Asked by Ryan
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?
When the second ion begins to precipitate, what is the remaining concentration of the first ion?
Answers
Answered by
DrBob222
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.
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.
Answered by
Ryan
I got it thanks
Answered by
anon
But how did you get the (Cl^-)?
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