Calculate the amount of $KCl$ $(MW=74.5 \ g \ mol^{-1})$ required to depress the freezing point of $500 \ g$ of water by $2 \ K$ (in $g$)? $(K_f=1.86 \ K \ kg \ mol^{-1})$

$17.4\% \text{ (mass/volume) } K_2SO_4$ solution at $27^\circ C$ is isotonic to $5.85\% \text{ (mass/volume) } NaCl$ solution at $27^\circ C$. If $NaCl$ is $100\%$ ionized,what is the $\%$ ionization of $K_2SO_4$ in aqueous solution? [Atomic weights: $K = 39, Na = 23, S = 32, O = 16, Cl = 35.5$]

$1 \ mol$ each of the following compounds is dissolved in $1 \ L$ of solution. Which will have the largest $\Delta T_b$ value?

Which of the following is not a non-electrolyte?

Consider the following solutions at $25\,^oC$:
$(I)$ $0.01\, M$ aqueous solution of glucose
$(II)$ $0.01\, M$ aqueous solution of $KNO_3$
$(III)$ $0.01\, M$ solution of acetic acid in benzene
Select the correct statement.

The addition of a polar solvent to a solid electrolyte results in