A saturated solution of iodine in water contain `0.330g I_(2) per litre`. More than this `I_(2)` can be dissolved in `KI` solution because of the following equilibrium.
`I_(2(g))+I^(-)hArrI_(3)^(-)`
A `0.100 M KI` solution actually dissolves `12.5 g "iodine per litre"`, most of which is converted to `I_(3)^(-)`. Assuming that the concentration of `I_(2)` in all saturated solution is the same, calculate the equilibrium constant for the above reaction. What is the effect of adding water to a clear saturated solution of `I_(2)` in the `KI` solution?

Explanation

`707 litre mol^(-1)` ,