Metals Reacting with Water & Acids (Edexcel IGCSE Chemistry (Modular))
Revision Note
Metals reacting with water & acids
The chemistry of the metals is studied by analysing their reactions with water and acids
Based on these reactions a reactivity series of metals can be produced
The series can be used to place a group of metals in order of reactivity based on the observations of their reactions with water and acids
Reactions of metal with cold water summary table
Metal | Reaction with water |
---|---|
Most reactive |
|
Potassium | Reacts violently |
Sodium | Reacts quickly |
Lithium | Reacts less strongly |
Calcium | Reacts less strongly |
Magnesium |
|
Zinc |
|
Iron | Slow rusting |
Copper |
|
Least reactive |
|
Reaction with water
The reactions of potassium and sodium have already been seen previously in the alkali metals, but the reaction with calcium and water is given here for reference:
Ca (s) + 2H2O (l) ⟶ Ca(OH)2 (aq) + H2(g)
calcium + water ⟶ calcium hydroxide + hydrogen
The reactions with magnesium, iron and zinc and cold water are very slow
Reaction with dilute sulfuric or hydrochloric acids
Only metals above hydrogen in the reactivity series will react with dilute acids
The more reactive the metal then the more vigorous the reaction will be
Metals that are placed high on the reactivity series such as potassium and sodium are very dangerous and react explosively with acids
When acids react with metals they form a salt and hydrogen gas:
The general equation is:
metal + acid ⟶ salt + hydrogen
Some examples of metal-acid reactions and their equations are given below:
Table of acid-metal reactions
Metal | Sulfuric acid | Hydrochloric acid |
---|---|---|
Magnesium | Mg (s) + H2SO4 (aq) → MgSO4 (aq) + H2 (g) | Mg (s) + 2HCl (aq) → MgCl2 (aq) + H2 (g) |
Zinc | Zn (s) + H2SO4 (aq) → ZnSO4 (aq) + H2 (g) | Zn (s) + 2HCl (aq) → ZnCl2 (aq) + H2 (g) |
Iron | Fe (s) + H2SO4 (aq) → FeSO4 (aq) + H2 (g) | Fe (s) + 2HCl (aq) → FeCl2 (aq) + H2 (g) |
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