Conductometric Titration of Weak Acid and Weak Base - QS Study
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Conductometric Titration of weak acid and weak base:

Conductance of electrolytes depends on the number of ions and their speeds. For conductometric titration experiments a known volume of the solution to be titrated is placed in a beaker and a conductivity cell dipped into it. The conductivity cell is now connected to one end of the Wheatstone’s bridge.

One major feature of weak acids and bases is that they do not dissociate completely in water, producing less free oxonium or hydroxide ions than strong acids and bases do.

For weak acid and weak base the conductance initially rises due to the formation of a salt, say ammonium ethanoate from Ammonium hydroxide (NH4OH) and Acetic acid (CH3COOH). On further addition of NH4OH the conductance continually raises till the neutral point is reached.

After this the conductance remains almost constant because NH4OH is a very weak base and contributes only very slightly to conductance. The titration cane for a weak acid – weak base is shown in Figure. The point of intersection of the two linear portions gives the neutral point. Almost all acid-base titrations can be performed conductometrically.

Fig: Titration of weak acid vs weak base

Similarly, if you titrate sodium hydroxide solution with ethanoic acid, at the equivalence point the pure sodium ethanoate formed has a slightly alkaline pH because the ethanoate ion is slightly basic. For example in Sodiumacetate, a weak base, there is an equilibrium where the reactions left to right and right to left occur at the same speed, hence cancelling each other.