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1h. A certain pure solvent freezes at 39.8°C and has a freezing point depression constant Kf...

1h. A certain pure solvent freezes at 39.8°C and has a freezing point depression constant Kf = 0.777°C/m. What is the predicted freezing point (in °C) of a solution made from this solvent that is (1.90x10^0) m in a non-electrolyte solute?

1i. When (8.23x10^1) g of a non-electrolyte is dissolved in (5.2600x10^2) g of a solvent (with Kb = 0.416°C/m) the boiling point of the solution is 1.50°C higher than the boiling point of the pure solvent. What is the molar mass (in g/mol) of the non-electrolyte solute?

1j. How many grams of Mg(NO3)2 (MM = 148.33 g/mol) would it take to lower the freezing point of (5.16x10^2) grams of water by 4.00°C? The freezing point depression constant of water is Kf = 1.86°C/m.

Please help, will rate, Thank you so much!

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