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11 Dec 2019

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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Patrina Schowalter
Patrina SchowalterLv2
13 Dec 2019

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Related questions

Based on your results of the boiling point elevation and melting point depressions, what is the experimental van't Hoff factor (i) for each listed solution? How does that compare to the theoretical van't Hoff factor? (Please show work) Thanks!

Solutions:

- 3.0 m NaCl in water (Exp. Boiling: 106.8 C) (Exp. Freezing: -12.4 C)

- 3.0 m MgCl2 in water ( Exp. Boiling: 107.1 C) (Exp. Freezing: -16.1 C)

- 3.0 m AlCl3 in water (Exp. Boiling: 108.5 C) (Exp Freezing: -8.4 C)

- 3.0 m ethylene glycol in water (Exp Boiling: 104.1 C) (Freezing: -7.8 C)

What is the freezing point and boiling point of an aqueous solution with 0.050 m of ? The cryoscopic constant () of water is 1.853 oC kg mol-1, while the ebullioscopic constant () of water is 0.512 oC kg mol-1. The van't Hoff factor of  is 2.7.

 

If the 3.90 m solution from Part A boils at 103.45 ^\circ {\rm C}, what is the actual value of the van't Hoff factor, i? The boiling point of pure water is 100.00 ^\circ {\rm C} and K_b is equal to 0.512 ^\circ {\rm C}/m

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