Acids and bases can conduct electricity because they form single dissociated ions
Alkali must have OH
Acids react with:
Acid + (some) metals → salt + hydrogen gas
- Displacement reaction,
- If metal is more reactive than acid, will displace to form salt
- Hydrochloric acid + magnesium → magnesium chloride + H2
- Testing for hydrogen gas with burning splint experiment
Acid + metal carbonate → Salt + CO2 + H2O
- Hydrochloric acid + sodium carbonate → NaCl + CO2 + H2O
- HCl + Na2CO3 → NaCl + CO2 + H2O
- Limewater test for CO2,
- Ca(OH)2, will go milky with CO2
Acid + metal hydroxide → salt and water
- Hydrochloric acid + sodium hydroxide → sodium chloride + water
Acid + metal oxide → salt + water reaction of base and acid
- Acid reacts with metal oxides because they are basic
- Metal oxide – basic Non-metal oxide – acidic
- HCl + sodium oxide → sodium chloride + water
- HCl + Copper oxide → copper chloride + water
Acid + ammonia → ammonium salt
- Sulfuric acid + ammonia → ammonium sulphate
Base reactions
Base(only alkali) + ammonium salt → salt + water + ammonia gas
- Alkali is a base that can dissolve in water to form OH-
- NaOH + NH4Cl → NaCl + water + NH3
Arrhenius definitions
- Acids: ionise in water to produce H+ ions
- HCl → H+ + Cl-
- HCl + H2O → H3O+ + Cl- (H+ ion is still formed)
- Bases: ionise in water to produce OH- ions
- KOH + H2O → K+ + OH-
In order for dissociation, solvent must be polar to break the bonds of the solute
, Bronsted lowry definitions
- Acid is a proton donor
- Fits with arrhenius, proton is H+
- H2SO4 + H2O → HSO4- + H3O+ (proton donor, donates hydrogen to water, therefore acid )
- Here water is behaving as a base, accepting protons
- Base is a proton acceptor
- Now includes NH3 because NH3 accepts proton, but does not form OH-
- H2O + NH3 → OH- + NH4+ (NH3 is base, accepts H+ from water)
- Here water donates proton, therefore acts as an acid
- Water can be both base and acid here
- Weak acids/base always reversible reactions, strong are completely dissociated (don't form back)
- When Hydrogen is lost, compound becomes more negative
- Conjugate base/acid are the acids or bases of the reverse reaction
- Acid and its conjugate (what it forms), acid pair (the acid and the conjugate acid )
- Amphiprotic: A substance that can either gain hydrogen or lose hydrogen (can be acid or base)
- E.g. HCO3
- Amphoteric: Can react with both acid and base
Lewis definitions
- Lewis acid is lone pair acceptor
- Lewis base is a lone pair donor
- Any ligand is a lewis base because they donate lone pair
Strong acid
- Will fully dissociate in water
- All molecules will dissociate
- Can not reverse
Weak acid
- Partially dissociate in water
- Very low percentage of acid will dissociate to form
product
Strong base
- Fully dissociates in water (always alkali because dissolves
in water)
- 100% of base broken down
Weak base
- Partially dissociates in water
Strong acids need to be remembered, weak acids in data booklet
Alkali must have OH
Acids react with:
Acid + (some) metals → salt + hydrogen gas
- Displacement reaction,
- If metal is more reactive than acid, will displace to form salt
- Hydrochloric acid + magnesium → magnesium chloride + H2
- Testing for hydrogen gas with burning splint experiment
Acid + metal carbonate → Salt + CO2 + H2O
- Hydrochloric acid + sodium carbonate → NaCl + CO2 + H2O
- HCl + Na2CO3 → NaCl + CO2 + H2O
- Limewater test for CO2,
- Ca(OH)2, will go milky with CO2
Acid + metal hydroxide → salt and water
- Hydrochloric acid + sodium hydroxide → sodium chloride + water
Acid + metal oxide → salt + water reaction of base and acid
- Acid reacts with metal oxides because they are basic
- Metal oxide – basic Non-metal oxide – acidic
- HCl + sodium oxide → sodium chloride + water
- HCl + Copper oxide → copper chloride + water
Acid + ammonia → ammonium salt
- Sulfuric acid + ammonia → ammonium sulphate
Base reactions
Base(only alkali) + ammonium salt → salt + water + ammonia gas
- Alkali is a base that can dissolve in water to form OH-
- NaOH + NH4Cl → NaCl + water + NH3
Arrhenius definitions
- Acids: ionise in water to produce H+ ions
- HCl → H+ + Cl-
- HCl + H2O → H3O+ + Cl- (H+ ion is still formed)
- Bases: ionise in water to produce OH- ions
- KOH + H2O → K+ + OH-
In order for dissociation, solvent must be polar to break the bonds of the solute
, Bronsted lowry definitions
- Acid is a proton donor
- Fits with arrhenius, proton is H+
- H2SO4 + H2O → HSO4- + H3O+ (proton donor, donates hydrogen to water, therefore acid )
- Here water is behaving as a base, accepting protons
- Base is a proton acceptor
- Now includes NH3 because NH3 accepts proton, but does not form OH-
- H2O + NH3 → OH- + NH4+ (NH3 is base, accepts H+ from water)
- Here water donates proton, therefore acts as an acid
- Water can be both base and acid here
- Weak acids/base always reversible reactions, strong are completely dissociated (don't form back)
- When Hydrogen is lost, compound becomes more negative
- Conjugate base/acid are the acids or bases of the reverse reaction
- Acid and its conjugate (what it forms), acid pair (the acid and the conjugate acid )
- Amphiprotic: A substance that can either gain hydrogen or lose hydrogen (can be acid or base)
- E.g. HCO3
- Amphoteric: Can react with both acid and base
Lewis definitions
- Lewis acid is lone pair acceptor
- Lewis base is a lone pair donor
- Any ligand is a lewis base because they donate lone pair
Strong acid
- Will fully dissociate in water
- All molecules will dissociate
- Can not reverse
Weak acid
- Partially dissociate in water
- Very low percentage of acid will dissociate to form
product
Strong base
- Fully dissociates in water (always alkali because dissolves
in water)
- 100% of base broken down
Weak base
- Partially dissociates in water
Strong acids need to be remembered, weak acids in data booklet
