The pH of 0.1M acetic acid is not equal to 1. Why?

The pH of 0.01 M solution of acetic acid is 5.0. What are the values of [H^(+)] and K_(a) respectively?

The pH of 0.05 M acetic acid is (K_(a) = 2 xx 10^(-5))

The pH of 0.1M monobasic acid is 4.50 . Calculate the concentration of species H^(+) . A^(-) and HA at equilibrium . Also, determine the value of K_(a) and pK_(a) of the monobasic acid.

Calculate pH of 0.1 M acetic acid having K_(a)=1.8xx10^(-5)

Calculate the pH of solution prepared by mixing 40 ml of 0.1 M acetic acid with 40 ml of 0.1 M sodium acetate, Given K_a = 10 ^(-5)

The conductivity of 0.001 M acetic acid is 5 xx 10^(-5) S cm^(-1) and ^^""^(0) is 390.5 S cm^(2) "mol" ^(-1) then the calculated value of dissociation constant of acetic acid would be

pH of a 0.1 M monobasic acid is found to be 2 . Hence , its osmotic pressure at a given temperature T K is :

What is the pH of acetic acid at equilibrium, given that acetic acid concentration is 0.1 M and it is 30% dissociated at equilibrium ? (log 3=0.47)

Calculate the pH of 0.002M aqueous acetic acid, if acid is 2.3% ionised in the given solution.