`0.01` M HA (aq.) is `2%` dissociated, `[OH^(-)]` of solution is :

The pH of a 0.1 M CH_(3)COOH which is 2% ionised in aqueous solution is

In a basic aqueous solution chloromethane undergoes a substitution reaction in which Cl is replaced by OH^(-) as. CH_3Cl(aq)+OH^(-) hArrCH_3OH(aq)+Cl^(-)(aq) The equilibrium constant of above reaction K_c=1xx10^(16) .If a solution is prepared by mixing equal volumes of 0.1 M CH_3Cl and 0.2M NaOH (100% dissociated) then [OH^(-)] concentration at equilibrium in mixture will be :

A weak acid HA is found to be 3% dissociated in 0.1 M solution . Calculate the value of K_a

At 25^(@) C dissociation constants of acid HA and base BOH in aqueous solution are same. The pH of 0.01 M solution of HA is 5. The pOH of 10^(-4) M solution of BOH at the same temperature is :

At 25^(@) C dissociation constants of acid HA and base BOH in aqueous solution are same. The pH of 0.01 M solution of HA is 5. The pOH of 10^(-4) M solution of BOH at the same temperature is :