Elevation in Boiling Point of the Solvent

Correct statements about the following solutions (Assuming equal amount of each solute is dissolved in $1\mathrm{L}$ solution)

$1\mathrm{L} \mathrm{NaCl}, 1\mathrm{L} {\left({\mathrm{NH}}_2\right)}_2\mathrm{CO}, 1\mathrm{L} {\mathrm{BaCl}}_2, 1\mathrm{L} {\mathrm{Ca}}_3{\left({\mathrm{PO}}_4\right)}_2$

Equimolal solutions of $\mathrm{NaCl}, {\mathrm{BaCl}}_2$ and ${\mathrm{Na}}_3{\mathrm{PO}}_4$ are prepared in water, then correct statements are

Value of $\frac{{\mathrm{\Delta T}}_{\mathrm{b}}}{{\mathrm{K}}_{\mathrm{b}}}$ of $9\%$ (w/w) of ${\mathrm{X}}_2\mathrm{Y}$ and $6\%$ (w/w) of ${\mathrm{XY}}_2$ is $1\mathrm{mole}{\mathrm{kg}}^{-1}$ in both cases. (Consider ${\mathrm{X}}_2\mathrm{Y}$ and ${\mathrm{XY}}_2$ are non-electrolytes). Hence, atomic masses of $\mathrm{X}$ and $\mathrm{Y}$ are respectively (approx.)

Which of the following aqueous solution has highest boiling point (If solute is non-volatile and non-electrolytic)?

A mixture weighing $228\mathrm{g}$ contain ${\mathrm{CaCl}}_2$ and $\mathrm{NaCl}$. If this mixture is dissolved in $10\mathrm{kg}$ of water and form ideal solution that boil at $100.364 °\mathrm{C}$. The $\mathrm{mol}\%$ of $\mathrm{NaCl}$ in mixture is [${\mathrm{K}}_{\mathrm{b}}$ of water $=0.52\mathrm{K}{\mathrm{mol}}^{-1}\mathrm{kg}$]

Among the following solutions

(a) $0.01\mathrm{M} \mathrm{NaCl}$

(b) $0.05\mathrm{M}$ glucose

(c) $0.01\mathrm{M} {\mathrm{CaCl}}_2$

(d) $0.02\mathrm{M} \mathrm{KCl}$

The correct order of decreasing boiling point can be given as (assuming same dissociation)

A water sample contains $9.5\% {\mathrm{MgCl}}_2$ and $11.7\%$ $\mathrm{NaCl}$ (by weight). Assuming $80\%$ ionisation of each salt. Boiling point of water will be approximately $\left({\mathrm{K}}_{\mathrm{b}}=0.52\right)$

'$\mathrm{A}$' gram of non-volatile, non-electrolyte (molar mass
$\mathrm{M}$) is dissolved in $200\mathrm{ml}$ of unknown solvent (density $=1.25\mathrm{gm}/\mathrm{ml}$ molal elevation constant is ${\mathrm{K}}_{\mathrm{b}}$). Elevation in boiling point of this solution can be given by

What should be the boiling point of $1.0$ molal aqueous $\mathrm{KCl}$ solution (assuming complete dissociation of $\mathrm{KCl}$), if ${\mathrm{K}}_{\mathrm{b}}\left({\mathrm{H}}_2\mathrm{O}\right)$ is $0.52 {\mathrm{Km}}^{-1}$ ?

An aqueous solution freezes at $-2.55°\mathrm{C}$. What is its boiling point $\left[{\mathrm{K}}_b\left({\mathrm{H}}_2\mathrm{O}\right)=0.52,{ \mathrm{K}}_1\left({\mathrm{H}}_2\mathrm{O}\right)=1.86\right]?$