1. Reactions of Acids Neutralisation
A neutral substance has a ph =7. It contains equal numbers of H+ and OH-
Neutralisation is when we reduce the number of H+ ions in an acid or reduce the number of OH- ions in an alkali – so that they become neutral.

2. Neutralising Acids If we add a BASE to and acid we can neutralise it.
There are 4 types of BASE:
Metals, Metal oxides, Metal hydroxides (soluble metal hydroxides are – alkali’s) and Metal Carbonates.
A new substance called a “salt” is always produced.

3. Naming Salts Acid Base Salt Hydrochloric Sodium hydroxide chloride
The first part of the name comes from the base – it will be a metal name.
The second part comes from the acid.
Salts usually end in “ ide” or “ ate
Acid
Base
Salt
Hydrochloric
Sodium
hydroxide
chloride
Sulphuric acid
Calcium
Hydroxide
sulphate

4. Bases Metals Metal + Acid —>Salt + Hydrogen Example
Magnesium + Hydrochloric Acid —>
Magnesium chloride ( salt) + Hydrogen

5. Metal oxides Metal oxide + Acid —> Salt + Water Example
Magnesium oxide + Carbonic Acid —>
Magnesium carbonate + Water
(salt)

6. Metal hydroxide ( alkali)
Metal hydroxide + Acid —>
Salt + Water
Example
Calcium hydroxide + Nitric Acid —>
Calcium nitrate + Water

7. Metal carbonate Metal carbonate + Acid —>
Salt + Water + Carbon dioxide
Example
Sodium carbonate + Sulphuric Acid —>
Sodium sulphate + Water + Carbon dioxide

8. Ionic Equations
Step 1.
Write down normal balanced equation, remember to use valency to work out formula of compounds.
Step 2
Put in the charges of the ions in the ionic compounds in the equations – remember – covalent compounds e.g. Water don’t have ions!

9. Example of Ionic Equation
Calcium oxide + Hydrochloric Acid —>
Calcium chloride + Water
Step 1
Ca O + H Cl —> Ca Cl2+ H2O
Step 2
Ca 2+ O 2- + H+ Cl- —> Ca 2+ (Cl-) H2O(l)

10. Spectator Ions These are ions which do not change
during the reaction – they are exactly the same on the left and fight side of the arrow!
Example
H+ CL- + Na+ OH- —> Na+ Cl- + H2O
The Na+ and Cl- ions have not changed – they are the spectator ions in this reaction.

11. Making Insoluble Salts
We can make an insoluble salt when we mix certain salt solutions.
This is called Precipitation!
Use p5 in Data booklet to check solubility of compounds!
Example
Barium nitrate(s) + Sodium sulphate(s)
They swap partners- Barium sulphate(i) and Sodium nitrate(s) are formed. Barium sulphate is insoluble – it is a precipitate!

12. Volumetric Titrations
This is when we work out the volume or concentration of an acid or alkali required for a neutralisation reaction.
C1 V1 = C2 V2
C1 = Concentration of Acid
V1 = Volume of Acid
C1 = Concentration of Alkali
V1 = Volume of Alkali

13. Examples!
Calculate the concentration of acid required id 20 cm3 neutralises 20 cm3 of 2mol/l alkali.
C1 V1 = C2 V2
We are wanting to calculate C1
C1 = C2 V2 / V1
C1 = 2 x 0.02 / 0.02
= 2 mol/l

14. Example 2
What volume of alkali, with a concentration of 3 mol/l, is required to neutralise 50 cm3 of 2 mol/l acid?
C1 V1 = C2 V2
V2 = C1 V1 / C2
= 2 x 0.05/ 3
= 0.03 Litres