I was just wondering about the following situation; if we had a solution containing 0.1M bromide and 0.1M chloride ions, and treated it with excess silver nitrate, what would happen and would quantitative precipitation of both silver salts be possible?
If I understood correctly, as AgBr is less soluble, it precipitates first. I know that the solubility product of AgBr is lower than AgCl, but why does it selectively precipitate first?
Anyway, it precipitates until the point where the remaining bromide (about 0.48% of 0.1M) remains; at this point, AgCl is more insoluble and starts precipitating, until AgBr is more insoluble again, that’s how I understood it.
So basically, am I correct in the assumption that quantitative precipitation of both salts in same solution is not possible because at some point both salts precipitate simultaneously although there is still a significant amount of bromide in solution?