1) Which will have the greatest affect on the colligative properties of a solution?

1) BeO 2) C6H12O6 3) Ca3N2 4) K2S

2) Which are electrolytes?

a) CoCl2b) CH4

c) C12H22O11

d) HBr

3) Compare and contrast solubility with the rate of solution. How are each affected?

WARM UP

ACIDS AND BASES

• Definition: aqueous solution of Hydrogen

containing compounds

Name the following:

HCl H2SO4 H2SO3 H2S

ACID

• Many contain the polyatomic ion OH- (hydroxide)

Name the following bases:

NaOH Ca(OH)2 Cu(OH)2 NH4OH

BASE

PROPERTIES OF ACIDS

• Ionize in water H3O+

• Corrosive to metals and skin. (React with most metals to form hydrogen gas.)

• Taste sour (like lemons)

• Frequently feel "sticky"

• pH less than 7.

• Neutralizes bases producing salt and water.

• Electrolytes.

• Acids effect indicators:1. Acids turn blue litmus to red

2. Acids turn bromothymol blue to yellow

3. Phenolthalein turns clear/cloudy

PROPERTIES OF BASES

• Ionize in water OH-

• Feel "slippery".

• Taste bitter (like soap)

• Electrolytes

• pH greater than 7.

• Neutralizes acids producing a salt and water.

• Bases effect indicators:

1. Bases turn red litmus to blue

2. Bases turn bromothymol blue to blue

3. Bases turn phenolphthalein to hot pink

ACIDS AND BASES ARE ELECTROLYTES!

• Ionization equation for HBr:

• Ionization equation for NH3:

• Concentration: amount of acid or base ÷ amount

of water or solution

• Strength: how well that particular acid or base

ionizes (amount of H3O+ or OH- )

• Strong acid/base: an acid/base that ionizes almost

completely

• Weak acid/base: an acid/base that only slightly

ionizes

STRENGTH VS. CONCENTRATION

WARM UP TURN IN YOUR LAB

1) Is it an acid or a base?

a) pH=3 b) HNO3 c) tastes bitter d)Ca(OH)2

2) Can an acid be both weak and concentrated? Explain (HINT HINT THIS IS IMPORTANT )

3) How many liters will it take to make a 0.25 M

solution of CaBr2 if you have 0.25 grams of solute?

Strong Weak

HCl H2SO4 HF H2SO3

HBr HClO3 H2S H3PO4

HI HClO4 HNO2

HNO3

LIST OF STRONG AND WEAK ACIDS

Organic acids: end in –COOH, weak

acidEx: vinegar CH3COOH

LIST OF STRONG AND WEAK BASES

Strong Weak

Group I and II

metals with

hydroxides

NH3 and any non-

group I or II

hydroxide

• Strong bases completely dissociates and are

strong electrolytes

• Weak bases only dissociate partially and are

weak electrolytes

KOH – Strong Base

KOH(s)K+(aq) + OH-

(aq)

Cu(OH)2 – Weak Base

Cu(OH)2(aq)↔ Cu2+(aq) + 2OH-

(aq)

Theory Acid

Definition

Base Definition

Arrhenius Releases H+

into solution

Releases OH-

into solution

Bronsted-

Lowery

Proton (H+)

donor

Proton (H+)

acceptor

ACID AND BASE THEORIES

Neutralization, producing a salt and water

General neutralization reaction:

Salt: Ionic compound from the cation of a base and

the anion of an acid

WHAT HAPPENS WHEN YOU MIX AN ARRHENIUS ACID WITH AN ARRHENIUS

BASE?

WaterSaltBaseAcid

COMPLETE AND NET IONIC EQUATIONS!

