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AIIMS 2004
Exam
AIIMS
Year
2004
Subject
Chemistry
Chapter
Ionic Equilibrium

AIIMS 2004 · Chemistry · Ionic Equilibrium

What is the pH of 0.01 M glycine solution? For glycine, K_ a_1 =4.5...

What is the pH\mathrm{pH} of 0.01M0.01 \mathrm{M} glycine solution? For glycine, Ka1=4.5×10−3K_{a_1}=4.5 \times 10^{-3} and Ka2=1.7×10−10K_{a_2}=1.7 \times 10^{-10} at 298 K298 \mathrm{~K} ?

Options

  1. A3.0
  2. B10.0
  3. C6.1
  4. D7.2

Correct answer

C. 6.1

Step-by-step solution

K=Ka1\timesKa2=4.5×10−3×1.7×10−10=7.65×10−13[H+]=KC=7.65×10−13×0.01=7.65×10−15=0.87×10−7pH=−log⁡0.87×10−7=7−0.93=6.07\begin{aligned}& K=K a_1 \timesK a_2=4.5 \times10^{-3} \times1.7 \times10^{-10} \\ & =7.65 \times10^{-13} \\ & {\left[\mathrm{H}^{+}\right]=\sqrt{K C}=\sqrt{7.65 \times 10^{-13} \times 0.01}} \\ & =\sqrt{7.65 \times 10^{-15}}=0.87 \times10^{-7} \\ & \mathrm{pH}=-\log0.87 \times10^{-7}=7-0.93=6.07 \\ & \end{aligned}
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