The freezing point of an equimolal aqueous solution will be highest for:

When $10^{-3} \ M$ solution of glucose in water freezes at $-0.0186^{\circ} C$,then at what temperature $10^{-3} \ M$ solution of $NaCl$ will freeze (in $^{\circ} C$)?

What is the percentage of dissociation of a $0.011 \ m$ aqueous solution of $K_3[Fe(CN)_6]$ having a freezing point of $-0.063 \ ^oC$? (Given: $K_f = 1.86 \ K \ kg \ mol^{-1}$ for water)

Which of the following aqueous solutions has the highest boiling point?

$12.25 \ g$ of $CH_3CH_2CHClCOOH$ is added to $250 \ g$ of water to make a solution. If the dissociation constant of the above acid is $1.44 \times 10^{-3}$,the depression in the freezing point of water in $^{\circ}C$ is ($K_f$ for water is $1.86 \ K \ kg \ mol^{-1}$)

$A$ compound contains $1.08 \ mol$ of $Na, 0.539 \ mol$ of $Cu$ and $2.16 \ mol$ of $F$. Its aqueous solution shows osmotic pressure which is three times that of urea having the same molar concentration. The formula of the compound is: