Using pH and pOH in calculations

What is the pH of a solution that has a [H+] of 2.5 x 10^-5?

• 4.60

• 5.00

• 2.50

• 7.00

What is the pOH of a solution where the [OH-] is 7.3 x 10^-2 M?

• -1.14

• 2.00

• 1.14

• 7.30

What is the [OH-] if the [H+] is 1.0 x 10^-3M?

• 1.0 x 10^-3 M

• 6.02 x 10^-23 M

• 1.0 x 10-¹⁴ M

• 1.0 x 10^-11 M

What is the [H+] if the pH is 4.0?

• 1 x 10^-10 M

• 1 x 10^-4 M

• 1 x 10^-14 M

• 1 x 10^-7 M

What is the pOH of a solution that has a pH of 2?

• 10
• 12
• 14
• 1

What is the [OH-] if the pH is 4.900?

• 7.94 x 10^-10 M

• 1.00 x 10^-4 M

• 7.940 x 10^-14 M

• 4.90 x 10^-10 M

The lower the pH, the greater the concentration of :

• OH-
• H+

The greater the pOH, the smaller the concentration of 

• OH-
• H+

What is the pH of a solution where the [H+] is 1 x 10^-11?

• 11.0

• 13.0

• 14.0

• 1.0

Calculate the hydronium ion concentration of a solution with a pOH of 11.20.

• 6.3 x 10 ^-12

• 1.6 x 10 ^-3

• 1.6 x 10¹¹

• 2.80