3.00 g of KCl is dissolved in 500.0 g of water to make an aqueous solution at 303 K. a. What is the concentration of KCl in ppm? b. What is the freezing point of this solution if 2.00 L of 0.100 M KCl (ρ = 1.05 g/mL) is added? The cryoscopic constant for water is 1.86 °C·kg/mol. Assume ideal behavior of the ions.

c. What is the vapor pressure in torr of the solution described in (b) at 303 K? You will need to look up the vapor pressure of water at this temperature.

the product of the pressure and volume is also constant

the best answer is d because the strong cohesion is caused by the ability of water molecules to undergo hydrogen bonding.

a is incorrect because when water solidifies, it becomes   ice, which expands and occupies a bigger volume for the same mass of water in its liquid state.

b is incorrect because water has high surface tension. besides bonding to itself it hydrogen bonds to other molecules at the top decreasing possibility for breaking of attractive forces.

c is incorrect because the water molecule has oxygen which is highly electronegative and so pulls the electron pair towards itself creating a dipole moment, making the molecule polar.

e is incorrect because water has strong adhesion, ability to stick to other molecules such as glass because of this molecules having stronger hydrogen bonding than water.