Question
In: Chemistry
Calculate the pH of a titration of 50.00 mL of 0.100 M Phenylacetic acid , Ka...
Calculate the pH of a titration of 50.00 mL of 0.100 M Phenylacetic acid , Ka = 4.9 x 10-5, with 0.100 M NaOH at the following points:
SHOW ALL WORK IN NEAT DETAIL ON A SEPARATE PAGE. (Be sure to write chemical equations and Ka or Kb expressions when needed.)
a. (4 Pts) Before any NaOH is added.
b. (4 Pts) After 18.7 mL of NaOH are added.
c. (4 Pts) After 25.00 mL of NaOH are added.
d. (4 Pts) After 50.00 mL of NaOH are added.
e. (4 Pts) After 53.00 mL of NaOH are added.
f. (1 Pt) What is the pKa of the acid (show calculation)?
Solutions
queen_honey_blossom answered 1 year agoRelated Solutions
caluclate the pH in the titration of 50.00 mL of 0.200 M HNO3 by 0.100 M...
caluclate the pH in the titration of 50.00 mL of 0.200 M HNO3 by
0.100 M NaOH after the addition to the acid of solutions of
(a) 0 mL NaOH
(b) 10.00 ml NaOH
(c) 100.00 ml Na OH
(d) 150 mL NaOH
Calculate pBa when 50.00 mL of 0.100 M EDTA is added to 50.00 mL of 0.100...
Calculate pBa when 50.00 mL of 0.100 M EDTA is added to 50.00 mL
of 0.100 M Ba2+. For the buffered pH of 10, the fraction of EDTA in
its fully deprotonated form is 0.30. Kf = 7.59 x 107 for BaY2-.
a) 7.36
b) 7.88
c) 1.30
d) 4.33
In the titration of 25.00 mL of 0.100 M acetic acid, what is the pH of...
In the titration of 25.00 mL of 0.100 M acetic acid, what is the
pH of the resultant solution after the addition of 15.06 mL of
0.100 M of KOH? Assume that the volumes of the solutions are
additive. Ka = 1.8x10-5 for acetic acid, CH3COOH.
In the titration of 25.00 mL of 0.100 M acetic acid, what is the pH of...
In the titration of 25.00 mL of 0.100 M acetic acid, what is the
pH of the resultant solution after the addition of 25.00 mL of
0.100 M KOH? Assume that the volumes of the solutions are additive.
Ka = 1.8x10-5 for CH3COOH.
calculate the pH during the titration of 50.00 ml of .400 M HCl with .800 M...
calculate the pH during the titration of 50.00 ml of .400 M HCl
with .800 M KOH after 0, 12.50, 25.00, and 40.00 ml of KOH have
been added. Graph the titration curve.
Calculate the pH of a solution produced during the titration of 50.00 mL of 2.0 M...
Calculate the pH of a solution produced during the titration of
50.00 mL of 2.0 M acetic acid with 1.0 M potassium hydroxide and
the following volumes of base added:
a) 0.00 mL
b) 25.0 mL
c) 50.0 mL
d) 100.0 mL
e) 125.0 mL
2.Calculate the pH of a solution made by mixing 50.00 mL of 0.100 M KCN with...
2.Calculate the pH of a solution made by mixing 50.00 mL of
0.100 M KCN with 4.33 mL of 0.425 M strong acid HCl. HCN pKa =
9.21.
Calculate the pH of a 0.100 M sodium benzoate, NaC6H5CO2, solution. The Ka of acetic acid...
Calculate the pH of a 0.100 M sodium benzoate, NaC6H5CO2,
solution. The Ka of acetic acid is 6.3 x 10-5
29). A 50.00-mL sample of 0.100 M KOH is titrated with 0.100 M HNO3. Calculate the...
29).
A 50.00-mL sample of 0.100 M KOH is titrated with 0.100
M HNO3. Calculate the pH of the solution after
52.00 mL of HNO3 is added.
1.29
2.71
11.29
12.71
None of these choices are correct.
Determine the pH during the titration of 24.3 mL of 0.310 M formic acid (Ka =...
Determine the pH during the titration of 24.3 mL of 0.310 M
formic acid (Ka = 1.8×10-4) by 0.442 M NaOH at the following
points. (a) Before the addition of any NaOH (b) After the addition
of 4.20 mL of NaOH (c) At the half-equivalence point (the titration
midpoint) (d) At the equivalence point (e) After the addition of
25.6 mL of NaOH
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