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?
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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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