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Explainer Video

Tutor: Aimee LeBrun

Summary

Formulae for crystals and salts

In a nutshell

Salts formed during a reaction can contain water molecules in their lattice structures. This water is known as the water of crystallisation.

Water of crystallisation

Definition

The water of crystallisation is known as the the water molecules embedded in the lattice structure of a salt.

When a salt contains water this salt is known as a hydrated salt. A salt that does not contain water is known as anhydrous. One mole of the hydrated salt is equal to the same number of moles as the water of crystallisation.

Example

Hydrated calcium chloride has the formula $CaCl_2\bullet6H_2O$ .

When hydrated salts are heated, they lose water and become fully anhydrous.

The formula of a hydrated salt can be found using the following method:

procedure

1.	First, find the mass of water that is lost.
2.	Use this to find the number of moles of water lost using the equation: $n \, = \, \frac{m}{M}$
3.	Find the number of moles of the anhydrous salt using the mass and molar mass of the salt: $n \, = \, \frac{m}{M}$
4.	Divide the number of moles of water by the number of moles of anhydrous salt to find the number of moles of water in the salt. This number will be placed before the ' $H_2O$ ' in the formula.

Example

$21.096 \, g$ of $CaSO_4\bullet XH_2O$ is heated to form $10.242 \, g$ of anhydrous calcium sulfate. What is the formula for the hydrated calcium sulfate?

Find the mass of the water that is lost:

$m \, = \, 21.096 \, - \, 10.242 \, = \, 10.854 \, g$ 

Use the following equation to find the number of moles of the water:

$n \, = \frac{m}{M}$ 

Find the molar mass of water ( $H_2O$ ):

$M \, (H_2O) \, = \, (1 \, \times \, 2) \, + \, 16 \, = \, 18 \, g \, mol^{-1}$

Substitute the values for the mass and molar mass to find the number of moles of the water that is lost:

$n \, = \, \frac{10.854}{18} \, = \, 0.603 \, mol$ 

Use the following equation to find the number of moles of the anhydrous salt:

$n \, = \frac{m}{M}$ 

Find the molar mass of the anhydrous salt ( $CaSO_4$ ):

$M \, (CaSO_4) \, = \, 40.1 \, + \, 32.1 \, + \, (16 \, \times \, 4) \, = \, 136.2 \, g \, mol^{-1}$

Substitute the values for the mass and molar mass to find the number of moles of anhydrous salt:

$n \, = \, \frac{10.242}{136.2} \, = \, 0.0752 \, mol$ 

Finally, divide the number of moles of water by the number of moles of the anhydrous salt:

$\frac{0.603}{0.0752}\, = \, 8.019 \, mol$

Therefore, the formula for the hydrated calcium sulfate is $\underline{CaSO_4\bullet 8H_2O}$ .

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Preparing soluble and insoluble salts

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