Acids, Bases and Neutralisation

Question	Answer
All acids contain	hydrogen
When an acid is dissolved in water it does what?	Releases H+ ions into the solution
Strong Acid	- Fully Dissociates - Releases all its H atoms into solution as H+ ions -Example: HCl
Weak Acid	- Partially Dissociates - Releases only a small proportion of its available H atoms as H+ ions in solution - Example: CH3COOH
Bases - definition	A base neutralises an acid to form a salt
Bases - Examples	- Metal Oxide -Metal Hydroxide - Metal Carbonate - Ammonia (NH3)
Alkali - Definition	An alkali is a base that dissolves in water releasing hydroxide ions (OH-) into the solution. An example of a base/alkali is sodium hydroxide.
Neutralising an acid with a base	H+ ions react with a base to form a salt and neutral water. H+ ions from the acid are replaced by metal or ammonium ions from the base.
Acid + Alkali -->	salt + water
Ionic Equation for neutralisation	H+ + OH- --> H2O
Acid + Metal Oxide -->	Metal Salt + Water
Acid + Metal Hydroxide -->	Metal Salt and Water
Neutralisation of sulphuric acid with Copper (II) Oxide =	sulphuric acid + Copper (II) Oxide --> Copper sulphate + Water H2SO4 (aq) + CuO (s) --> CuSO4 (aq) + H2O (l)
Acid + Metal Carbonate -->	Metal Salt + Water + Carbon Dioxide
Neutralisation of Zinc Carbonate with Sulphuric Acid	Zinc Carbonate + Sulphuric Acid --> Zinc Sulphate + Water + Carbon Dioxide ZnCO3 (s) + H2SO4 (aq) --> ZnSO4 (aq) + H2O (l) + CO2 (g)

Resource summary

	Created by Bee Brittain about 8 years ago