What is the boiling point of a decimolal aqueous solution of glucose if the molal elevation constant for water is $0.52 \ ^{\circ}C \ kg \ mol^{-1}$ (in $^{\circ}C$)?

If the boiling point of water is $100 \,^{\circ}C$,how many grams of $NaCl$ must be added to $500 \,g$ of water to increase the boiling point by approximately $1 \,^{\circ}C$ (in $,g$)? Given $(K_{b})_{H_2O} = 0.52 \,K \cdot kg/mol$.

The molal elevation constant is the ratio of the elevation in $B.P.$ to

Calculate the molality of a solution of a non-volatile solute if the boiling point elevation is $1.75 \ K$ and the $K_b$ for the solvent is $3 \ K \ kg \ mol^{-1}$. (in $m$)

When $0.01 \ mol$ of nonvolatile solute is dissolved in a certain solvent,calculate the mass of the solvent in $kg$ if $\Delta T_{b} = 0.6 \ K$ and $K_{b}$ for the solvent $= 2 \ K \ kg \ mol^{-1}$. (in $kg$)

What is the molal elevation constant if one gram mole of a nonvolatile solute is dissolved in $1 \ kg$ of ethyl acetate? $(\Delta T_{b} = x \ K)$