Buffer solutions

Front

The buffer solution is able to maintain pH by some events, except . . .

• The addition of a little acid
• The addition of a little base
• Dilution
• Addition of water
• The addition of excess acid

Back

The addition of excess acid

Front

Mixture of solutions that form a buffer solution: 50 mL CH₃COOH 0.2 M and 50 mL NaOH 0.1 M, 50 mL CH₃COOH 0.2 M and 100 mL NaOH 0.1 M, 50 mL HCl 0.2 M and 100 mL NH₄OH 0.1 M, 50 mL HCl 0.2 M and 50 mL NH₄OH 0.1 M, 50 mL HCl 0.2 M and 100 mL NaOH 0.1 M

Back

50 mL CH₃COOH 0.2 M and 50 mL NaOH 0.1 M

Front

The pH solution that consist of CH₃COOH 0.01 M and CH₃COONa 0.01 M with Ka = 10^-5 is . . .

Back

5

Front

Acidic buffer is made up of

Back

weak acid and its conjugate base

Front

Which solution A and B of equal volume and concentration mixed together to form a buffer? Options: Nitric acid and potassium hydroxide, Nitric acid and potassium nitrate, Propanoic acid and potassium hydroxide, Propanoic acid and potassium propanoate

Back

Propanoic acid and potassium propanoate

Front

Which combination will form a buffer solution? Options: 100ml of 0.1M HCI with 50ml of 0.1M NaOH, 100ml of 0.1M CH₃COOH with 50ml of 0.1M NaOH, 50ml of 0.1M HCI with 100ml of 0.1M NaOH, 50ml of 0.1M CH₃COOH with 100ml of 0.1M NaOH

Back

100ml of 0.1M CH₃COOH with 50ml of 0.1M NaOH

Front

What could be added to a solution of ethanoic acid to prepare a buffer?

Back

NaOH

Front

What statement is true about basic buffer?

Back

basic buffer usually works effectively at pH range of above 7

Front

What reaction takes place in a buffer solution of HCOOH and NaHCOO to resist pH change when NaOH is added?

Back

HCOOH + OH^- → HCOO^- + H₂O

Front

Reaction in buffer solution to resist pH change when HCl is added: CH₃COOH ↔ CH₃COO^- + H⁺

Back

CH₃COO^- + H⁺ → CH₃COOH