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CBSE Class 11 Chemistry MCQs: Acids, Bases, and Equilibrium Practice Test
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Introduction
Mastering Acids, Bases, and Equilibrium Applications is essential for every CBSE Class 11 Chemistry student aiming for top marks in the board exams. This topic, from Chapter 7 – Equilibrium (Part A: Physical Chemistry), explores the dynamic balance between forward and reverse reactions, acid-base theories, and practical equilibrium concepts crucial for higher studies and competitive exams like NEET and JEE.
This online practice test offers carefully crafted CBSE Class 11 Chemistry MCQs, designed strictly according to the NCERT syllabus. Each question includes instant feedback, clear explanations, and aligns with the latest CBSE exam pattern. These multiple-choice questions help strengthen conceptual understanding of acid-base equilibria, buffer action, and Le Chatelier’s principle.
Take this free CBSE Class 11 Chemistry Equilibrium quiz to test your knowledge, analyze your preparation, and identify key learning areas for improvement — all in a timed, interactive environment.
Sample MCQs (with Answers & Explanations)
Q1. Which of the following pairs represents a conjugate acid-base pair?
A) HCl and Cl₂ B) NH₄⁺ and NH₃ C) NaOH and NaCl D) H₂O and OH⁻
Answer: B) NH₄⁺ and NH₃
Explanation: NH₄⁺ donates a proton to form NH₃, making them a conjugate acid-base pair under the Brønsted-Lowry concept.
Q2. The pH of a 0.001 M HCl solution is approximately:
A) 2 B) 3 C) 4 D) 5
Answer: B) 3
Explanation: For strong acids like HCl, [H⁺] = 0.001 M → pH = –log(10⁻³) = 3.
Q3. A buffer solution resists changes in pH due to:
A) High ion concentration B) Presence of strong acid C) Weak acid and its conjugate base D) Dilution
Answer: C) Weak acid and its conjugate base
Explanation: Buffers contain a weak acid and its conjugate base that neutralize small additions of acids or bases.
Q4. When NaOH is added to CH₃COOH solution, equilibrium shifts:
A) Right B) Left C) No change D) Both sides equally
Answer: B) Left
Explanation: OH⁻ ions combine with H⁺, decreasing [H⁺]; Le Chatelier’s principle shifts equilibrium left to restore balance.
Q5. The pKa of acetic acid is 4.76. For equal [CH₃COOH] and [CH₃COO⁻], the pH of buffer is:
A) 4.76 B) 7.00 C) 5.76 D) 3.76
Answer: A) 4.76
Explanation: Using Henderson–Hasselbalch equation, pH = pKa + log([A⁻]/[HA]) = 4.76 + log(1) = 4.76.