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).
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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