Question

A 100 g sample of a hydrate containing cobalt, sulfur, oxygen, and water lost 44.70 g...

A 100 g sample of a hydrate containing cobalt, sulfur, oxygen, and water lost 44.70 g of water when heated. The remaining anhydrous salt found to contain 21.24 g Co, 11.38 g S, and 22.68 g O. What is the empirical formula of the hydrate?

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Homework Answers

Answer #1

mass of water = 44.70 g

moles of water = 44.70 / 18 = 2.5

% Co = (21.47 / 100) x 100 = 21.47

% of S = 11.38

% of O = 22.68

convert % to atomic ratio by dividing with atomic masses

atomic ratio of Co = 21.24 / 58.9 = 0.36

atomic ratio of S = 11.38 / 32 = 0.36

atomic ratio of O = 22.68 / 16 = 1.42

now convert atomic ratio to simplest ratio by dividing with small value.

Co = 0.63 / 0.36 = 1

S = 0.36 /0.36 =1.0

O = 1.42 / 0.36 = 4.0

empirical formula of anhydrate salt = CoSO4

empirical formula of hydrated salt

CoSO4 .2.5H2O

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