Question

The Slability product of Baso4 is
1.08 x 10^-10. What is the minimum
conc. of So4^2- required to precipitats Baso4
from a 0.001 sol of Bacl2​

Answer 1

Answer:

If the ionic product in the solution starts exceeding thr value of the solubility product of Barium Sulpthate then, Barium Sulphate will start precipitating.

However, already Barium Chloride salt has been added to the solution of concentration 0.001 Molar.

So, this concentration of Barium Ions In the solution will be already there as a constant now.

So, now,

By definition, Solubility Product of Barium Sulphate = Concentration of Barium Ions * Concentration of Sulphate ions

However here, Minimum concentration of Sulphate ions that'll be needed for precipitation will therefore, be

Solubility product / Constant concentration of Barium Ions in the solutions

= 1.08*10^-10 / 0.001 = 1.08*10^-10/10^-3 = 1.08*10^-7 molar.

It is clear that if the concentration of Sulphate ions is any higher than this Val then, the ionic product of barium sulphate in the solution (viz. [Ba2+][SO4 2-] will be higher than solubility product and hence Precipitation of Barium Sulphate will surely take place.