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 $1:2$ electrol

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$3$

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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 $AgCl = 0.0206 \ mol 	imes 143.5 \ g \ mol^{-1} = 2.956 \ g \approx 3 \ g$.

Similar Questions

Which of the following outer octahedral complexes have the same number of unpaired electrons?
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$2$. $[FeF_6]^{3-}$
$3$. $[CoF_6]^{3-}$
$4$. $[Ni(NH_3)_6]^{2+}$

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$C$. $[Ni(CN)_4]^{2-}$
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$E$. $Ni(PPh_3)_4$
Choose the correct answer from the options given below:

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Due to the presence of ambidentate ligands,coordination compounds show isomerism. Palladium complexes of the type $[Pd(C_6H_5)_2(SCN)_2]$ and $[Pd(C_6H_5)_2(NCS)_2]$ are

The magnetic moment of the complex $[Cr(CN)_6]^{3-}$ is ..... (in $BM$)

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