A one litre contains `0.08` moleof acetic acid `(K_(a) = 1.75 xx 10^(-5))`. To this solution of resulting solution is `[log 1.75 = 0.243]`

A one litre solution contains 0.08 mole of acetic acid ( K_(a) = 1.75 xx 10^(-5) ) . To this solution , 0.02 mole of NaOH is added . Then the pH of resulting solution is[log 1.75 =0.243 ]

A one litre solution contains 0.08 mole of acetic acid (K_(a)=1.75xx10^(-5)) . To the solution, 0.02 mole of NaOH is added. Then the P^(H) of resulting solution is [log 1.75=0.273]

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

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

0.2 M NaOH are added to 50 ml of 0.2 M acetic acid ( K_(a) = 1.8 xx 10^(-5)) . The volume of 0.2 M NaOH required to make the pH of solution 4.74 ( -log 1.8 xx 10^(-5) = 4.74 )

A basic buffer contains 0.8 mole of NH_(4)Cl and 0.2 mole of NH_(4)OH for litre of a solution the K_(b) of base is 1.8 xx 10^(-5) . Then the P^(H) of the buffer solution is (log 1.8 = 0.2553)

A monoprotic acid in 0.1 M solution has K_(a)=1.0xx10^(-5) . The degree of dissociation for acid is

The acid dissociation constant K_(a) of acetic acid is 1.74 xx 10^(-5) at 298 K. The pH of a solution of 0.1 M acetic acid is