1) Assuming ideal behavior, what is the ionic concentration of a 0.135 M solution of trisodium phosphate?

2) What is the boiling point of a solution (in oC) that was prepared by dissolving 13.38 g of MgCl2 in 250.0 g water. MgCl2 is an ionic solid with a measured van't Hoff factor of 2.7. KbH2O= 0.52 oC.kg/mol

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Hubert KochLv2

20 Feb 2019

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What is the freezing point in âC of a solution prepared by dissolving 7.40 g of MgCl2 in 110 g of water? The value of Kf for water is 1.86 (âCâ kg)/mol, and the van't Hoff factor for MgCl2 is i = 2.7.

PART A

A solution is prepared from 4.5730 g of magnesium chloride and 43.232 g of water. The vapor pressure of water above this solution is found to be 0.3624 atm at 348.0 K. The vapor pressure of pure water at this temperature is 0.3804 atm.

Find the value of the van't Hoff factor i for magnesium chloride in this solution.

PART B

Use the van't Hoff factors in the table below to calculate each colligative property.

-the melting point of a 6.00Ã10^â2m iron(III) chloride solution

-the osmotic pressure of a 0.087 M potassium sulfate solution at 298 K

-the boiling point of a 1.25 % by mass magnesium chloride solution

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.