Question

consider two hypothetical pure substances, AB(s) and XY(s). when equal molar amounts of these substances are placed in separate 500 ml samples of water they undergo the following reactions, AB(s)=A+(aq)+B-(aq) and XY(s)=XY(aq). which solution would you expect to have the lower boiling point and why?

I am having trouble identifing trends that would help me to understand the question.

Answer 1

AB is strong electrolyte and XY is weak electrolyte.AB has more boiling point as compared to XY.

When the only volatile component of a solution is the solvent, then the vapor pressure of the solution is less than the vapor pressure tat the solvent has at any given temperature.   At the temperature at which the pure solvent normally boils, the vapor pressure of the solution is still not equal to the atmospheric pressure. So to make the vapor pressure of the solution come up to atmospheric pressure, we have to increase the temperature of the solution further. The presence of a nonvolatile solute thus elevates the boiling point of the solution.