#12.1
know that a Brønsted–Lowry acid is a proton donor and a Brønsted–Lowry base is a proton acceptor
#12.6
be able to calculate the concentration of hydrogen ions, in mol dm-3, in a solution from its pH, using the expression [H+] = 10–pH
#12.7
understand the difference between a strong acid and a weak acid in terms of degree of dissociation
#12.9
be able to deduce the expression for the acid dissociation constant, Ka,for a weak acid and carry out relevant calculations
#12.12
be able to calculate the pH of a strong base from its concentration, using Kw
#12.14
be able to analyse data from the following experiments:
i) measuring the pH of a variety of substances, e.g. equimolar solutions of strong and weak acids, strong and weak bases, and salts
ii) comparing the pH of a strong acid and a weak acid after dilution 10, 100 and 1000 times
#12.15
be able to calculate Ka for a weak acid from experimental data given the pH of a solution containing a known mass of acid
#12.16
be able to draw and interpret titration curves using all combinations of strong and weak monobasic acids and bases
#12.17
be able to select a suitable indicator, using a titration curve and appropriate data
#12.21
be able to calculate the concentrations of solutions required to prepare a buffer solution of a given pH
#12.22
understand how to use a weak acid–strong base titration curve to:
i) demonstrate buffer action
ii) determine Ka from the pH at the point where half the acid is neutralised
#12.23
understand why there is a difference in enthalpy changes of neutralisation values for strong and weak acids
#12.24
understand the roles of carbonic acid molecules and hydrogencarbonate ions in controlling the pH of blood