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12 Dec 2019

1. A buffer solution contains 0.393 M CH₃NH₃Br and 0.463 M CH₃NH₂ (methylamine). Determine the pH change when 0.095 mol HNO₃ is added to 1.00 L of the buffer.

pH after addition â pH before addition = pH change =

2. An aqueous solution contains 0.346 M nitrous acid. How many mL of 0.318 M potassium hydroxide would have to be added to 125 mL of this solution in order to prepare a buffer with a pH of 3.160?

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13 Dec 2019

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A buffer solution contains 0.312 M CH₃NH₃Cl and 0.363 M CH₃NH₂ (methylamine). Determine the pH change when 0.081 mol KOH is added to 1.00 L of the buffer.

pH after addition ? pH before addition = pH change =

a) A buffer solution contains 0.455 M NaHSO₃ and 0.254 M K₂SO₃. Determine the pH change when 0.096 mol NaOH is added to 1.00 L of the buffer.

pH after addition â pH before addition = pH change = ___________

b) Determine the pH change when 0.131 mol KOH is added to 1.00 L of a buffer solution that is 0.460 M in CH₃COOH and 0.280 M in CH₃COO^-.

pH after addition â pH before addition = pH change = ___________

c) When a 25.0 mL sample of a 0.369 M aqueous acetic acid solution is titrated with a 0.311 M aqueous sodium hydroxide solution, what is the pH at the midpoint in the titration?
pH = _________

d) A 17.3 mL sample of a 0.427 M aqueous hypochlorous acid solution is titrated with a 0.441 M aqueous potassium hydroxide solution. What is the pH at the start of the titration, before any potassium hydroxide has been added?

pH = __________

1) A buffer solution is 0.460 M in H2CO3 and 0.280 M in KHCO3 . If Ka1 for H2CO3 is 4.2 x 10^-7 , what is the pH of this buffer solution?

2)How many grams of solid potassium nitrite should be added to 1.00 L of a 0.300 M nitrous acid solution to prepare a buffer with a pH of 4.184 ?

3)How many grams of solid ammonium chloride should be added to 1.50 L of a 0.250 M ammonia solution to prepare a buffer with a pH of 9.960 ?

4) An aqueous solution contains 0.460 M acetic acid.
Calculate the pH of the solution after the addition of 3.74Ã10^-2 moles of potassium hydroxide to 225 mL of this solution.
(Assume that the volume does not change upon adding potassium hydroxide)

5)An aqueous solution contains 0.379 M ammonia.
Calculate the pH of the solution after the addition of 1.76Ã10^-2 moles of nitric acid to 125 mL of this solution.
(Assume that the volume does not change upon adding nitric acid.)

6)An aqueous solution contains 0.460 M acetic acid.
Calculate the pH of the solution after the addition of 3.74Ã10^-2 moles of potassium hydroxide to 225 mL of this solution.
(Assume that the volume does not change upon adding potassium hydroxide).

7)An aqueous solution contains 0.379 M ammonia.
Calculate the pH of the solution after the addition of 1.76Ã10^-2 moles of nitric acid to 125 mL of this solution.
(Assume that the volume does not change upon adding nitric acid).

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