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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. 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.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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: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.
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.
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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