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Summary Edexcel A level Chemistry Topic 12: Acid-Base Equilibria questions
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Edexcel A level Chemistry Topic 12: Acid-Base Equilibria questions
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Edexcel A level Chemistry Topic 12: Acid-Base Equilibria questions
Bronsted-Lowry base? - proton acceptor
Bronsted-Lowry acid? - proton donor
H+ ions are never by themselves in water. Instead... - they combine with water to
form H3O +
Define a strong acid/bases. - Strong acids/bases completely dissociate in water
Define weak acids/bases. - Acids dissociate only slightly in water
Bases only slightly protonate in water
- only small numbers of H+ ions are formed.
- equilibrium lies very far to the left
What are conjugate acid-base pairs? - - species linked by the transfer of a proton.
- species which has lost the proton will become the conjugate base
- species which has gained a proton becomes the conjugate acid.
How to write ionic equations? - - show the H+ ions being donated
, Edexcel A level Chemistry Topic 12: Acid-
Base Equilibria questions
- show the ion that accepts the H+
- show the products formed in the process
- balance charges
When an acid and base react, if conc of H+ = concn of OH-, reaction is known as a
- neutralisation reaction.
When an acid and base react, if conc of H+ > concn of OH-, solution will be - acidic
When an acid and base react, if conc of H+ < concn of OH-, solution will be - basic
Why is the standard enthalpy of neutralisation similar for all reactions of strong
acids with strong bases? - - strong acids and bases fully dissociate in solution
- when they react in a neutralisation rtn, no dissociation enthalpy for acid or base
- only enthalpy for reaction between H+ and OH- which will be the same every
time.
What is the pH scale a measure of? - - measure of the hydrogen ion concentration
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