1. Examine this Titration Curve: a. Suppose this is a titration curve for the titration of a strong acid (analyte) with a strong base (titrant). The equivalence point is reached in the experiment when exactly 50.00 mL of the base is used. Label each axis. Then label the equivalence point on the curve (dot). Finally, add values on both axes that correspond to the equivalence point. b. Suppose the acid solution used in part (a) was more concentrated than the base that was used. This means that the volume of acid used must have been [less than; equal to; greater than] 100 milliliters. c. Write a net ionic equation for the reaction taking place in the flask below the buret.
1. Examine this Titration Curve: a. Suppose this is a titration curve for the titration of a strong acid (analyte) with a strong base (titrant). The equivalence point is reached in the experiment when exactly 50.00 mL of the base is used. Label each axis. Then label the equivalence point on the curve (dot). Finally, add values on both axes that correspond to the equivalence point. b. Suppose the acid solution used in part (a) was more concentrated than the base that was used. This means that the volume of acid used must have been [less than; equal to; greater than] 100 milliliters. c. Write a net ionic equation for the reaction taking place in the flask below the buret.
Transcribed Image Text:Hint: You should NOT pick alkali metals. Or even really alkali earth metals as electrodes. They react with
water. Even aluminum is a little iffy but people do it anyway. Also avoid H, gas for this.
TABLE 17.1 Standard Reduction Potentials at 25 °C
Reduction Half-Reaction
E (V)
Flg) + 2e-
H,0,(aq) + 2H (aq) + 2 e
Mnolog) + 8 H (ag) + 5e
Weaker
Stronger
oxidizing
agent
+2F(aq)
2.87
reducing
2H,01)
+ Mn"(aq) + 4H,0(1)
2 CI(og)
1.78
1.51
agent
Clg) + 2e
1.36
Cr,0,7(aq) + 14 H"(aq) + 6e-2 Cr "lag) + 7 H,0(1)
O,lg) + 4H (aq) + 4e
Bralaq) + 2e
Ag *(og) + e
Fe"(aq) + e
Olg) + 2H (aq) + 2e
Ils) + 2e
O,l9) + 2H,0() + 4e
Cu"(aq) + 2e
Sn*(aq) + 2e
1.33
+2H,01)
1.23
+2 Br (aq)
Ag(s)
Fe (aq)
H,02 (aq)
2r(aq)
1.09
0.80
0.77
0.70
0.54
4 OH (ag)
Cul s)
- Sn*laq)
0.40
0.34
0.15
2H (aq) + 2 e
(6)H+
Pb(s)
Pb"laq) + 2e"
Ni *(aq) + 2e
Cd"(aq) + 2e
Fe(ag) + 2e
Zn"laq) + 2e
2H,0() + 2e
AI"(aq) + 3e
Mg"laq) + 2e
Na *(ag) + e
Li*(aq) + e
- 0.13
+ Ni( s)
+ Cd(s)
+ Fe(s)
- 0.26
-0.40
- 0.45
- 0.76
(b0) HOZ + (6•
- 0.83
Zn(s)
+ Al( s)
+ Mg(s)
+ Na( s)
Li(s)
• 1.66
- 2.37
- 2.71
- 3.04
Weaker
oxidizing
agent
Stronger
reducing
agent
Table 17-1 Chemistry, S/e
0 2008 Pearson Prentice Hall, Inc.
Transcribed Image Text:1. Examine this Titration Curve:
a. Suppose this is a titration curve for the titration of a strong acid (analyte) with a strong base
(titrant). The equivalence point is reached in the experiment when exactly 50.00 mL of the base
is used. Label each axis. Then label the equivalence point on the curve (dot). Finally, add values
on both axes that correspond to the equivalence point.
b. Suppose the acid solution used in part (a) was more concentrated than the base that was used.
This means that the volume of acid used must have been [less than; equal to; greater than] 100
milliliters.
с.
Write a net ionic equation for the reaction taking place in the flask below the buret.
d. In a separate but related experiment with the same reactants, suppose 25.0 mL of 0.500 M HA
and 3.0 mL of 0.800 M(OH) react. What is the pH of the final solution?
In a separate but related experiment with the same reactants, suppose 25.0 mL of 0.500 M HA
and 25.0 mL of 0.800 M(OH) react. What is the pH of the final solution?
е.
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![1. Examine this Titration Curve:
a. Suppose this is a titration curve for the titration of a strong acid (analyte) with a strong base
(titrant). The equivalence point is reached in the experiment when exactly 50.00 mL of the base
is used. Label each axis. Then label the equivalence point on the curve (dot). Finally, add values
on both axes that correspond to the equivalence point.
b. Suppose the acid solution used in part (a) was more concentrated than the base that was used.
This means that the volume of acid used must have been [less than; equal to; greater than] 100
milliliters.
с.
Write a net ionic equation for the reaction taking place in the flask below the buret.
d. In a separate but related experiment with the same reactants, suppose 25.0 mL of 0.500 M HA
and 3.0 mL of 0.800 M(OH) react. What is the pH of the final solution?
In a separate but related experiment with the same reactants, suppose 25.0 mL of 0.500 M HA
and 25.0 mL of 0.800 M(OH) react. What is the pH of the final solution?
е.](https://content.bartleby.com/qna-images/question/310fa1be-a638-47b3-9316-1b971054d314/94cf6a52-e3cd-4365-84df-5b5241eec5bd/esxghon_processed.jpeg)
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