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The aim of this practical experiment is to calculate the formula of hydrated Iron(II) Sulphate crystals, using two methods.

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  • Essay length: 1237 words
  • Submitted: 07/11/2003
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GCSE Aqueous Chemistry

The first 200 words of this essay...

Chemistry practical

Date: 26th September 2003

Name: Frazar Ngosa

Aim: the aim of this practical experiment is to calculate the formula of hydrated Iron(II) Sulphate crystals, using two methods.

Abstract

Introduction and Theory

Hydrated Iron(II) Sulphate crystals contains water of crystallization. Water of crystallization is the fixed amount of water that an hydrated salt contains.

The formula of an hydrated salt is generally written as M.xH2O, where the M is an hydrous salt formula, and x is the number of moles of water per mole of hydrated salt.

In this experimental investigation, we are going to determine the formula of hydrated Iron(II) Sulphate, which is given to us in the instruction as FeSO4.xH2O. Our main objective is to determine the value of x.

Determining the value of x will involve the use of two different methods then comparing the results.

One of the methods involves heating the hydrated to decompose it into an hydrous salt of Fe+2 and water, the calculating the value of x, employing the method called 'formula of calculating the empirical method'. This involves assuming the FeSO4 as an element, lets call

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