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  3. 3. a) calculate the ph of a sodium acetate-acetic

3. a) Calculate the pH of a sodium acetate-acetic acid buffer solution (Ka= 1.78 x 10-5)...

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Chemistry

3. a) Calculate the pH of a sodium acetate-acetic acidbuffer solution (Ka= 1.78 x 10-5) in
which the concentration of both components is 1.0 M. What would bethe pH of the
solution if 1.5 mL of 0.50 M NaOH was added to 35.0 mL of thebuffer? How much
does the pH change?

b) If the same amount and concentration of NaOH wasadded to 35.0 mL of pure water
(initial pH = 7), what would be the resulting pH change?

Answer & Explanation Solved by verified expert
4.4 Ratings (949 Votes)

3)

a) pH of acidic buffer = pka + log(ch3coona+NaOH/ch3cooh-NaOH)

pka of ch3cooh = -logKa = -log(1.78*10^-5) = 4.75

No of mole of acetic acid present in buffer = 35*1 = 35 mmole

No of mole of sodium acetate = 35*1 = 35 mmol

No of mole of NaOH added = 1.5*0.5 = 0.75 mmole

pH = 4.75 + log((35+0.75)/(35-0.75))

   = 4.77

pH change = 4.77-4.75 = 0.02

b)

Concentration of NaOH solution = n/v

                               = 1.5*0.5/(35+1.5)

                               = 0.0205 M
pOH = - log[OH-]

    = -log0.0205

    = 1.7

pH = 14-pOH = 14-1.7 = 12.3

initial pH of water = 7

pH change = 12.3 - 7 = 5.3
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