1. Reactions of metals with acid
Wednesday 27th July
Reactions of metals with acid

2. Reaction of metals All acids contain Hydrogen
Metal + acid  salt + hydrogen
The salt formed depends on the acid used
HNO3 forms Nitrate salts
H2SO4 forms Sulphate salts
HCl forms Chloride salts

3. Reactivity series of metals
Potassium
sodium
calcium
magnesium
aluminium
zinc
Iron
Lead
(Hydrogen)
copper
silver
gold
Decreasing activity
Even though hydrogen is not a metal it can be placed in the reactivity series due to its reactivity
Metals above hydrogen in the reactivity series will react with acid to make a salt + hydrogen.
Metals below hydrogen will not react with acids.

4. Why do metals react with acid?Cl H
Metal more reactive than H Na Cl + H

5. The more reactive the metal, the more vigorous the reaction.
The least reactive metals do not react at all.
Potassium
sodium
calcium
magnesium
aluminium
zinc
Iron
Lead
(Hydrogen)
copper
silver
gold
Decreasing activity
Which metal fits the description silver; potassium; iron
Explodes in acid
Bubbles slowly in warm acid
Doesn’t react

6. Name of Salt Formula Contains calcium chloride CaCl2 Ca Cl
Formula of salts
How many of each type of atom does the formula of the salt represent?
Name of Salt
Formula
Contains
calcium chloride
CaCl2 Ca Cl
sodium sulphate
Na2SO4 Na S O
magnesium sulphate
MgSO4 Mg
magnesium nitrate
Mg(NO3)2 N
calcium sulphate
CaSO4

7.         + magnesium magnesium chloride + Mg + HCl MgCl2 H2 2
hydrochloric acid +
copper
No reaction Cu +
HCl  - 2 
hydrochloric acid + +
hydrogen Al +
HCl 
AlCl3 H2 6 2 
hydrochloric acid +
calcium + Ca +
HCl 
CaCl2 H2

8. 
sulphuric acid +
zinc + Zn +
H2SO4 
ZnSO4 H2  
nitric acid +
magnesium + Mg +
HNO3 
Mg(NO3)2 H2 
nitric acid +
iron + Fe +
HNO3 
Fe(NO3)3 H2 2 6 2 3 
sulphuric acid +
calcium + Ca +
H2SO4 
CaSO4 H2 