Water of Crystallisation
- Water of crystallisation is when some compounds can form crystals which have water as part of their structure
- A compound that contains water of crystallisation is called a hydrated compound
- The water of crystallisation is separated from the main formula by a dot when writing the chemical formula of hydrated compounds
- E.g. hydrated copper(II) sulfate is CuSO4∙5H2O
- A compound which doesn’t contain water of crystallisation is called an anhydrous compound
- E.g. anhydrous copper(II) sulfate is CuSO4
- A compound can be hydrated to different degrees
- E.g. cobalt(II) chloride can be hydrated by six or two water molecules
- CoCl2 ∙6H2O or CoCl2 ∙2H2O
- The conversion of anhydrous compounds to hydrated compounds is reversible by heating the hydrated salt:
- The degree of hydration can be calculated from experimental results:
- The mass of the hydrated salt must be measured before heating
- The salt is then heated until it reaches a constant mass
- The two mass values can be used to calculate the number of moles of water in the hydrated salt - known as the water of crystallisation
Worked example
Calculating water of crystallisation
11.25 g of hydrated copper sulfate, CuSO4.xH2O, is heated until a constant mass of 7.19 g.
Calculate the formula of the hydrated copper(II) sulfate.
Ar (Cu) = 63.5 Ar (S) = 3. Ar (O) = 16 Ar (H) = 1
Answer:
1. Salt and water | CuSO4 | H2O |
2. Value | 7.19 | 11.25 - 7.19 = 4.06 |
3. Mr | 63.5 + 32 + (16 x 4) = 159.5 |
(1 x 2) + 16 = 18 |
4. Moles = | = 0.045 | = 0.226 |
5. Salt : water ratio | = 1 | = 5 |
6. Formula of hydrated salt | The formula is CuSO4•5H2O |
Examiner Tip
- Instead of elements, you start with the salt and water
- Instead of dividing by atomic masses, you divide by molecular / formula masses
- The rest of the calculation works the same way as the empirical formula calculation