• LiOH(aq) + HBr(aq) LiBr(aq) + H2O(l)

1. Sodium hydroxide and hydrochloric acid

2. Calcium hydroxide and sulfuric acid

3. Potassium hydroxide and nitric acid

NAME THE SALT PRODUCED AND WRITE THE BALANCED REACTION:

BRONSTED-LOWERY ACID AND BASE

• HCl +NH3 NH4+ + Cl-

• H2O(l) + NH3(aq) ↔ NH4+

(aq) + OH-(aq)

• Monoprotic acid: only has one ionizable hydrogen

ex: HCl, HBr, HC2H3O2, HNO3

• Polyprotic acid: more than one ionizable hydrogen

ex: H2SO4, H3PO4

• Amphoteric: substance that can act as an acid or

as a base

ex: H2O

DEFINITIONS

WATER AS AN ACID OR BASE

Base

H2SO4(aq) + H2O(l) H3O+

(aq) + HSO4-(aq)

Acid

NH3(aq) + H2O(l) ↔ NH4+

(aq) + OH-(aq)

WARM-UP

• Write the complete and net ionic equations for the

neutralization of sulfuric acid and sodium hydroxide

• Compare and contrast Arrhenius and Bronsted-

Lowery acids/bases. Be sure to give an example of

each.

B-L CONJUGATE ACIDS AND BASES

• Conjugate acid: The species that is formed when a

B-L (Bronsted-Lowery) base gains a proton

• Conjugate base: The species that remains after a B-

L acid has given up a proton

IDENTIFY THE CONJUGATES

• NH3 + H3O+ NH4

+ + H2O

• CH3OH + NH2- CH3O

- + NH3

TRY THESE!

• OH- + H3O+ H2O + H2O

• H2O + NH2- OH- + NH3

WRITE THE CONJUGATE BASE

•H3O+

•H2SO4

•HCO3-

•HOCl

•NH4+

WRITE THE CONJUGATE ACID

•I-

•SO32-

•PO43-

•C2H3O2-

•H2BO3-

STRENGTH OF CONJUGATES

•The stronger an acid is, the

weaker its conjugate base; the

stronger a base is, the weaker

its conjugate acid.

• Pure water ionize slightly according to:

The product of molar concentrations of the ions is

equal to a constant Kw.

Kw = 1 * 10-14

IONIZATION OF WATER

OHOHOHOH 322

][][ 3

OHOH

In a neutral solution:

In an acidic solution:

In a basic solution:

RELATIONSHIPS

7

3 10*1][][ OHOH

][][ 3

OHOH

][][ 3

OHOH

pH and pOH

[H+] M [OH-] M pH value

Acidic >1.0x10-7 <1.0X10-7 <7.00

Neutral =1.0x10-7 =1.0x10-7 =7.00

Basic <1.0x10-7 >1.0x10-7 >7.00

• A change in [H+] by a factor of 10 causes the pH to change by 1.

• Solution with a pH of 6 has 10x the [H+] as a solution with a pH

of 7.

pH: measure of [H3O+] in a solution, measure of

“acidity”

pOH: measure of [OH-] in a solution, measure of

“basicity”

PH AND POH

Neutral

0 7 14

Acid Base

Neutral

0 7 14

Base Acid

ACID BASE INDICATORS

1 4

2 5

3 6

IMPORTANT FORMULAS

]log[ 3

OHpH ]log[ 1 OHpOH

pHOH 10][ 3pOHOH 10][ 1

14 pOHpH ]][[ 3

OHOHKW

[H3O+] =

FIND THE PH OF THE FOLLOWING:

a. 1.00 * 10-3 M d. 7.01 * 10-6 M

b. 1.00 * 10-6 M e. 9.47 * 10-8 M

c. 6.59 * 10-10 M f. 6.89 * 10-14 M

a. d.

b. e.

c. f.

• Warm UP!

• 1) how many valence electrons are in the element aluminum?

