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Acids and Bases - Coggle Diagram

- - - - For example:
        Hydrochloric acid → hydrogen ion + chloride ion
        HCl (aq)→ H+ (aq) + Cl- (aq)
        sulfuric acid → hydrogen ion + sulfate ion
        H₂So₄(aq) → 2H+ (aq) + SO₄²- (aq)
  - - - general equation
        
        metal + acid → salt + hydrogen
        
        E.g.
        magnesium + dilute sulfuric acid → magnesium sulfate + hydrogen
        Mg(s) + H₂SO₄ (aq) → MgSO₄ (aq) + H₂ (g)
    - - general equation (for metal oxides)
        
        metal oxide + acid → salt + water
        
        zinc oxide + dilute sulfuric acid → zinc sulfate + water
        ZnO(s) + H SO (aq) → ZnSO (aq) + H O (l)
      - general equation (for metal hydroxides)
        
        metal hydroxide + acid → salt + water
        
        zinc hydroxide + dilute nitric acid → zinc nitrate + water Zn(OH) (s) + 2HNO (aq) → Zn(NO) (aq) + 2H O (l)
    - - general equation (for carbonate)
        
        carbonate + acid → salt + water + carbon dioxide
        
        E.g.
        calcium carbonate + dilute hydrochloric acid → calcium carbonate + water + carbon dioxide CaCO₃(s) + 2HCl (aq) → CaCl₂ + H₂O (l) + CO₂ (g)
      - general equation (for hydrogen carbonate)
        
        hydrogen carbonate + acid → salt + water + carbon dioxide
        
        E.g.
        sodium hydrogen carbonate + dilute hydrochloric acid → sodium chloride + water + carbon dioxide
        NaHCO₃ (s) + HCl (aq) → NaCl (aq) + H₂O (l) + CO₂ (g)
  - - - Meaning
        
        an acid that is completely ionised in aqueous solution
        
        HCl (aq) → H+ (aq) + Cl- (aq)
        
        Hydrochloric acid (HCl) is an example of a strong acid. All the HCl molecules will ionise in aqueous solution
    - - Meaning
        
        an acid that is only partially ionised in aqueous solution
        
        CH₃COOH (aq) ⇌ CH₃COO- (aq) + H+ (aq)
        
        Example of a weak acid:
        Ethanoic Acid (CH₃COOH)
        ONLY SOME CH₃COOH molecules will ionise in aqueous solution
- - - - E.g.
        Copper (II) Oxide neither reacts with, nor dissolved in, water
    - - copper (II) oxide + dilute sulfuric acid → copper (II) sulfate + water
        CuO(s) + H₂SO₄(aq) → CuSO₄ (aq) + H₂O (l)
      - Ionic Equation
        
        CuO (s) + 2H+ (aq) → Cu₂+ (aq) + H₂O (l)
- - - - The oxides of most metals are basic oxides. Most basic oxides are insoluble in water. A few oxides, such as sodium oxide and potassium oxide, dissolve readily in water to form alkalis
        
        E.g. Calcium oxide + nitric acid → calcium nitrate + water
        CaO(s) + 2HNO₃ (aq) → (aq) + H O (l)
    - - Metallic oxides that react with both acids and bases to form salt and water
        
        E.g.
        Aluminum Oxide (Al₂O₃)
        Lead (II) Oxide (PbO)
    - - Some non-metals form oxides that show neither basic nor acidic properties. They are insoluble in water (except for water itself)
        
        E.g. Water ( H₂O)
        Carbon monoxide (CO)
        Nitric Oxide (NO)
    - - Most oxides of non-metals are acidic oxides
        
        E.g. sulfur dioxide + water → sulfurous acid
        SO₂(aq) + H₂O (l) → H₂SO₃ (aq)
- - - - General Equation
        
        alkali + acid → salt + water
        
        sodium hydroxide + dilute hydrochloric acid → sodium chloride + water
        NaOH (aq) + HCl (aq) → NaCl (aq) + H₂O (l)
    - - General Equation
        
        alkali + ammonium salt → salt + water + ammonia
        
        calcium hydroxide + ammonium chloride → calcium chloride + water + ammonia
        Ca(OH)₂ (aq) + 2NH₄Cl (s) → CaCl₂ (aq) + 2H₂O (l) + 2NH₃ (g)
    - - General Equation
        
        alkali (containing metal A) + salt (of metal B) → salt (of metal A) + metal hydroxide (of metal B)
        
        sodium hydroxide + iron (II) sulfate → sodium sulfate + iron (II) hydroxide
        2NaOH (aq) + FeSO₄ (aq) → Na₂SO₄ + Fe(OH)₂ (s)