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Assuming ideal behavior, find the boiling point of a solution made by dissolving 32.8 g of calcium nitrate in 108 g of water. Use 0.512 (oC)/m as the molal boiling point elevation constant for this solution. 

What are the Moles Ca(NO3)2 

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Related questions

A solution is prepared by dissolving 125.0 g sucrose (C12H22O11) in 502.0 g water. At what temperature, in °F, would this solution boil? (The boiling point of pure water is 100°C (exactly) at 1 atm pressure and molal boiling-point-elevation constant for water is 0.513°C/m.)

What mass of salt would have to be added to 750.0 mL of water inorder to raise the boiling point of the solution by 0.5 C? Assumethe ideal van't Hoff factor for NaCl.

Hint:
The boiling point elevation constant of water is 0.512 C/m.


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