When $1.8 \ g$ of glucose is dissolved in $100 \ g$ of solvent,the boiling point of the solution increases by $0.1 \ ^\circ C$. The molal elevation constant of the solvent is ............ $\frac{K}{m}$.

Calculate the amount of water evaporated if $2.8 \ kg$ of $2 \ m$ $CaBr_2$ solution is heated to $110 \ ^oC$ at $1 \ atm$ .......... $gm$.
(Given: $K_b$ of water $= 0.5 \ K \ kg/mol$; Atomic mass of $Ca = 40$,$Br = 80$)

The elevation in boiling point for a $0.1 \ m$ solution of a solute in $500 \ g$ of benzene is $0.51 \ K$. If $1000 \ g$ of a $0.1 \ m$ solution of the same solute in benzene is added to the above solution,the $\Delta T_b$ for the resulting solution will be ............... $K$.

Two different solutions were prepared by dissolving sucrose in water having concentrations of $1 \ m$ and $2 \ m$ respectively. The value of $(T_2 - T_1)$ will be ........... $K$. (Given: $K_b$ for water $= 0.52 \ K \ kg \ mol^{-1}$)

What is the boiling point of a $0.5 \ m$ aqueous solution of sucrose if a $0.1 \ m$ aqueous solution of glucose boils at $100.16^{\circ} C$ (in $^{\circ} C$)?

Which of the following formulas correctly gives the value of the ebullioscopic constant $(K_{b})$?