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11 Dec 2019

13. Consider the titration of a 20.00 mL sample of 0.105 M CH3COOH (acetic acid) with
0.125 M NaOH. The Ka for acetic acid is 1.8 × 10-5. Calculate the pH after 10.00 mL of
NaOH is added. The volume needed of base to reach the equivalence point/end point is
16.80 mL.
(A) pH = 4.74 (B) pH = 4.91 (C) pH = 4.57 (D) pH = 8.75

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Collen Von
Collen VonLv2
13 Dec 2019

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Related questions

Hello, I need help with Part D only

Consider the titration of a 25.0 mL sample of 0.105 molL−1 CH3COOH (Ka=1.8×10−5) with 0.125 molL−1 NaOH. Determine each quantity:

Part A

Part complete

the volume of added base required to reach the equivalence point

V =

21.0

 mL

Part B

Part complete

the pH at 6.0 mL of added base

Express your answer using two decimal places.

pH =

4.35

Part C

Part complete

the pH at the equivalence point

Express your answer using two decimal places.

pH =

8.75

Part D

the pH after adding 6.0 mL of base beyond the equivalence point

Express your answer using two decimal places.

pH = ?

Consider the titration of a 20.0 mL sample of 0.105 M HC2H3O2 with 0.125 NaOH. Determine:

a) the initial pH

b) the volume of added base required to reach the equivalence point

c) the pH at 5.0 mL of added base

d) the pH at one-half of the equivalence point

e) the pH at the equivalence point

f) the pH after adding 5.0ml of base beyond the equivalence point

A 20.0 mL sample of 0.105 M HC2H3O2 is titrated with 0.125 M NaOH. The Ka of HC2H3O2 is 1.8 x 10-5

a) Write a balanced reaction for the titration mentioned above.

b) Calculate the volume (in mL) of NaOH required to reach the equivalence point.

c) Calculate the pH of the titration when 20.0 mL of NaOH is added to the mixture.

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