Chemistry

posted by .

You have amisture that is 0.100mol/L in each of the following ions: Cl-, Br-, and I-.


(a) Which substance will precipitate first?
AgCl, AgBr, AgI?
(b)what is the concentration of Ag+ required to start the precipitation of the first substance?

ksp (AgCl)= 1.77*10^-10
ksp (AgBr)= 5.35*10^-13
ksp (AgI)= 8.51*10^-17

Could you please help me understand how to do this problem? I am so lost.

  • Chemistry -

    Look up Ksp for AgCl, AgBr and AgI.
    The salt with the smallest Ksp will ppt first.(this comparison is true only when the salts have the same ratio. In this case all are 1:1).

    The following shows you how to calculate Ag^+ at the time EACH ppts. However, AgCl will not ppt first and that's the one you are calculate. AgI ppts first.
    ......AgCl(s) ==> Ag^+(aq) + Cl^-(aq)
    I.......solid......0..........0
    C.......solid......x..........x
    E.......solid......x..........x

    Ksp = whatever = (Ag^+)(Col^-)
    Ksp = (x)(x)
    Solve for x = (Ag^+).

  • Chemistry -

    i got 4.46*10^-4??

  • Chemistry -

    No, that isn't right; however, I may have led you down the wrong path. I see at the top that the solution is 0.1M in I^- so
    AgI==> Ag^+ + I^-
    ........x.....x
    Ksp = (Ag^+)(I^-)
    Ag^+ is x from AgI.
    I^= 0.1M from the problem.
    8.51E-17 = (0.1)(x)
    Solve for x.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. chemistry

    The values of Ksp for AgBr and AgCl, are 7.7x10^-13 and 1.6 x 10^-10. A solution containing a mixture of 2.0x10^-2 M Br and 2.0 x 10^-2M Cl is a candidate for separating using selective precipitation. Solid AgNO3 is added, with a miniature …
  2. Chemistry

    The values of Ksp for silver bromide, AgBr is 7.7x10^-13, and silver chloride, AgCl is 1.6x10^-10. A solution containing a mixture of 2.0x10^-2 M Br^- and 2.0x10^-2 M Cl^- is a candidate for separation using selective precipitation. …
  3. chemistry

    The solubility products of AgBr and Ag3PO4 are 5.0 10-13 and 1.8 10-18, respectively. If Ag+ is added (without changing the volume) to 1.00 L of a solution containing 0.31 mol Br ‾ and 0.31 mol PO43-, calculate the molarity of …
  4. Chemistry

    Which of the following pairs of compounds will give a precipitate in a diluted solution?
  5. Chemistry

    A solution contains 0.022 M Ag and 0.033 M Pb2 . If you add Cl–, AgCl and PbCl2 will begin to precipitate. What is the concentration of Cl– required, in molarity, when A. AgCl precipitation begins?
  6. Chemistry

    Why does AgCl dissolve in NH3 but AgBr and AgI don't?
  7. College Chemistry

    Arrange the following compounds in the order of increasing Ksp: AgCl, AgBr, AgI. Explain your reasoning. I got AgI<AgBr<AgCl but I looked at the actual Ksp. I do not know how else to explain it besides looking at the Ksp. Like …
  8. Chemistry

    Solid AgNo3 is added slowly to solution of 0.001M Cl,Br,and I a) at what concentration of Ag will AgI precipitating?
  9. Chemistry

    Solid AgNo3 is added slowly to solution of 0.001M Cl,Br,and I a) at what concentration of Ag will AgI precipitating?
  10. Chemistry

    A solution contains 2.2×10−4 M Ag+ and 1.3×10−3 M If NaI is added, will AgI(Ksp=8.3×10−17) or PbI2(Ksp=7.9×10−9) precipitate first?

More Similar Questions