~

Also known as SI notation, we use scientific /

exponential notation to write very large and very

small numbers in a shorter, more convenient form.

For example, Avogadro's number is given as :

602,200,000,000,000,000,000,000 per mol

Instead of writing it out, we shorten it down to:

6.022 x 1023

or 6.022e23

To create SI notation, move the decimal of a

number until only ONE non-zero digit is in front of

the decimal. The number of times you have to

move the decimal and the direction determine the

power of ten. Left = + Right = -

7000 = 7 x 103 0.00007 = 7 x 10

-5

You can shorten this using exponential notation:

2.54 x 106 = 2.54e6 6.6 x 10

-34 = 6.6e-34

1.5.1 Introduction to Sci/Expo Notation

~ 19 ~

Convert each of the following "expanded" large

numbers into SI notation by moving the decimal left:

Ex.1) 430 =

Ex.2) 14509000 =

Ex.3) 2540000 =

Ex.4) 8300000000000000000 =

Convert the following "expanded" small numbers

into SI notation by moving the decimal right:

Ex.5) 0.0005 =

Ex.6) 0.69 =

Ex.7) 0.000000078 =

Ex.8) 0.041 =

~ 20 ~

There are six major "landmarks" in exponential

notation which will allow you to better understand

the sizes of the numbers with which you work:

e3 = thousands e-3 = thousandths

e6 = millions e-6 = millionths

e9 = billions e-9 = billionths

Knowing these, you can infer the units in between...

Ex.1) e4 Ex.4) e-2

Ex.2) e8 Ex.5) e1

Ex.3) e-5 Ex.6) e2

...which allows you to easily translate expo notation

back into expanded numbers.

Ex. 1.2e3 = 1.2 thousand = 1200

1.5.2 Using Landmarks in Sci-Expo Notation

~ 21 ~

Convert the following into expanded form:

Ex.7) 4.5e2 =

Ex.8) 7.21e-5 =

Ex.9) 1e-8 =

Ex.10) 4.38e6

Ex.11) 9e-4

Ex.12) 3.5e3 =

~ 22 ~

Find the button on your TI-Nspire labeled EE in the

bottom left corner of the calculator. This is what we

use to get the "e" used in exponential notation.

Using your Nspire, convert the following back into

their expanded forms:

Ex.1) 7.6e-3 →

Ex.2) 7.6e3 →

Ex.3) 1e6 →

Ex.4) 9.3e-4 →

Ex.5) 2.00e2 →

Ex.6) 1e-1 →

Ex.6) 7.89e5 →

1.5.3 Using Sci/Expo Notation on a TI-Nspire

~ 23 ~

In science, the way a number is written indicates

both the size and precision of that number. The last

digit in a number is said to be uncertain, meaning

that its value could be one more or less than what is

shown. For example, the number "three" could be

written as shown with the following meanings:

Written as... 3 3.0 3.00

Precision: Low Med Higher

Uncertainty: 3 ± 1 3.0 ± 0.1 3.00 ± 0.01

Range: 2 - 4 2.9 - 3.1 2.99 - 3.01

More digits = more precise = less uncertain

When you make measurements in lab, your

precision is limited by the quality of the equipment

used. The scales used in year 1 measure mass out

to two decimal places (ex. 54.06 g), while analytical

scales used in AP/IB chemistry work out to four or

more (ex. 54.0597 g). Similarly, graduated cylinders

are far superior to beakers for measuring volume.

1.6.1 The Role of Rounding in Science

When these measurements are used to make

calculations, your answer cannot be more precise

than the measurements used to create it:

+

(35 ml)

(Imprecise) + (Precise)

In this chapter, you'll learn to round your answers

like a true scientist using the concept of

figures or "sigfigs

us in deciding the precision of our answers and will

often keep you from having to write

long numbers that are sometimes given by the

calculator.

