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What is the effect of adding H⁺ ions to a solution containing a compound with a basic conjugate base (A⁻)?
The H⁺ ions react with A⁻ to form HA, reducing [A⁻] and shifting the equilibrium towards dissolution.
What is the effect of adding OH⁻ ions to a solution containing a compound with an acidic conjugate acid (NH₄⁺)?
The OH⁻ ions react with NH₄⁺ to form NH₃ and H₂O, reducing [NH₄⁺] and shifting the equilibrium towards dissolution.
What is the effect of adding OH⁻ ions to a solution containing a salt with a basic conjugate base (CH₃COO⁻)?
The equilibrium $CH_3COO^- + H_2O
ightleftharpoons CH_3COOH + OH^-$ shifts left due to the added OH⁻, decreasing solubility.
What is the effect of increasing the acidity (adding H⁺) on the solubility of Fe(OH)₃?
The solubility of Fe(OH)₃ increases because H⁺ ions react with OH⁻, reducing [OH⁻] and pushing the dissolution equilibrium to the right: $Fe(OH)_3
ightleftharpoons Fe^{3+} + 3OH^-$.
What is the effect of adding a common ion to a solution of a sparingly soluble salt?
The solubility of the salt decreases, shifting the equilibrium towards the formation of the solid salt.
What are the differences between the effect of pH and the common ion effect on solubility?
pH changes involve reactions with H⁺ or OH⁻, while the common ion effect involves adding an already present ion.
Compare the solubility of salts with basic conjugate bases in acidic vs. basic solutions.
Acidic solutions: Solubility increases. Basic solutions: Solubility decreases (due to common ion effect).
Compare the solubility of salts with acidic conjugate acids in acidic vs. basic solutions.
Acidic solutions: Solubility decreases. Basic solutions: Solubility increases.
Compare the effect of pH on NaCl vs. CaF₂.
NaCl: Solubility is not affected by pH. CaF₂: Solubility is affected by pH because F⁻ is the conjugate base of a weak acid.
Compare the effect of adding HCl vs. NaOH on the solubility of Mg(OH)₂.
Adding HCl: Increases solubility. Adding NaOH: Decreases solubility.
Define pH.
pH indicates the concentration of H⁺ ions in a solution.
Define solubility.
Solubility describes how much of a substance dissolves in a solution, representing an equilibrium process.
What is Le Chatelier's Principle?
Le Chatelier's Principle states that if a condition changes (like pH), the equilibrium will shift to counteract that change.
What is the common ion effect?
The common ion effect influences solubility by adding an ion already present in the equilibrium.
Define conjugate base.
A conjugate base is what remains after an acid has donated a proton (H⁺).