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(B) Ammonium hydroxide $(NH_4OH)$ is a weak base and ammonium chloride $(NH_4Cl)$ is its salt with a strong acid,forming a basic buffer solution.For a

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$9.0 	imes 10^{-4}$

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(B) Ammonium hydroxide $(NH_4OH)$ is a weak base and ammonium chloride $(NH_4Cl)$ is its salt with a strong acid,forming a basic buffer solution.For a basic buffer,the concentration of $OH^-$ ions is given by the formula: $[OH^-] = K_b 	imes \frac{[Base]}{[Salt]}$Given: $K_b = 1.8 	imes 10^{-5}$,$[Base] = 0.05 \, M$,$[Salt] = 0.001 \, M$.Substituting the values: $[OH^-] = 1.8 	imes 10^{-5} 	imes \frac{0.05}{0.001}$$[OH^-] = 1.8 	imes 10^{-5} 	imes 50$$[OH^-] = 90 	imes 10^{-5} = 9.0 	imes 10^{-4} \, M$.

What is the $OH^-$ ion concentration of a solution containing $0.05 \, M$ ammonium hydroxide and $0.001 \, M$ ammonium chloride? Given $K_b(NH_4OH) = 1.8 \times 10^{-5}$.

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