Elevation in Boiling Point of the Solvent

If an equimolar solution of ${\mathrm{CaCl}}_2$, and ${\mathrm{AlCl}}_3$ in water have boiling point of ${\mathrm{T}}_1$ and ${\mathrm{T}}_2$ respectively then

Define elevation in boiling point. How can you calculate the molecular mass of a non-volatile solute with it ?

If the boiling points of two solvents $\mathrm{X}$ and $\mathrm{Y}$ (having same molecular weights) are in the ratio $\text{2: 1}$ and their enthalpy of vaporizations are in the ratio $1: 2$, then the boiling point elevation constant of $\mathrm{X}$ is $\mathrm{m}$ times the boiling point elevation constant of $\mathrm{Y}$. The value of $\mathrm{m}$ is (nearest integer).

Sea water contains $29.25\%\mathrm{NaCl}$ and $19\%{\mathrm{MgCl}}_2$ by weight of solution. The normal boiling point of the sea water is ${}^{\circ }\mathrm{C}$ (Nearest integer) Assume $100\%$ ionization for both $\mathrm{NaCl}$ and ${\mathrm{MgCl}}_2$ Given: ${\mathrm{K}}_{\mathrm{b}}\left({\mathrm{H}}_2\mathrm{O}=0.52 \mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1}\right)$ Molar mass of $\mathrm{NaCl}$ and ${\mathrm{MgCl}}_2$ is $58.5$ and $95 \mathrm{g}$ ${\mathrm{mol}}^{-1}$ respectively.

$60 \mathrm{g}$ of a non-volatile solid $\mathrm{AB}$(having crystals like $\mathrm{NaCl}$) is dissolved in $0.50 \mathrm{kg}$ water. The normal boiling point of solution is found to be $102.08°\mathrm{C}$. The molal elevation of water is $0.52 \mathrm{K}-\mathrm{kg} {\mathrm{mol}}^{-1}$. The density of solid $\mathrm{AB}$ is $6.25 \mathrm{g}/{\mathrm{cm}}^3$ and the edge-length of unit cell is $400 \mathrm{pm}$. The effective number of atoms per unit cell is (Use Avogadro's number $=6\times {10}^{23}$)

Calculate the elevation in boiling point of an aqueous solution of $0.1$ molal monobasic acid, which undergoes $25\%$ ionization is $\left({\mathrm{K}}_{\mathrm{b}}\right({\mathrm{H}}_2\mathrm{O})=0.52 {\mathrm{Kmolal}}^{-1})$

$2\mathrm{g}$ of non-electrolyte solute dissolved in $200\mathrm{g}$ of water shows an elevation of boiling point of $0.{026}^{\mathrm{o}}\mathrm{C}$. ${\mathrm{K}}_{\mathrm{b}}$ of water is $0.52\mathrm{K}. {\mathrm{mole}}^{-1} \mathrm{Kg}$ then the molecular weight of solute is $\mathrm{x}\times 100$. What is the value of '$\mathrm{x}$'?

Calculate the molal elevation boiling point constant of a solution containing $1.0 \mathrm{g}$ of urea $(\mathrm{M}=60)$ in $75 \mathrm{g}$ water and boils at $100.{114}^{\circ }\mathrm{C}$.

The molal elevation constant for water is $0.56 \mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1}$. Calculate the boiling point of solution made by dissolving$6.0 \mathrm{g}$ of urea (${\mathrm{NH}}_2{\mathrm{CONH}}_2$) in $200 \mathrm{g}$ of water.

The rise in boiling point of a solution containing $1.8 \mathrm{g}$ of glucose in $100 \mathrm{g}$ of solvent is $0.1°\mathrm{C}$. The molal elevation constant of the liquid is

The aqueous solution that shows the maximum boiling point elevation is [Assume identical conditions]

Calculate the boiling point of solution when $4 \mathrm{g}$ of ${\mathrm{MgSO}}_4 \left(\mathrm{M}=120 \mathrm{g} {\mathrm{mol}}^{-1}\right)$ was dissolved in $100 \mathrm{g}$ of water, assuming ${\mathrm{MgSO}}_4$ undergoes complete ionization. $({\mathrm{k}}_{\mathrm{b}} \mathrm{for} \mathrm{water}=0.52 \mathrm{K} \mathrm{Kg} {\mathrm{mol}}^{-1})$

$6 \mathrm{g}$ of urea and $1 \mathrm{g}$ of glucose are dissolved $300 \mathrm{g}$ of water find the boiling point of solutions and pure water boiling point is ${100}^{\circ }\mathrm{C}$. ${\mathrm{k}}_{\mathrm{b}}$ for water is $0.52 \mathrm{kkg}/\mathrm{mol}$.

A student observed that the boiling of the water containing $10 \mathrm{g}/\mathrm{l}$ of $\mathrm{NaCl}$ was $101.5^{\circ }\mathrm{C}$. If more water is added to the solution, will its boiling point increase or decrease? Give reason.

$1\mathrm{L}$ of aq. Solution of urea having density $= 1.060 \mathrm{gm}/\mathrm{mL}$is found to have ${\mathrm{\Delta T}}_{\mathrm{b}} = 0.5°\mathrm{C}$, if temperature of this solution increase to $101.5°\mathrm{C}$ then calculate amount of water which must have gone into vapour state up to this point. Given${\mathrm{K}}_{\mathrm{b}}= 0.5 {\mathrm{Kkgmol}}^{-1}$for water

Which of the following aqueous solutions should have the minimum boiling point?

What will happen to the boiling point of a solution if the weight of the solute dissolved is doubled but the weight of solvent taken is halved?

Which solution has maximum boiling point?