Question

A solution containing $1g$ of the complex $\left[Cr\right(H_{2}O{)}_{5}Cl]C{l}_2\cdot H_{2}O$ was passed through a cation exchanger. The acid liberated was made up to $1L$. Find the strength of the acid formed in $g/L$. (Write your answer up to two decimal places)

Answer 1

While passing through the cation exchanger there is formation of
$HCl$. Molar mass of the complex $Cr(H_{2}O{)}_{6}C{l}_2=52+108+106.5$
$=266.5g$ $mo{l}^{-1}$
$\underset{\underset{\frac{1}{266.5}}{1mol}}{\left[Cr\right(H_{2}O{)}_{5}Cl]C{l}_2}\cdot H_{2}O\to \underset{\underset{\frac{2}{266.5}mol}{2mol}}{2HCl}$
$\left[HCl\right]=7.5\times {10}^{-3}M$
$7.50\times {10}^{-3}\times 36.5g{L}^{-1}$
$=0.24g{L}^{-1}$