Equilibrium Question 149
Question: What is the pH of 0.01 M glycine solution’ For glycine, $ Ka_1=4.5\times {10^{-3}} $ and $ Ka_2=1.7\times {10^{-10}} $ at 298 K [AIIMS 2004]
Options:
3.0
B) 10.0
6.1
7.2
Show Answer
Answer:
Correct Answer: C
Solution:
$ K=Ka_1\times Ka_2 $
$ =4.5\times {10^{-3}}\times 1.7\times 10^{10} $
${H^{+}}=\sqrt{K_{a}c} $
$ =\sqrt{4.5\times {10^{-3}}\times 1.7\times {10^{-10}}\times .01} $
$ = 0.87\times {10^{-7}} $
$ pH=-\log \ (0.87\times {10^{-7}})$
$ =7-0.93=6.07 $ .
BETA
