A student determined the molar mass of an unknown ionic solid by the method used in this experiment.  She found the equilibrium temperature of the ice water mixture (THE FREEZING POINT) to be 0.50°C on her thermometer.  When she added 3.10 g of her solid to the mixture, the temperature fell to -4.30°C. She then poured off the solution into a beaker.  The mass of the solution was 34.59 g.  Kf = 1.86°C/m What was the freezing point depression ∆Tf (celsius) What was the molality of the unknown solution? How much water was in the solution? What did she find to be the observed molar mass of the ionic solid, assuming she made the calculation properly?

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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.