In depth and simple to understand class notes taken over the course of 2 years in a highly accredited IB school for Chemistry HL, in regards to the topic of Acids and Bases.
This includes diagrams, annotations, extensive notes and explanations and they are the notes that have solely led me to an ...
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
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
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