Figure 6.19
Conductometric titration curves
(a) Titration of strong acid with NaOH.
(b) Titration of acetic acid, Ka = 1.75 × 10 –^5 mol dm–^3 with NaOH.^
(c) Titration of boric acid Ka = 6 × 10 –^10 mol dm–^3 with NaOH.^
(d) Titration of sodium acetate with HCl.background concentration of H 3 O+ and other electrolytes usually present. Conductometric titrations are
especially useful for very dilute solutions as the percentage change in conductance is independent of
concentration. Unlike potentiometric and visual indicator methods, measurements need not be made
close to the equivalence point so that there is an advantage in conductometric methods when the
chemical reactions involved are relatively incomplete.
Problems
(1) Calculate the theoretical cell potentials for the following systems:
(a) Pb|Pb2+ (0.100 M)||Cd2+ (0.001 M)|Cd(b) Ag|AgBr (saturated), Br– (0.01 M), H+ (10 M)|H 2 (1 atmosphere) Pt