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AIIMS 2010
Exam
AIIMS
Year
2010
Subject
Chemistry
Chapter
Ionic Equilibrium

AIIMS 2010 · 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. C7.06
  4. D8.2

Correct answer

C. 7.06

Step-by-step solution

Glycine H3 N+CH2COO−\mathrm{H}_3 \mathrm{~N}^{+} \mathrm{CH}_2 \mathrm{COO}^{-}is more acidic than basic. Instead of KbK_b value, the second given KaK_a value is corresponding to the KbK_b value \left(\because K_a \times K_b=10^{-14}\right).Hence,overallionizationconstant,. Hence, overall ionization constant,K=Ka1\timesKa2=4.5×10−3×1.7×10−10=7.65×10−13H+=KC=7.65×10−13×0.01=0.765×10−14=0.87×10−7MpH=−log⁡(0.87×10−7)=7.06\begin{aligned}& K=K_{a_1} \timesK_{a_2}=4.5 \times10^{-3} \times1.7 \times10^{-10} \\ & =7.65 \times10^{-13} \\ & \mathrm{H}^{+}=\sqrt{K C}=\sqrt{7.65 \times 10^{-13} \times 0.01}\\ & =\sqrt{0.765 \times 10^{-14}}=0.87 \times10^{-7} \mathrm{M}\\ & \mathrm{pH}=-\log \left(0.87 \times10^{-7}\right)=7.06 \\ & \end{aligned}$
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