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The pH of buffer of NH4OH + NH4Cl - type...

The pH of buffer of `NH_4OH + NH_4Cl` - type is given by -

A

Solochrome black

B

Eriochrome blackT

C

Eosin

D

Both 1&2

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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_(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. The amount of (NH_(4))_(2)SO_(4) to be added to 500 mL of 0.01M NH_(4)OH solution (pK_(a) for NH_(4)^(+) is 9.26) prepare a buffer of pH 8.26 is:

Assertion : Buffer solutions are those which resist change in pH value on the addition of a small amount of acid or a base to it. Reason: Mixture of NH_4OH and NH_4 Cl acts as basic buffer.

1 lit of buffer solution contains 0.1 mole each of NH_(4)OH and NH_(4)Cl . What will be the P^(H) of the solution when 0.01 mole of HCl is added to it [ P^(Kb) of NH_(4)OH = 4.74 ]

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 :

NH_4Cl is a salt of a

The pH of a buffer solution of 0.1 M NH_(4)OH [ pK_(a)=4.0] and 0.1 M NH_(4)Cl is

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