Observe the following four solutions :P : 10 | vedclass

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(D) buffer solution is a mixture of a weak acid and its conjugate base or a weak base and its conjugate acid.$P$: $10 \ mL, 0.1 \ M \ NaOH$ (strong ba

Vedclass · Accepted Answer

$Q$,$R$,$S$ only

Vedclass · Answer

(D) buffer solution is a mixture of a weak acid and its conjugate base or a weak base and its conjugate acid.$P$: $10 \ mL, 0.1 \ M \ NaOH$ (strong base) + $5 \ mL, 0.1 \ M \ HCl$ (strong acid). This results in a solution of $NaCl$ and excess $NaOH$. It is not a buffer.$Q$: $10 \ mL, 0.1 \ M \ NaOH$ + $15 \ mL, 0.1 \ M \ CH_3COOH$. $NaOH$ reacts with $CH_3COOH$ to form $CH_3COONa$ (conjugate base) and remaining $CH_3COOH$ (weak acid). This is an acidic buffer.$R$: $10 \ mL, 0.1 \ M \ NH_3$ (weak base) + $10 \ mL, 0.1 \ M \ NH_4Cl$ (conjugate acid). This is a basic buffer.$S$: $10 \ mL, 0.05 \ M \ NaF$ (conjugate base) + $5 \ mL, 0.1 \ M \ HF$ (weak acid). This is an acidic buffer.Therefore,$Q$,$R$,and $S$ act as buffers.

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Observe the following four solutions :$P : 10 \ mL, 0.1 \ M \ NaOH + 5 \ mL, 0.1 \ M \ HCl$$Q : 10 \ mL, 0.1 \ M \ NaOH + 15 \ mL, 0.1 \ M \ CH_3COOH$$R : 10 \ mL, 0.1 \ M \ NH_3 + 10 \ mL, 0.1 \ M \ NH_4Cl$$S : 10 \ mL, 0.05 \ M \ NaF + 5 \ mL, 0.1 \ M \ HF$Which of above solutions act as buffer?