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Assertion : The pH of a basic buffer mix...

Assertion : The `pH` of a basic buffer mixture is given by: `pH=pK_(a)+log(([Base])/([conjugate acid]))`
Reason : The `pH` of an acidic buffer mixture is given by: `pH=pK_(a)+log(([conjugate acid])/([Acid]))`

A

If both assertion and reason are true and the reason is the correct explantion of the assertion.

B

If both assertion and reason are true but reason is not the correct explanation of the assertion.

C

If assertion is true but reason is false.

D

If assertion is false but reason is true.

Text Solution

Verified by Experts

The correct Answer is:
D
For basic buffer
`pH=pK_(a)+log=([Base])/([Conjugate acid])`
` :. pH=pK_(w)-pOH`
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pH of an acidic buffer is given by

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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 volume of 0.2M NaOH needed to prepare a buffer of pH 4.74 with 50 mL of 0.2M acetic acid is: (pK_(a) of CH_(3)COO^(-)= 9.26)

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:

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 weak acid HA after treatment with 12 mL of 0.1M strong base BOH has a pH=5 . At end point, the volume of same base required is 26.6mL K_(a) of acid 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 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^(+)] :

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