Homework Chapter 16
Acid-Base Titration and pH


16.1

1. Determine the hydronium and hydroxide ion concentrations in a solution that is
1 x 10-4 M HCl. soln ( [H3O+1] = 1 X 10-4 M; [OH-1] = 1 X 10-10 M )

2. Determine the hydronium and hydroxide ion concentrations in a solution that is
1.0 x 10-3 M HNO3. soln ( [H3O+1] = 1.0 X 10-3 M; [OH-1] = 1 X 10-11 M )

3. Determine the hydronium and hydroxide ion concentrations in a solution that is
3.0 x 10-2 M NaOH. soln ( [H3O+1] = 3.3 X 10-13 M; [OH-1] = 3.0 X 10-2 M )

4. Determine the hydronium and hydroxide ion concentrations in a solution that is
1.0 x 10-4 M Ca(OH)2. soln ( [H3O+1] = 5.0 X 10-11 M; [OH-1] = 2.0 X 10-4 M )

16.2

1. Determine the pH of the following solutions:

a) 1 x 10-3 M HCl soln (3.0)

b) 1 x 10-5 M HNO3 soln (5.0)

c) 1 x 10-4 M NaOH soln (10.0)

d) 1.0 x 10-2 M KOH soln (12.00)

16.3

1. What is the pH of a solution if the [H3O+1] is 6.7 x 10-4 M? soln (3.17)

2. What is the pH of a solution with a hydronium ion concentration of 2.5 x 10-2 M? soln (1.60)

3. Determine the pH of a 2.5 x 10-6 M HNO3 solution. soln (5.60)

4. Determine the pH of a 2.00 x 10-2 M Sr(OH)2 solution. soln (12.60)

16.4

1. The pH of a solution is determined to be 5.0. What is the hydronium ion concentration of this solution? ( 1 x 10-5 M) soln

2. The pH of a solution is determined to be 12.0. what is the hydronium ion concentration of this solution? (1 x 10-12 M) soln

3. The pH of an aqueous solution is measured as 1.50. Calculate the [H3O+1] and the [OH-1]. ( [H3O+1] = 3.2 x 10-2 M and [OH-1] = 3.2 x 10-13 M ) soln

4. The pH of an aqueous solution is 3.67. Determine [H3O+1]. (2.1 x 10-4 M) soln

16.5

1. What is the concentration of hydronium and hydroxide ions in pure water at 25oC?

2. Why does the pH scale generally range from 0 to 14 in aqueous solutions?

3. Why does a pH of 7 represent a neutral solution at 25oC?

4. Idenitfy each of the following as being true of acidic or basic solutions at 25oC:
a) [H3O+1] = 1 x 10-3 M
b) [OH-1] = 1 x 10-4 M
c) pH = 5.0
d) pH = 8.0

5. A solution contains 4.5 x 10-3 HCl. Determine the following for the solution:
a) [H3O+1]
b) [OH-1]
c) pH soln

6. A Ca(OH)2 solution has a pH of 8.0. Determine the following for the solution:
a) [H3O+1]
b) [OH-1]
c) pH soln

16.6

1. A 15.5 mL sample of 0.215 M KOH solution required 21.2 mL of aqueous acetic acid solution in a titration experiment. Calculate the molarity of the acetic acid solution.
( 0.157 M ) soln

2. By titration, 17.6 mL of aqueous H2SO4 neutralized 27.4 mL of 0.0165 M LiOH solution. What was the molarity of the aqueous acid solution? ( 0.0128 M ) soln

3. Name an appropriate indicator for titrating the following:
a) a strong acid and a weak base;
b) a strong base and a weak acid

4. Suppose you have an NaOH solution of unknown concentration. Name three possible substances that could be used in known solutions to titrate the NaOH solution.

5. If 20.0 mL of 0.0100 M aqueous HCl is required to neutralize 30.0 mL of an aqueous solution of NaOH, determine the molarity of the NaOH solution. ( 6.67 x 10-3 M ) soln

6. Suppose that 20.0 mL of 0.010 M Ca(OH)2 is required to neutralize 12.0 mL of aqueous HCl solution. What is the molarity of the HCl solution? ( 0.33 M ) soln