Homework Answers
You are titrating 100.0 mL of 0.0400 M Fe2+ in 1 M HCIO4 with 0.100 M...
You are titrating 100.0 mL of 0.0400 M Fe2+ in 1 M HCIO4 with 0.100 M Ce4+ to give Fe3+ and Ce3+ using Pt and calomel electrodes to find the endpoint. (a) Write the balanced titration reaction. > (b) Complete the two half reactions for the Pt electrode. Ce té E° = 1.70 V Fe +e = E° = 0.767 V [Fe2+11 1 - 0.241 E= 0.767 – 0.05916) (c) From the list in the column at the right, select...
A 100.0 mL solution of 0.0400 M Fe2+ in 1 M HCIO s titrated with 0.100 M Ce4+ resulting in the fo...
A 100.0 mL solution of 0.0400 M Fe2+ in 1 M HCIO s titrated with 0.100 M Ce4+ resulting in the formation of Fe3+ and Ce3+. A Pt indicator electrode and a saturated calomel electrode are used to monitor the titration. Write the balanced titration reaction titration reaction:> Complete the two half-reactions that occur at the Pt indicator electrode. Write the half-reactions as reductions half-reaction: Ce e half-reaction: Fe e- E 0.767 V Select the two equations that can be...
A 100.0 mL solution of 0.0400 M Fe2+ in 1 M HCIO, is titrated with 0.100...
A 100.0 mL solution of 0.0400 M Fe2+ in 1 M HCIO, is titrated with 0.100 M Ce*+ resulting in the formation of Fe+ and Ce3+. APt indicator electrode and a saturated calomel electrode are used to monitor the titration Write the balanced titration reaction. titration reaction:-> Complete the two half reactions that occur at the Pt indicatorelecrode Write the half-reactions as reductions half-reaction: Ice + e-→ We were unable to transcribe this imageсез+] . 0.241 (Ce+] 「 0.241 E...
ans A C B how ? 14. Consider the titration of 25.00 mL of 0.0500 M...
ans A C B how ?
14. Consider the titration of 25.00 mL of 0.0500 M Sn2+ with 0.100 M Fe3+ in 1 M HCl to give Fe2+ and Sn4+, using Pt and saturated calomel electrodes SCE l Sn4+, Sn2+, Fe3+, Fe3 | Pt(s) The titration reaction: 2Fe3 + Sn2+Snt+ 2Fe2+ The two half-reactions for the indicator electrode: Fe3+e Sn 2e Sn2+ Indicate the two Nernst equations for the cell voltage. E 0.732 V E 0.139 V Fe2+ IFe2 log...
Мар You are performing a titration of 25.0 mL of 0.0100 M Sn4 in 1 M HCI with 0.0500 M Ag* to give Sn2 anu 3+ Ags using...
Мар You are performing a titration of 25.0 mL of 0.0100 M Sn4 in 1 M HCI with 0.0500 M Ag* to give Sn2 anu 3+ Ags using a Pt indicator electrode and a saturated calomel electrode (SCE) as the reference electrode. A) Write the balanced titration reaction B) Complete the two half-reactions that occur at the indicator electrode (shown is their corresponding reduction potential) Sn E 0.139 V 3+ Ag® Eo 1.90 V C) Choose the two different expressions...
- A40.0 mL. solution of 0.600 M Cu' in 1 M HNO was t titrated with...
- A40.0 mL. solution of 0.600 M Cu' in 1 M HNO was t titrated with 0.400 M Cef to give Cu and Ce The saturated calomel electrode was the reference e lectrode. (a) Write down the BALANCED titration reaction (b) Determine the equivalence volume. (c) Write the analyte half-reaction for the indicator electrode. (d) Write the titrant half-reaction for the indicator electrode (e) Write the analyte Nernst equation for the net cell reaction. (t) Write the titrant Nernst equation...
Consider the titration of 25.0 mL of 0.01000 M Sn2+ by 0.0500 M Tl3+ in 1...
Consider the titration of 25.0 mL of 0.01000 M Sn2+
by 0.0500 M Tl3+ in 1 M HCl, using Pt and saturated
calomel electrodes to find the endpoint.
a.) Write the balanced titration reaction.
b.) Write two different half-reactions for the indicator
electrode.
c.) Write two different Nernst equations for the cell
voltage.
d.) Calculate E at the following volumes of Tl3+:
1.00, 2.50, 4.90, 5.00, 5.10, and 10.0 mL.
(This is problem 3 in Chapter 15 from Eigth Edition...
3. (20 points) Consider the titration of 25.0 mL of 0.05 M Sna' with 0.100 M...
3. (20 points) Consider the titration of 25.0 mL of 0.05 M Sna' with 0.100 M Fell in 1 M HCl to give Fe2+ and Sn" using Pt and calomel electrodes. a) Write a balanced titration reaction. b) Write two half-reactions for the indicator electrode. c) Write two Nernst equations for the cell voltage d) Calculate E at the following volumes of Fe3+: 1.0, 5.0, 10.0, 12.5, 17.5, 20.0, 24.0, 25.0, 26.0 and 30.0 mL. Make the titration curve graph.
5. Consider the titration of 25.0 mL of 0.0100 M Sn2 by 0.0500 M Ti Pt and saturated calomel electrodes to find the end point. (total 15 pt) M HCI, using (c) Write two different Nernst equations for...
5. Consider the titration of 25.0 mL of 0.0100 M Sn2 by 0.0500 M Ti Pt and saturated calomel electrodes to find the end point. (total 15 pt) M HCI, using (c) Write two different Nernst equations for the cell voltage. (3 pt) (d) Calculate E at the following volumes of TI: 1.0, 2.5,4.9,5.0,5.1, and 10.0 mL. (6 pt)
5. Consider the titration of 25.0 mL of 0.0100 M Sn2 by 0.0500 M Ti Pt and saturated calomel electrodes to...
At 25 C, a titration of 15.00 mL of a 0.0440 M A^NO, solution with a...
