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What is the pH of a solution containing $\mathrm{0.1\ M\ NH_4OH}$ and $\mathrm{0.1\ M\ NH_4Cl}$ ?

$\mathrm{(Given,\ k_b\ of\ NH_4OH = 10^{-5})}$
Option: 1
4

Option: 2
5

Option: 3
8

Option: 4
9

Answers (1)

best_answer

$\mathrm{NH_4Cl}$ is a strong electrolyte and it will furnish $\mathrm{NH_4^+}$ ions

$\mathrm{[NH_4^+]_{NH_4Cl}=0.1\ M}$

Now, let us consider the dissociation of $\mathrm{NH_4OH}$

$\mathrm{NH_4OH\ \ \rightleftharpoons \ \ NH_4^+ +OH^-}$

$0.1$ $0.1$ $-$

$\mathrm{(0.1-x)}$ $\mathrm{(0.1+x)}$ $\mathrm{(x)}$

$\mathrm{\approx 0.1}$ $\mathrm{\approx 0.1}$

Writing the expression for equilibrium constant

$\mathrm{\frac{(x) \times 0.1}{0.1}=10^{-5}}$

$\Rightarrow\mathrm{x=10^{-5}}$

Thus, $\mathrm{[OH^-]=10^{-5}}$

Hence, $\mathrm{pOH =5\ or\ pH =9}$

Therefore, the correct answer is Option (4)

Posted by

vishal kumar

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