Chemistry Question!!!!?

Suppose 50.00 mL of 2.0 x 10^-6 M Fe(NO3)3 is added to 50.00 mL of 2.0 x 10^-4 M KIO3.

Which of the following statements is true? For Fe(IO3)3, ksp = 1.0 x 10^-4

a) A precipitate forms because Qc > Ksp

b) A precipitate forms because Qc < Ksp

c) No precipitate forms because Qc < Ksp

d) No precipitate forms because Qc = Ksp

3) No precipitate forms because Qc > Ksp

Can you guys explain your thought process so I can understand the problem?

Thanks!!

2 Answers

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  • 4 years ago

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  • 8 years ago

    1)Write chemical equation

    Fe(NO3)3 +KIO3 -->Fe(IO3)3 + KNO3

    [IO3] = (50mL)(2.0x10^-4M) / 100mL =1.0x10^-4 M

    [Fe^3+]= (50mL)(2.0x10^-6M)/100mL = 1.0 x10^-6 M

    Fe(IO3)s <----> Fe^3+(aq) +(IO3)-(aq)

    Q=[Fe][IO3]

    Q=(1.0x10^-4)(1.0x10^-6) = 1.0 x10^-10

    Ksp for Fe(IO3)3 is 1.0x10^-4. Notice that Q is smaller than Ksp, so the solution is unsaturated in Fe(IO3)3 and a precipate will not form.

    answer is C

    Source(s): chemistry student
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