Q 1201401328.     Experiment - 1: A solution of `KI` and `KCl` of unknown concentration is provided to an student. In order to determine the concentration
of each soluble salt, he titrated the solution with `AgNO_3` , using an electrode to measure the change in the electrode potential as
`AgNO_3` was added. The data obtained is shown in Figure-2 as given below.
Electron Potential for addition of titrant not knowing which endpoint belonged to Kl and which to `KCl`, the student consulted a table of
solubility constants, as shown in below table.
Compound Ksp
Agl `8.3×10^(-17)`
AgBr `5.0×10^(-13)`
AgCI `1.8×10^(-10)`
Experiment-2 : Another student performed a titration of a solution of `KCl`, but had no way of measuring the current in the solution.
Consequently, he had no way of knowing if he had reached the endpoint. In order to determine concentration of `KCl`, he used a titration
method known as the Volhard titration . First, he titrated the solution of `KCl` with `AgNO_3` excess and filtered out the solid precipitate. He
then titrated the solution with `KSCN` in the presence of `Fe(III)`, The solution turned red in color when the endpoint was reached.
At which point in Figure 2 does the silver chloride begin to precipitate out of solution?