Reactions of Acids

Reactions of Acids

General Properties of Acids

• Acids are substances that produce hydrogen ions (H+) when dissolved in water.
• Acids are known for their corrosive nature and ability to change the colour of litmus paper from blue to red.
• They have a sour taste and a pH less than 7.

Common Acids and their Formulas

• Sulphuric acid (H2SO4), hydrochloric acid (HCl), and nitric acid (HNO3) are all examples of commonly encountered strong acids.
• Ethanoic acid (CH3COOH) and carbonic acid (H2CO3) are examples of weak acids.

Reactions with Metals

• Acids react with metals to produce a salt and hydrogen gas.
• The general equation for this reaction is: Acid + Metal -> Salt + Hydrogen.
• For example, with zinc and hydrochloric acid: 2HCl + Zn -> ZnCl2 + H2.

Reactions with Metal Oxides and Metal Hydroxides

• Acids also react with metal oxides and metal hydroxides to produce a salt and water.
• The general equation for this reaction is: Acid + Metal oxide/hydroxide -> Salt + Water.
• For example, with copper(II) oxide and sulphuric acid: H2SO4 + CuO -> CuSO4 + H2O.

Reactions with Carbonates

• Acids react with carbonates and hydrogen carbonates to produce a salt, water, and carbon dioxide.
• The general equation for this reaction is: Acid + Carbonate/Hydrogen Carbonate -> Salt + Water + Carbon Dioxide.
• For example, with calcium carbonate and hydrochloric acid: 2HCl + CaCO3 -> CaCl2 + H2O + CO2.

Neutralisation Reactions

• A neutralisation reaction occurs when an acid reacts with a base to produce a salt and water.
• The general equation for this reaction is: Acid + Base -> Salt + Water.
• For example, with hydrochloric acid and sodium hydroxide: HCl + NaOH -> NaCl + H2O.

Knowing about the reactions of acids can help in understanding many important chemical processes. Always remember to handle acids with care, since they can be corrosive or harmful.