Difference between revisions of "Neutralisation"
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| − | + | ==Key Stage 3== | |
| + | ===Meaning=== | ||
| + | [[Neutralisation]] is a [[Chemical Reaction|chemical reaction]] in which an [[acid]] and a [[base]] [[Chemical Reaction|react]] to produce a [[Neutral (Chemistry)|neutral]] [[product]]. | ||
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| + | ===About Neutralisation=== | ||
| + | : [[Neutralisation]] can reduce the danger from a [[corrosive]] spill. | ||
| + | : An [[acid]] can be '''neutralised''' by adding a [[base]]. | ||
| + | : A [[base]] can be '''neutralised''' by adding an [[acid]]. | ||
| + | : When there is a dangerous [[acid]] spill it is better to use an [[insoluble]] base to '''neutralise''' it than an [[alkali]] because if too much is used the [[insoluble]] [[base]] will not make the [[solution]] go above [[pH]] [[Neutral (Chemistry)|7]] but an [[alkali]] may '''neutralise''' and then replace the [[acid]] with another [[corrosive]] [[chemical]] with a high [[pH]]. | ||
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| + | ===Examples=== | ||
| + | : [[Hydrochloric Acid]] + [[Lithium Oxide]] → [[Lithium Chloride]] + [[Water]] | ||
| + | : [[Hydrochloric Acid]] + [[Iron Oxide]] → [[Iron Chloride]] + [[Water]] | ||
| + | |||
| + | : [[Sulphuric Acid]] + [[Potassium Hydroxide]] → [[Potassium Sulphate]] + [[Water]] | ||
| + | : [[Sulphuric Acid]] + [[Aluminium Hydroxide]] → [[Aluminium Sulphate]] + [[Water]] | ||
| + | |||
| + | : [[Nitric Acid]] + [[Magnesium Carbonate]] → [[Magnesium Nitrate]] + [[Carbon Dioxide]] + [[Water]] | ||
| + | : [[Nitric Acid]] + [[Titanium Carbonate]] → [[Titanium Nitrate]] + [[Carbon Dioxide]] + [[Water]] | ||
Revision as of 17:16, 29 September 2018
Key Stage 3
Meaning
Neutralisation is a chemical reaction in which an acid and a base react to produce a neutral product.
About Neutralisation
- Neutralisation can reduce the danger from a corrosive spill.
- An acid can be neutralised by adding a base.
- A base can be neutralised by adding an acid.
- When there is a dangerous acid spill it is better to use an insoluble base to neutralise it than an alkali because if too much is used the insoluble base will not make the solution go above pH 7 but an alkali may neutralise and then replace the acid with another corrosive chemical with a high pH.
Examples
- Hydrochloric Acid + Lithium Oxide → Lithium Chloride + Water
- Hydrochloric Acid + Iron Oxide → Iron Chloride + Water