Question

an unknown hydrate, AC*XH2O, has a mass of 1.000 g before heating, and a mass of...


an unknown hydrate, AC*XH2O, has a mass of 1.000 g before heating, and a mass of 0.738 g after heating what is the experimental percentage of water in the hydrate? If the anhydrous compound (AC) in the preceding problem has a molar mass of 101 g/mol, what is the water of crystallization(X) and the formula for the hydrate?

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Answer #1

During heating, water is lost.

Mass of unknown hydrate is 1.000 g before heating. After heating, the mass of anhydrous compound is 0.738 g.

Mass of water lost during heating

The expermental percentage of water in hydrate

Molar mass of anhydrous compound (AC) is 101 g/mol

Mass of anhydrous compound (AC) is 0.738 g

Number of moles of anhydrous compound (AC)

Mass of water of crystallisation is 0.262 g.

Molar mass of water is 18 g/mol.

Number of moles of water of crystallisation is

The ratio of number of moles of anhydrous compound (AC) to number of moles of water of crystallisation is or

Hence, the water of crystallisation (X) is 2. The formula for the hydrate is

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