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(A) The formula of the complex is $[Cr(H_2O)_5Cl]Cl_2$. Each mole of the complex releases $2 \ mol$ of ionizable $Cl^-$ ions. Number of moles of compl

Vedclass · Accepted Answer

$287 	imes 10^{-3}$

Vedclass · Answer

(A) The formula of the complex is $[Cr(H_2O)_5Cl]Cl_2$. Each mole of the complex releases $2 \ mol$ of ionizable $Cl^-$ ions. Number of moles of complex = $Molarity 	imes Volume (L) = 0.01 \ M 	imes 0.1 \ L = 0.001 \ mol$. Number of moles of $Cl^-$ ions = $2 	imes 0.001 \ mol = 0.002 \ mol$. Reaction: $Ag^+(aq) + Cl^-(aq) ightarrow AgCl(s)$. Moles of $AgCl$ formed = $0.002 \ mol$. Molar mass of $AgCl = 108 + 35.5 = 143.5 \ g/mol$. Mass of $AgCl = 0.002 \ mol 	imes 143.5 \ g/mol = 0.287 \ g = 287 	imes 10^{-3} \ g$.

Excess of silver nitrate solution is added to $100 \ mL$ of $0.01 \ M$ pentaaqua chloro chromium $(III)$ chloride solution. The mass of silver chloride obtained in grams is [Atomic mass of silver is $108$].

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