• 2) what is the pH for the following examples

• a) [H+]= 5.6 x 10-3 M

• b) pOH= 2.11

• 3) use the solubility curve in your hw packet to answer these questions:

a) How many grams of KI can be dissolved in 300 grams of water at 10°C?

a) What type of solution do you have if you dissolve 50 grams of NaCl and 40°C in 100 grams of water?

pH =

FIND THE [H3O+]

a. 3.000 d. 2.523

b. 10.000 e. 6.149

c. 6.61 f. 7.662

a. d.

b. e.

c. f.

pOH =

FIND THE PH FOR THE FOLLOWING:

a. 2 d. 4.98

b. 7 e. 9.71

c. 1.26 f. 3.04

a. d.

b. e.

c. f.

[OH-] =

FIND THE PH FOR THE FOLLOWING:

a. 1.00 * 10-11 M d. 3.45 * 10-8 M

b. 1.00 * 10-6 M e. 4.97 * 10-10 M

c. 2.64 * 10-13 M f. 2.93 * 10-2 M

a. d.

b. e.

c. f.

FIND THE [H3O+]

a. 1.00 * 10-11 M d. 3.45 * 10-8 M

b. 1.00 * 10-6 M e. 4.97 * 10-10 M

c. 2.64 * 10-13 M f. 2.93 * 10-2 M

a. d.

b. e.

c. f.

[OH-] =

WARM-UP

• Find the pH if [H+] is 2.97 x 10-4 M

• Find the [OH-] if the pOH is 6.12

• Find the pOH if [H+] is 8.21 x 10-10 M

• Find the [OH-] if [H+] is 1.26 x 10-2 M

PH CONTINUED

• Find the pH of the following:

• 0.01 M HNO3

• 0.05 M KOH

• 3.0 M HF (8.1% dissociation)

TITRATION INTRO

• Go to page 497 and read to page 502.

• Summarize each section.

• Write the definitions in your own words

• Pages 500 and 501 talk about titration procedures

and techniques. You will be doing this on Tuesday!

• Write the procedure for titrations in your own words

WARM-UP

• What is the conjugate acid for H2O?

• What is the conjugate base of HNO2?

• What is the acid and base that

neutralize to make CaSO4?

• What is an indicator? Give examples

with colors.

BUFFERED SOLUTION

• A solution that can resist changes in pH

• Made up of a weak acid and its

conjugate base

TITRATIONS

• An acid-base titration is a neutralization reaction

that is performed in the lab in order to determine an

unknown concentration of acid or base.

• The moles of acid will equal the moles of base at

the equivalence point.

• Remember this: nBMAVA= naMBVB

M molarity (M)

V volume (V)

• n moles (mol) (coefficients in balanced

reactions)

TITRATIONS

• Endpoint: When you actually stop doing the

titration. This is determined by a color change in the

indicator or an indication from a pH probe.

• Equivalence point: When the solution is neutralized.

• Indicator: weak acid or base; whose color

changes in different pH’s (because the

conjugate base/acid is a different color)

• Standard solution: solution of known

concentration used as the titrant

TITRATION TERMS

TITRATION CURVES

On the following slide you you will see 3 different

curves.

The relationships are:

Strong Acid titrated with Strong Base

Weak Acid titrated with Strong Base

Strong Acid titrated with Weak Base

Using those graphs compare the pH values of each

substance as well as the equivalence points

MORE TITRATION CURVES

Strong base

and weak

acid curve

Strong acid

and weak

base curve

Strong acid

and strong

base curve

MORE CURVES

DIPROTIC ACID CURVE

TITRATIONS

1) If it takes 54mL of 0.1M NaOH to neutralize 125mL

of an HCl solution, what is the concentration of the

HCl?

2) If it takes 25mL of 0.05M HCl to neutralize 345mL of

NaOH solution, what is the concentration of NaOH

solution?

If 26.4 mL of LiOH solution are required to neutralize

21.7 mL of 0.5M HBr, what is the concentration of

the basic solution?

PRACTICE PROBLEM 3

COMMON ACIDS!

• Go to pages 456 and 457.

• Read about each of the acids and

their common uses.

• Summarize the uses for each acid

• Be sure to know this for your test! (and life )