Question

Metallic tin in the presence of $HCl$ is oxidized by $K_{2}C{r}_2{O}_7$ to stannic chloride, $\left(SnC{l}_4\right)$. What volume of decinormal dichromate solution would be reduced by $1$ g of tin?

• A. $70$ mL
• B. $85$ mL
• C. $30$ mL
• D. $40$ mL

Answer 1

The correct option is D $40$ mL

$1$ g $Sn=\frac{1}{119}=0.0084$ moles

The oxidation number of $Sn$ changes from $0$ to $4$.

Hence, 1 mole $Sn$ corresponds to 4 equivalents. It will reduce 4 equivalnets of dichromate solution. Volume of decinormal dichromate solution $=\frac{4}{0.1}=40ml$.