Calculate the pH of a 0.02 M ammonia solutio | vedclass

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(B) Ammonia $(NH_3)$ is a weak base. The ionization reaction is: $NH_3 + H_2O \rightleftharpoons NH_4^+ + OH^-$. Given concentration $C = 0.02 \ M$ an

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$11$

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(B) Ammonia $(NH_3)$ is a weak base. The ionization reaction is: $NH_3 + H_2O ightleftharpoons NH_4^+ + OH^-$. Given concentration $C = 0.02 \ M$ and degree of ionization $\alpha = 5\% = 0.05$. The concentration of hydroxide ions $[OH^-] = C 	imes \alpha = 0.02 	imes 0.05 = 0.001 \ M = 10^{-3} \ M$. Calculate $pOH = -\log[OH^-] = -\log(10^{-3}) = 3$. Since $pH + pOH = 14$ at $25^{\circ}C$,we have $pH = 14 - 3 = 11$.

Calculate the $pH$ of a $0.02 \ M$ ammonia solution that is $5\%$ ionized.

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