topic 4 and 5. Acids and Bases

• what is a Bronsted-Lowry acid?

  a proton donor.
• what is a Bronsted-Lowry base?

  a proton accepter.
• what do acid-base equilibrium reactions involve?


  the transfer of protons where acids donate them and bases accept them.
• what is an equation to show a reaction between an acid and a base?

  HA + H2O = A- + H3O +
• how could you describe acids?


  strong or weak depending on the extent to which they can dissociate to donate protons when added to water.
• what will happen to a strong acid when added to water?

  will undergo complete dissociation donating all its available protons in an irreversible reaction.
• how can you tell if a reaction is irreversible by looking at the equation?

  will use a single headed arrow.
• what is an example of a strong acid?

  Hydrochloric acid HCL
• what is an example of a strong monoprotic acid?

  HCL. HCL —> H+ + Cl-
• what is a monoprotic acid?


  an acid that will only donate 1 proton per mole of acid during dissociation.
• what is an example of a strong diprotic acid?

  sulphuric acid H2SO4
• what is a diprotic acid?

  an acid that only produces 2 protons per mole of acid during dissociation.
• what is an example of a strong triprotic acid?

  phosphoric acid H3PO4
• what is a triprotic acid?

  an acid that produces 3 protons per mole of acid during dissociation.
• what is a weak acid?

  an acid that will only undergo partial dissociation when added to water.
• what is an example of a weak acid?

  carboxylic acids, eg: methanoic acid, ethanoic acid and propanoic acid.
• what is the formula for methanoic acid?

  HCOOH
• what is the formula for ethanoic acid?

  CH3COOH
• what is the formula for propanoic acid?

  CH3CH2COOH
• what will a weak acid do in a reversible reaction where the acid and dissociation products are in equilibrium with each other?

  weak acids only donate 1 proton per mole of acid.
• what does a base do when added to water?

  a base will dissociate when added to water to produce positive ions and aqueous hydroxide ions (OH-).
• what does the presence of hydroxide ions cause for a solution?

  the solution will become alkaline in nature.
• how may Bronsted-Lowry bases be described?


  strong or weak depending on the extent to which they can dissociate to produce these OH- ions when added to water.
• what will a strong base do in water?

  a strong base will dissociate completely in water to produce hydroxide ions and a positively charged metal ion.
• what are 3 common examples of strong bases?

  sodium hydroxide, potassium hydroxide and lithium hydroxide.
• what is the formula for sodium hydroxide?


  NaOH
• what is the formula for potassium hydroxide?

  KOH
• what is the formula for lithium hydroxide?

  LiOH
• what is a strong monobasic base?

  they only produce 1 hydroxide ion per mole when they dissociate in water.
• what is an example of strong monobasic bases?


  sodium hydroxide.
• what is the equation for NaOH's dissociation?

  NaOH --> Na+ + OH-
• what is a dibasic base?

  they only produce 2 hydroxide ions per mole when they dissociate in water.
• what is an example of a strong dibasic base?

  calcium hydroxide.
• what is the formula for calcium hydroxide?

  Ca(OH)2
• what is a strong tribasic base?

  they only produce 3 hydroxide ions per mole when they dissociate in water.
• what is an example of a strong tribasic base?

  aluminium hydroxide.
• what is the formula for aluminium hydroxide?

  Al(OH)3
• what is a weak base?

  they only partially dissociate in a reversible reaction when added to water to produce hydroxide ions.
• what is a common example of a weak base?

  ammonia
• what is the formula for ammonia?

  NH3