~ 24 ~


our answer cannot be more precise

than the measurements used to create it:

= 47.55 ml

(12.55 ml) 48 ml

(Imprecise) + (Precise) = Imprecise total


like a true scientist using the concept of significant

sigfigs". The rules for sigfigs help guide


often keep you from having to write the ridiculously



our answer cannot be more precise

47.55 ml

Imprecise total


significant

". The rules for sigfigs help guide


the ridiculously


~ 25 ~

Significant figures, or "SigFigs", are a system of

rounding based on the precision of measurements

made in lab. The basic rules are below:

• Non-zero numbers are always significant:

589 = 3 significant figures

298,741 = 6 significant figures

• Zeros are significant based on the following:

"Leading" "Between" "Trailing"

- Leading zeros (placeholders) are never significant

- Zeros between numbers are always significant.

- Trailing zeros are only significant if a decimal is

present somewhere (anywhere) in the number.

1.6.2 Identifying Significant Figures

000 ## 000 ## 000

~ 26 ~

Ex.1) Label the zeros in each of the following as leading,

trailing, or between (L, T, or B):

450 0.0023 0.00230

5,800,600 0.000008

360. 90.08 0.06070

Ex.2) How many sigfigs are present in each of the

numbers in Ex.1?

Ex.3) Determine the number of sigfigs in the following:

1,000,000.

3,450 754,230

~ 27 ~

Ex.4) How many sigfigs are present in the following?

0.9000 0.00310 7.6080

1,000,000 0.004500

In SI notation, the same rules apply for sigfigs.

However, the 10 and its power do NOT count as

they represent "placeholder zeros".

Ex.5) Determine the number of significant figures in each

of the following numbers:

5.6090 x 10-10

2.750e10

3.61e120 105 x 10-9

1.9000 x 1024

8.3e-6

~ 28 ~

In science, your answer can only be as precise

(significant) as the measurements used to calculate

it. You will often need to round answers.

Round the numbers below to the listed number of

sigfigs.

Ex.1) (5 sigfigs) 12847.9 →

(4 sigfigs) 12847.9 →

(3 sigfigs) 12847.9 →

(2 sigfigs) 12847.9 →

(1 sigfig) 12847.9 →

Ex.2) Convert the final 3 answers to Ex.1 into SI notation.

Ex.3) (4 sigfigs) 0.080725 →

(3 sigfigs) 0.080725 →

(2 sigfigs) 0.080725 →

(1 sigfigs) 0.080725 →

1.6.3 How to Round with Sigfigs

~ 29 ~

For really large or small numbers, you'll find it easier

to convert your answer into SI notation before

rounding. I typically do this for anything larger than

1000 or smaller than 0.001.

Ex.4) 2830067 →

(6 sigfigs) 2830067 →

(5 sigfigs) 2830067 →

(4 sigfigs) 2830067 →

(3 sigfigs) 2830067 →

(2 sigfigs) 2830067 →

(1 sigfig) 2830067 →

Ex.5) 0.00007601329 →

(6 sigfigs) 0.00007601329 →

(5 sigfigs) 0.00007601329 →

(4 sigfigs) 0.00007601329 →

(3 sigfigs) 0.00007601329 →

(2 sigfigs) 0.00007601329 →

(1 sigfig) 0.00007601329 →

~ 30 ~

When adding or subtracting, round your answer to

the lowest amount of decimal places used. All

digits, including 0, after a decimal count as a

decimal place.

120.09 → (2 decimal places)

- 45.2 _ → (1 decimal place)

= 74.89 → Round to 1 decimal, so 74.9

Ex.1) 809 + 1.523 = 810.523 →

Ex.2) 0.854 + 10.9 = 11.754 →

Ex.3) 134.2 + 250.943 = 385.143 →

Ex.4) 12 + 24.4 = 36.4 →

Ex.5) 6.00167 + 0.92 - 4.2095 = 2.71217 →

Ex.6) 45.67 - 12.091 + 89.00154 = 122.58054 →

1.6.4 Rounding When Adding/Subtracting

~ 31 ~

When multiplying or dividing, round your answer to

the lowest number of sigfigs used.

