Drill: Calculate the pH of: [H + ] = 3.0 x 10 -5 M [HI] = 2.0 x 10 -4 M

Drill: Calculate the pH of:

[H+] = 3.0 x 10-5 M [HI] = 2.0 x 10-4 M

Acid-Base Equilibria

Ionization of WaterH2O(l)

H+(aq)+ OH-

(aq)

2 H2O(l)

H3O+(aq) + OH-

(aq)

Water Ionization Constant

Kw = [H+][OH-] or

Kw = [H3O+][OH-]

Kw = 1.00 x 10-14

Memorize this

Kw CalculationsIn pure water [H+] = [OH-]

Kw = [H+][OH-]

= 1.0 x 10-14

Let [H+] = x = [OH-]

Kw CalculationsKw = [H+][OH-] = x2

Kw = x2 =1.0 x 10-14

Thus x = 1.0 x 10-7 M

[H+] = x = 1.0 x 10-7 M

pH of Pure Water[H+] = 1.0 x 10-7 M

pH = -log[H+]

pH = -log[1.0 x 10-7]

pH = 7 -log 1

Thus pH = 7.00

Calculate the pH of

3.3 x 10-8 M HI

Calculate [H+],[OH-], pH, &

pOH of 0.020 M HCl

Calculate [H+] of 0.050 M H2SO4

Weak Acid Ionization

HA(aq) H+(aq) + A-

(aq)

HA(aq) + H2O(l)

H3O+(aq) + A-

(aq)

Acid Dissociation Constant

HA(aq) H+(aq) + A-

(aq)

[H+][A-]

[HA]Ka =

Weak Base Ionization

NH3(aq) + H2O(l)

NH4+

(aq) + OH-(aq)

Base Dissociation Constant

NH3(aq) + H2O(l)

NH4+

(aq) + OH-(aq)

[NH4+][OH-]

[NH3]Kb =

Calculate [H+], [OH-], pH, & pOH of 2.0 M

HC2H3O2 (HAc)Ka = 1.8 x 10-5

Drill: Calculate [H+],[OH-], pH, &

pOH of 0.025 M KOH

Acid-Base Equilibria Problems

Calculate [H+], [OH-], pH, &

pOH of0.50 M NH3

Kb = 1.8 x 10-5

Calculate [H+],[OH-], pH, & pOH of 0.010 M HC7H5O2 (HBz)

Ka = 6.4 x 10-5

Calculate the Ka of 0.10 M Hquack

when it ionized 5.0 % in an aqueous

solution.

The pH of a 0.79 M solution of Hnut is 3.10.

Calculate its Ka

Drill: Calculate [H+] & pH of 0.50 M NaOH

Drill: Calculate [H+] & pH of

2.0 M C6H5NH2

Kb = 3.2 x 10-5

Calculate the pH of a solution of

0.00050 M HBS : Ka = 5.0 x 10-12

PolyproticAcid

Equilibria

Calculate [H2CO3], [HCO3

-], [CO3-2], [H+],

[OH-], & pH of 0.44 M H2CO3 Ka1 = 4.4 x 10-7

Ka2 = 4.7 x 10-11

Calculate [H2SeO3], [HSeO3

-1], [SeO3-2],

[H+],[OH-], & pH of 0.27 M H2SeO3 Ka1 = 2.7 x 10-7

Ka2 = 5.4 x 10-11

Calculate [H3A],[H2A-], [HA-2],[A-3],[H+], &pH of 0.30 M H3A

Ka1 = 3.0 x 10-7

Ka2 = 5.0 x 10-11

Ka3 = 4.0 x 10-15

Calculate the pH of

0.025 M HF:Ka = 6.4 x 10-4

Drill: Calculatethe pH of

0.025 M QOH:Kb = 2.0 x 10-4

You have 10 identical coins with 1 coin having a slight mass difference. Determine the odd coin with only 3 uses of an

equal arm balance.

Drill: Calculate the pH of

0.25 M HAz Ka = 2.5 x 10-3

Drill: Calculate the pH of

0.25 M HAz Ka = 2.5 x 10-3

Calculate the pH of

0.10 M HClO Ka = 2.5 x 10-8

Calculatethe pH of

0.025 M QOH:Kb = 2.0 x 10-4

Drill: Calculate the pH of 0.020

M QOH.Kb = 3.2 x 10-7

TestReview

Arrhenius Bronsted-Lowry

Lewis

Be able to name:•Acids

•Bases

Be able to describe & Identify:

•Strong Acids

•Strong Bases

Show the ionization of

HClin solution

Show the ionization of

NH3

in solution

Calculate the [H+], [OH-], pH,

& pOHof 0.1 M HNO3

Calculate the [H+], [OH-], pH,

& pOHof 0.02 M NaOH

Calculate the [H+], [OH-], pH,

& pOH of 2.0 M NH3

Kb = 1.8 x 10-5

Calculate the pH, & pOH of

0.10 M HNO2 Ka = 6.0 x 10-4

Calculate the volume of 0.30 M Ba(OH)2 required to titrate

50.00 mL of 0.40 M H3PO4 to its

equivalence point.

Calculate [H2A], [HA-], [A-2], [H+], & pH of 0.20 M H2A

Ka1 = 2.0 x 10-7

Ka2 = 5.0 x 10-11

Calculate the pH of a solution of 0.20 M QNH2.Kb = 2.0 x 10-3

Drill: 831 mL NH3 was bubbled through 2.0 L of water at 27.0oC under 150 kPa pressure. 80.0 % of

the ammonia dissolves in the water. Calculate the pH

of the final solution.