CHEM 1202 Chapter : SI Chem 2 27 13 Devin

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15 Mar 2019

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1 004 moles of hcl is added to a acetic acid buffer solution that is . 45 m acetic acid and. The volume of the buffer was . 268 l. calculate the new ph of the solution after the addition of hcl. Calculate the new ph of an ammonia buffer in 1. 5l after the addition of . 05 moles of. Ammonia is . 56 m and ammonium is . 67 m. kb of ammonia is 1. 8e -5. 4)total volume: concentration of salt, ph of salt: Calculate the ph at all 3 major points when 400 ml of . 15m ammonia is titrated with . 04 m. Calculate the ph at all 3 major points when 380 ml of . 1m ammonia and . 13m ammonium is titrated with . 04m hbr (kb ammonia = 1. 8e 5). Find the ph at the 3 major points in a titration of acetic acid (50 ml at . 35m) titrated with . 15m barium hydroxide. Ka value of acetic acid is 1. 8e 5.

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PART ONE:

A buffer solution contains 0.22 mol of acetic acid (HC2H3O2) and 0.77 mol of sodium acetate (NaC2H3O2) in 3.40 L.

The Ka of acetic acid (HC2H3O2) is Ka = 1.8e-05.

(a) What is the pH of this buffer?

pH = ____

(b) What is the pH of the buffer after the addition of 0.16 mol of NaOH? (assume no volume change)

pH = ____

pH =____

PART TWO:

(a) Calculate the percent ionization of 0.00180 M hypochlorous acid (K_a = 3e-08).

% ionization = ______%

(b) Calculate the percent ionization of 0.00180 M hypochlorous acid in a solution containing 0.0120 M sodium hypochlorite.

% ionization = ______%

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. How many grams of dry NH4Cl need to be added to 1.50 L of a0.200 M solution of ammonia, NH3, to prepare a buffer solution thathas a pH of 8.60? Kb for ammonia is 1.8e-5

2 Part A:.What is the pH of a buffer prepared by adding 0.45 molof the waek acid HA to 0.608 mol of NaA in 2.00 L of solution? Thedissociation constant Ka of HA is 5.66e-7

3.Part B: What is the pH after 0.150mol of HCl is added to thebuffer from part A? Assume no volume change on the addition of theacid.

4.Part C: What is the pH after 0.195mol of NaOH is added to thebuffer from Part A? Assume no volume change on the addition of thebase.

CHEM 1202 Chapter : SI Chem 2 27 13 Devin

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