0.0049 x 560.3 = 2.74547 → 2.7

(2 sigfigs) (4 sigfigs) → (Round to 2 sigfigs)

Ex.1) 855 x 0.90 = 769.5 →

Ex.2) 9180. x 0.4 = 3672 →

Ex.3) 4.2 / 23.00 = 0.182608695 →

Ex.4) 4507.3 / 2.31 = 1951.08225 →

Ex.5) (70.30)(0.50040) = 35.17812 →

Ex.6) 0.00860 / 0.00133 x 1.7 = 10.99248 →

Ex.7) (3.00e8) / (4.7e6) = 63.829787 →

1.6.5 Rounding when Multiplying/Dividing

~ 32 ~

Lab calculations can often involve multiple steps.

When doing so, follow the order of operations and

any time you switch from one set of rules (mult/div)

to another (add/sub), round first. If no " rule

switching" occurs, you can round at the end.

Ex.1) 1.4 + 17 x 120.4 =

Ex.2) 90.3 x 5.6 / 4.51 =

Ex.3) 2.0 + 14.56 - 0.135 =

Ex.4) (1.2 • 0.196) / (0.500)(228.2 + 273) =

Ex.5) 9.503 • (12.1 - 3.45) + 14.391 =

1.6.6 Multi-Step Calcs and Constants

~ 33 ~

Constants and whole number values do not

contribute to sigfigs when rounding.

Ex.6) In lab, you measure the mass of a platinum strip 3

times, recording it as: 12.14 g, 11.9 g, and 12.098 g.

Calculate the average mass:

Ex.7) The wavelength of light is found by dividing the

speed of light by its measured frequency. If the

speed of light is a constant at 3e8 m/s and the

frequency is found to be 5.790e17, what is the

wavelength?

~ 34 ~

In chemistry, we use dimensional analysis, or DA, to

solve a variety of complex problems. To do so, we

use conversion factors (something = something

else) to "swap" labels. The goal is to create a new

number with different dimensions - but still equal in

value to the original number and dimension.

Ex.1) Let's say that I asked you to determine the number

of seconds in 2.5 minutes.

What is our starting dimension/label? ___________

Give the relationship between minutes and seconds.

This will be our conversion factor:

__________ minutes = _________ seconds

(DA)

=

1.7.1 Introduction to Dimensional Analysis

~ 35 ~

Ex.2) Calculate the number of nickels found in $6.35:

=

Ex.3) How many minutes are contained by 8.5 hours?

=

Ex.4) If 1 mol of carbon (1 mol C) has a mass of 12.011 g,

what is the mass of 82.3 mol C?

=

~ 36 ~

Ex.5) A kilogram (kg) is equal to 2.2 pounds (lbs). What is

my mass in kilograms if I weigh 285 lbs?

=

Ex.6) Tablespoons (tbsp) and milliliters (mL) are both

ways of measuring volume. If 1 tbsp = 14.8 mL, how

many tbsp are found in a 354 mL bottle of cough

syrup?

=

Ex.7) 2.54 cm (centimeters) = 1 inch. If my height is 76

inches, what is this in cm?

=

~ 37 ~

Most problems will require you to use multiple

conversion factors, not just one. In these instances,

you will first need to find a "path" from your current

label to the one you desire:

Ex.1) Days to minutes:

Ex.2) Seconds to weeks:

Ex.3) Inches to yards:

Once you've found a path, create a DA using labels

ONLY, such that the labels cancel to give the final

unit.

Ex.4) Days to minutes:

Ex.5) Seconds to weeks:

1.7.2 Multi-Step Dimensional Analysis

~ 38 ~

Ex.6) Inches to yards:

Once you have the labels in place, add in the

conversion factors and solve!

Ex.7) 140 months would be equal to ________ centuries:

=

Ex.8) How many seconds are in a year?

CFs: 1 year = 365.25 days 1 day = 24 hours

1 hour = 60 min 1 min = 60 s

=

~ 39 ~

Ex.9) My truck gets about 22 miles per gallon. If gas

costs $2.50 per gallon, how much would it cost me

to drive to my parent's house in Minneapolis if it is

1105.8 miles away?

