A 0.070 M solution of the salt NaB has a pH of 9.60. Calculate the pH of a 0.010 M solution of HB.

Or, what is the Kb of HB?

Question

Chemistry

Jovani Bryan

25 October, 22:08

A 0.070 M solution of the salt NaB has a pH of 9.60. Calculate the pH of a 0.010 M solution of HB.

Or, what is the Kb of HB?

+3

Answers (1)

Know the Answer?

Ciara Kent · Answer 1

B - + H2O HB + OH-

pOH = 14 - 9 = 5

[OH-] = [HB] = 10^-5 M

Kb = (10^-5) ^2 / 0.050 - 10^-5 = 2 x 10^-9

Ka = Kw/Kb = 5 x 10^-6 = x^2 / 0.0010-x

x = [H+] = 0.000071 M

pH = 4.2

A 0.070 M solution of the salt NaB has a pH of 9.60. Calculate the pH of a 0.010 M solution of HB.Or, what is the Kb of HB?

A 0.070 M solution of the salt NaB has a pH of 9.60. Calculate the pH of a 0.010 M solution of HB.

Or, what is the Kb of HB?