Answer: The formula for this hydrate is [tex]CuSO_4.5H_2O[/tex]
Explanation:
Decomposition of hydrated copper sulphate is given by:
[tex]CuSO_4.xH_2O\rightarrow CuSO_4+xH_2O[/tex]
Molar mass of [tex]CuSO_4[/tex] = 160 g/mol
According to stoichiometry:
(160+18x) g of [tex]CuSO_4.xH_2O[/tex] decomposes to give 160 g of anhydrous [tex]CuSO_4[/tex]
Thus 42.75 g of [tex]CuSO_4.xH_2O[/tex] decomposes to give=[tex]\frac{160}{160+18x}\times 42.75[/tex]g of anhydrous [tex]CuSO_4[/tex]
[tex]\frac{160}{160+18x}\times 42.75=27.38[/tex]
[tex]x=5[/tex]
Thus the formula for this hydrate is [tex]CuSO_4.5H_2O[/tex]
