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_(1) + log.(["Salt"])/(["Acid"]). Addition of little acid or base although shows no change in pH for all practical purposes , but since the ratio (["Base"])/(["Salt"]) for (["Salt"])/(["Acid"]) changes, a slight decrease or increase in pH results. A solution containing 0.2 mole of dichloroacetic acid litre solution has [H^(+)]

The pH of basic buffer mixtures is given by pH = pK_(a) + log.(["Base"

1.	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_(1) + log.(["Salt"])/(["Acid"]). Addition of little acid or base although shows no change in pH for all practical purposes , but since the ratio (["Base"])/(["Salt"]) for (["Salt"])/(["Acid"]) changes, a slight decrease or increase in pH results. A solution containing 0.2 mole of dichloroacetic acid litre solution has [H^(+)]
Answer» 0.05 M 0.025 M 0.10 M 0.005 M Solution :Since `CHCl_(2).COOH` is relatively strong ACID having more `K_(a)`. `{:(CHCl_(2).COONA,rarr,CHCl_(2)COO^(-),+,Na^(+)),(,,0.1,,0.1),(CHCl_(2).COOH ,hArr,CHCl_(2)COO^(-) ,+,H^(+)),(0.2,,0,,0),((0.2 - x),,(x + 0.1),,x):}` `:. K_(a) = ([CHCl_(2)COO^(-)][H^(+)])/([CHCl_(2)COOH])` or `5 xx 10^(-2) = ([0.1 + x][x])/([0.2 - x])` `:. x = 0.05`.