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Heat of Solution

# Heat of Solution - Heat of Solution Objective To determine...

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Heat of Solution Objective : To determine and interpret the heats of solution in water of Lithium Chloride, Potassium Chloride, and Calcium Chloride. Experimental Data : T 1 T 2 -*C LiCl 23.12 23.24 1.18 KCl 24.49 23.31 2.07 CaCl 2 23.25 27.23 3.09 Sample Calculations : LiCl: q surroundings = (m 1 + m 2 ) C soln (T 2 – T 1 ) q surroundings = (1.18 g + 100 g)(4.100 × 10 ^ -3)(23.24 - 23.12) q surroundings = -q salt q salt = 0.0498 ∆H soln = (q salt / m 1 )(molar mass) ∆H soln = (.0.498/1.18)(42.5) ∆H soln = -1.79 ∆H soln = ∆H lattice + ∆H hydration -1.79 = 853 + X X = -854.79 = ∆H hydration Results and Conclusions : Salt ∆H lattice (KJ/mol) ∆H soln (KJ/mol) ∆H hydration (KJ/mol) C soln (KJ g-1 deg-1) LiCl 853 -1.79 -854.8 4.100 × 10 ^ -3 NaCl 786 3.9 -782 4.092 × 10 ^ -3 KCl 715 17.5 -697.5 4.038 × 10 ^ -3 CaCl 2 2258 -60.7 -2318.7 4.125 × 10 ^ -3 The higher the specific heat capacity, the lower the heat of solution value. The metals, Li, Na, and K, all follow a path in the graph. Also, in the graph the Ca metal does not lie in the path of the other metals because the heat of solution is so low in CaCl 2 . Discussion of Experimental Uncertainty : There are a few uncertainties with this experiment. One, being that the water can be

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