Elevation in Boiling Point of the Solvent

$18 \mathrm{g}$ of glucose $\left({\mathrm{C}}_6{\mathrm{H}}_{12}{\mathrm{O}}_6\right)$ dissolved in $1 \mathrm{kg}$ of water is heated to boiling. The boiling point (in $\mathrm{K}$) measured at $1 \mathrm{atm}$ pressure is closest to [Ebullioscopic constant, ${\mathrm{K}}_{\mathrm{b}}$ for water is $0.52 \mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1}$. Consider absolute zero to be $-273.15°\mathrm{C}$]

The molal boiling point elevation constant depends upon

A solution of $122 \mathrm{g}$ of benzoic-acid in $1000 \mathrm{g}$ of benzene shows a boiling point elevation of $1.4°$$.$ If the solute is dimerized to an extent of $80\%$$,$ the boiling point of pure benzene will be_________  (Molar enthalpy of vaporization of benzene $=7.8\mathrm{kcal}.{\mathrm{mol}}^{-1}$ )

The elevation in boiling point of a solution of $10 g$ of a binary electrolyte (of molecular mass $100$) in $100 \mathrm{g}$ of water is ${\mathrm{\Delta T}}_{\mathrm{b}}$. Then the value of ${\mathrm{K}}_{\mathrm{b}}$ for water is

Molal elevation constant is the elevation in boiling point produced by

The boiling point (in ${}^{\circ }\mathrm{C}$) of $0.1$ molal aqueous solution of ${\mathrm{CuSO}}_4.5{\mathrm{H}}_2\mathrm{O}$ at $1$ bar is closest to: [Given: Ebullioscopic (molal boiling point elevation) constant of water, $\left.{\mathrm{K}}_{\mathrm{b}}=0.512 \mathrm{K} {\mathrm{kgmol}}^{-1}\right]$

The molal elevation constant for water is $0.52$. What will be the boiling point of $2$ molar sucrose solution at $1 \mathrm{atm}$ pressure? (Assume that the boiling point of pure water is $100 \mathrm{℃}$)

The boiling point of benzene is $353.23\mathrm{K}$. When $1.80 \mathrm{g}$ of a non-volatile, non-ionisable solute was dissolved in $90\mathrm{g}$ of benzene, the boiling point raised to $354.11 \mathrm{K}$. Calculate molar mass of the solute in ${\mathrm{gmol}}^{-1}$( ${\mathrm{K}}_{\mathrm{b}}$ for benzene= $2.53 \mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1}$)

(Report your answer upto 1 decimal value)

The boiling point of $0.001 \mathrm{M}$ aqueous solutions of $\mathrm{NaCl}, {\mathrm{Na}}_2{\mathrm{SO}}_4, {\mathrm{K}}_3{\mathrm{PO}}_4$ and ${\mathrm{CH}}_3\mathrm{COOH}$ should follows the order.

Latent heat of vaporization for a liquid solvent is $500 \mathrm{cal} {\mathrm{g}}^{-1}.$ Let the boiling point be ${\mathrm{T}}_{\mathrm{b}} \mathrm{K}.$ Find the value of ${\mathrm{K}}_{\mathrm{b}}$ of the solvent in $\mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1}$. 

$58.5 \mathrm{g} \mathrm{of} \mathrm{NaCl} \mathrm{and} 180 \mathrm{g}$of glucose were separately dissolved in $1000 \mathrm{mL}$ of water. Identify the correct statement regarding the elevation of boiling point (b.pt.) of the resulting solutions.

The molal elevation constant is the ratio of the elevation in boiling point to:

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

The unit of an ebullioscopic constant is ______.

Boiling point of a solvent is $80.2°\mathrm{C}$. When $0.419 \mathrm{g}$ of the solute of molar mass $252.4 \mathrm{g} {\mathrm{mol}}^{-1}$ was dissolved in $75 \mathrm{g}$ of the solvent, the boiling point of the solution was found to be $80.256°\mathrm{C}$. Find the molal elevation constant.

Calculate the mass in grams of an impurity of molar mass $100 \mathrm{g} {\mathrm{mol}}^{-1}$ which would be required to raise the boiling point of $50 \mathrm{g}$ of chloroform by $0.30 \mathrm{K}$. $({\mathrm{K}}_{\mathrm{b}}$ for chloroform = $3.63 \mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1})$

If mass is expressed in gram then ${\mathrm{K}}_{\mathrm{b}}$ is given by.

The determination of molar mass from elevation in boiling point is called as

When $\mathrm{NaCl}$ is added to water.