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Acids Bases and Salts MCQs for MDCAT Practice

Chemistry section, Acids Bases and Salts chapter. Up to eight free sample questions, each with the correct answer and a worked explanation. The full chapter opens in the app.

The bank has 545 active questions on this chapter. Your first 500 practice attempts are free, and every attempt includes a worked explanation.

  1. Question 1
    The pH of a solution contains 10-4 M{H+}
    • 4 (correct answer)
    • 3
    • -3
    • 0
    Correct answer: A
    Calculate the pH of a solution given its hydrogen ion concentration using the fundamental pH definition.
  2. Question 2
    Which of the following is the Henderson-Hasselbalch equation?
    • pH = pKb + Log([Salt]/[Acid])
    • pH = pKa + Log([Salt]/[Acid]) (correct answer)
    • pH = pKb + Log([Acid]/[Salt])
    • pH = pKa + Log([Acid]/[Salt])
    Correct answer: B
    The Henderson-Hasselbalch equation relates pH, pKa, and the concentrations of a weak acid and its conjugate base (salt) in a buffer solution.
  3. Question 3
    Sodium benzoate and benzoic acid of equimolar mixed to form buffer if pKa is 2 what will be pH?
    • 1
    • 2 (correct answer)
    • 0
    • None of these
    Correct answer: B
    Buffer pH equals pKa when the weak acid and its conjugate base are present in equimolar amounts, as demonstrated by the Henderson-Hasselbalch equation.
  4. Question 4
    What volume of 0.4 M Ba(OH)2 (aq) is needed to exactly neutralize 100 milliliters of 0.2 M HBr (aq)?
    • 25 mL (correct answer)
    • 50 mL
    • 100 mL
    • 200 mL
    Correct answer: A
    Stoichiometric calculation to determine the volume of a strong base needed for complete neutralization of a strong acid, considering molarity and stoichiometry.
  5. Question 5
    Which of the following combination is used to make buffer?
    • NaOH and HCI
    • KOH and H2SO
    • CH3COOH and CH3COONa (correct answer)
    • CH3COOH and NH4OH
    Correct answer: C
    Buffers resist pH change by combining a weak acid/base with its conjugate partner. Option C exemplifies this crucial principle.
  6. Question 6
    Which one f the following has the lowest pH?
    • 1 M HF
    • 1 M HCL
    • 1 m CH3COOH (correct answer)
    • 1 M NaOH
    Correct answer: C
    Acids have lower pH than bases. Among acids, the weaker the acid, the lower its pH for equimolar solutions due to increased H+ concentration. Strong acids fully dissociate, weak acids partially dissociate.
  7. Question 7
    If the degree of ionization of water be 1.8 × 10-9 at 298 K. Its ionization constant will be :
    • 1.8 × 10-16 (correct answer)
    • 1 × 10-14
    • 1 × 10-16
    • 1.67 × 10-14
    Correct answer: A
    Calculate water's ionization constant (KwK_w) using its degree of ionization (α\alpha) and concentration. This tests understanding of ionic equilibria in water.
  8. Question 8
    Strong acids give leveling effect in
    • Protogenic solvent
    • Protophilic solvent (correct answer)
    • Aprotic solvent
    • Organic solvent
    Correct answer: B
    Strong acids show the same acidic strength in protophilic solvents due to the leveling effect, where the solvent accepts protons and limits the acid's dissociation.

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