What is the pH of a solution with [OH- ] = 1.60x10-9 M? Include two digits past the decimal in your answer.
What is the pH of a solution if [H3O+] = 2.00x10-5 M? Include two digits past the decimal in your answer.
A solution has a pH value of 3.90. What is the pOH for the solution? Include one digit past the decimal in your answer.

1) pH = 5.20

2) pH = 4.70

3) pOH = 10.1

Explanation:

What is the pH of a solution with [OH- ] = 1.60x10-9 M?

Step 1: Data given

[OH-] = 1.60 * 10^-9 M

Step 2: Calculate pOH

pOH = -log[OH-]

pOH = -log [1.60*10^-9]

pOH = 8.80

Step 3: Calculate pH

pH = 14 - pOH

pH = 14 - 8.8 = 5.20

What is the pH of a solution if [H3O+] = 2.00x10-5 M?

[H3O+] = [H+] = 2.00 * 10^-5 M

pH = -log[H+]

pH = -log[2.00*10^-5]

pH = 4.70

A solution has a pH value of 3.90. What is the pOH for the solution?

pOH = 14 - pH

pOH = 14 -3.90 = 10.1

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