Free Buffer Solutions MCQs with Answers
30 Buffer Solutions MCQs from Chemistry, each with the correct answer and a written explanation of why it is correct. Free and unlimited, with no account needed.
Buffer solutions resist changes in pH when small amounts of acid or base are added, using a weak acid and its conjugate base or a weak base and its conjugate acid. Work includes buffer action, the common-ion effect, Henderson-Hasselbalch calculations, buffer capacity, and the difference between acidic and basic buffers.
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30 questions · page 2 of 2
- A. Standard solution
- B. buffer solution
- C. acidic buffer solution
- D. both B & C
Explanation: CH3COOH is a weak acid and CH3COONa supplies its conjugate base, CH3COO-, so their mixture forms an acidic buffer.
Correct answer: both B & C- A. Lowrys
- B. Lewis
- C. Arrhenius
- D. None of these
Explanation: The Brønsted-Lowry concept defines a base as a proton, H+, acceptor. The Lewis concept instead defines a base as an electron-pair donor…
Correct answer: Lowrys- A. pH
- B. pOH
- C. pKa
- D. pKw
Explanation: pH is defined as the negative logarithm of the hydrogen-ion concentration: pH = -log[H+].
Correct answer: pH- A. more than 7
- B. less than 7
- C. equal to 7
- D. no effect
Explanation: Adding a base increases the concentration of OH- ions and lowers the concentration of H+ ions, so pH rises above 7 in ordinary aqueous…
Correct answer: more than 7- A. 1 x 10^-1
- B. 1 x 10^-14
- C. 1 x 10^-7
- D. 1
Explanation: Using pH = -log[H+], a pH of 0 gives [H+] = 10^0 mol/L = 1 mol/L. Thus the hydrogen-ion concentration is 1 mol/L.
Correct answer: 1- A. Acetic acid & sodium acetate
- B. Acetic acid & ammonia
- C. Acetic acid and its ammonium acetate
- D. Ammonia & ammonium acetate
Explanation: .Acetic acid acts a good buffer with its salt because it is a weak acid.Acetic acid and sodium acetate form a buffer solution due to their…
Correct answer: Acetic acid & sodium acetate- A. pH = pKa + log [salt]/[acid].
- B. pH = pKa-log [acid]/[salt].
- C. pH = pKa - log [salt]/[acid].
- D. Pka =pH-log[salt]/[acid].
Explanation: The only incorrect form is:pH=pKa−log[salt]/[acid]
Correct answer: pH = pKa - log [salt]/[acid].- A. CH3COOH + CH3COONa
- B. H2CO3 + NaHCO3
- C. HCl + NaCl
- D. H3PO4 + Na2HPO4
Explanation: An acidic buffer solution is prepared by mixing weak acid and salt of it with a strong base.
Correct answer: HCl + NaCl- A. 43
- B. 48
- C. 0.43
- D. 4.3
Explanation: pH=pKa+ Log NaHCO3/H2CO3 7=4.3*10^-7+ Log NaHCO3/H2CO3 Log NaHCO3/H2CO3=7 NaHCO3/H2CO3=10^7 NaHCO3=10^7* H2C03 NaHCO3=10^7*4.3^-7 NaHCO3=4.3
Correct answer: 4.3- A. pH = pKa + log([Acid]/[Salt])
- B. pH = pKa - log([Salt]/[Acid])
- C. pH = pKa + log([Salt]/[Acid])
- D. pH = pKa - log([Acid]/[Salt])
Explanation: Henderson-Hasselbalch equation to calculate the pH of a buffer solution ispH=pka+log[salt]/[Acid]
Correct answer: pH = pKa + log([Salt]/[Acid])