A chromium complex with a formula CrCl_3 cdot | vedclass

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(A) The spin-only magnetic moment of $3.87 \ BM$ corresponds to $3$ unpaired electrons, indicating $Cr^{3+}$ in an octahedral field. The $1:2$ electro

Vedclass · Accepted Answer

$3$

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(A) The spin-only magnetic moment of $3.87 \ BM$ corresponds to $3$ unpaired electrons, indicating $Cr^{3+}$ in an octahedral field. The $1:2$ electrolyte behavior implies the formula is $[Cr(H_2O)_5Cl]Cl_2 \cdot H_2O$. When passed through a cation exchanger, the complex cation $[Cr(H_2O)_5Cl]^{2+}$ is retained, and the $2Cl^-$ ions are released into the solution. The molar mass of $[Cr(H_2O)_5Cl]Cl_2 \cdot H_2O = 52 + (5 	imes 18) + (3 	imes 35.5) + 18 = 266.5 \ g \ mol^{-1}$. Moles of complex = $\frac{2.75 \ g}{266.5 \ g \ mol^{-1}} \approx 0.0103 \ mol$. Since each mole of complex releases $2$ moles of $Cl^-$, moles of $AgCl$ formed = $2 	imes 0.0103 = 0.0206 \ mol$. Mass of $AgCl = 0.0206 \ mol 	imes 143.5 \ g \ mol^{-1} = 2.956 \ g \approx 3 \ g$.

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