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Buffer Solutions MCQs
1. Buffer solution is destroyed when _____________
a) addition of weak base
b) addition of strong acid or base
c) addition of weak acid
d) addition of a salt
Answer: addition of weak base
2. What is the buffer capacity if 3 moles are added in 5 litres of the solution to change the pH by 2 units?
3. Buffer capacity of a buffer is given as two units for a change in pH by Unity. Then what is the number of moles of acid or base, added in one litre of the solution?
4. If 0.20 mol/L CH3COOH and 0.50 mol/L CH3COO– together make a buffer solution, calculate the pH of the solution if the acid dissociation constant of CH3COOH is 1.8 × 10-5.
5. Note that the pKa here is given by 4.752, a buffer is made using 0.8 M acetic acid and 1 M Sodium Acetate what do you think its pH is(log10/8 = 0.097)?
6. If the pH of a substance is given by 3 then what is the pOH of the substance?
7. Which of the following do you think is a correct statement?
a) Ammonium hydroxide / ammonium chloride is an acidic buffer
b) boric acid / borax is an acidic buffer
c) henderson hasselbalch equation is given by pH = pKb + log[salt]/[acid]
d) PH + pOH = 4
Answer: boric acid / borax is an acidic buffer
8. Carbonic acid and sodium bicarbonate are present in blood as a buffer.
9. Which of the following is not an acidic buffer?
a) Acetic Acid-Sodium acetate
b) Boric acid-borax
c) Ammonium hydroxide-ammonium chloride
d) All are acidic buffers
Answer: Ammonium hydroxide-ammonium chloride
10. Which of the following is an equation used to calculate the pH of a buffer solution for an acidic buffer?
a) pH = pKa + log[salt]/[acid]
b) pOH = pKa + log[salt]/[acid]
c) pH = pKb + log[salt]/[acid]
d) pH = pKa + log[salt][acid]
Answer: pH = pKa + log[salt]/[acid]