## Calculations of pH, pOH, [H^{+}] and [OH^{-}]

### You will need a calculator or log table to complete this activity

Choose the correct answer for each question.

### pH Problem Solving Diagram

The pH of a 0.0001-M solution of NaOH is:

- 4
- -4
- 11
- 10

What is the [OH^{-}] of a solution whose [H^{+}] = 0.001M

- 1 x 10
^{-3} M - 1 x 10
^{-11} M - 1 x 10
^{11} M - 1 x 10
^{3} M

The [H^{+}] of a solution is 8.34 x 10^{-5} mole/liter. The pH of this solution lies between:

- 2 and 3
- 3 and 4
- 4 and 5
- 5 and 6

Which of the following hydrogen ion concentrations represents a solution with acidic properties?

- 1 x 10
^{-2} M - 1 x 10
^{-8} M - 1 x 10
^{-10} M - 1 x 10
^{-14} M

The [H^{+}] of an acid solution that has a pH of 3 is:

- 1 x 10
^{3} M - 1 x 10
^{-3} M - 1 x 10
^{11} M - 1 x 10
^{-11} M

The pH of a 0.01-M solution of HCl is:

- 2
- -2
- 12
- -12

The pH of a solution is 3.0. What is the [OH^{-}]?

- 11 M
- 3 M
- 1 x 10
^{-3} M - 1 x 10
^{-11} M

What is the pH of a 0.001 M NaOH solution?

- 3
- -3
- 10
- 11

The pH of a softdrink is determined to be 4.0. What is the [OH^{-}] of the drink?

- 10 M
- 4 M
- 1.0 x 10
^{-4} M - 1.0 x 10
^{-10} M

In aqueous solutions, [H^{+}][OH^{-}] is equal to:

- 1 x 10
^{-7} M - 1 x 10
^{-14} M - 7 M
- 1 x 10
^{14} M

The normal pH of human blood is 7.4. Human blood is:

- slightly basic
- slightly acidic
- strongly basic
- strongly acidic

What is the pOH of a solution whose pH is 3.45?

- -3.45
- 17.45
- 10.55
- 3.45

What is the pH of a solution whose [H^{+}] is 2.75 x 10^{-4} M?

- 3.56
- 3.636 x 10
^{-11} - 3.64
- 10.44

What is the pOH of a solution whose [H^{+}] is 2.75 x 10^{-4} M?

- 3.56
- 3.636 x 10
^{-11} - 3.64
- 10.44

What is the pOH of a solution whose [OH^{-}] is 9.31 x 10^{-2} M?

- 1.03
- 12.97
- 1.07 x 10
^{-13} - 15.03

What is the pH of a solution whose [OH^{-}] is 9.31 x 10^{-2} M?

- 1.03
- 12.97
- 1.07 x 10
^{-13} - 10.44

What is the [H^{+}] of a solution whose [OH^{-}] is 9.31 x 10^{-2} M?

- 9.31 x 10
^{-16} M - 9.31 x 10
^{12} M - 1.07 x 10
^{-13} M - 10.44

What is the pH of a solution whose pOH is 11.09?

- 2.91
- 15.09
- 25.09
- -11.09

What is the [H^{+}] of a solution whose pH = 5.43 ?

- 3.72 x 10
^{-6} M - 2.69 x 10
^{-9} M - 8.57
- 269153

What is the [OH^{-}] of a solution whose pH = 5.43 ?

- 3.72 x 10
^{-6} M - 2.69 x 10
^{-9} M - 8.57
- 269153

What is the [OH^{-}] of a solution whose pOH = 2.86 ?

- 1.38 x 10
^{-3} M - 7.24 x 10
^{-12} M - 724 M
- 3.50 x 10
^{-15} M

What is the [H^{+}] of a solution whose pOH = 2.86 ?

- 1.38 x 10
^{-3} M - 7.24 x 10
^{-12} M - 724 M
- 3.50 x 10
^{-15} M