Common AcidsSulfuric Acid H2SO4

Nitric Acid HNO3

Phosphoric Acid H3PO4

Hydrochloric Acid HCl

Acetic Acid CH3COOH

Carbonic Acid H2CO3

Battery acid

Used to make fertilizersand explosives

Food flavoring

Stomach acid

Vinegar

Carbonated water

Sulfuric acid is the most commonly produced industrial chemical in the world.

Uses: petroleum refining, metallurgy, manufacture of fertilizer, many industrial processes: metals, paper, paint, dyes, detergents

Sulfuric acid is used in automobile batteries.

H2SO4

“oil of vitriol”

Nitric acid stains proteins yellow (like your skin).

Uses: make explosives, fertilizers, rubber, plastics, dyes, and pharmaceuticals.

HNO3

“aqua fortis”

The stomach produces HCl to aid in the digestion of food.

Uses: For ‘pickling’ iron and steel.Pickling is the immersion of metals in acid solution to removesurface impurities.

A dilute solution of HCl is called muriatic acid (available in many hardwarestores). Muriatic acid is commonly used to adjust pH in swimming pools and in the cleaning of masonry.

HCl(g) + H2O(l) HCl(aq)hydrogen chloride water hydrochloric acid

Sodium hydroxide NaOH lye or caustic soda

Potassium hydroxide KOH lye or caustic potash

Magnesium hydroxide Mg(OH)2 milk of magnesia

Calcium hydroxide Ca(OH) 2 slaked lime

Ammonia water NH3 H2O household ammonia

Name Formula Common Name

.NH4OH

Bases are ionic compound. They follow the rules for naming ionic compounds and you have to use criss cross method to write the chemical formula. (The “+” ion first followed by the “-” ion.)

Ex. 1 sodium hydroxide

Na+ OH-

NaOH

Ex. 2 KOH

K+ OH-

Potassium hydroxide

Acids donate hydrogen ions (H+) and their chemical formulas have a hydrogen written at the beginning.

Names of acid depend on the negative ion and its ending.

Anion ends with –ide :

Ex. 1 acid formed with anion bromide

if anion ends with –ide:

To write name use prefix hydro + root of anion+ change –ide ending to –ic + word “acid”

NAME: hydrobromic acid

Anion ends with –ate :

Ex. 2 acid formed with anion carbonate

if anion ends with –ate:

To write name Use root of anion+ change –ate ending to –ic + word “acid”

NAME: carbonic acid

Anion ends with –ite :

Ex. 3 acid formed with anion nitrite

if anion ends with –ite:

To write name Use root of anion+ change –ite ending to –ous + word “acid”

NAME: nitrous acid

All acids have as the positive ion the hydrogen ion (H+) and a negative ion that can be identified by the name of the acid.

Ex. 4 hydrochloric acid

if name of ion includes prefix hydro and has an -ic ending, then the anion has an -ide ending.

From ion sheet determine which ion has root like the anion and an -ide ending. For the example is the chloride ion which formula is Cl-

H+ Cl- HCl

Ex. 4 phosphoric acid

if name of ion has an -ic ending, then the anion has an -ate ending.

From ion sheet determine which ion has root like the anion and an -ate ending. For the example is the phosphate ion which formula is PO4 3-

H+ PO4 3- H3 PO4

Ex. 4 phosphorous acid

if name of ion has an -ous ending, then the anion has an -ite ending.

From ion sheet determine which ion has root like the anion and an -ite ending. For the example is the phosphite ion which formula is PO3 3-

H+ PO3 3- H3 PO3

Acids properties1. Conduct electricity (strong

acids)2. Change blue litmus to red 3. Have a sour taste 4. React with bases to

neutralize their properties 5. React with active metals

to liberate hydrogen6. pH values <7

AcidsAcids are defined as: Substances which ionize

to form hydrogen ions (H+) in aqueous solution. (Arrhenius)

Substances that act as proton donors, H+ (Bronsted-Lowry) or as electron-pair acceptors (Lewis)

Examples HCl, H2SO4

Bases properties Base properties

1. Conduct electricity (strong bases)

2. Change red litmus to blue

3. Have a slippery feeling (like soap)

4. React with acids to neutralize their properties

5. pH values >7

BasesBases are defined as:Substances which ionize to

form hydroxide ions OH(-) in aqueous solution

Substances that act as proton receptors (Bronsted-Lowry) or as electron-pair donors (Lewis)

Examples: NH3OH, NaOH, CaCO3 , NaHCO3 (baking

soda)

AMMONIAcleaner

pH ScaleThe pH scale is used to

measure how acidic or basic a liquid is.

pH measures the concentration of hydrogen ions (H+) and hydroxide ions (OH-).

