Reactions of metals with acid

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Presentation transcript:

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

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

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.

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

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

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

        + 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

 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 