If the Kb of a weak base is 4.6 × 10-6, what is the pH of a 0.32 M solution of this base?

Answers

Answer 1

Answer: Assuming that the given base is a weak monoprotic base, the pH of the solution can be calculated as follows:

Write the balanced reaction and ice chart:

BOH --> OH- + B+

i 0.32 0 0
c -x x x
e 0.32-x x x

Kb = x^2/ (0.32-x)
x = 1.21x10^-3 = [OH-]
pOH = -log[OH-] = -log[1.21x10^-3] = 2.917
pH = 14 - pOH = 14 - 2.917 = 11.08

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Answers

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. . .. . . . .. . . . . .. . . . . .
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Answers

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Answers

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Answer:

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Explanation:

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