A solution of 22.0g CaCl2 in 100.0 cm^3 of water has a vapor pressure of 22.8 torr at 26 celsius. Why does this result supprt the view that CaCl2 is completely ionized to Ca 2+ and Cl - in aqueous solution?(At 26 C(celsius) the vapor pressure of H2O is 25.2 torr and the density of H2O is 1.00g/cm^3; CaCl2 is non-volatile)