David is trying to determine the enthalpy of vaporization of water. In a closed container, which is emptied of atmospheric air, he measures corresponding values of pressure and temperature. He only makes two measurements around the boiling point, and assumes that the enthalpy of vaporization is independent of the temperature.

Temperatur (oC)	Pressure (bar)
90,34	0,707
95,92	0,866

1. From the data in the table, determine the enthalpy of vaporization of the water in David's experiment. David also knows that water has an entropy of vaporization of 109.1 J/(mol K) at its normal boiling point.

2. Determine the normal boiling point of water based on David's experiment.

3. How many grams of the easily soluble salt CaCl₂ must be added to 800.00 g of water to raise its boiling point by 2.5C? You can assume that the equations for dilute solutions apply.

4. Calculate the ionic strength of the resulting solution of CaCl₂ in water. The density of water is 0.958 g/mL at its normal boiling point.