TOPIC 9 Reactions of acids Acids and Alkalis All Acids contain H + ions. Common examples are: Hydrochloric acid: H + Cl - Sulphuric Acid: H 2 + SO 4.

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Presentation transcript:

TOPIC 9 Reactions of acids

Acids and Alkalis All Acids contain H + ions. Common examples are: Hydrochloric acid: H + Cl - Sulphuric Acid: H 2 + SO 4 2- Nitric Acid : H + NO 3 - All Alkalis contain OH - ions. Common examples are: Sodium Hydroxide: Na + OH - Potassium Hydroxide: K + OH - Barium Hydroxide: Ba 2+ (OH - ) 2

Reactions of Acids 1. With Metals Metals above hydrogen in the activity series react with acids. Acid + MetalSalt + Hydrogen 2H + Cl - + Mg Mg 2+ (Cl - ) 2 + H 2 2H + NO Zn Zn 2+ (NO 3 - ) 2 + H 2 Metals below Hydrogen in the Activity Series, such as copper, silver and gold, do not react with dilute acid.

Reactions of Acids (continued) 2. With Alkalis Acid + AlkaliSalt + Water H + Cl - + Na + OH - Na + Cl - + H 2 O Note: The Main Reaction taking place is between the H+ H+ ion and the OH - ion which react to produce H 2 O. This is a Neutralisation reaction which produces heat energy ie an Exothermic Reaction. Na + and Cl - are said to be Spectator ions ie they remain unchanged and don’t take part in the reaction

Reactions of Acids (continued) 3. With Metal Carbonates: Acids react with metal Carbonates to produce Salt, Carbon Dioxide and water. Acid + Metal CarbonateSalt + CO 2 +Water 2H + Cl - + CaCO 3 Ca 2+ (Cl - ) 2 + CO 2 + H 2 O The test for CO 2 is that it turns limewater milky.

Reactions of Acids (continued) 4. With Metal Oxides Acid + Metal OxideSalt + Water 2H + Cl - + CuOCu 2+ (Cl - ) 2 +H 2 O Note: Alkalis, Metal Carbonates and Metal Oxides can be regarded as Bases. This because they can all remove H + ions from solution and produce water.

Precipitation Reactions Salts can be regarded as Acids whose H + ions has been replaced with metal ions.eg. NaCl, KNO 3 and BaSO 4 Salts can be prepared by the four methods mentioned earlier but they can also be made by adding two salts together which results in their ions crossing over. Na + Cl - + Ag + NO - 3 AgCl (s) + Na + NO - 3

Titrations A Burette filled with HCl acid which is added slowly until the End-Point is reached ie.The colour changes from purple to green. A Pipette is used to fill a conical flask with 25ml of Alkali of known concentration 25ml of NaOH +five drops of Universal Indicator. The purpose of a Titration is to accurately determine the volume of acid required to neutralise an alkali of known volume and concentration and vice versa.