Is the solubility of Fe(OH)3 increased, decreased, or unchanged on addition of each of the following substances? Write a balanced net ionic equation for each dissolution reaction. (See Appendix C.6 for formulas of complex ions.) (b) NaOH(aq)

Name: Chemistry
Author: McMurry
ISBN: 9781292336145

Verified step by step guidance

Identify the dissolution reaction of Fe(OH)_3 in water: Fe(OH)_3(s) \(\rightleftharpoons\) Fe^{3+}(aq) + 3OH^{-}(aq).

Recognize that adding NaOH(aq) increases the concentration of OH^- ions in the solution.

Apply Le Chatelier's Principle: Increasing the concentration of a product (OH^-) will shift the equilibrium to the left, favoring the formation of more Fe(OH)_3(s).

Conclude that the solubility of Fe(OH)_3 decreases with the addition of NaOH(aq) due to the common ion effect.

Write the net ionic equation for the dissolution of Fe(OH)_3: Fe(OH)_3(s) \(\rightleftharpoons\) Fe^{3+}(aq) + 3OH^{-}(aq).

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Solubility Product Constant (Ksp)

The solubility product constant (Ksp) is an equilibrium constant that applies to the solubility of sparingly soluble ionic compounds. It represents the product of the molar concentrations of the ions, each raised to the power of their coefficients in the balanced dissolution equation. For Fe(OH)3, the Ksp value helps predict how changes in ion concentration, such as the addition of NaOH, will affect its solubility.

Common Ion Effect

The common ion effect refers to the decrease in solubility of a salt when a common ion is added to the solution. In this case, adding NaOH introduces OH- ions, which are common to Fe(OH)3. This increase in hydroxide ion concentration shifts the dissolution equilibrium to the left, reducing the solubility of Fe(OH)3 due to Le Chatelier's principle.

Net Ionic Equations

A net ionic equation represents the chemical species that are involved in a reaction, excluding spectator ions that do not participate. For the dissolution of Fe(OH)3 in the presence of NaOH, the net ionic equation will show the formation of Fe(OH)4- ions, highlighting the interaction between Fe(OH)3 and the added hydroxide ions. Writing this equation helps clarify the chemical changes occurring in the solution.

Related Practice

Textbook Question

Dissolution of 5.0 x 10^-3 mol of Cr(OH)3 in 1.0 L of 1.0 M NaOH gives a solution of the complex ion [Cr(OH)4]- (Kf = 8 x10^29). What fraction of the chromium in such a solution is present as uncomplexed Cr3+?

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Textbook Question

Write a balanced net ionic equation for each of the follow-ing dissolution reactions, and use the appropriate Ksp and Kf values in Appendix C to calculate the equilibrium constant for each.(a) AgI in aqueous NaCN to form [Ag(CN)2]-

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Textbook Question

Is the solubility of Zn(OH)₂ increased, decreased, or unchanged on addition of each of the following substances? Write a balanced net ionic equation for each dissolution reaction. (See Appendix C.6 for formulas of complex ions.) (a) HCl

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