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Prove the buffer action of acetic acid and sodium acetate by the addition of 0.01 mol of solid sodium hydroxide.

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1. Consider one litre of buffer solution containing 0.8 m CH3COOH and O.8 m CH3COONa. Assume that the volume change due to the addition of 0.01 mol of solid NaOH is negligible. Ka for CH3COOH is 1.8 x 10-5.

2. 

3. The dissociation constant for CH3COOH is given by

The above expression shows that the concentration of H+ is directly proportional to

degree of dissociation of CH3COOH = α

5. Given that Ka for CH3COOH is 1.8 x 10-5 

[H+] = 1.8 x 10-5 

pH = – log [H+

= – log [1.8 x 10-5

= 5 – log 1.8 

= 5 – 0.26 pH 

= 4.74

6. After adding 0.01 moI NaOH to I litre of buffer. Given that volume change due to the addition of NaOH is negligible. [OH-] = 0.01 M. The consumption of OH- are expressed by the following equation.

7. The addition of a strong base (0.01 M NaOH) increased the pH only slightly i.e., from 4.74 to 4.75. So the buffer action is verified.

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