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  • An excess of AgNO3 is added to 100 mL of a 0.01M solution of dichlorotetraaquachromium(lll) chloride. The number of moles of AgCl ppt?

An excess of AgNO3 is added to 100 mL of a 0.01M solution of dichlorotetraaquachromium(lll) chloride.
The number of moles of AgCl ppt?

How is the Molar concentration of dichlorotetraaquachromium(III) chloride coming as 0.001M?

Shouldn't it be 0.01? 

Can you explain it a bit.

Answers (1)

\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{4}(\mathrm{Cl})_{2}\right] \mathrm{Cl} \quad \overset{\text{excess }AgNO_{3}}{\rightarrow}{}\quad\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{4}(\mathrm{Cl})_{2}\right]^{+}+\mathrm{AgCl} \downarrow

\text { Using formula, Molarity }=\frac{\text { No.of }}{\text { Volume }} \times 1000

0.01=\frac{\text { No.of moles }}{100} \times 1000

\\\text {No. of moles of } \mathrm{AgCl}=0.001\\ \text{That is number of moles, not molar concentration.}

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lovekush

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