An aqueous solution freezes at $-0.186\,^\circ C$ ($K_f = 1.86\, K\, kg\, mol^{-1}$; $K_b = 0.512\, K\, kg\, mol^{-1}$). What is the elevation in boiling point?

For $0.1 \ M$ solutions of urea and $Al_2(SO_4)_3$,which of the following statements is correct? $(a)$ $i$ for urea is $1$ and $i$ for $Al_2(SO_4)_3$ is $5$. $(b)$ $Al_2(SO_4)_3$ has a higher elevation in boiling point. $(c)$ $Al_2(SO_4)_3$ has a higher depression in freezing point. $(d)$ Urea has a higher vapor pressure.

Calculate the osmotic pressure in $atm$ of an aqueous solution of urea at $37\,^oC$,which has a freezing point of $0.52\,^oC$. Assume molality and molarity are numerically equal. $(K_f = 1.86\,^oC\, m^{-1})$

Identify the false statement:

$A$ solution of urea (molar mass $60 \, g \, mol^{-1}$) boils at $100.18 \, ^oC$ at atmospheric pressure. If $K_f$ and $K_b$ for water are $1.86$ and $0.512 \, K \, kg \, mol^{-1}$ respectively,the above solution will freeze at ........... $^oC$.

The only incorrect statement regarding Henry's law for a gas dissolving in water is