Unit 10: Calculating pH and pOH (5.6)

If a solution has a [H⁺] of 9.3x10^-11, what is the pH?

• 10.0

• 4.0

• 3.5

• 8.2

A  pH and a pOH will add up to:

• 0
• 7
• 14
• 1.0 x 10^-14

What is the equation for calculating pH?

• pH = [H⁺]

• pH = log [H⁺]

• pH = -log[OH^-]

• pH = -log [H⁺]

If the [H+] of a solution is 6.8 x 10^-9 mol/L the pH is

• 8.17
• 8.2
• 9.99
• 8.62

if the [H+] of a solution is 8.4 x 10^-3 mol/L the pOH of the solution will be

• 2.08
• 11.92
• 1.02
• 12.98

If the hydronium ion H₃O⁺ concentration is equal to the hydroxide ion OH^- concentration, the solution is a(n)

• acid

• base

• salt

• neutral solution

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

• 11

• -3

• 3

• 1

When the hydrogen ion concentration goes up, the pH ___

• gets lower

• stays the same

• gets higher

• goes toward 7

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

When a water molecule loses a hydrogen ion, or proton, it becomes ___

• a hydronium ion, H₃O⁺

• a hydroxide ion, OH^-

• a hydronium ion, OH^-

• a hydroxide ion, H₃O⁺