2. Ions in aqueous solution
ā Many reactions in industrial processes and in living systems take place in aqueous
solution.
ā Water is a very good solvent and therefore many substances can dissolve in it.
ā The microscopic structure of water makes it possible to dissolve other substances.
3. Polarity of water
ā The water molecule is polar.That is it has a slightly positive end and a slightly negative
end.
ā The atoms in a water molecule are held together strongly by covalent bonds to form
an angular molecule.
ā Oxygen attracts electrons to itself.
ā¢ It becomes slightly negatively charged.
ā¢ Hydrogen becomes slightly positively charged.
4. Polarity of water
ā The shape of the water molecule is important for its polarity.
ā Polarity is a difference in charges on molecules.
ā Water molecules are dipole ( they have two poles).
ā The negative and positive charges are equal, so they cancel each other and the overall
charge on a water molecule is zero.
5. Dissolution process
ā When ionic salts dissolve in water, their ions dissociate from each other.
ā This can be represented by ionic equation:
6. Dissolution processes
ā Acids are important group of covalent compounds that dissolve in water.
ā When acids dissolve in water, they ionise.
ā The new product form and so the process is a chemical change
7. Solubility in water
ā Ionic compounds are made of positive and negative ions that are tightly packed in a
crystal lattice.
ā Strong ionic bonds consists of electrostatic forces and hold the ions in position in the
solid phase.
ā Solubility is defined as the amount of a given substance that can be dissolved in a
certain amount of solvent.
ā Dissolving is a process of a solid ionic crystal breaking into its ions.
8. Solubility
Substances fall into three main categories of solubility
1. Generally, a substance is considered āsolubleā if it dissolves into solution completely.
2. āSparingly (or slightly) solubleā substances are partially soluble. A limited amount of
substance dissolves.
3. āInsolubleā substances do not dissolve at all (or a very tiny amount dissolves.)
9. Solubility of salts
ā Salts are ionic compounds that are made up of metals and none metals.
ā Salts can be soluble, sparingly soluble, and insoluble, depending on the identity of the
cation and anion.
11. Precipitation reactions
Precipitation reactions happen when:
Two soluble salts are mixed
An exchange reaction occurs
And one of the salts formed is insoluble
ā¢ This insoluble substance is called a precipitate.
12. Reference
ā Itutor (2013) Solutions & solubility. Retrieved September 1, 2018, from
https://www.slideshare.net/itutor/solution-solubility
ā Janetra (2007) 9 Aqueous solutions. Retrieved 01 September 2018, from
https://www.slideshare.net/janetra/9-aqueous-solutions
ā Lauralici (2007) Solutions. Retrieved 01 September 2018, from
https://www.slideshare.net/lauralici/solutions