A 200 mL solution X contains 0.02 mol of [C | vedclass

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(D) $1$. Reaction with excess $AgNO_3$: Only the chloride ions outside the coordination sphere will precipitate as $AgCl$. $[Co(NH_3)_5Br]Cl_2$ provid

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$0.04, 0.02$

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(D) $1$. Reaction with excess $AgNO_3$: Only the chloride ions outside the coordination sphere will precipitate as $AgCl$. $[Co(NH_3)_5Br]Cl_2$ provides $2 	imes 0.02 = 0.04 \ mol$ of $Cl^-$. $[Co(NH_3)_5Cl]SO_4$ does not provide any $Cl^-$ ions outside the coordination sphere. Thus,moles of $AgCl$ $(Y)$ = $0.04 \ mol$. $2$. Reaction with excess $BaCl_2$: Only the sulfate ions outside the coordination sphere will precipitate as $BaSO_4$. $[Co(NH_3)_5Cl]SO_4$ provides $0.02 \ mol$ of $SO_4^{2-}$. $[Co(NH_3)_5Br]Cl_2$ does not provide any $SO_4^{2-}$ ions. Thus,moles of $BaSO_4$ $(Z)$ = $0.02 \ mol$.

$A$ $200 \ mL$ solution $X$ contains $0.02 \ mol$ of $[Co(NH_3)_5Br]Cl_2$ and $0.02 \ mol$ of $[Co(NH_3)_5Cl]SO_4$. If solution $X$ is treated with excess $AgNO_3$ and excess $BaCl_2$,what will be the number of moles of precipitates $Y$ and $Z$ formed,respectively?

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