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JEE Mains · Chemistry · STD 11 - 6.2. Equilibrium - II (icon Equilibrium)
What would be the \(pH\) of a solution obtained by mixing \(5\,g\) of acetic acid and \(7.5\,g\) of sodium acetate and making the volume equal to \(500\, mL\) ? \((K_a = 1.75 \times 10^{-5},pK_a =4.76)\)
- A \(pH=4.70\)
- B \(pH < 4.70\)
- C \(pH\) of solution will be equal to \(pH\) of acetic acid
- D \(4.76 < pH < 5.0\)
Answer & Solution
Correct Answer
(D) \(4.76 < pH < 5.0\)
Step-by-step Solution
Detailed explanation
\(pH = p{K_a} + \log \,\frac{{[salt]}}{{[acid]}}\) \( = 4.76 + \log \,\frac{{\frac{{7.5}}{{500}}}}{{\frac{5}{{500}}}} = 4.7 + \log \,1.5 = 4.87\) Hence correct answer is \(4.76 < pH < 5.0\)
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