chemistry

AgCl <==> Ag^+ + Cl^-
NaCl ==> Na^+ + Cl^-

Ksp = (Ag^+)(Cl^-) = 1.8 x 10^-10
Let S = solubility of AgCl, then
(Ag^+) = S
(Cl^-) = S+0.01
Solve for S.
Note: A similar problem to this post (0.1 M NaCl instead of 0.01 M NaCl) was on a couple of days ago; the one who posted said that the answer came back incorrect. Check my work. Check myu thinking.


Should the continuing work look like this?
S = 1.8 x 10^-10 + 1
= 1.00?

Please help I am very confused

  1. 0
  2. 0
  3. 16
asked by Claus
  1. I don't understand how you can be confused.
    (S)(S + 0.01) = 1.8 x 10^-10
    You can solve the quadratic, OR you can make the simplifying assumption that S + 0.01 is about 0.01 (that is, that S is very small in comparison so 0.01 is not really different than S + 0.01).
    If we make the assumption, then
    S(0.01) = 1.8 x 10-^-10
    and S = 1.8 x 10^-8 M = (AgCl).

    1. 0
    2. 0
    posted by DrBob222

Respond to this Question

First Name

Your Response

Similar Questions

  1. chemistry

    What is the solubility of AgCl when it is in a solution of 0.15 M NaCl? (AgCl has Ksp = 1.8 x 10-10.) Make a reaction table. Include rows for initial concentration, change in concentration, and equilibrium concentration. Write

    asked by Anonymous on May 4, 2012
  2. chemistry

    What is the solubility of AgCl when it is in a solution of 0.15 M NaCl? (AgCl has Ksp = 1.8 x 10-10.) Make a reaction table. Include rows for initial concentration, change in concentration, and equilibrium concentration. Write

    asked by Anonymous on April 23, 2012
  3. 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? Ksp for AgCl= 1.8 x 10^-10 Ksp for AgI= 1.5 x 10^-16

    asked by Audrey on November 13, 2010
  4. Chemistry

    Calculate the mass of NaCl required to cause dissolution of 0.010 moles of AgCl in 100 mL of solution. Consider that the addition of NaCl does not cause increased volume in the solution KSP (AgCl) = 1.0 x 10 ^ -10 KF (AgCl2) = 3.0

    asked by Monica on April 15, 2016
  5. Chemistry

    Calculate the mass of NaCl required to cause dissolution of 0.010 moles of AgCl in 100 mL of solution. Consider that the addition of NaCl does not cause increased volume in the solution KSP (AgCl) = 1.0 x 10 ^ -10 KF (AgCl2) = 3.0

    asked by Monica on April 15, 2016
  6. Chemistry

    Combine the Ksp and Kf equilibria for AgCl and Ag(NH3)2+ respectively and demonstrate Hess's law to determine the equilibrium constant for the dissolution of AgCl in NH3. AgCl + 2NH3 --> Ag(NH3)2 + Cl- K= (Ksp)(Kf) If there is

    asked by Kaitlin on April 8, 2016
  7. Chemistry

    Calculate solubility of AgCl (in g/L) in a 6.5*10^-3 M silver Nitrate solution ksp= 1.8 * 10^-10 (AgCl molecular mass is 143.3g) any idea on how to do this this is what i tried> AgCl--> Ag + Cl I 6.5*10^-3 0 C same x E same x ksp

    asked by Steve on February 19, 2016
  8. Chemistry

    Calculate solubility of AgCl (in g/L) in a 6.5*10^-3 M silver Nitrate solution ksp= 1.8 * 10^-10 (AgCl molecular mass is 143.3g) any idea on how to do this this is what i tried> AgCl--> Ag + Cl I 6.5*10^-3 0 C same x E same x ksp

    asked by Steve on February 19, 2016
  9. chemistry

    Most Soluble compound CuS, Ksp = 1.27 x10^-36 PbS, Ksp = 9.04 x 10^-29 AgCl,Ksp = 1.77 X 10^-10 AgI, Ksp = 8.51 x 10^17 My book states that AgCl is insoluble in water and so are MOST phosphates and Sufides, So am I reasonable to

    asked by Sarah on November 13, 2011
  10. chemistry

    what one is the Most Soluble compound 1) CuS, Ksp = 1.27 x10^-36 2) PbS, Ksp = 9.04 x 10^-29 3) AgCl,Ksp = 1.77 X 10^-10 4) AgI, Ksp = 8.51 x 10^17 5) Not enough information. My book states that AgCl is insoluble in water and so

    asked by Ashley on November 13, 2011

More Similar Questions