1.615 g of anhydrous $Z n S O_{4}$ was places in moist air. After a few days, its mass was found to be 2.875g. The molecular formula for hydrated zinc sulphate is

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Solution

The correct option is C
Molecular mass of anhydrous $Z n S O_{4} = 65.5 + 32 + (4 \times 16) = 161.5$
1.615 g of anhydrous $Z n S O_{4}$ combines with (2.875 - 1.615) g = 1.260 g of water
Hence 161.5 g of $Z n S O_{4}$ combines with 126 g of water = $\frac{126}{18} = 7$ moles of water
Hence formula of hydrate $Z n S O_{4}$ is $Z n S O_{4} .7 H_{2} O$

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1.615g of an anhydrous salt was placed in moist air.After a few days it was found to be 2.875g.Assuming that complete hydration has taken place ,calculate the simplest formula of hydrated salt.The composition of anhydrous salt is(Zn=40.6%,S=19.8%,O=39.6%)

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1.615 g of anhydrous ZnSO4 was places in moist air. After a few days, its mass was found to be 2.875g. The molecular formula for hydrated zinc sulphate is

The correct option is C Molecular mass of anhydrous ZnSO4=65.5+32+(4×16)=161.5 1.615 g of anhydrous ZnSO4 combines with (2.875 - 1.615) g = 1.260 g of water Hence 161.5 g of ZnSO4 combines with 126 g of water = 12618=7 moles of water Hence formula of hydrate ZnSO4 is ZnSO4.7H2O

1.615 g of anhydrous $Z n S O_{4}$ was places in moist air. After a few days, its mass was found to be 2.875g. The molecular formula for hydrated zinc sulphate is