Calculate `[H^(+)]` in a `0.2M` solution of dichloriacetic acid `(K_(a)=5xx10^(-2))` that also contains `0.05M H_(2)SO_(4)` .Report your answer after multiflying it by `4000`.

Calculate [H^(+)] in a 0.20M solution of dichloriacetic acid (K_(a)=5xx10^(-2)) that also contains 0.1M sodium dichloroacetate.Neglect hydrolysis of sodium salt.

The pH of 0.5 M aqueous solution of HF (K_(a)=2xx10^(-4)) is

A solution containing 0.2 mole of dicholoracetice acid (K_(a)=5xx10^(-2)) and0.1 mole sodium dicholoroacetate in one litre solution has [H^(+)] :

Calculate the pH of 0.01 M H_2SO_4

Calculate [H^+],[HCOO^(-)] and [OCN^(-)] in a solution that contains 0.1 M HCOOH (K_a=2.4xx10^(-4)) and 0.1 M HOCN (K_a=4xx10^(-4)) .

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

Calculate pH of 0.05 M Acetic acid solution , if K_(a)(CH_(3)COOH) = 1.74 xx 10^(-5) .

Calculate the hydrogen ion concentration ( "in mol"//dm^3 ) in a solution containing 0.04 mole of acetic acid and 0.05 mole of sodium acetate in 500 mL of solution.Dissociation constant for acetic acid is 1.75xx10^(-6) Report your answer after multiplying by 2xx10^(6)

If osmotic presssure of 1M aqueous solution of H_(2)SO_(4) at 500 K is 90.2 atm. Calculate K_(a2) of H_(2)SO_(4) . Give your answer after multiplying 1000 with K_(a_(2)) . (Assumme ideal solution) [Given : K_(a_(1)) of H_(2)SO_(4)=oo ,R=0.082 L atm // mol-K]

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)) :