K L Chugh Solutions for Chapter: Solutions, Exercise 6: Follow Up Problems

A solution containing $7.5 \mathrm{g}$ of urea (Mol. wt. $60$) in one $\mathrm{kg}$ of water freezes at the same temperature as another solution containing $15 \mathrm{g}$ of solute $\mathrm{S}$ in the same amount of water. Calculate molecular mass of $\mathrm{S}.$

Water is used in car radiators. In winter season, ethylene glycol is added to water so that water may not freeze:
Assuming ethylene glycol to be non-volatile, calculate minimum amount of ethylene glycol that must be added to $6.0 \mathrm{kg}$ of water to prevent it from freezing at $-0.3°\mathrm{C}.$ The molal depression constant of water is $1.86°.$

$45 \mathrm{g}$ of ethylene glycol ${\mathrm{C}}_2{\mathrm{H}}_6{\mathrm{O}}_2$ is mixed with $600 \mathrm{g}$ of water. Calculate the freezing point depression.

$45 \mathrm{g}$ of ethylene glycol, ${\mathrm{C}}_2{\mathrm{H}}_6{\mathrm{O}}_2$ is mixed with $600 \mathrm{g}$ of water. Calculate the freezing point of the solution.

$1.00 \mathrm{g}$ of a non electrolyte solute dissolved in $50.0 \mathrm{g}$ of benzene lowered the freezing point of benzene by $0.40 \mathrm{K}.$ The freezing point depression constant of benzene is $5.12 \mathrm{K} \mathrm{kg} \mathrm{mol}{ }^{-1}.$ Find the molecular mass of the solute.