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7 November, 01:51

If 147 g of znf2 (ksp = 0.0300) is added to water to make a 1.00 l solution, what is the [f-] concentration in the solution in molarity?

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  1. 7 November, 02:15
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    When the balanced reaction equation is:

    and by using the ICE table:

    ZnF2 (s) ↔Zn2 + (aq) + 2 F - (aq)

    initial 0 0

    change + X + 2X

    Equ X 2X

    so we have the Ksp expression of this reaction as the following:

    Ksp = [Zn2+][F-]^2

    when we have Ksp = 0.03

    and we assumed [Zn2+] = X

    and [F-] = 2X

    so, we can substitute and solve to get the value of X:

    0.03 = X * (2X) ^2

    0.03 = X * 4X^2

    0.03 = 4X^3

    ∴X = 0.196 M

    and when the [F-] = 2X

    ∴[F-] = 2 * 0.196 = 0.192 M
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