Question

What is the pH of a weak base solution that has an [OH–] of 2.1 g 10–6 M? (4 points)

APEX

Answer 1

• 8.3

Step-by-step explanation:

1) Data:

a) [OH⁻] = 2.1 × 10⁻⁶ M . . . (the symbol g shown in the question is a typo)

b) pH = ?

2) Formulae:

• pH + pOH = 14

• pOH = log 1 /[OH⁻]

3) Solution:

• pOH = log ( 1 / 2.1 × 10⁻⁶ ) = 5.7

• pH = 14 - pOH = 14 - 5.7 = 8.3