Potassium perchlorate (KClO4) has a lattice energy of -599 kJ/mol and a heat of hydration of -548 kJ/mol. Find the heat of solution for potassium perchlorate and determine the temperature change that occurs when 10.0 g of potassium perchlorate is dissolved with enough water to make 100.0 mL of solution. (Assume a heat capacity of 4.05 J/g°C for the solution and a density of 1.05 g/mL.)

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1. Identify the given values: lattice energy of KClO4 is -599 kJ/mol, heat of hydration is -548 kJ/mol.
2. Calculate the heat of solution using the formula: \( \Delta H_{solution} = \Delta H_{lattice} + \Delta H_{hydration} \).
3. Convert the mass of KClO4 (10.0 g) to moles using its molar mass.
4. Calculate the total heat change (q) using the formula: \( q = n \times \Delta H_{solution} \), where n is the number of moles.
5. Determine the temperature change (\( \Delta T \)) using the formula: \( q = m \times C \times \Delta T \), where m is the mass of the solution and C is the heat capacity.