Calculate the molalities, the change in boiling points (ΔTbp), and the change in freezing points (ΔTfp) of water at 1 atm if 0.500 moles of each of the following compounds are dissolved in 200.00 g of water. (Round your answer to 3 sig figs) (a) Fructose, C6H12O6 (a non-electrolyte)
m = mol/kg
ΔTbp = °C
ΔTfp = °C

(b) Sodium chloride
m = mol/kg
ΔTbp = °C
ΔTfp = °C

(c) Barium nitrate
m = mol/kg
ΔTbp = °C
ΔTfp = °C

A0.10 m aqueous solution of sodium sulfate is a better conductor of electricity than a 0.10 m aqueous solution of sodium chloride. which of the following best explains this observation? (a) sodium sulfate is more soluble in water than sodium chloride. (b) sodium sulfate has a higher molar mass than sodium chloride. (c) to prepare a given volume of 0.10 m solution, the mass of sodium sulfate needed is more than twice the mass of sodium chloride needed. (d) more moles of ions are present in a given volume of 0.10 m sodium sulfate than in the same volume of 0.10 m sodium chloride. (e) the degree of dissociation of sodium sulfate in solution is significantly greater than that of sodium chloride.