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JIPMER 2016
Exam
JIPMER
Year
2016
Subject
Chemistry
Chapter
Ionic Equilibrium

JIPMER 2016 · Chemistry · Ionic Equilibrium

100 mL of a solution contains 2 g of acetic acid and 3 g of sodium...

100 mL of a solution contains 2 g of acetic acid and 3 g of sodium acetate providing Ka=1.8×10−5K_a=1.8 \times 10^{-5}, then choose the correct option.

Options

  1. AThis solution is basic in nature
  2. BThis solution is acidic in nature
  3. CThis solution is amphoteric in nature
  4. DThis solution is neutral in nature

Correct answer

B. This solution is acidic in nature

Step-by-step solution

We have the formula for pH pH=−log⁡Ka+log⁡[ Salt ][ Base ][\mathrm{pH}=-\log K_a+\log \frac{[\text{ Salt }]}{[\text{ Base }]} [ Salt ]=3×100082×100molL−1and]=\frac{3 \times 1000}{82 \times 100} \mathrm{ mol} \mathrm{ L}^{-1} and[ Acid ]=2×100060×100molL−1pH=−log⁡1.8×10−5+log⁡3×100082×1002×100060×100pH=4.7851\begin{aligned} {[\text{ Acid }] } & =\frac{2 \times 1000}{60 \times 100} \mathrm{ mol} \mathrm{ L}^{-1} \\ \mathrm{pH} & =-\log 1.8 \times 10^{-5}+\log \frac{ \frac{3 \times 1000}{82 \times 100}}{\frac{2 \times 1000}{60 \times 100}}\\ \mathrm{pH} & =4.7851\end{aligned}$
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