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CHE 111

Laboratory 3
Hydrates

Introduction

Hydrates
Water molecules combine with the molecules of certain substances, forming loose chemic combinations called hydrates. An example of a hydrate is MgSO47H2O. This formula means 7 water system molecules argon loosely attached to a magnesium sulfate molecule. Other examples of hydrates are Na2SO410H2O and Ba(OH)28H2O. When the hydrate is heated, it easily loses water molecules attached and becomes an anhydrous salt. The corresponding chemical reaction for hydrous magnesium sulfate smoke be written as

|MgSO47H2O ( MgSO4 + 7H2O |(1) |

where MgSO4 is the anhydrous salt.

Usually, when the hydrate is losing water as the result of heating, changes of physical properties (color, appearance) can be observed.

Reversible and Irreversible reactions

Some reactions of dehydration are reversible, others are irreversible.



For example, the reaction

|BaCl22H2O ( BaCl2 + 2H2O |(2) |

is reversible, and if water is added to the anhydrous salt BaCl2, formation of BaCl22H2O takes emerge:

|BaCl2 + 2H2O ( BaCl22H2O |(3) |

The reaction of dehydration of hydrated ferrous sulfate

|FeSO47H2O ( FeSO4 + 7H2O |(4) |

is irreversible. The simple amplification of water to FeSO4 will non lead to the formation of FeSO47H2O.

inclination of the number of molecules of water in a hydrate.
If you do not know how many molecules of water are in unmatchable molecule of hydrate and want to find this out, it can be done by measuring the masses of the hydrate and anhydrous compound formed after the heating. For example, lets...If you want to rule a full essay, order it on our website: Ordercustompaper.com



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