chemistry

Im really sorry I got sidetracked:P This is the question I wanted to ask you

In a saturated solution of silver sulfite, the concentration of silver ion is 3.6 x 10^-4 mol/L. The Ksp of silver sulfite willl be what?

Sorry about that

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asked by MikeSo
  1. Do you mean silver sulfite or silver sulfide. I will assume you mean what you wrote. Nothing will change, except the formula, if it is Ag2S.
    Ag2SO3 ==> 2Ag^+ + SO3=
    Ksp = (Ag^+)^2(SO3^=)
    (Ag^+) = 3.6 x 10^-4 from the problem.
    (SO3^=) = 1/2 that.
    Plug into the Ksp expression and calculate Ksp.

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    posted by DrBob222
  2. Ksp = [SO3][Ag]^2 / [Ag2SO3]

    = [1.8 x 10^-4][3.6 x 10^-4]^2 /
    [ ]


    Would I divide by 1.8 x 10^-4 since there is one mole of Ag2So3?

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    posted by MikeSo
  3. Ksp = (Ag^+)^2(SOc^=).
    The denominator is 1, not (Ag2SO3).
    This is not an equilibrium constant. No Ksp has anything on the bottom except 1.

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    posted by DrBob222
  4. AHHH help i have no idea!!!

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    posted by sasha
  5. KSP for Au2 S

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