Specific heat, CaCl2 solutions

The dissolution of CaCl2(s) in water is exothermic, with AHso]n = —81.3 kj/mol. If you were to prepare a 1.00 m solution of CaCl2 beginning with water at 25.0°C, what would the final temperature of the solution be (in °C) Assume that the specific heats of both pure H2O and the solution are the same, 4.18 J/(K g). 

An 11.0-g sample of CaCl2 is dissolved in 125 g of water, with both substances at 25.0°C. Calculate the final temperature of the solution assuming no heat lost to the surroundings and assuming the solution has a specific heat capacity of 4.18 J °C 1 g-1. 

Solid CaCl2-6H20 and liquid water at 298.15 K (25°C) are mixed adiabatically in a continuous process to form a brine of 15-mass-% CaCl2. Using data from Pb. 12.37, determine the temperature of the brine solution fonned. The specific heat of a 15 mass-% aqueous CaCls solution at 298.15 K (25°C) is 3.28 kJ kg °K . 

A U. luO-L solution is made by dissolving u.44i gof CaCl2(s) in water, (a) Calculate the osmotic pressure of this solution at 27 "C, assuming that it is completely dissociated into its component ions, (b) The measured osmotic pressure of this solution is 2.56 atm at 27 C. Explain why it is less than the value calculated in (a), and calculate the van t Hoff factor, i, for the solute in this solution. (See the A Closer Look box on Colligative Properties of Electrolyte Solutions in Section 13.5.) (c) The enthalpy of solution for CaCl2 is AH = —81.3 kj/mol. If the final temperature of the solution is 27 °C, what was its initial temperature (Assume that the density of the solution is 1.00 g/mL, that its specific heat is 4.18 J/g-K, and that the solution loses no heat to its surroundings.)... 

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