Multiple Choice
A 370.0 mL buffer solution is 0.150 M in HF and 0.150 M in NaF. What mass of NaOH can this buffer neutralize before the pH rises above 4.00? (Ka(HF) = 3.5 × 10⁻⁴.)
17. Acid and Base Equilibrium
Acids Introduction
Struggling with General Chemistry?
Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
Which of the following equations correctly shows how the Cr^{3+} cation acts as an acid in water?
A
Cr^{3+} + H_2O → CrO_4^{2-} + 2H^+
B
Cr^{3+} + H_2O → Cr(OH)^{2+} + H^+
C
Cr^{3+} + 3H_2O → Cr(OH)_3 + 3H^+
D
Cr^{3+} + 2H_2O → CrO_2^{+} + 2H^+
Verified step by step guidance1
Step 1: Understand the concept of a cation acting as an acid in water. A cation can act as an acid by donating protons (H^+) to water molecules, forming hydroxide complexes.
Step 2: Analyze the given options to determine which equation correctly represents the behavior of Cr^{3+} in water. The Cr^{3+} cation can interact with water to form a hydroxide complex and release protons.
Step 3: Consider the chemical behavior of Cr^{3+}. Chromium(III) ions can form complexes with water, often resulting in the formation of hydroxide ions and the release of protons.
Step 4: Evaluate the stoichiometry of each equation. The correct equation should balance the number of water molecules and protons released, reflecting the formation of a hydroxide complex.
Step 5: Identify the correct equation based on the chemical behavior and stoichiometry. The equation that shows Cr^{3+} forming a hydroxide complex and releasing protons is the correct representation of its acidic behavior in water.
2:29mWatch next
Master Acid Structure and Types with a bite sized video explanation from Jules
Start learningRelated Videos
Related Practice
Acids Introduction practice set
Problem sets built by lead tutorsExpert video explanations