Assertion : Addition of NH_4OH to an aqueous | vedclass

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(D) The presence of $NH_4Cl$ (a strong electrolyte) suppresses the dissociation of $NH_4OH$ (a weak base) due to the common ion effect ($NH_4^+$ ions)

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If the Assertion is incorrect but the Reason is correct.

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(D) The presence of $NH_4Cl$ (a strong electrolyte) suppresses the dissociation of $NH_4OH$ (a weak base) due to the common ion effect ($NH_4^+$ ions).This significantly reduces the concentration of $OH^-$ ions in the solution.For the precipitation of $Ba(OH)_2$ to occur,the ionic product $[Ba^{2+}][OH^-]^2$ must exceed the solubility product constant $(K_{sp})$ of $Ba(OH)_2$.Since the concentration of $OH^-$ is kept very low,the ionic product does not exceed $K_{sp}$,and no precipitation occurs.Furthermore,$Ba(OH)_2$ is actually a strong base and is soluble in water.Therefore,the Assertion is incorrect and the Reason is incorrect.

Assertion : Addition of $NH_4OH$ to an aqueous solution of $BaCl_2$ in the presence of $NH_4Cl$ (excess) precipitates $Ba(OH)_2$.
Reason : $Ba(OH)_2$ is insoluble in water.

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Assertion : Addition of $NH_4OH$ to an aqueous solution of $BaCl_2$ in the presence of $NH_4Cl$ (excess) precipitates $Ba(OH)_2$.Reason : $Ba(OH)_2$ is insoluble in water.