7.10 Heat of Dilution

The amount of heat evolved or absorbed when solution containing one mole of solute is diluted from one concentration to another. For example,

HCl(g) + 10H2O ® HCl.10H2O; DH1 = – 69.01 kJ/mol

HCl(g) + 25H2O ® HCl.25H2O; DH2 = – 72.03 kJ/mol

HCl(g) + 40H2O ® HCl.40H2O; DH3 = – 72.79 kJ/mol

HCl(g) + ¥H2O ® HCl.¥H2O; DH¥ = – 74.85 kJ/mol

If we subtract first equation from the second in the above set, we get

HCl.10H2O + 15H2O ® HCl.25H2O; DH = (DH2 – DH1) = – 3.02 kJ/mol

This value of DH is the heat of dilution. The heat of dilution of a solution is dependent on the original concentration of the solution and on the amount of the solvent added.

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