![сез+] . 0.241 (Ce+] 「 0.241 E = 1.70-0.059 16log E = 1.70-0.059 1610g Calculate the values of E for the cell after each of th](http://img.homeworklib.com/questions/bd8617e0-9877-11ea-bf3b-d3e3e85edfb9.png?x-oss-process=image/resize,w_560)
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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 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...
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...
Ce Ce Ce Ce You are titrating 100.0 mL of 0.0400 M Fe2 in 1 M...
Ce Ce Ce Ce You are titrating 100.0 mL of 0.0400 M Fe2 in 1 M HCIO4 with 0.100 M Ce to give Fe and Ce E E-0.767-0.05916log 0.24I using Pt and calomel electrodes to find the endpoint. (a) Write the balanced titration reaction. Fe aq)Ce (aq)Fe (b) Complete the two half reactions for (d) Calculate the values of E for the cell when the following volumes of the Ce titrant have been added: (Activity coefficients may be ignored as...
- 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...
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...
A 20.0 mL solution of a 0.00500 M Sn2 solution in 1.0 M HCI was titrated...
A 20.0 mL solution of a 0.00500 M Sn2 solution in 1.0 M HCI was titrated with 0.0200M Ce solution to give Sn and Csalomel 0.241 V and E (Sn /Sn2)-0.139 V) a) Write the balanced titration reaction. b) Calculate the potential (versus S.C.E) after the addition of 5.00 mL of the titrant. c) Calculate the potential (versus S.C.E) after the addition of 12.00 mL of the titrant.
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.
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...
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...
Consider the titration of 60.0 mL of 0.0400 M HONH2 (a weak base; Kb = 1.10e-08) with 0.100 M HIO4. Calculate the pH aft...
Consider the titration of 60.0 mL of 0.0400 M HONH2 (a weak base; Kb = 1.10e-08) with 0.100 M HIO4. Calculate the pH after the following volumes of titrant have been added: (a) 0.0 mL pH = (b) 6.0 mL pH = (c) 12.0 mL pH = (d) 18.0 mL pH = (e) 24.0 mL pH = (f) 40.8 mL pH =
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...
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...
Ce Ce Ce Ce You are titrating 100.0 mL of 0.0400 M Fe2 in 1 M HCIO4 with 0.100 M Ce to give Fe and Ce E E-0.767-0.05916log 0.24I using Pt and calomel electrodes to find the endpoint. (a) Write the balanced titration reaction. Fe aq)Ce (aq)Fe (b) Complete the two half reactions for (d) Calculate the values of E for the cell when the following volumes of the Ce titrant have been added: (Activity coefficients may be ignored as...
- 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...
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...
A 20.0 mL solution of a 0.00500 M Sn2 solution in 1.0 M HCI was titrated with 0.0200M Ce solution to give Sn and Csalomel 0.241 V and E (Sn /Sn2)-0.139 V) a) Write the balanced titration reaction. b) Calculate the potential (versus S.C.E) after the addition of 5.00 mL of the titrant. c) Calculate the potential (versus S.C.E) after the addition of 12.00 mL of the titrant.
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.
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...
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...
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