Session 31. Chapter 12.6 4/14/2013

Ch 12.7 Acids and Bases
Supplemental Instruction
Iowa State University
Grant DeRocher
Chem 167
Know Kw= 1.0 x 10-14
1. Write the formula of the conjugate base of each of the following acids: (a)HNO3 (b)H2O
(c) HSO4- (d) H2CO3 (e) H3O+
2. For each of the following reactions, indicate the Bronsted-Lowry acids and bases. What
are the conjugate acid-base pairs?
(a) CN-(aq) + H2O(l)
HCN(aq) + OH-(aq)
(b) HCO3-(aq) + H3O+(aq)
H2CO3-(aq) + H2O(l)
(c) CH3COOH(aq) + HS-(aq)
CH3COO-(aq) + H2S(aq)
3. What are the products of the following acid-base reactions? Indicate the acid and its
conjugate base and the base and its conjugate acid.
(a) HClO4 + H2O
(b) NH4+ + H2O
(c) HCO3- + OH-
4. Write chemical equations and equilibrium expressions for the reactions of each of the
following weak acids with water:
(b) C2H5COOH
(c) HF
(d) HClO
(e) H2CO3
5. Hydrofluoric acid is a weak acid used in the building industry to etch patterns into glass
for elegant windows. Because it dissolves glass, it is the only inorganic acid that must be
stored in plastic containers. A 0.1 M solution of HF has a pH of 2.1. Calculate [H3O+] in
this solution.
6. Calculate the pH of a 0.10 solution of propanoic acid and determine its present ionization.
The ionization constant Ka for propanoic acid is 1.3x10-5.
7. Acrylic acid is used in the polymer industry in the production of acrylates. Its Ka is
5.6x10-5 . What is the pH of a 0.11 M solution of acrylic acid, CH2CHCOOH?
8. Morphine, an opiate derived from opium poppy, has the molecular formula C7H19NO3. It
is a weakly basic amine, with a Kb of 1.6x10-6. What is the pH of a 0.0045 M solution of