Freezing point depression can be used to experimentally determine the van 't Hoff factor of a solute in solution. Given the data in the table, answer the questions below and determine the "real" van 't Hoff factor of the solute. Experimental Results Mass of solvent (water) 8.413 g Freezing point of water 0.00°C Freezing point depression constant (Kf) of water     1.86°C/m Mass of solution 9.226 g Freezing point of solution −4.73°C (a) What mass of solute was used?   g (b) What is the freezing point depression ΔTf of the solution?   °C (c) What is the colligative molality mc of the solution?   m (d) How many moles of solute particles are present in solution?   mol (e) If the solute has a molar mass of 144.02, what is the van 't Hoff factor i for the solute? (Remember that experimentally, i does not have to be an integer.)

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Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.