pH and pOH

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

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

• 1.77

• 12.23

• 10.91

• 3.09

Ammonia has a pOH of 2. Ammonia is a(n) __________.

• acid

• base

• neutral

• metal

Find the pH of a solution with [OH-] = 8.41 x 10^-4.

• 3.08

• 10.92

• 9.88

• 11.23

What is the pOH of a solution with [H⁺] = 1.24 x 10 ^-2?

• 1.91

• 1.61

• 12.09

• 12.39