Magnesium – reacts rapidly with dilute acids to make colourless solutions of magnesium salts. Zinc – reacts readily to make colourless salts. Aluminium – does not react due to impervious aluminium oxide coating. Iron – reacts slowly to form pale solutions of Iron (II) chloride or Iron (III) sulphate. Acid + Metal Oxide → Salt + Water Acid + Metal Carbonate → Salt + Water + Carbon Dioxide Acid + Metal Hydroxide → Salt + Water ACID + PRODUCTS METAL SALT + HYDROGEN METAL OXIDE SALT + WATER METAL CARBONATE SALT + CARBON DIOXIDE + WATER METAL HYDROXIDE SALT + WATER Definitions Acids are substances which dissociate in water and form an H+(aq) ion. Acids are proton donors. Acids only behave like acids when dissolved in water. Hydrogen chloride dissolves in water to form hydrochloric acid, in methylbenzene is does not dissociate, and so does not behave like an acid. Bases are substances which react with acids and form a salt and water. This includes metal oxides, metal carbonates and metal hydroxides. Alkalis are bases which dissolve in water to form the OH-(aq) ion. Most alkalis are metal hydroxides, but ammonia is also an alkali. Salts are formed when the hydrogen in the acid is replaced by a different positive ion – usually a metal ion. Neutralisation is the reaction of an acid with a base. A salt and water is always produced. Salt Preparation Rules for Solubility: All sodium, potassium and ammonium compounds are soluble. All chlorides except silver chloride are soluble. All sulphates are soluble, except for barium and calcium sulphate. All hydroxides are insoluble, except sodium, potassium and ammonium.
Magnesium – reacts rapidly with dilute acids to make colourless solutions of magnesium salts. Zinc – reacts readily to make colourless salts. Aluminium – does not react due to impervious aluminium oxide coating. Iron – reacts slowly to form pale solutions of Iron (II) chloride or Iron (III) sulphate. Acid + Metal Oxide → Salt + Water Acid + Metal Carbonate → Salt + Water + Carbon Dioxide Acid + Metal Hydroxide → Salt + Water ACID + PRODUCTS METAL SALT + HYDROGEN METAL OXIDE SALT + WATER METAL CARBONATE SALT + CARBON DIOXIDE + WATER METAL HYDROXIDE SALT + WATER Definitions Acids are substances which dissociate in water and form an H+(aq) ion. Acids are proton donors. Acids only behave like acids when dissolved in water. Hydrogen chloride dissolves in water to form hydrochloric acid, in methylbenzene is does not dissociate, and so does not behave like an acid. Bases are substances which react with acids and form a salt and water. This includes metal oxides, metal carbonates and metal hydroxides. Alkalis are bases which dissolve in water to form the OH-(aq) ion. Most alkalis are metal hydroxides, but ammonia is also an alkali. Salts are formed when the hydrogen in the acid is replaced by a different positive ion – usually a metal ion. Neutralisation is the reaction of an acid with a base. A salt and water is always produced. Salt Preparation Rules for Solubility: All sodium, potassium and ammonium compounds are soluble. All chlorides except silver chloride are soluble. All sulphates are soluble, except for barium and calcium sulphate. All hydroxides are insoluble, except sodium, potassium and ammonium.
fullchemnotes.docx