Calculate the pH of `0.2M` sodium butyrate, `(K_(a)` for butyric acid is `2.0xx10^(-5))`

Calculate the pH of a buffer solution containing 0.1 mole of acetic acid and 0.15 mole of sodium acetate. K_(c) for acetic acid is 1.75 xx 10^(-5) .

Calculate the concentration of H_3O^+ ions in a mixture of 0.02 M acetic acid and 0.1 M sodium acetate. K_alpha for acetic acid is 1.8 xx 10^(-5) .

Calculate the pH at equivalence point when a solution of 0.10 M acetic acid is titrated with a solution of 0.10 M hydroxide (K_(a) " for acetic acid is " 1.9 xx10^(-5))

Calculate the ratio of sodium formate and cormic acid (K_(a)=2xx10^(-4)) in a buffer solution of pH=4.3.

Calculate the hydrolysis constant for 0.1 M sodium acetate solution. (K_a=1.8xx10^(-5))

a. Calculate the percentage hydrolysis of 0.003M aqueous solution of NaOH. K_(a) for HOCN = 3.3 xx 10^(-4) . b. What is the pH and [overset(Theta)OH] of 0.02M aqueous solution of sodium butyrate. (K_(a) = 2.0 xx 10^(-5)) .

A small quantity of phenolphthalein (an acid indicator) is added a decimolar solution of Sodium butyrate.Calculate the ratio of the ration of the coloured form of the indicator. K_(a) for butyric acid =1.5xx10^(-5),K for the indicator =3.075xx10^(10) and K_(W)=10^(-14) .Take log 1.23=0.09 .

Calculate the pH of a 0.01 M solution of benzoic acid, the K_a being 7.3xx10^(-5)