An aqueous solution is obtained by mixing of with of . What would be the precise pH of the resulting solution at ? (Given for and ).

Question

An aqueous solution is obtained by mixing $100 	ext{ mL}$ of $0.2 	ext{ M } CH_3COOH$ with $100 	ext{ mL}$ of $0.2 	ext{ M } NaOH$. What would be the precise pH of the resulting solution at $25^\circ C$? (Given $pK_a$ for $CH_3COOH = 4.74$ and $\log 2 = 0.30$).

Prashant Kotian · Accepted Answer

Correct answer: B. Mixing equal volumes of weak acid and strong base results in complete neutralization, forming a solution of sodium acetate () with a total volume of . This salt undergoes anionic hydrolysis. The pH is given by . Here, . .

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