The Ksp for Fe(OH)2 is 1.8 x 10-11. Will a precipitate form if an 0.4M solution of FeCl2, has its pH raised to 8.3?

What is the solubility of Mg+2 in 0.03M HF? Ka for hydrofluoric acid is 6.6 x 10-4. The Ksp for magnesium fluoride is 3.7 x 10-8

Also:
Complete the following reactions:

a. H2PO4^- +H^+ ->

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The Ksp for Fe(OH)2 is 1.8 x 10-11. Will a precipitate form if an 0.4M solution of FeCl2, has its pH raised to 8.3?

Response:

First, we write out the relevant chemical equation.

Fe(OH)2 ------> Fe2+ + 2 OH-

Second, we write the solubility product expression.

Ksp = [OH-]^2[Fe2+]

Third, since the concentration of FeCl2 is 0.4 M, then we also know that the concentration of Fe2+ is 0.4 M. Therefore, we can use this information to solve for the [OH-] in the Ksp expression.

Fourth, we write out the Ksp expression with what we know.

1.8x10^-11 = (x^2)(0.4), where x is [OH-]

Fifth, we solve for x.

x = 6.7x10^-6 M

Therefore, if the [OH-] > 6.7x10^-6 M, ...

Solution Summary

This solution calculates a solubility of a given equation and completes a given reaction

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