Solutions freezing points

Tfp) the freezing point of a solution is always lower than the freezing point of the pure solvent. The freezing point depression is roughly proportional to the molality of solute particles in the solution. Freezing point depression is an example of a colligative property of a solution. 

A solution of 5.000 g of a solute in 100.0 g of water is heated slowly at a constant pressure of 1.00 atm and is observed to boil at 100.421°C. Estimate the molecular weight of the solute, the effective solvent vapor pressure at 25°C and the solution freezing point at 1 atm. The necessary properties of water can be found in Table B.I. 

This paper reports cryoscopic measurements for NiS04 aqueous solutions in saturated potassium chlorate solution (freezing point 272.55 K) and saturated potassium nitrate solution (freezing point 270.32 K). The eutectic freezing point depressions, AT, are between 0.0296 K and 0.178 K. Thus, together with the measurements reported in [56KEN], the variation in the complexation constant, K, with ionic strength was examined. 

A solutions freezing point depression, ATf, is the difference in temperature between its freezing point and the freezing point of its pure solvent. Molal freezing point depression constants (Kf) for several solvents are shown in Table 14.6. For nonelectrolytes, the value of the freezing point depression is directly proportional to the solutions molality. 

Ethylenedlamlnes Aqueous Solutions, Freezing Point vs. Composition... 

Osmotic pressure is a colligative property. A colligative property solely depends on the concentration of the dissolved molecules or ions and is independent of the nature of the solute. Freezing point depression is also a colligative property and can be indirectly used to determine osmotic pressure. In practice, it is much more difficult to determine the osmotic pressure of a solution than to measure its freezing point depression. The freezing point of a solution can be measured and the osmotic pressure can be calculated from it. 

Freezing point of solution Freezing point of solvent... 

Freezing-Point Depression Solid/Liquid Equiiibrium Freezing-Point Depression Addition of a Solute Freezing-Point Depression Solid/Solution Equilibrium... 

Plan (a) We find the numbers of cations and anions per formula unit from the name and compare it with the three scenes, (b) We convert the given mass to amount (mol), use the answer from part (a) to find moles of chloride ions (green spheres), and divide by the number of green spheres to get moles/sphere. (c) We find the molality (m) from amount (mol) of solute divided by the given mass of water (changed to kg). We multiply for water (Table 13.5) by m to get ATf, and then subtract that from 0.000°C to get the solution freezing point. 

The Phase Rule — Theory of Solutions — Supersatured Solutions — Freezing-Points of Solutions — Raoult — Vapour Pressure Lowering — Osmotic Pressure — Van t Hoff s Theory of Solutions — Van t Hoff — Chemical Kinetics — Abegg. Tammann. 

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