# Chemistry

posted by .

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?
B. AgCl precipitation is 99.99% complete?
C. PbCl2 precipitation begins?
D. PbCl2 precipitation is 99.99% complete?
Finally, give the concentration range of Cl– for the complete separation of Ag and Pb2 .
E. Concentration of Cl– at the start: F. Concentration of Cl– once complete

For A I got 8.18x10^-9 and for B I got 0.0227. A is wrong but I'm not sure why..? and I need help on how to approach the rest of this question please! Really confused.

• Chemistry -

Oh and the Ksp values for AgCl and PbCl2 is 1.8x10^-10 and 1.7x10^-5, respectively.

• Chemistry -

Thanks for the Ksp values. My book had them slightly different. This way I can compare your values.
For A, I think your answer is right; you just reported too many significant figures. You're using Ksp and (Ag^+) with 2 s.f.; I suspect 8.2E-9 is what you are to report.
B. When AgCl is 99.99% that means the Ag^+ is 0.01% in solution or 0.0001 x 0.022 = ? that is left in solution. Use Ksp to calculate Cl^- at this point. I think 8.2E-5M is B.
For C I would round that to 0.023M.That should get you started.

## Similar Questions

1. ### Chemistry

Given the two reactions 1.PbCl2 <--->Pb^2+ + 2 Cl^-, K1= 1.82×10^−10 2. AgCl <----> Ag^+ + Cl^-, K2 = 1.15×10−4 what is the equilibrium constant Kfinal for the following reaction?
2. ### chemistry

[Cl-] in PbCl2 solution, M? [Pb2+] in PbCl2 solution, M?
3. ### Chemistry

i need to find the; [Cl-] in PbCl2 solution,[Pb2+] in PbCl2 solution, and the ksp given: PbCl2(s)--> Pb2+(aq)+2Cl-(aq) Temp of solution =20.2 volume of Pbcl2 solution=25.00ml mass of dry AgCl2(g)=0.2543g #moles : AgCl(s)=1.77e-3 …
4. ### 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 …
5. ### chemistry

If solid AgNO3 is slowly added to a solution that is .05 M in NaI and .12 M in NaCl, what is the concentration of I- when AgCl just begins the precipitate?
6. ### chemistry

if heat of precipitation of AgCl=-36k.j/mole find heat of precipitation of 287 gm of AgCl knowing that (Ag=108 . CL35.5)
7. ### chemistry

Consider the following reaction CaCl2(aq) + 2Ag2SO4(aq) ! CaSO4(?
8. ### Chemistry

You have amisture that is 0.100mol/L in each of the following ions: Cl-, Br-, and I-. (a) Which substance will precipitate first?
9. ### Chem Help

Consider a solution that contains Ag+ , Ba2+, and Pb2+ each at a concentration of .2M a) You add NaCl until the concentration of Cl- is 5.0 x 10^-3 M. A white precipitate forms. How do you determine whether that precipitate was AgCl …
10. ### Chem

HCl is slowly added to a solution that is .250 M in Pb^2+ and .00150 M in Ag+. Which precipitate forms first, PbCl2 or AGCl?

More Similar Questions