Balancing
Write a balanced equation showing the reaction of carbon dioxide with water to produce aqueous carbonic acid.
CO2(g) + H2O (l) ⇌ H2CO3 (aq)
Identify whether the solution is acidic, basic, or neutral.
a. [H+] = 1.0 x 10-8 M
b. [H+] = 2.5 x 10-12 M
c. [OH-] = 1.0 x 10-7 M
d. [OH-] = 8.21 x 10-11 M
a. Basic
b. Basic
c. Neutral
d. Acidic
Determine the pH for each of these strong-acid solutions
a. 0.27 M aq. HClO4
b. 0.035 M aq. HNO3
c. 5.3 x 10 -3 M aq. HI
a. pH = 0.57
b. pH = 1.46
c. pH = 2.28
Definition of Ka and Kb
Ka is the equilibrium constant for acid ionization and Kb is the equilibrium constant for base ionization
pH + pOH =
14
Write a balanced equation showing the reaction of gaseous sulfur trioxide with water to form aqueous sulfuric acid.
SO3 (g) + H2O (l) --> H2SO4 (aq)
Find the concentration of hydroxide ions in each of the solutions
a. a solution with a pOH of 4.7
b. a solution with a pOH of 10.3
c. a solution with a pH of 6.2
d. a solution with a pH of 13.4
a. 2.0 x 10-5 M
b. 5.0 x 10-11 M
c. 1.6 x 10-8 M
d. 0.25 M
Trifluoroacetic acid (HC2F3O2) is a weak acid. Construct an ICE table and find [H+] and the pH for a 0.150 M HC2F3O2 solution.
HC2F3O2 (aq) ⇌ H+ (aq) + C2F3O2- (aq) Ka = 0.30
[H+] = 0.11 M
pH = 0.96
Bronsten lowry definition of acids and bases
An acid gives up an H+ proton and a base accepts an H+
Kw =
1.0 x 10-14
a. HBr(aq) + KOH (aq) -->
b. Ba(OH)2 (aq) + HBr (aq) -->
c. HBr (aq) + Fe(OH)2 (s) -->
d. H3PO4 (aq) + KOH (aq) -->
a. HBr(aq) + KOH (aq) --> H2O (l) + KBr (aq)
b. Ba(OH)2 (aq) + 2HBr (aq) --> 2H2O (l) + BaBr2 (aq)
c. 2HBr (aq) + Fe(OH)2 (s) --> 2H2O (l) + FeBr2 (aq)
d. H3PO4 (aq) + 3KOH (aq) --> 3H2O (l) + K3PO4 (aq)
Which has a lower pH, a 1.0 x 10-4 M solution of HCl, or a 1.0 x 10-4 M solution of H2CO3? Explain.
HCl
Using the equilibrium data given, find the pH of a 1.20 M aq. (CH3)2NH solution.
(CH3)2NH (aq) + H2O (l) ⇌ (CH3)2NH2+ (aq) + OH- (aq) Kb = 1.9 x 10-11
pH = 8.68
Arrhenius definition of acid and base
Acids produce H+ ions and Bases produce OH- ions
Percent ionization equation for an acid in terms of [HA] and [A-]
[A-] / [HA-]initial x 100%
Show all the steps for a neutralization reaction of aqueous Triprotic Acid (H3PO4)
1. H3PO4 (aq) + H2O (l) ⇌ H2PO4- (aq) + H3O+ (aq)
2. H2PO4- (aq) + H2O (l) ⇌ HPO42- (aq) + H3O+ (aq)
3. HPO42- (aq) + H2O (l) ⇌ PO43- (aq) + H3O+
Find the concentration of [OH-] ions in each of these situations:
a. a strongly acidic solution where [H+] = 1.0 x 10-2 M
b. a neutral solution where [H+] = 1.0 x 10-7 M
c. a basic solution where [H+] = 4.28 x 10-11
a. 1.0 x 10-12 M
b. 1.0 x 10-7 M
c. 2.34 x 10-4
0.280-M solution of a monoprotic acid is 1.32% ionized. What is the pH for this solution? What is the Ka for this acid?
pH = 2.43
Ka = 4.94 x 10-5
Definition of autoionization
A process that occurs in water when a water molecule fragments to produce H+ and OH- ions.
When acids react with metals it produces
Metal cations and Hydrogen gas
Complete ionic equation and net ionic equation for this neutralization reaction:
H2SO4 (aq) + 2KOH (aq) --> K2SO4 (aq) + 2H2O (l)
Ionic equation: 2H+ (aq) + SO42- (aq) + 2K+ (aq) + 2OH- (aq) --> 2K+ + SO42- + 2H2O (l)
Net ionic equation: H+ (aq) + OH- (aq) --> H2O (l)
Identify each solution as acidic, basic, or neutral:
a. an aqueous solution where the hydroxide ion concentration is greater than the hydronium ion concentration
b. a solution of vinegar in water, with a pH of 5.2
c. a solution with [OH-] = 5.2 x 10-2 M
d. a solution where the -log[H+] = 7.0
e. a solution with a pOH of 4.0
a. Basic
b. Acidic
c. Basic
d. Neutral
e. Basic
A 0.105-M aqueous solution of a compound with the formula HC7H5O2 has a pH of 4.29. Find the Ka for this compound.
Ka = 2.5 x 10-8
What is produced in a neutralization reaction
Water and an ionic compound (or salt)
Nonmetal oxides react with water to produce
Acidic compounds