The scale goes from 0 through 14. Distilled water is 7, so is called neutral.

lemon juice

0 1 2 3 4 5 6 7 8 9 10 11 12 13 14

pH Acidic

Neutral

Basic

vinegar

d water

baking soda

ammonia

detergent

Indicators

Indicator Acid Base

Red litmus paper Stays same Turns blue

Blue litmus paper Turns red Stays same

Bromophenol blue Yellow Stays blue

Phenolphtalein Colorless Pink

An indicator is a large organic molecule that works somewhat like a "color dye."

Natural indicatorsThere are natural

indicators for acids and bases, and we may find them in our kitchen or garden! Red rose flowersBougainvillea flowersRed cabbageBlue berries

Practice: identifying acid and bases1) HCl + H2O H3O+ + Cl–

HCl is the acid because it is donating a H+ to H2O

H2O is the base because it is accepting a H+ from HCl

Cl- is the conjugate base because it’s what’s left after the acid donates a H+

H+

H3O+ is the conjugate acid because it’s what’s left after the base accepts a H+

Practice: identifying acid and bases2) CN- + H2O OH- + HCN

H2O is the acid because it is donating a H+ to CN-

CN- is the base because it is accepting a H+ from H2O

OH- is the conjugate base because it’s what’s left after the acid donates a H+

H+

HCN is the conjugate acid because it’s what’s left after the base accepts a H+

Practice: identifying acid and bases3) OH- + HI

H+

The acid can donate a H+ and its chemical formula has a H at the beginning

acidDonates a H+

H2O + I-

Classwork :handout conjugate acids and bases

Common Acids

Strong Acids

stomach acid;

(dissociate ~100%)

pickling: cleaning metals w/conc. HCl

sulfuric acid: H2SO4 2 H1+ + SO42–

-- #1 chemical; (auto) battery acid

explosives;

nitric acid: HNO3 H1+ + NO31–

-- fertilizer

Common Acids (cont.)

Weak Acids (dissociate very little)

acetic acid: CH3COOH H1+ + CH3COO1–

--

hydrofluoric acid: HF H1+ + F1–

--

citric acid, H3C6H5O7

--

ascorbic acid, H2C6H6O6

--

lactic acid, CH3CHOHCOOH

--

vinegar; naturally made by apples

used to etch glass

lemons or limes; sour candy

vitamin C

waste product of muscular exertion

carbonic acid, H2CO3

-- carbonated beverages

-- CO2 + H2O H2CO3

dissolveslimestone(CaCO3)

rainwaterin air

H2CO3: cave formation H2CO3: natural acidity of lakes

H2CO3: beverage carbonation

Formation of Hydronium Ions1+

hydronium ion

H3O+

+

hydrogen ion

H+

water

H2O

1+

(a proton)

1+

pH Scale

Acid Base

0

7

14

Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 515

[H[H++] pH] pH

10-14 14

10-13 13

10-12 12

10-11 11

10-10 10

10-9 9

10-8 8

10-7 7

10-6 6

10-5 5

10-4 4

10-3 3

10-2 2

10-1 1

100 0

1 M NaOH

Ammonia(householdcleaner)

