2.1.4

• sulfuric acid?

  H2SO4
• Nitric acid

  HNO3
• hydrochloric acid?

  HCl
• ethanoic acid?

  CH3COOH
• Ammonia?

  NH3
• Sodium hydroxide?

  NaOH
• Potassium hydroxide?

  KOH
• Acids release H+ ions
• Alkalis release OH- ions
• Acid is a proton donor
• base is a proton acceptor
• alkali: a base that dissolves in water to form a solution with a pH above 7
• strong acids fully dissociate in water
• weak acids partially dissociate in water as the reverse reaction is favoured
• neutralisation reaction: H+ + OH- -> H2O
• acid + base = salt + water
• acid + metal = metal salt + hydrogen
• acid + metal oxide = salt + water
• acid + metal hydroxide = salt + water
• acid + metal carbonate = metal salt + water + carbon dioxide
• acid + ammonia (NH3) = ammonium salt
• a strong acid fully disassociates
• amphoteric substances can act as an acid or base
• salt: a compound formed when a H+ of an ion is replaced by a metal ion or a positive ion
• chlorine is toxic
• making standard solution: weigh 2.1g of alkali, wash all equipment used into final volumetric flask to make up 250cm, stopper and shake
• titration: 25cm standard solution in conical flask with dye, acid in burette, add until colour change, record initial and final burette, repeat until concordant, find mean titre of acid, find moles in standard solution used, find moles and concentration of acid using balanced equation of reaction