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Solubility and mass dissolved

  1. Apr 28, 2015 #1
    1. The problem statement, all variables and given/known data
    What mass of AgCl will dissolve in 1 L of water containing 0.0144 moles of NaCl. Ksp = 1.7 x 10^-10

    2. Relevant equations
    Ksp = [x][x] and ICE table

    3. The attempt at a solution
    So, the common ion effect is taking place here and the equilibrium taking place is:
    AgCl(s) ↔ Ag+ + Cl-

    Since excess Cl- will be present from the NaCl, the Na+ is just a spectator ion.

    ICE table:
    AgCl(s) ↔ Ag+ + Cl-
    x 0 0.0144 M
    -x x x
    0 x 0.0144 + x

    Ksp = [Ag+][Cl-] = 1.7 x 10^-10

    (x)(0.0144 + x) = 1.7 x 10^-10

    I assume that I can eliminate the x in the parentheses because it would be very small, thus:
    0.0144x = 1.7 x 10^-10
    x = 1.2 x 10^-8 mol/L
    Converting to grams gives me 1.8 x 10^-6 g/L

    I was wondering if someone wouldn't mind checking to see if my steps are accurate. Thanks in advance!
     
  2. jcsd
  3. Apr 29, 2015 #2

    Borek

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    Staff: Mentor

    What have you used for molar mass of AgCl? I got a slightly different result.
     
  4. Apr 29, 2015 #3
    I used 144 g/mol. I will recheck my math.
     
  5. Apr 29, 2015 #4
    Yes, x = 1.2x10^-8 mol/L
    Thus, (1.2x10^-8 mol/L)(144 g/L) = 1.8x10^-6 g/L
     
  6. Apr 29, 2015 #5

    Borek

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    Staff: Mentor

    No matter how many times you will write it, it won't get correct. Sorry.
     
  7. Apr 29, 2015 #6
    Wait! The steps are more important! Can I get any advice on how I am approaching these problems?
     
  8. Apr 29, 2015 #7

    Borek

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    Staff: Mentor

    Your approach is OK, the final result is not.
     
  9. May 16, 2015 #8

    James Pelezo

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    Gold Member

    Borek is right, recheck your formula wt.
     
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