BloodPure waterMilk

VinegarLemon juiceStomach acid

1 M HCl

Aci

dic

N

eutr

al

Bas

ic

pH of Common Substances

Timberlake, Chemistry 7th Edition, page 335

1.0 MHCl0

gastricjuice1.6

vinegar2.8

carbonated beverage3.0

orange3.5

apple juice3.8

tomato4.2

lemonjuice2.2 coffee

5.0

bread5.5

soil5.5

potato5.8

urine6.0

milk6.4

water (pure)7.0

drinking water7.2

blood7.4

detergents8.0 - 9.0

bile8.0

seawater8.5

milk of magnesia10.5

ammonia11.0

bleach12.0

1.0 MNaOH(lye)14.0

8 9 10 11 12 14133 4 5 621 70

acidic neutral basic[H+] = [OH-]

Acid – Base ConcentrationspH = 3

pH = 7

pH = 11

OH-

H3O+OH-

OH-H3O+

H3O+

[H3O+] = [OH-] [H3O+] > [OH-] [H3O+] < [OH-]

acidicsolution

neutralsolution

basicsolution

co

nc

en

trat

ion

(m

ole

s/L

)

10-14

10-7

10-1

Timberlake, Chemistry 7th Edition, page 332

pH Calculations

pH

pOH

[H3O+]

[OH-]

pH + pOH = 14

pH = -log[H3O+]

[H3O+] = 10-pH

pOH = -log[OH-]

[OH-] = 10-pOH

[H3O+] [OH-] = 1 x10-14

[ ] are used to represent concentration, usually molarity (mol/L) or (mol/dm3).

pH has no units.

Example 1What is the pH of a solution that contains

1.00x10-4 mol H3O+/dm3?

Given [H3O+ ]=1.00x10-4 mol H3O+/dm3

Unknown: pH

pH = -log[H3O+]

pH = -log[1.00x10-4]

pH = 4.00

Example 2What is the pH and pOH of a solution that

contains 0.00350mol H3O+/dm3?

Given [H3O+ ]=0.00350mol H3O+/dm3

Unknown: pH and pOH

pH = -log[H3O+]

pH = -log[0.00350]

pH = 2.46

pH + pOH = 14

pOH = 14 – pH= 14 - 2.46 = 11.54

Example 3What is the [H3O+ ] and [OH- ] of a solution if

pOH=4.40Given: pOH= 4.40 Unknown: [H3O+ ] and [OH- ]

[OH-] = 10-pOH

[OH-] = 10-4.40

[OH-] = 3.98x10-5 M

[H3O+] [OH-] = 1 x10-14

[H3O+] = 1 x10-14 = 1 x10-14 = 2.51x10-10M

[OH-] 3.98x10-5

classworkP 184 #15,16,17

Strengths of acids and basesStrong acids and bases : ionize completely in

aqueous solution.HCl (g) + H2O (l) H3O+ (aq) + Cl- (aq)

(100% ionized)Examples: HCl, HNO3, H2SO4, KOH, NaOH

Weak acids and bases: ionize slightly in aqueous solution. CH3COOH (aq) + H2O (l) H3O+ (aq) + CH3COOH - (aq)

(partially ionized)Examples: HClO, H3PO4 , NH3

Reactions between acids and bases

When and acid and a base react with each other it is called neutralization reaction.

Reactions between acids and bases

General formula for acid base reaction:

Acid + Base → H2O +Salt“Salt” means any ionic compound formed from an acid/base reaction

NOT JUST NaCl !!

Acids and bases reactionsThe acids react with bases, forming salts

ACID + BASE → SALT + WATER

HHCl + NaOHOH → NaCl + H2O

H-OH

TitrationEquivalence point: when number of moles of

hydrogen ions equals the number of moles of hydroxide ions.

Titration: adding a known amount of a solution of known concentration to determine the concentration of another solution.

Standard solution: solution of known concentration

End point: point at which the indicator changes color

Point of neutralization is the end point of the titration.

Ex. 1 How many milliliters of 0.45M HCl will neutralize 25.0 mL of 1.00M KOH?

mL HCl= 25.0mL x 1.00M KOH 0.45 M HCl

mL HCl= 55.6mL HCl

Ex. 2 What is the molarity of a NaOH solution if 20.0 mL of the solution is neutralized by 28.0mL of 1.00 M HCl? M NaOH= 1.00 M HCl x 28.0 mL

20.0 mL

M NaOH = 1.40 M

Classwork: p 189 # 23 (a,c,d), 25, 26