pH and [H+] Calculations

For a solution, pH + pOH =

• 7

• 14

• 1.0 x 10^-14

• -log (1.0 x 10 ^-14)

If the pH of a solution is 4.0, what is the pOH?

• 4.0

• 10.0

• 1.0 x 10 ^-4

• cannot be determined from the information

The pH of a solution is 8.43. What is the [H₃O⁺]concentration?

• 3.7 x 10 ^-9

• 1.0 x 10^-8.43

• 2.7 x 10^-6

• 1.0 x 10^-14

If the [H₃O⁺] of a solution is 1 x 10^-3 M, the pH is

• 11

• -3

• 3

• 1

If the pH of a solution is 8 the [H₃O⁺] is

• 1.0 x 10⁶ M

• 8.0 x 10¹ M

• 1.0 x 10⁸ M

• 1.0 x 10^-8 M

If the [OH^-] of a solution is 2.7 x 10^-4 M, the pOH of the solution is

• 10.44

• 1.00

• 3.57

• -4.43

If the [H₃O⁺] of a solution is 6.8 x 10^-8 M, the pH is

• 7.17

• 3.2 x 10^-5

• 7.2

• 7.62

If the [H₃O⁺] of a solution is 9.3 x 10^-3 M, the pOH of the solution will be

• 2.03

• 1.02

• 11.97

• 12.98

If a solution has a pOH of 3.7 the [OH-] of the solution is

• 5.0 x 10^-11

• 2.0 x 10^-4

• 10.3

• 14

Oranges have a [H₃O⁺] of 1.7 x 10^-2 M. Their pOH is

• 1.77

• 12.23

• 10.91

• 3.09