NAME:
MODS:
Acid-Base Equilibria Practice
Ka/Kb and Salt Solutions
16.1-16.4
1.
Write the chemical equations for the ionizations of the following weak acid and weak base
in water, and write the Ka or Kb expressions.
a)
HNO2 (nitrous acid)
b)
CH3NH2 (methylamine)
2.
Nicotinic acid (niacin, HNic) is a monoprotic acid with the formula HC6H4NO2. A solution
that is 0.012 M in nicotinic acid has a pH of 2.89 at 25°C. What is the Ka for this acid at
25°C? Also, what is the degree of ionization of nicotinic acid in this solution?
3.
Quinine (Quin) is an alkaloid (naturally occurring base) that is used to treat malaria. A
0.0015 M solution of quinine has a pH of 9.84 at 25°C. What is the Kb for this base at 25°C?
4.
A solution of acetic acid, HC2H3O2 (HAc) on a lab shelf is of an undetermined
concentration. If the pH of the solution was found to be 2.68, what is the concentration
of the acetic acid? Ka for acetic acid = 1.7 x 10-5
5.
What is the [H3O+] of a 0.20 M solution of ammonia in water at 25°C? Kb = 1.8 x 10-5
6.
What are the concentrations of the hydronium ion and the acetate ion (Ac -) in a solution
of 0.10 M acetic acid, HC2H3O2 (HAc) at 25°C? Also, what is the pH of the solution and
the degree of ionization? Ka = 1.7 x 10-5
7.
What is the [H3O+], [OH-] and pH of a 2.00 M solution of 2,6-dinitrobenzoic acid (DNBA),
(NO2)2C6H3COOH? Ka = 0.0794 *You will need to use the quadratic equation here! 
8.
Determine whether or not hydrolysis will occur for the following ions:
a)
Cl-
9.
For the following salts, determine whether the aqueous solution will be acidic, basic or
neutral:
b)
OCl-
c)
PO4-3
d)
NO3-
e)
NH4+
a)
Na2CO3
b)
Fe(NO3)3
c)
KBr
d)
Cu(ClO4)2
e)
CaCl2
f)
Ba(CN)2
10.
Use Table 16.1 (pg. 656) and Table 16.2 (pg. 665) to determine the following Ka or Kb:
a)
Kb for NO2-
b)
Ka for C6H5NH3+
c)
Kb for ClO-
d)
Kb for C7H5O2-
e)
Ka for N2H5+
e)
Kb for C3H3O3-
11.
What is the pH of a 0.025 M aqueous solution of sodium proprionate, NaC3H5O2? Also,
what is the concentration of propionic acid (HPr, Ka = 1.3 x 10-5) in the solution?
12.
Calculate the concentration of pyridine, C5H5N (PyN, Kb = 1.4 x 10-9) in a solution that is
0.15 M pyridinium bromide, C5H5NHBr. Also, what is the pH of the solution?