Question
In: Chemistry
what are the effects of acid concentration and Ka on pH and titration curves?
what are the effects of acid concentration and Ka on pH and titration curves?
Solutions
queen_honey_blossom answered 1 year agoRelated Solutions
The pH at the half-equivalence point is 3.15 in an acid-base titration. What is the Ka...
The
pH at the half-equivalence point is 3.15 in an acid-base titration.
What is the Ka of the acid?
What are the components of an acid-base buffer? What do these
buffers do?
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....
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
Determine the pH during the titration of 65.9 mL of 0.410 M hypochlorous acid (Ka =...
Determine the pH during the titration of 65.9
mL of 0.410 M hypochlorous acid
(Ka = 3.5×10-8) by
0.410 M NaOHat the following
points.
(a) Before the addition of any NaOH-?
(b) After the addition of 16.0 mL of
NaOH-?
(c) At the half-equivalence point (the titration midpoint) -?
(d) At the equivalence point -?
(e) After the addition of 98.9 mL of
NaOH-?
Determine the pH during the titration of 56.0 mL of 0.389 M hydrofluoric acid (Ka =...
Determine the pH during the titration of 56.0 mL of 0.389 M
hydrofluoric acid (Ka = 7.2×10-4) by 0.389 M NaOH at the following
points. (Assume the titration is done at 25 °C.)
(a) Before the addition of any NaOH
(b) After the addition of 14.0 mL of NaOH
(c) At the half-equivalence point (the titration midpoint)
(d) At the equivalence point
(e) After the addition of 84.0 mL of NaOH
Determine the pH during the titration of 66.6 mL of 0.468 M hypochlorous acid (Ka =...
Determine the pH during the titration of 66.6
mL of 0.468 M hypochlorous acid
(Ka = 3.5×10-8) by
0.468 M NaOH at the following
points. (Assume the titration is done at 25 °C.)
(a) Before the addition of any NaOH ?
(b) After the addition of 16.0 mL of
NaOH ?
(c) At the half-equivalence point (the titration midpoint) ?
(d) At the equivalence point ?
(e) After the addition of 99.9 mL of
NaOH ?
Determine the pH during the titration of 62.1 mL of 0.445 M benzoic acid (Ka =...
Determine the pH during the titration of 62.1
mL of 0.445 M benzoic acid
(Ka = 6.3×10-5) by
0.445 M NaOH at the following
points. (Assume the titration is done at 25 °C.)
(a) Before the addition of any NaOH
(b) After the addition of 15.0 mL of
NaOH
(c) At the half-equivalence point (the titration midpoint)
(d) At the equivalence point
(e) After the addition of 93.2 mL of
NaOH
Determine the pH during the titration of 22.7 mL of 0.406 M hydrocyanic acid (Ka =...
Determine the pH during the titration of 22.7
mL of 0.406 M hydrocyanic acid
(Ka = 4.0×10-10) by
0.492 M KOH at the following
points.
(a) Before the addition of any KOH
(b) After the addition of 4.60 mL of
KOH
(c) At the half-equivalence point (the titration midpoint)
(d) At the equivalence point
(e) After the addition of 28.1 mL of
KOH
Given Ka for acetic acid = 1.8 x 10-5, calculate the pH in the titration of...
Given Ka for acetic acid = 1.8 x
10-5,
calculate the pH in the titration of 50.0 mL of 0.120 M
acetic acid by 0.240 M sodium hydroxide after the addition
of the following:
0.00 mL of the base.
10.0 mL of base.
25.0 mL of the base.
35.0 mL of the base.
Please show all work
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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