At 25 C, a titration of 15.00 mL of a 0.0440 M A^NO, solution with a 0.0220 M Nal solution is conducted within the cell SCE | titration solution | Ag(s) For the cell as written, what is the potential after the addition of each volume of Nal solution? The reduction potential for the saturated calomel electrode is E = 0.241 V. The standard reduction potential for the reaction Ag+ + e _» Ag(s) is E = 0.79993 V. The...
You are titrating 100.0 mL of 0.0400 M Fe2+ in 1 M HCIO4 with 0.100 M Ce4+ to give Fe3+ and Ce3+ using Pt and calomel electrodes to find the endpoint. (a) Write the balanced titration reaction. > (b) Complete the two half reactions for the Pt electrode. Ce té E° = 1.70 V Fe +e = E° = 0.767 V [Fe2+11 1 - 0.241 E= 0.767 – 0.05916) (c) From the list in the column at the right, select...
A 100.0 mL solution of 0.0400 M Fe2+ in 1 M HCIO s titrated with 0.100 M Ce4+ resulting in the formation of Fe3+ and Ce3+. A Pt indicator electrode and a saturated calomel electrode are used to monitor the titration. Write the balanced titration reaction titration reaction:> Complete the two half-reactions that occur at the Pt indicator electrode. Write the half-reactions as reductions half-reaction: Ce e half-reaction: Fe e- E 0.767 V Select the two equations that can be...
A 100.0 mL solution of 0.0400 M Fe2+ in 1 M HCIO, is titrated with 0.100 M Ce*+ resulting in the formation of Fe+ and Ce3+. APt indicator electrode and a saturated calomel electrode are used to monitor the titration Write the balanced titration reaction. titration reaction:-> Complete the two half reactions that occur at the Pt indicatorelecrode Write the half-reactions as reductions half-reaction: Ice + e-→ We were unable to transcribe this imageсез+] . 0.241 (Ce+] 「 0.241 E...
ans A C B how ?
14. Consider the titration of 25.00 mL of 0.0500 M Sn2+ with 0.100 M Fe3+ in 1 M HCl to give Fe2+ and Sn4+, using Pt and saturated calomel electrodes SCE l Sn4+, Sn2+, Fe3+, Fe3 | Pt(s) The titration reaction: 2Fe3 + Sn2+Snt+ 2Fe2+ The two half-reactions for the indicator electrode: Fe3+e Sn 2e Sn2+ Indicate the two Nernst equations for the cell voltage. E 0.732 V E 0.139 V Fe2+ IFe2 log...
Мар You are performing a titration of 25.0 mL of 0.0100 M Sn4 in 1 M HCI with 0.0500 M Ag* to give Sn2 anu 3+ Ags using a Pt indicator electrode and a saturated calomel electrode (SCE) as the reference electrode. A) Write the balanced titration reaction B) Complete the two half-reactions that occur at the indicator electrode (shown is their corresponding reduction potential) Sn E 0.139 V 3+ Ag® Eo 1.90 V C) Choose the two different expressions...
- A40.0 mL. solution of 0.600 M Cu' in 1 M HNO was t titrated with 0.400 M Cef to give Cu and Ce The saturated calomel electrode was the reference e lectrode. (a) Write down the BALANCED titration reaction (b) Determine the equivalence volume. (c) Write the analyte half-reaction for the indicator electrode. (d) Write the titrant half-reaction for the indicator electrode (e) Write the analyte Nernst equation for the net cell reaction. (t) Write the titrant Nernst equation...
Consider the titration of 25.0 mL of 0.01000 M Sn2+
by 0.0500 M Tl3+ in 1 M HCl, using Pt and saturated
calomel electrodes to find the endpoint.
a.) Write the balanced titration reaction.
b.) Write two different half-reactions for the indicator
electrode.
c.) Write two different Nernst equations for the cell
voltage.
d.) Calculate E at the following volumes of Tl3+:
1.00, 2.50, 4.90, 5.00, 5.10, and 10.0 mL.
(This is problem 3 in Chapter 15 from Eigth Edition...
3. (20 points) Consider the titration of 25.0 mL of 0.05 M Sna' with 0.100 M Fell in 1 M HCl to give Fe2+ and Sn" using Pt and calomel electrodes. a) Write a balanced titration reaction. b) Write two half-reactions for the indicator electrode. c) Write two Nernst equations for the cell voltage d) Calculate E at the following volumes of Fe3+: 1.0, 5.0, 10.0, 12.5, 17.5, 20.0, 24.0, 25.0, 26.0 and 30.0 mL. Make the titration curve graph.
5. Consider the titration of 25.0 mL of 0.0100 M Sn2 by 0.0500 M Ti Pt and saturated calomel electrodes to find the end point. (total 15 pt) M HCI, using (c) Write two different Nernst equations for the cell voltage. (3 pt) (d) Calculate E at the following volumes of TI: 1.0, 2.5,4.9,5.0,5.1, and 10.0 mL. (6 pt)
5. Consider the titration of 25.0 mL of 0.0100 M Sn2 by 0.0500 M Ti Pt and saturated calomel electrodes to...
At 25 C, a titration of 15.00 mL of a 0.0440 M A^NO, solution with a 0.0220 M Nal solution is conducted within the cell SCE | titration solution | Ag(s) For the cell as written, what is the potential after the addition of each volume of Nal solution? The reduction potential for the saturated calomel electrode is E = 0.241 V. The standard reduction potential for the reaction Ag+ + e _» Ag(s) is E = 0.79993 V. The...
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