=

Ex.10) How much of a week is contained in 2.0 seconds?

=

~ 40 ~

The metric system and its prefixes form a sort of

"universal language" for scientists worldwide. You

will want to memorize the base units and prefixes!

nano (n) a billionth 1e-9 or 0.000000001

micro (µ) a millionth 1e-6 or 0.000001

milli (m) a thousandth 1e-3 or 0.001

centi (c) a hundredth 1e-2 or 0.01

deci (d) a tenth 1e-1 or 0.1

Base Unit: length = meters (m)

time = seconds (s)

volume = liters (L)

mass = grams (g)

deca (da) ten 1e1 or 10

hecto (h) a hundred 1e2 or 100

kilo (k) a thousand 1e3 or 1,000

mega (M) a million 1e6 or 1,000,000

giga (G) a billion 1e9 or 1,000,000,000

1.7.3 Creating Metric Conversion Factors

~ 41 ~

The prefix always comes first, followed by the base

unit. Knowing this, interpret the following labels:

Ex. mg = milligrams, thousandths of a gram

Ex.1) kg =

Ex.2) ms =

Ex.3) mm =

Ex.4) dL =

Ex.5) nm =

We can also use our knowledge of prefixes to "build"

metric conversion factors relating our prefixes back

to their base unit. For larger prefixes:

Ex. A kg (kilogram) literally means "1000 grams", so

1 kg = 1000 g OR 0.001 kg = 1 g

~ 42 ~

Ex. cm (centimeter) means a hundredth of a meter:

1 cm = 0.01 m OR 100 cm = 1 m

Ex.6) Create conversion factors for each of the following:

mL / L ________ mL = _________ L

________ mL = _________ L

dg / g ________ g = _________ dg

________ g = _________ dg


dL / L ________ L = _________ dL

________ L = _________ dL

Mm / m ________ Mm = _________ m

________ Mm = _________ m

mg / g ________ g = _________ mg

________ g = _________ mg

~ 43 ~


nm / m ________ nm = _________ m

________ nm = _________ m

km / m ________ km = _________ m

________ km = _________ m

μg / g ________ g = _________ μg

________ g = _________ μg


Gs / s ________ s = _________ Gs

________ s = _________ Gs

HL / L ________ HL = _________ L

________ HL = _________ L

dam ________ dam = _________ m

________ dam = _________ m

~ 44 ~

Metric conversions work the same way as normal

DAs - determine your path/labels, complete the

conversion factors, and solve:

Ex.1) Let's say that you needed to convert 4.5 kg

(kilograms) into g (grams). Create the necessary

conversion factor and solve the problem:

___________ kg = _______ g

=

Ex.2) 80.9 mL is equal to ______ L?

Ex.3) How many cm are found in 7.9e3 m?

1.7.4 Simple Metric Dimensional Analysis

~ 45 ~

Ex.4) 3.4e10 ns = ? s

Ex.5) 78.0 cg → g:

Ex.6) Convert 670 grams into kilograms:

Ex.7) How many meters are equilvalent to 370 nm?

Ex.8) 45.7 L → ? mL

~ 46 ~

In order to convert from one prefix to another, you

”bounce" off the base unit in your DA.

Ex. 45 km = ? cm Path: km → m → cm

45 km 1000 m 100 cm

1 km 1 m

Ex.1) How many kilobytes (MB) are present in a 256 GB

computer hard drive?

Ex.2) Convert 4.6e9 mg into kg:

Ex.3) 2.54e10 nm would be equal to _____ cm:

1.7.5 Advanced Metric DA

~ 47 ~

Metric and general conversion factors can be used in

the same DA to solve more complex problems:

Ex.4) How long is 1.5 days, in ms?

Ex.5) The tip of a pencil lead is made of carbon and has a

mass of 10.8 mg. If a mole of carbon has a mass of

0.012011 k g and a mole of carbon also contains

6.022e23 atoms of carbon, how many atoms are

found in the tip of a pencil?

~ 48 ~

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1.1 Lab Safety Highlights

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