The number of water molecules associated with copper sulphate molecule to form crystals is
5
Understanding Water Molecules in Copper Sulfate Crystals
When certain salts crystallize from an aqueous solution, water molecules become an integral part of the crystal structure. These water molecules are known as water of crystallization.
Copper sulfate is a well-known example of a salt that forms hydrated crystals. The most common crystalline form of copper sulfate is copper(II) sulfate pentahydrate.
The chemical formula for copper(II) sulfate pentahydrate is \(\text{CuSO}_4 \cdot 5\text{H}_2\text{O}\).
This formula indicates that for every one molecule of copper sulfate (\(\text{CuSO}_4\)), there are five molecules of water (\(\text{H}_2\text{O}\)) associated with it within the crystal structure.
Therefore, the number of water molecules associated with the copper sulfate molecule to form crystals is 5.
Copper(II) sulfate pentahydrate is commonly known as blue vitriol due to its characteristic bright blue color.
Copper Sulfate Crystal Formula
The hydrated form of copper sulfate clearly shows the water molecules bonded within its structure. The formula \(\text{CuSO}_4 \cdot 5\text{H}_2\text{O}\) explicitly shows the presence of five water molecules. The dot (\(\cdot\)) in the formula signifies that the water molecules are associated with the salt but are not covalently bonded to the anion or cation in the same way the sulfate ion is bonded to copper.
The properties of hydrated copper sulfate, such as its color and crystal shape, are due to the presence of these water molecules.
Revision Table: Copper Sulfate Hydration Facts
| Property | Details |
|---|---|
| Chemical Name | Copper(II) Sulfate Pentahydrate |
| Chemical Formula | \(\text{CuSO}_4 \cdot 5\text{H}_2\text{O}\) |
| Number of Water Molecules | 5 |
| Common Name | Blue Vitriol |
| Appearance | Blue crystals |
Additional Information: Dehydration of Copper Sulfate
When hydrated copper sulfate is heated, it loses its water of crystallization in steps.
- Heating \(\text{CuSO}_4 \cdot 5\text{H}_2\text{O}\) removes water molecules, changing its color.
- Partial dehydration occurs first, leading to less hydrated forms.
- Strong heating removes all water molecules, resulting in anhydrous copper sulfate (\(\text{CuSO}_4\)), which is a white powder.
- The dehydration process is reversible; anhydrous copper sulfate turns blue again when it absorbs water. This property is sometimes used as a test for the presence of water.
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