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The pH of basic buffer mixtures is given...

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^(+)]` :

A

`0.05M`

B

`0.025M`

C

`0.10M`

D

`0.005M`

Text Solution

AI Generated Solution

To solve the problem, we need to calculate the concentration of hydrogen ions \([H^+]\) in a buffer solution containing dichloroacetic acid and sodium dichloroacetate. Here are the steps to arrive at the solution: ### Step 1: Identify the components of the buffer We have a buffer solution made up of: - Weak acid: Dichloroacetic acid (DCA) - Salt: Sodium dichloroacetate (NaDCA) ### Step 2: Write the formula for pH of an acidic buffer ...
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