An excess of AgNO_3 is added to 100 mL of a | vedclass

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(A) The chemical formula of tetraaquadichloridochromium$(III)$ chloride is $[Cr(H_2O)_4Cl_2]Cl \cdot 2H_2O$.Upon ionization in water, the complex diss

Vedclass · Accepted Answer

$5$

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(A) The chemical formula of tetraaquadichloridochromium$(III)$ chloride is $[Cr(H_2O)_4Cl_2]Cl \cdot 2H_2O$.Upon ionization in water, the complex dissociates as: $[Cr(H_2O)_4Cl_2]Cl \cdot 2H_2O ightarrow [Cr(H_2O)_4Cl_2]^+ + Cl^- + 2H_2O$.Only the chloride ion outside the coordination sphere reacts with $AgNO_3$ to form $AgCl$ precipitate.Number of moles of the complex = $	ext{Molarity} 	imes 	ext{Volume (in L)} = 0.05 \ M 	imes 0.1 \ L = 0.005 \ 	ext{moles}$.Since $1 \ 	ext{mole}$ of the complex releases $1 \ 	ext{mole}$ of $Cl^-$, the moles of $AgCl$ precipitated = $0.005 \ 	ext{moles}$.Converting to the required format: $0.005 = 5 	imes 10^{-3} \ 	ext{moles}$.Thus, the answer is $5$.

An excess of $AgNO_3$ is added to $100 \ mL$ of a $0.05 \ M$ solution of tetraaquadichloridochromium$(III)$ chloride. The number of moles of $AgCl$ precipitated will be . . . . . . $\times 10^{-3}$. (Nearest integer)

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