Pre-Lab Activities: After reading the lab, complete items a, b, c, and d (title, purpose, chemicals and equipment, and summary of procedure) as described on page 10 of Exp. 1 on an 8 1/2 x 11 sheet of paper. Answer the following questions on 8 1/2 x 11 sheet of paper or in your laboratory notebook if one is required by your instructor: 1. Write the oxidation and reduction half reactions; a. Fe2+, Fe3+ || Br2, Br b. Mg , Mg2+ || Cr³+, Cr2* 2. If E°H92+,Hg = +0.80V and E°co2+,Co = -0.28V, then what is the E°cell for the reaction Co + HgCl2 → CoCl2 + Hg? 3. If you assume the E°Ag*,Ag = 0.00 volts, then what is E°Cu2+,Cu when the voltage measured across the electrochemical cell below is +0.46 volts? E°cell = +0.46V for Cu,Cu2+ || Ag*,Ag 4. Using the information above, what is E°Cl2 C- given the system below? • E°cell = +1.02V for Cu,Cu2+ || Cl2,CI- 5. A student measures the potential of a cell made up with 1 M CuSO4 in one solution and 1 M AGNO3 in the other. There is a Cu electrode in the CuSO4 and an Ag electrode in the AgNO3, and the cell is set up as in Figure 6-1. She finds that the potential, or voltage, of the cell, E°cell, is 0.45V, and that the Cu electrode is negative. a. At which electrode is oxidation occurring? b. Write the equation for the oxidation reaction c. Write the equation for the reduction reaction. d. If the potential of silver, silver ion electrode, E°Ag*,Ag is taken to be 0.000 V in oxidation or reduction, what is the value of the potential for the oxidation reaction: • E°cu,Cu2+oxid? E°cell = E°oxid + E°red
Pre-Lab Activities: After reading the lab, complete items a, b, c, and d (title, purpose, chemicals and equipment, and summary of procedure) as described on page 10 of Exp. 1 on an 8 1/2 x 11 sheet of paper. Answer the following questions on 8 1/2 x 11 sheet of paper or in your laboratory notebook if one is required by your instructor: 1. Write the oxidation and reduction half reactions; a. Fe2+, Fe3+ || Br2, Br b. Mg , Mg2+ || Cr³+, Cr2* 2. If E°H92+,Hg = +0.80V and E°co2+,Co = -0.28V, then what is the E°cell for the reaction Co + HgCl2 → CoCl2 + Hg? 3. If you assume the E°Ag*,Ag = 0.00 volts, then what is E°Cu2+,Cu when the voltage measured across the electrochemical cell below is +0.46 volts? E°cell = +0.46V for Cu,Cu2+ || Ag*,Ag 4. Using the information above, what is E°Cl2 C- given the system below? • E°cell = +1.02V for Cu,Cu2+ || Cl2,CI- 5. A student measures the potential of a cell made up with 1 M CuSO4 in one solution and 1 M AGNO3 in the other. There is a Cu electrode in the CuSO4 and an Ag electrode in the AgNO3, and the cell is set up as in Figure 6-1. She finds that the potential, or voltage, of the cell, E°cell, is 0.45V, and that the Cu electrode is negative. a. At which electrode is oxidation occurring? b. Write the equation for the oxidation reaction c. Write the equation for the reduction reaction. d. If the potential of silver, silver ion electrode, E°Ag*,Ag is taken to be 0.000 V in oxidation or reduction, what is the value of the potential for the oxidation reaction: • E°cu,Cu2+oxid? E°cell = E°oxid + E°red
Chapter16: Applications Of Neutralization Titrations
Section: Chapter Questions
Problem 16.2QAP
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Transcribed Image Text:Pre-Lab Activities:
After reading the lab, complete items a, b, c, and d (title, purpose, chemicals and
equipment, and summary of procedure) as described on page 10 of Exp. 1 on an
8 1/2 x 11 sheet of paper.
Answer the following questions on 8 1/2 x 11 sheet of paper or in your laboratory
notebook if one is required by your instructor:
1. Write the oxidation and reduction half reactions;
a. Fe2+, Fe3+ || Br2, Br
b. Mg , Mg2+ || Cr³+, Cr2*
2. If E°H92+,Hg = +0.80V and E°co2+,Co = -0.28V, then what is the E°cell for the reaction
Co + HgCl2 → CoCl2 + Hg?
3. If you assume the E°Ag*,Ag = 0.00 volts, then what is E°Cu2+,Cu when the voltage
measured across the electrochemical cell below is +0.46 volts?
E°cell = +0.46V for Cu,Cu2+ || Ag*,Ag
4. Using the information above, what is E°Cl2 C- given the system below?
• E°cell = +1.02V for Cu,Cu2+ || Cl2,CI-
5. A student measures the potential of a cell made up with 1 M CuSO4 in one
solution and 1 M AGNO3 in the other. There is a Cu electrode in the CuSO4 and
an Ag electrode in the AgNO3, and the cell is set up as in Figure 6-1. She finds
that the potential, or voltage, of the cell, E°cell, is 0.45V, and that the Cu electrode
is negative.
a. At which electrode is oxidation occurring?
b. Write the equation for the oxidation reaction
c. Write the equation for the reduction reaction.
d. If the potential of silver, silver ion electrode, E°Ag*,Ag is taken to be 0.000 V
in oxidation or reduction, what is the value of the potential for the oxidation
reaction:
• E°cu,Cu2+oxid? E°cell
= E°oxid + E°red
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