chemistry

The Ksp for silver sulfate (Ag2SO4) is 1.2 10-5. Calculate the solubility of silver sulfate in each of the following.
A)water
B)0.14 M AgNO3
C)0.33 M K2SO4
the answer in mol/L

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  1. This is the common ion effect. In part a there is no common ion, part b as the Ag+ as the common ion, and part c has the SO4^= as the common ion.
    Ag2SO4 ==> 2Ag^+ + SO4^=
    ..x........2x........x
    Ksp = (Ag^+)^2(SO4^=)
    Substitute Ksp, Ag^+ = 2x and SOr^= = x. Solve for x = solubility

    b) AgNO3 ==> Ag^+ + NO3^-
    ....0.14M.....0......0
    equil..0......0.14...0.14
    Use Ksp as before but not
    (Ag^+) 0.14 + 2x
    (SO4^=) = x
    Solve for x

    c) K2SO4 ==> 2K^+ + SO4^=
    ...0.33........0.....0
    .....0........0.66...0.33
    Use Ksp as before but
    (Ag^+) = 2x
    (SO4^=) = x + 0.33
    Solve for x
    Post your work if you get stuck.

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