Exercise 16.108p Consider a solution that is 2.4×10 2 M in Fe2+ and 1.5×10 2 M i

Question

Exercise 16.108p

Consider a solution that is 2.4×102 M in Fe2+ and 1.5×102 M in Mg2+.

Part A

If potassium carbonate is used to selectively precipitate one of the cations while leaving the other cation in solution, which cation will precipitate first?

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Part B

What minimum concentration of K2CO3 is required to cause the precipitation of the cation that precipitates first?

Express your answer using two significant figures.

1.3×109

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Part C

What is the remaining concentration of the cation that precipitates first, when the other cation just begins to precipitate?

Express your answer using two significant figures.

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please be hurry cos this is due today at 11:59pm

Exercise 16.108p

Consider a solution that is 2.4×102 M in Fe2+ and 1.5×102 M in Mg2+.

Part A

If potassium carbonate is used to selectively precipitate one of the cations while leaving the other cation in solution, which cation will precipitate first?

Fe2+ Mg2+

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Correct

Part B

What minimum concentration of K2CO3 is required to cause the precipitation of the cation that precipitates first?

Express your answer using two significant figures.

[K2CO3] =

1.3×109

M

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Correct

Part C

What is the remaining concentration of the cation that precipitates first, when the other cation just begins to precipitate?

Express your answer using two significant figures.

Explanation / Answer

Solution-

(b) Ksp of MgCO3 = 6.82 x 10-6

6.82 x 10-6 = [Mg+2][CO3-2]

6.82 x 10-6 = 1.5×102 [CO3-2]

[CO3-2] = 0.00045 M

Ksp of FeCO3 = 3.07 x 10-11

3.07 x 10-11 = [Fe+2]*0.00045

[Fe+2] = 6.67 x 10-8 M

a)Fe+2 will be precipitated first also the minimum concentration of K2CO3 required to precipitate would be 0.00045 M.

(c) Remaining concentration of the cation that precipitates first, is Fe+2 is 6.67 x 10-8 M

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