Question

Which is the value of Ka for the weak acid HA if a 0.35 M solution of HA has a pH of 5.95?

Answer 1

3.6 x 10^-12

Step-by-step explanation:

[H+]= 10^-5.95= 1.12 x 10^-6 M

HA -> H+ + A-

k= [H+] [A-]/[HA]

k= (1.12 x10^-6)^2/0.35M

k= 3.6 x 10^-12