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16 Nov 2019

Consider 1.0 L of a solution which is 0.80 M NH4Cl and 0.50 M NH3. (Ka for NH4+ = 5.6×10-10).

Part 1 Calculate the pH of this solution.

pH =

Part 2 Calculate the pH after 0.10 mol of HCl has been added to the original buffer solution. Assume no volume change on addition of HCl.

pH =

Part 3 Calculate the pH after 0.20 mol of NaOH has been added to the original buffer solution. Assume no volume change on addition of NaOH.

pH =

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15 Jul 2019
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Related questions

Consider 1.0 L of a soluiton which is 0.65 M NH4Cl and 0.90 MNH3. (Ka for NH4+=5.6e-10)

a) calculate the ph for this solution.

b) calculate the pH after 0.10 mol of HCl has been added to theoriginal solution. Assume no volume change on addition of HCl.

c) calculate the pH after 0.20 mol of NaOH has been added to theoriginal buffer solution. Assume no volume change on addition ofNaOH.

Part A

Consider a buffer solution that is 0.50 M in NH3 and 0.20 M in NH4Cl. For ammonia, pKb=4.75.​

Calculate the pH of 1.0 L of the original buffer, upon addition of 0.190 mol of solid NaOH.

Part B

A 1.0-L buffer solution contains 0.100 mol HC2H3O2 and 0.100 mol NaC2H3O2. The value of Ka for HC2H3O2 is 1.8×10−5.​

Calculate the pH of the solution, upon addition of 0.030 mol of NaOH to the original buffer.

(I will leave a good rating, thank you)

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 = ____

(c) What is the pH of the original buffer after the addition of 0.41 mol of HI? (assume no volume change)

pH =____

PART TWO:

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

% ionization = ______%



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

% ionization = ______%

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