Question

An aqueous solution has a pOH of 4.41 (1) What is the pH of this solution? (2) What is the hydroxide ion concentration in this solution? (3) What is the hydrogen ion concentration in this solution?

Answer 1

a. 1. pH = 14 - pOH = 14 - 4.41 = 9.59

2. pOH = -log([OH-])

4.41 = -log([OH-])

Solving, [OH-] = 3.89 * 10-5 M

3. pH = -log([H+]) = 9.59

SOlving, [H+] = 2.57 * 10-10 M

b.

1. pOH = 14 - pH = 14 - 4.41 = 9.59

2. pOH = -log([OH-]) = 9.59

SOlving, [OH-]= 2.57 * 10-10 M

3. pH = -log([H+])

4.41 = -log([H+])

Solving, [H+] = 3.89 * 10-5 M

c. We have the relation: [OH-] * [H+] = 10-14

2.62 * 10-2 * [H+] = 10-14

Solving [H+] = 3.82 * 10-13 M

pOH = -log([OH-]) = 1.58

pH = -log([H+]) = 12.42