Chemistry

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An aqueous solution that 2.10 M in AgNO3 is slowly added from a buret to an aqueous solution that is 1.20×10^−2 M in Cl- and 0.260 M in I- .

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

  • Chemistry -

    You should have typed in the Ksp for AgCl and AgI. The Ksp I look up probably aren't the same as in your text. I will use approximations.
    Ksp for AgI = about 10^-17.
    Ksp for AgCl = about 10^-10
    Therefore, AgI will ppt first. AgCl will ppt second.
    What will be the (Ag^+) when AgCl just starts to ppt.
    That will be (Ag^+) = Ksp/(Cl^-) = 10^-10/0.012 = ?
    Now what will be the (I^-) at this point? That will be (I^-) = Ksp/(Ag^+) just calculated.
    Post your work if you still need help.

  • Chemistry -

    I got it thanks

  • Chemistry -

    But how did you get the (Cl^-)?

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