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25 July, 09:01

Use your experimentally determined value of ksp and show, by calculations, that ag2cro4 should precipitate when 5ml of 0.004m agno3 are added to 5ml of 0.0024 m k2cro4.

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  1. 25 July, 10:43
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    When the value of Ksp = 3.83 x 10^-11 (should be given - missing in your Q)

    So, according to the balanced equation of the reaction:

    and by using ICE table:

    Ag2CrO4 (s) → 2Ag + (Aq) + CrO4^2 - (aq)

    initial 0 0

    change + 2X + X

    Equ 2X X

    ∴ Ksp = [Ag+]^2[CrO42-]

    so by substitution:

    ∴ 3.83 x 10^-11 = (2X) ^2 * X

    3.83 x 10^-11 = 4 X^3

    ∴X = 2.1 x 10^-4

    ∴[CrO42-] = X = 2.1 x 10^-4 M

    [Ag+] = 2X = 2 * (2.1 x 10^-4)

    = 4.2 x 10^-4 M

    when we comparing with the actual concentration of [Ag+] and [CrO42-]

    when moles Ag + = molarity * volume

    = 0.004 m * 0.005L

    = 2 x 10^-5 moles

    [Ag+] = moles / total volume

    = 2 x 10^-5 / 0.01L

    = 0.002 M

    moles CrO42 - = molarity * volume

    = 0.0024 m * 0.005 L

    = 1.2 x 10^-5 mol

    ∴[CrO42-] = moles / total volume

    = (1.2 x 10^-5) mol / 0.01 L

    = 0.0012 M

    by comparing this values with the max concentration that is saturation in the solution

    and when the 2 values of ions concentration are >>> than the max values o the concentrations that are will be saturated.

    ∴ the excess will precipitate out
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