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JIPMER 2014
Exam
JIPMER
Year
2014
Subject
Chemistry
Chapter
Ionic Equilibrium

JIPMER 2014 · Chemistry · Ionic Equilibrium

A buffer solution is prepared in which the concentration of NH_3 is...

A buffer solution is prepared in which the concentration of NH3\mathrm{NH}_3 is 0.30 M and the concentration of NH4+\mathrm{NH}_4^{+}is 0.20 M . If the equilibrium constant, KbK_b for NH3\mathrm{NH}_3 equals 1.8×10−51.8 \times 10^{-5}, what is the pH of this solution? (log⁡2.7=0.43)(\log 2.7=0.43)

Options

  1. A9.439.43
  2. B11.7211.72
  3. C8.738.73
  4. D9.089.08

Correct answer

A. 9.439.43

Step-by-step solution

pOH=pKb+log⁡[ Salt ][ Base ]=−log⁡Kb+log⁡[ Salt ][ Base ]\begin{aligned} \mathrm{pOH}=\mathrm{p} K_b & +\log \frac{[\text{ Salt }]}{[\text{ Base }]} \\ & =-\log K_b+\log \frac{[\text{ Salt }]}{[\text{ Base }]}\end{aligned}=−log⁡1.8×10−5+log⁡0.200.30=5−0.25+(−0.176)=4.75−0.176=4.57\begin{aligned} & =-\log 1.8 \times 10^{-5}+\log \frac{0.20}{0.30} \\ & =5-0.25+(-0.176) \\ & =4.75-0.176=4.57\end{aligned} \therefore \quad \mathrm{pH}=14-4.57=9.43$
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