BUFFER SOLUTION

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

The following incorrect statement of the buffer solution is that the pH of the buffer solution . . .

• Relatively constant

• Not changed by the addition of a small amount of acid solution

• Not changed by dilution

• Not changed by the addition of a little base

• Same as pKa or pKb

The following solution mixture which is not buffer is . . .

• NaH₂PO₄ and Na₂HPO₄

• NH₃ and (NH₄)₂SO₄

• HCOOH and Ba(HCOO)₂

• H₃PO₄ and NaH₂PO₄

• NaOH and Ba(HCOO)₂

The following mixture of solutions that form a buffer solution is . . .

• 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

The pH solution that consist of NH₄OH 0.2 M and (NH₄)₂SO₄ 0.1 M with Kb NH₄OH = 10^-5 is . . .

• 5 – log 2

• 5

• 7

• 9

• 9 + log 2

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

• 4

• 5

• 6

• 8

• 9

To produce buffer solution with pH = 5, then ratio volume of propionat acid 0.2 M with sodium propionat 0.1 M (Ka = 2 x 10^-5) is . . .

• 1 : 1

• 2 : 1

• 4 : 1

• 1 : 2

• 1 : 4

1000 mL CH₃COOH 0.1 M is mixtured with 1000 mL CH₃COONa 0.1 M (Ka = 10^-5), then the pH of that solution if added 10 mL HCl 0.1 M is . . .

• 5

• 5 – log 1.02

• 7

• 6 – log 9.8

• 6

1000 mL CH₃COOH 0.1 M is mixtured with 1000 mL CH₃COONa 0.1 M (Ka = 10^-5), then the pH of that solution if added 20 mL NaOH 0.05 M is . . .

• 5

• 5 – log 1.02

• 7

• 6 – log 9.8

• 6

1000 mL CH₃COOH 0.1 M is mixtured with 1000 mL CH₃COONa 0.1 M (Ka = 10^-5), then the pH of that solution if added 4 L water is . . .

• 5

• 5 – log 1.02

• 7

• 6 – log 9.8

• 6