Acid-base reactions

• Lowry-Brønsted Theory

  An acid is a proton donorA base is a proton acceptor.
• Ampholyte


  substance that can act as either acid or base
• Acid Base Indicator

  Describe an acid-base indicator as a weak acid, or a weak base, which colour changes as the H+ion concentration or the OH+ion concentration in a solution changes
• Equivalence Point of a Titration


  the point at which the acid/base has completely reacted with the base/acid.
• Endpoint of a Titration


  Define the endpoint of a titration as the point where the indicator changes colour
• Reddox Reaction


  Describe a redox (oxidation-reduction) reaction as involving an electron transferalways involving changes in oxidation numbers
• Oxidation

  A loss of electrons. OR An increase in oxidation number.
• Reduction

  A gain of electrons. OR A decrease in oxidation number
• Oxidising Agent


  A substance that is reduced/that gains electrons/whose oxidation number decreases
• Reduction Agent


  A substance that is oxidised/that loses electrons/whose oxidation number increases
• Arrhenius Theory

  (A) hydrogen ions (H+ /H3O + /hydronium ions) & (B) hydroxide ions (OH- ) in (aq).
• Strong Acids


  o Strong acids ionise completely in water to form a high concentration of (H3O+)ions.
• Weak Acids


  Weak acids ionise incompletely in water to form a low concentration of (H3O+)ions.
• Strong Bases


  Strong bases dissociate completely in water to form a high concentration of (OH-)ions.
• Weak bases


  Weak bases ionise incompletely in H2O to form a low concentration of (OH-)ions.