A solution of iron(III) chlorate was poured into a lithium phosphate solution. Would you expect a precipitate to form if 354.0 mL of the iron(III) chlorate solution (2.52 x 10-9 M) was mixed with 520.0 mL of a 4.65 x 10-11 M lithium phosphate solution? A. Yes, because Qsp = Ksp for iron(III) phosphate B. Yes, because Qsp < Ksp for iron(III) phosphate C. No, because Qsp < Ksp for iron(III) phosphate D. No, because Qsp = Ksp for iron(III) phosphate E. Yes, because Qsp < Ksp for lithium chlorate F. Yes, because Qsp = Ksp for lithium chlorate G. No, because Qsp > Ksp for iron(III) phosphate H. No, because Qsp < Ksp for lithium chlorate I. No, because Qsp > Ksp for lithium chlorate J. No, because Qsp = Ksp for lithium chlorate K. Yes, because Qsp > Ksp for iron(III) phosphate L. Yes, because Qsp > Ksp for lithium chlorate

K. Yes, because Qsp > Ksp for iron(III) phosphate

Explanation:

Lithium chlorate is very soluble in water, that means has a big ksp.

Iron (III) phosphate has a ksp of 1.3x10⁻²²

Ksp formula of iron (III) phospate is:

FePO₄(s) ⇄ Fe³⁺(aq) + PO³⁻(aq)

Ksp = [Fe³⁺] [PO₄³⁻] = 1.3x10⁻²²

Molar concentration of Fe³⁺ and PO₄³⁻ is:

[Fe³⁺] = 0.340L ₓ (2.52x10⁻⁹mol / L) ÷ (0.354L + 0.520L) = 9.8x10⁻¹⁰M

[PO₄³⁻] = 0.520L ₓ (4.65x10⁻¹¹mol / L) ÷ (0.354L + 0.520L) = 2.78x10⁻¹¹M

Replacing in Ksp formula:

Qsp = [9.8x10⁻¹⁰] [2.78x10⁻¹¹M] = 2.72x10⁻²⁰

As Qsp > Kps, the equlibrium will shift to the right decreasing the ions concentrations producing FePO₄(s), a precipitate

The ions decreases its concentration until Q = Kps

Thus, right answer is:

K. Yes, because Qsp > Ksp for iron(III) phosphate

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