[" A decrease or increase in pH results."],[" Which containing "0.2" mole of dichloroacetic acid "(K_(0)=5times10^(-2))" and "0.1" mole sodium "],[" loras un in a solution has "[H']" : "],[[" (B) "0.025M," (C) "0.10M," (D) "0.005M]]

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^(+)] :

The concentration of H^(+) in a solution containing 0.2 mol of dichloroacetic acid (Ka=5 times 10^(-2)) and 0.1 mol of sodium dichloroacetate in 1L of the solution is

The Ph of basic buffer mixtures is given by : Ph=Pk_(a)+ log (["Base"])/(["Salt"]) whereas Ph of acidic buffer mixtures is given by : Ph = pK_(a)+"log"(["Salt"])/(["Acid"]) . Addition of little acid or base although shows no appreciable change in Ph for all practical purposes, but sicne the ratio (["Base"])/(["Salt"]) or (["Salt"])/(["Acid"]) changes, a slight decrease or increase in pH results. A solution containing 0.2 mole of dichloroacetic acid (K_(a)=5xx10^(-2)) and 0.1 mole sodium dichloracetate in one litre solution has [H^(+)] :

The pH of basic buffer mixtures is given by : pH=pK_(a)+log((["Base"])/(["Salt"])) , whereas pH of acidic buffer mixtures is given by: pH= pK_(a)+log((["Salt"])/(["Acid"])) . Addition of little acid or base although shows no appreciable change for all practical purpose, but since the ratio (["Base"])/(["Salt"]) or (["Salt"])/(["Acid"]) change, a slight decrease or increase in pH results in. A solution containing 0.2 mole of dichloroacetic acid (K_(a)=5xx10^(-2)) and 0.1 mole sodium dichloroacetate in one litre solution has [H^(+)] :

The pH of basic buffer mixtures is given by : pH=pK_(a)+log((["Base"])/(["Salt"])) , whereas pH of acidic buffer mixtures is given by: pH= pK_(a)+log((["Salt"])/(["Acid"])) . Addition of little acid or base although shows no appreciable change for all practical purpose, but since the ratio (["Base"])/(["Salt"]) or (["Salt"])/(["Acid"]) change, a slight decrease or increase in pH results in. A solution containing 0.2 mole of dichloroacetic acid (K_(a)=5xx10^(-2)) and 0.1 mole sodium dichloroacetate in one litre solution has [H^(+)] :

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 [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.

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]