Astudent weighs out 3.23 g of fe(no3)3 • ? h2o and heats it. the remaining anhydrous salt has a mass of 1.93 g. calculate the empirical formula for the hydrate.

The empirical formula is :

Explanation:

Let us assume the moles of hydration in ferric nitrate is ''

Thus the formula of the compound becomes :

Now when its heated , the reaction proceeds like  :

⇒

Given ,

The mass of anhydrated

Molar mass of respectively.

The mass of 1 mol of

The number of moles =

Therefore the number of hydrated moles must also be 0.008

Given ,

The mass of hydrated

The molecules contain like 54 of water 

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