Are the crystals of salts really dry

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Solution

Yes, the crystals of salts are really dry as the water molecules present in them don't act as water but instead give them a crystalline structure.
Example: Copper sulphate crystals(blue) which seem to be dry contain water of crystallization.
Copper sulphate crystals look dry but contain water for crystallization. When we apply some heat to these copper sulphate crystals(blue) the water comes out and copper sulphate turns white in color. If we are going to add water to the white color copper sulphate, it regains its blue color.
Equation : $C u S O_{4} .5 H_{2} O (B l u e) h e a t - -- \to C u S O_{4} (w h i t e) + 5 H_{2} O$

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Q. Are the crystals of salts really dry

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N H_{3}

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[N i {(N H_{3})}_{6}] B r_{2}

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If you are given some copper sulphate crystals, how would you proceed to prepare its saturated solution at room temperature? Give practical details. How can you show that your solution is really saturated?

Q. Copper sulphate crystals which seem to be dry contain water of crystallization. When we heat the crystals, this water is removed and the salt turns white. If you moisten the crystals again with water, you will find that blue colour of the crystals reappears.

The water of crystallization is the fixed number of water molecules present in one formula unit of a salt. Five water molecules are present in one formula unit of copper sulphate. The chemical formula for hydrated copper sulphate is

C u {S O}_{4}

5 H_{2} O

. Now you would be able to answer the question whether the molecule of

{N a}_{2} {C O}_{3}

10 H_{2} O

is wet. One other salt, which possesses water of crystallization is gypsum. It has two water molecules as a water of crystallization. It has the formula

C a {S O}_{4}

2 H_{2} O

What are the uses of this salt?

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