Which of the following solutions,upon complete dissociation,exhibits the maximum elevation in boiling point?

If $10 \ g$ of a solute (molar mass $= 100 \ g/mol$) is dissolved in $100 \ g$ of water,then the molal elevation constant $K_b$ of the solvent will be equal to:

For water,$K_b = 0.513 \ ^oC \ kg \ mol^{-1}$. If $0.1 \ mol$ of sugar $(C_{12}H_{22}O_{11})$ is dissolved in $200 \ mL$ of water,at what temperature will the resulting solution boil at $1 \ atm$ pressure (in $^oC$)?

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

Molal elevation constant is the elevation in boiling point produced by

When $174.5 \ mg$ of octatomic sulfur $(S_8)$ is added to $78 \ g$ of bromine $(Br_2)$,the boiling point of bromine becomes ............. $K$. Given: $K_b$ for $Br_2 = 5.2 \ K \ kg \ mol^{-1}$ and the boiling point of pure $Br_2 = 332.15 \ K$.