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At 25ºC the osmotic pressure of an aqueous CaCl2 solution is 9545.4 torr; the solution has...

At 25ºC the osmotic pressure of an aqueous CaCl2 solution is 9545.4 torr; the solution has a density of 1.71 g/mL. Calculate the new boiling point of this solution in Celsius. Assume the normal boiling point of water is 100ºC. (MMCaCl2 = 110.984 g/mol; Kb, H2O = 0.512 ºC/m; Kf, H2O = 1.86ºC/m)

Expert Solution

Calcium chloride is strong electrolyte. In water, it dissociates into ions

The vant Hoff factor

The osmotic pressure

The molar concentration

1 L (1000 mL) of solution contains 0.171 moles of calcium chloride.

Molar mass of calcium chloride is 110.984 g/mol

Mass of calcium chloride

Mass of solution

Mass of water

Convert unit from g to kg

The molality

The elevation in the boiling point

The normal boiling point of water is 100 deg C.

The new boiling point of the solution is

queen_honey_blossom answered 1 year ago

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