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. The amount of `(NH_(4))_(2)SO_(4)` to be added to 500mL of 0.01 M `NH_(4)OH` solution `(pH_(a)NH_(4)^(+)` is 9.26) to prepare a buffer of pH 8.26 is :A. 0.05 moleB. 0.025 moleC. 0.10 moleD. 0.005 mole

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_(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. The amount of `(NH_(4))_(2)SO_(4)` to be added to 500mL of 0.01 M `NH_(4)OH` solution `(pH_(a)NH_(4)^(+)` is 9.26) to prepare a buffer of pH 8.26 is :A. 0.05 moleB. 0.025 moleC. 0.10 moleD. 0.005 mole
Answer» Correct Answer - b

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