In a typical conductometric titration of a strong acid with a weak base, the curve resembles (Conductance vs volume of base graphs as shown in the question)
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Strong acid + weak base titration gives a sharp decrease first, then a slight rise in conductance.
Step 1: Nature of species during titration.
A strong acid initially provides a high concentration of H$^+$ ions, giving high conductance. When a weak base is added, H$^+$ neutralizes to form the weak conjugate acid of the weak base, lowering conductance because the weak conjugate acid ionizes poorly. Step 2: Change in conductance with added base.
Before the equivalence point, conductance drops sharply because highly mobile H$^+$ is removed. After the equivalence point, excess weak base (which ionizes partially) increases conductance only slightly—much less than a strong base would. Step 3: Identifying the curve.
Thus, the correct graph must show:
– A steep fall initially (due to loss of H$^+$).
– A slow rise after equivalence (weak base contributes ions slowly).
Graph (C) shows this exact pattern.
