Unit 10: Solutions: pH and pOH

For a solution at 25^oC, 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

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

When the hydrogen ion concentration goes up, the pH ___

• gets lower

• stays the same

• gets higher

• goes toward 7

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

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

What is the numerical value of K_w, the water dissociation constant?

• 14.0 x 10^-1

• 7.0 x 10^-2

• 2.0 x 10^-7

• 1.0 x 10^-14

If a solution has a pOH of 1 what is the pH? Is it an acid or base? (pick 2)

• acid

• base

• 13

• 1

• neutral

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