reaction of acids

• • METAL OXIDES & METAL HYDROXIDES are classified as BASES, which are typically substances that can NEUTRALISE ACIDS.
• The type of SALT formed depends on the acid used in the reaction:

  • Hydrochloric acid (HCl) -> Chloride Salt (Cl-)
  • Nitric acid (HNO3) -> Nitrate Salt (NO3-)
  • Sulfuric Acid (H2SO4) -> Sulfate Salt (SO4 2-)
• Acid + Metal oxide -> Salt + Water
• Hydrochloric Acid + Calcium Oxide -> Calcium Chloride + water

  2HCl + CaO -> CaCl2 + H2O
• Acid + metal hydroxide -> salt + water
• Nitric acid + sodium hydroxide -> sodium nitrate + water

  HNO3 + NaOH -> NaNO3 + H2O
• Acid + metal carbonate -> salt + water + carbon dioxide
• Sulfuric acid + calcium carbonate -> calcium sulfate + water+ carbon dioxide

  H2SO4 + CaCO3 -> CaSO4 + H2O + CO2
• • green solid / powder
  • colourless solution
  • blue solution formed
  • copper carbonate disappears
  • fizzing
  • bubbles of gas
  • stops fizzing
  • powder left at the end
  • temperature increases

  
• The excess copper carbonate can be removed by filtration.

  
• The pH of the solution changes during the reaction, at the end of the reaction, the pH is 7, as it's an exothermic, neutralisation reaction.

  
• The state symbol would be (Aq)

  
• • zinc hydroxide
  • zinc carbonate

  
• Hydrochloric acid reacts with copper carbonate to produce copper chloride and carbon dioxide.
• 2HCl + Na2O -> 2 NaCl + H2O

  The positive sodium ions & negative chloride ions would combine to form sodium chloride (salt).

  • While the hydrogen & oxygen would form water.
• H2SO4 + 2KOH -> K2SO4 + 2H2O

  Each of the negative sulfate ions (2-) would combine with 2 of the potassium ions (1+).
• During a neutralisation reaction: 

  • The negative ion from the acid react with the positive ion from the base to form a salt.
  • The positive hydrogen ions from the acid react with the negative ions from the base to form molecules of water.
• 2HNO3 + CaCO3 -> Ca(NO3)2 + H2O + CO2

  The positive calcium ion from the base reacts with the negative nitrate ions from the acid.

  • But since the nitrate has a 1- charge while the calcium has a 2+ charge, we’d need 2 nitrates.
• H2SO4  +  Na2O  ➔  Na2SO4  +  H2O
• HCl + KOH ➔ KCl + H2O
•  Soluble salts:

  • NaCl 
  • K2SO 
  • Ca(NO3)2 
• Insoluble base:


  • Metal hydroxide
  • Metal oxide
  • Metal carbonate
• Acid + insoluble base = soluble salt
• ammonia + hydrochloric acid -> ammonium chloride

  • NH3 + HCl -> NH4CL
  • alkali + acid -> neutral salt + no water