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InterviewSolution
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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. The ratio of pH of solution (I) containing 1 mole of `CH_(3)COONa` and 1 mole of acetic acid in one litre isA. `1:2`B. `2:1`C. `1:3`D. `3:1` |
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Answer» Correct Answer - A `{:(CH_(3)COONa+,HCl rarr,CH_(3)COOH+,NaCl,),(" "1," "1," "0," "0,),(" "0," "0," "1," "1,):}` `:. [CH_(3)COOH] = (1)/(2) =1`. `:. [H^(+)] = C alpha = C sqrt((K_(a))/(C)) = sqrt(K_(a).C) = sqrt(K_(a))` or `pH_(1) = -(1)/(2) log K_(a) = (1)/(2) pK_(a)` `{:(CH_(3)COOH+,CH_(3)COONa),(" "1," "1):}` `:. pH = pK_(a) + log.(1)/(1) rArr pH_(2) = pK_(a) :. (pH_(1))/(pH_(2)) = (1)/(2)`. |
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