chemistry

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Can Anyone Help Me With This Solubility Problem?
An aqueous solution of 1.90 M AgNO3 is slowly added from a buret to an aqueous solution of 0.0100 M Cl- and 0.250 M I-.
b) When the second ion begins to precipitate, what is the remaining concentration of the first ion?

Reposting this because i already know how to do the other ones. for part B, what is the setup i use to solve this? thx

  • chemistry -

    Bob Pursley gave you a hint this morning. Here is another one.
    Divide Ksp AgCl/Ksp AgI =
    (Ag^+)(Cl^-)/(Ag^+)(I^&-) = (KspAgCl)/(Ksp AgI).
    (Ag^+) cancels so you can get a ratio of
    (Cl^-)/(I^-) = ??
    Substitute numbers and solve for (Cl^-)

  • chemistry -

    the ksp for AGCL is 1.8*10^-11, and the ksp for AGI came out to 8.5*10^-11. when i divided the numbers and set them equal to CL/0.250, the number came out really large? is that right?

  • chemistry -

    Yes, the number is a large one. A couple of words of caution.
    1. AGCL and AgCl are two different things. The same goes for AGI versus AgI. You need to use more caps to begin a sentence and fewer caps for symbols.
    2. I don't believe either of your values for Ksp and that will affect the ratio you calculated (although, I agree it is a large number).

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