When 0.020 mol of a weak acid HA is dissolved in enough water to make 1.0 L of solution, [H+] is 3.6 Ã10-3M. Calculate the freezing point of this solution. Assume that the molarity concentration is equal to the molality concentration, and assume ideal behavior. Kf (H2O) is 1.86Â°C kg/mol.

Ans: -.044Â°C

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Deanna HettingerLv2

17 Dec 2019

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A 0.100-g sample of the weak acid HA (molar mass=100.0 g/mol) is dissolved in 500.0 g water. The freezing point of the resulting solution is -0.0056°C. What is the value of for this acid? Assume molality equals molarity in this solution.

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A 0.100-g sample of the weak acid HA (molar mass = 100.0 g/mol) is dissolved in 500.0 g water. The freezing point of the resulting solution is −0.0056°C. Calculate the value of K a for this acid. Assume molality equals molarity in this solution.