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Licemer1 [7]
3 years ago
10

A chemist is given a sample of the CuSO4 hydrate and asked to determine its the empirical formula. The original sample weighed 4

2.75 g. After heating to remove the waters of hydration, the sample weighed 27.38 g. Determine the formula for this hydrate.
Chemistry
1 answer:
Firlakuza [10]3 years ago
8 0

Answer: The formula for this hydrate is CuSO_4.5H_2O

Explanation:

Decomposition of hydrated copper sulphate is given by:

CuSO_4.xH_2O\rightarrow CuSO_4+xH_2O

Molar mass of CuSO_4 = 160 g/mol

According to stoichiometry:

(160+18x) g of CuSO_4.xH_2O decomposes to give 160 g of anhydrous CuSO_4

Thus 42.75  g of CuSO_4.xH_2O decomposes to give=\frac{160}{160+18x}\times 42.75g of anhydrous CuSO_4

\frac{160}{160+18x}\times 42.75=27.38

x=5

Thus the formula for this hydrate is CuSO_4.5H_2O

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