The `[H^(+)]` of a resulting solution that is 0.01 M acetic acid `(K_(a)=1.8xx10^(-5))` and 0.01 M in benzoic acid `(K_(a)=6.3xx10^(-5))` :

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

Calculate PH Of 0.01 M acetic acid . K_a = 1.8 xx 10^-5 at 298 K.

Calculate the percent ionization of 0.10M acetic acid (K_a=1.8xx10^(-5)) .

Calculate [H^(+)], [CH_(3)COO^(-)] and [C_(7)H_(8)O_(2)^(-)] in a solution that is 0.02M in acetic acid and 0.01M in benzoic acid. (K_(a_(A A))= 1.8xx10^(-5), K_(a_(BA)) = 6.4xx10^(-5))

Degree of dissociation of 0.1 molar acetic acid at 25^(@)C (K_(a) = 1.0 xx 10^(-5)) is

Degree of dissociation of 0.1 molar acetic acid at 25^(@)C (K_(a) = 1.0 xx 10^(-5)) is

What is the percentage dissociation of 0.1 M solution of acetic acid ? (K_(a)=10^(-5))

The values of ionisation constants for some pairs of acids and bases are given which of them is stronger ? (a) Acetic acid (K_(a) =1.8 xx 10^(5)), boric acid (K_(a) =5,8 xx 10^(-10)) (b) Hydrofluoric acid (K_(a)= 6.7 xx 10^(-4)), benzoic acid (K_(a) =6.3 xx 10^(-5)) (c) Ammonium hydroxide (K_(b) =1.8 xx 10^(-5)) Magensium hydroxide (K_(b) =8.1 xx 10^(-3))