A 0.100 M solution of a weak base has a pH of 9.95. What is...

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Chemistry

A 0.100 M solution of a weak base has a pH of 9.95. What is thebase hydrolysis constant, Kb, for the weak base?

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4.1 Ratings (817 Votes)

pH + pOH = 14

pOH = 14 -9.95

pOH = 4.05

[OH-] = 10^-4.05

[OH-] = 8.9 x 10^-5 M

x = [OH-] = 8.9 x 10^-5 M

B + H2O ----------------------> BH+Â Â Â + OH-

0.10Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â 0Â Â Â Â Â Â Â Â 0Â Â ------------------> initial

-xÂ Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â + xÂ Â Â Â Â Â Â Â +x -----------------> changed

0.10-xÂ Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â Â xÂ Â Â Â Â Â Â Â Â Â x ----------------------> equilibrium

Kb = [BH+][OH-]/[B]

Kb = x^2 / 0.1-x

Kb = (8.9 x 10^-5)^2 / (0.1-8.9 x 10^-5)

Kb = 7.93 x 10^-8

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A 0.100 M solution of a weak base has a pH of 9.95. What is...

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Chemistry

A 0.100 M solution of a weak base has a pH of 9.95. What is thebase hydrolysis constant, Kb, for the weak base?

Answer & Explanation Solved by verified expert

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