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sammy [17]
3 years ago
5

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

Chemistry
1 answer:
Amiraneli [1.4K]3 years ago
5 0

Answer:

  • <u><em>8.3</em></u>

Explanation:

<u>1) Data:</u>

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

b) pH = ?

<u>2) Formulae:</u>

  • pH + pOH = 14

  • pOH = log 1 /[OH⁻]

<u>3) Solution:</u>

  • pOH = log ( 1 / 2.1 × 10⁻⁶ ) = 5.7
  • pH = 14 - pOH = 14 - 5.7 =  8.3
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