Unit 2 Topic 2 ✓

A dative bond is a covalent bond in which one of the atoms supplies both of the electrons

An acid is a proton donor NOTE: A proton is a hydrogen ion

A base is a proton acceptor NOTE: A proton is a hydrogen ion

A conjugate base is the substance that is left behind after an acid has donated its proton NOTE: The stronger the acid, the weaker the conjugate base

An amphoteric substance is a substance that can react as an acid or a base e.g. Water

pH is the ‘potential of hydrogen’ -it measures [hydronium] in solution NOTE: square brackets [ ] = concentration As the concentration of hydronium increases, the pH decreases

pOH is the ‘potential of hydroxide’ -it measures [OH]

A strong acid is an acid that completely dissociates into ions in solution High acid dissociation content (Ka) e.g. Hydrochloric acid, Nitric acid, Sulfuric acid NOTE: Diluting a strong acid by a factor of 10, changes its pH by 1

A weak acid is an acid that only partially dissociates into ions in solution Low acid dissociattion content (Ka) e.g. Ethanoic acid (most organic acids) NOTE: Diluting a weak acid by a factor of 10, changes it pH by 0.5

A polyprotic acid is an acid with more than one ionisible proton NOTE: Each ionisible proton is removed one by one

Equimolar means that two substances have an equal number of moles

Monoprotic means that an acid has one transferrable proton per molecule (Diprotic means two protons are transferable)

A strong base is a base that ionises completely in solution e.g. Potassium hydroxide, potassium oxide etc. NOTE: A strong base doesn’t need to contain hydroxide ions as it can gain them from the solution

A weak base is a base that only partially dissociates into ions in solution e.g. Ammonia and amines

A salt is a substance that is produced when the proton of an acid is replaced by a positive ion NOTE: The positive ion is usually a metal or an ammonium ion

The end point of a titration reaction is the point that is shown by a change in indicator colour

The equivalence point of a neutralisation reaction is the point when the moles of base = moles of acid, so the solution only contains salt and water

Indicators are weak acids that change colour in response to pH

A buffer solution is a solution in which the pH remains approximately constant when small volumes of acid/base/water are added NOTE: If a large amount is added, pH wont remain consistent

An acid buffer is a buffer made up of a weak acid and one of it’s salts from a strong base e.g. Sodium hydroxide or Potassium Hydroxide

A basic buffer is a solution consiting of a weak base and one of it’s salts e.g. Ammonium chloride