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During a lab, you heat 1.62 g of a CoCl2 hydrate over a Bunsen burner. After heating, the final mass of the dehydrated compound is 0.88 g. Determine the formula of the hydrate and also give the full name of the hydrate.
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Answer is: formula of hydrate is CoCl₂· 6H₂O -cobalt(II) chloride hexahydrate
m(CoCl₂· xH₂O) = 1,62 g.
m(CoClâ‚‚) = 0,88 g.
n(CoCl₂) = m(CoCl₂) ÷ M(CoCl₂)
n(CoCl₂) = 0,88 g ÷ 130 g/mol
n(CoClâ‚‚) = 0,0068 mol.
m(Hâ‚‚O) = 1,62 g - 0,88 g.
m(Hâ‚‚O) = 0,74 g.
n(H₂O) = m(H₂O) ÷ m(H₂O) 
n(H₂O) = 0,74 g ÷ 18 g/mol
n(H₂O) = 0,041 mol.
n(CoCl₂) : n(H₂O) = 0,0068 mol : 0,041 mol.
n(CoCl₂) : n(H₂O) = 1 : 6.

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