In the laboratory, an aqueous solution that is 4.00 M in Pb(NO3)2 is slowly added from...

In the laboratory, an aqueous solution that is 4.00 M in Pb(NO₃)₂ is slowly added from a buret to an aqueous solution that is 0.005 M in Cl^- and also 0.0500 M in Br^-.

PbCl₂_(s) <-> Pb⁺²_(aq) + 2 Cl^-_{(aq) ,} Ksp = 1.6 x 10^-5

PbBr_{2 (s)} <-> Pb⁺²_(aq) + 2 Br^-_(aq) , Ksp = 4.0 x 10^-5

1. Which ion, Cl^- or Br^-, is the first to precipitate from solution?

2. When the second ion begins to precipitate, what is the remaining concentration of the first ion?

3. Is the separation of the first two ions by selective precipitation feasible?

Please show the work included, thank you!

Expert Solution

queen_honey_blossom answered 2 years ago

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