Calculating pH, pOH, H+ and OH- concentration

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

• 10.0

• 4.0

• 3.5

• 8.2

If a solution has a [OH^-] of 2.3x10^-4, it must be a(n) (a)  

• Acid
• Base
• Neutral

pH and a pOH add up to:

• 0
• 7
• 14
• 1.0 x 10^-14

If the pH of a solution is 5.6 the pOH is

• 6.5
• 12.4
• 8.4
• 5.6

If the [OH-] of a solution is 2.7 x 10^-4 mol/L the pOH of the solution is

Mathematical Equivalence

ON

pH =

(a)  

• 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)

(a)   .

• acid

• base

• salt

• neutral solution

The pH of a solution is 8.43. What is the hydronium ion H₃O⁺ concentration?

• 3.7 x 10^-9 M

• 2.7 x 10^-6 M

• 1.0 x 10^-8.43 M

• 1.0 x 10^-14