A solution containing $2.5 \times 10^{-3}\, kg$ of a solute dissolved in $75 \times 10^{-3} \,kg$ of water boils at $373.535$ $K$. The molar mass of the solute is $.....\,g\, mol ^{-1}$. [nearest integer] (Given: $K _{ b }\left( H _{2} O \right)=0.52 \,K\, Kg\,mol ^{-1}$, boiling point of water $=373.15 \,K$ )
→$'x' + H_2O \xrightarrow[{{H_2}S{O_4}}]{{HgS{O_4}}}$ $\begin{array}{*{20}{c}}
{C{H_3} - C - C{H_2} - C{H_3}} \\
{|\,|\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,} \\
{O\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,}
\end{array}$ reactant $'x'$ in above reaction is-
→At higher altitude, boiling point of water is $95\,^oC$. The amount of $NaCl$ added to $1\, kg$ of water $(K_b = 0.52\, K\, mol^{-1}\,kg)$ in order to raise the boiling point of solution to $100\,^oC$ (assuming $90\%$ ionisation of $NaCl$) ........... $g$
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