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A base is any substance that reacts with an acid to form a salt and water only. This means that metal oxides and metal hydroxides are bases.
Some bases are soluble in water. An alkali is a soluble base - it dissolves in water to form an alkaline solution. For example:
copper oxide is a base but it is not an alkali because it is insoluble in water
sodium hydroxide is a base and it dissolves in water, so it is also an alkali
Example
Explain why all alkalis are bases but not all bases are alkalis.
Alkalis are soluble bases, but only some bases are soluble in water, so these are not alkalis.
Neutralisation reactions
Neutralisation involves an acid reacting with a base or an alkali, forming a salt and water.
Reactions with metal oxides
In general:
acid + metal oxide → salt + water
For example:
sulfuric acid + copper(II) oxide → copper(II) sulfate + water
H2SO4(aq) + CuO(s) → CuSO4(aq) + H2O(l)
Reactions with metal hydroxides
In general:
acid + metal hydroxide → salt + water
For example:
nitric acid + sodium hydroxide → sodium nitrate + water
HNO3(aq) + NaOH(s) → NaNO3(aq) + H2O(l)
Aqueous neutralisation reactions
Remember:
acids in solution form hydrogen ions, H+
solutions of alkalis contain hydroxide ions, OH-
Acid-alkali neutralisation reactions involve the reaction between hydrogen ions from the acid, and hydroxide ions from the alkali:
H+(aq) + OH-(aq) → H2O(l)
Pure water is neutral (its pH is 7). A neutral solution can be produced if the correct amounts of acid and alkali react together.
Neutralisation reactions in solution can be generalised to hydrogen ions reacting with hydroxide ions to form water.
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Glossary
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