Question

# Given an acetate buffer with pH 4.9, do you expect the solution to contain predominantly more...

Given an acetate buffer with pH 4.9, do you expect the solution to contain predominantly more undissociated acetic acid or more dissociated acetate ions? explain.

Henderson - Hasselbach equation is

pH = pKa + log([A-]/[HA])

where,

A- = conjucate base , CH3COO-

HA = weak acid , CH3COOH

pKa of CH3COOH = 4.75

4.9 = 4.75 + log([CH3COO-]/[CH3COOH])

log([CH3COO-] / [CH3COOH]) = 0.15

[CH3COO-] / [CH3COOH] = 1.413

Therefore,

The solution should contain predominentally more dissociated acetate ions.

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