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.)
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17. Acid and Base Equilibrium
Acids Introduction
Multiple 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.
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