The pH of a 1.00 M solution of urea, a weak organic base, is 7.050.?

Calculate the ka of the protonated urea

Urea is a base, so we will denote it as “B”.

B + H2O <---> BH+ + OH-

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

[B] = 1.00 M

pH = 7.050; pOH = 6.95; [OH-] = 1.12E-7 M = [BH+]

Kb = (1.12E-7)^2 / (1.00) = 1.26E-14

Ka = 1E-14 / Kb = 1.26

Weak bases tend to have strong conjugate acids.

H+ = 10^ -PH
H+ = 10^ – 7.05
H+ = 8.91 * 10^-8 mol
so the answer is 8.91 * 10^-8 L

0.794