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Experiment to Find the Amount of Water in a Hydrated Compound

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| Experiment to find the amount of water in a hydrated compound | Calculating Reacting Quantities and Formulae | |

Contents

Aim 2 Introduction 2 Hypothesis 3 Apparatus 3 Method 3 Results 4 Calculation 4 Conclusion 5 Evaluation 5 Bibliography 6

Aim

The aim of this experiment is to find the number of molecules of water of crystallisation combined with one molecule of magnesium sulphate and to ultimately find the formula of the hydrated salt.
Introduction

Within crystals of certain salts, there are a fixed number of water molecules, combined chemically in a fixed proportion. When a salt crystallises from a solution, it forms hydrated salts which contain water molecules that are loosely bonded together. The name for this is the water of crystallisation or water of hydration.
Magnesium sulphate contains seven molecules of water (H2O) for each formula unit of MgSO4 and can be written like this: - MgSO4.7H2O
The dot shows the weak salt/chemical bond in the formula.
To determine the formula of a hydrated salt, it must be heated so that the water of crystallisation evaporates.
When magnesium sulphate has been heated, the water is removed to form an anhydrous salt. This can be reversed by adding water to the anhydrous salt to make it hydrated which will cause the water to reattach itself to the salt.
Other substances that act similarly to hydrates, but have distinct individual characteristics are:- * Hygroscopic – substances that are able to absorb moisture or water molecules from the air. These include ethanol, methanol and sulfuric acid. * Deliquescent – substances that melt or dissolve by absorbing moisture from the atmosphere. This can be seen in calcined calcium chloride which is used in settling road dust and soluble salts. * Efflorescent – hydrates that lose water when exposed to the atmosphere.

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