Textbook Question
A 1.000 L sample of HF gas at 20.0 °C and 0.601 atm pressure was dissolved in enough water to make 50.0 mL of hydrofluoric acid. (b) To what volume must you dilute the solution to triple the percent dissociation?
17. Acid and Base Equilibrium
Acids Introduction
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Which of the following compounds will form an aqueous solution with a pH higher than 7?
A
NaClO4
B
KIO2
C
FeBr2
D
None of the above
Verified step by step guidance1
Identify the nature of each compound: Determine if each compound is a salt, acid, or base. NaClO4, KIO2, and FeBr2 are all salts.
Consider the ions produced in solution: When dissolved in water, salts dissociate into their constituent ions. For example, NaClO4 dissociates into Na⁺ and ClO₄⁻ ions.
Evaluate the potential for hydrolysis: Determine if the anions or cations can react with water to form acidic or basic solutions. Anions from strong acids (like ClO₄⁻ from HClO₄) do not hydrolyze, while anions from weak acids (like IO₂⁻ from HIO₂) can hydrolyze to form OH⁻, making the solution basic.
Analyze the hydrolysis of KIO2: The IO₂⁻ ion can react with water in a hydrolysis reaction: IO₂⁻ + H₂O ⇌ HIO₂ + OH⁻. The production of OH⁻ ions increases the pH, making the solution basic.
Conclude which compound forms a basic solution: Since KIO₂ produces OH⁻ ions through hydrolysis, it will form an aqueous solution with a pH higher than 7, unlike NaClO₄ and FeBr₂, which do not increase the pH.
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