of copper (II) sulfate 

You are provided with : The aim of this activity is to measure the enthalpy of hydration of copper sulfate using Hess's Law . 

The enthalpy of hydration is difficult to calculate as it is not possible to measure the chemical potential energy directly as the CuSO_{4}.5H_{2}O crystallizes.  
We can calculate the ΔH of equation 3 if we know the ΔH of equation 1 and 2. You will perform this practical in two stages. Then you will use a calorimeter to measure the ΔH of equation 2. 

Using Hess's Law you will then work out the ΔH of equation 3. This has two parts.
Part one  reverse equation 1 Part two  add it to equation 2.


Step 1 measure the mass of a crucible  
Step 2 Measure accurately about 23.0 g of copper sulfate pentahydrate (CuSO_{4}.5H_{2}O )  
Step 3 Add 100 mL of distilled water to the calorimeter  
Step 4 Measure the temperature of the water.  
Step 5 Add the CuSO_{4}.5H_{2}O to the water and seal the calorimeter. Stir the the water to allow for the CuSO_{4}.5H_{2}O to dissolve.  
Step 6 Record the final temperature of the water.  
Step 7 Calculate the ΔH. of the reaction below CuSO_{4} .5H_{2}O (s) + (aq) => CuSO_{4}(aq) + H_{2}O(l) 