Consider the titration of 25.0ml 0.0100M Sn2+ by 0.0500M Tl3+ in 1M HCl using Pt and saturated calomel electrodes , calculate E at following volumes of Tl3+ : 1, 5 and 10ml
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Consider the titration of 25.0ml 0.0100M Sn2+ by 0.0500M Tl3+ in 1M HCl using Pt and saturated calomel electrodes , calculate E at following volumes of Tl3+ : 1, 5 and 10ml
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- A titration of 50.0 mL of 0.10 M Sn2+ with 0.2 M Fe3+ in 1 M HCl to give Fe2+ and Sn4+ using Pt and calomel electrodes. Assuming the standard potential for Sn2+/Sn4+ = 0.139V ; calomel, 0.241 V; Fe2+/Fe3+ = 0.732 V. Calculate the voltage (E) at 25 ml, 50 ml, and 70 ml.Consider the titration of 25.0mL 0.0100M Sn2+by 0.0500M Tl3+in 1M HCl, using Pt and saturated calomel electrodes. 1)Calculate E at the following volumes of Tl3+: 1, 2.5, 4.9, 5, 5.1, and 10 mL12.00 mL of 0.1234 M Fe 2+ is titrated with 0.1234 M BrO - 3 and monitored usingpotentiometry (an SCE reference and a Pt indicator electrode). Both solutions are at pH2.00. 1. Calculate the cell potential 2.00 mL before Ve . 2. Calculate the cell potential at Ve.
- A titration of 50.0 mL of 0.10 M Sn2+ with 0.2 M Fe3+ in 1 M HCl to give Fe2+ and Sn4+ using Pt and calomel electrodes. Assuming the standard potential for Sn2+/Sn4+ = 0.139V ; calomel, 0.241 V; Fe2+/Fe3+ = 0.732 V. This my cathode reaction: Fe3+ (aq) + 1 electron <-> Fe2+(s) and anode reaction: Sn2+(s) <-> Sn4+(aq) + 2 electrons. How will I write my Nernst equation for the cell voltage for the oxidation reaction?Consider the titration of 100.0 mL of 0.010 0 M Ce4+ in 1 M HClO4 by 0.040 0 M Cu+ to give Ce3+ and Cu2+, using Pt and saturated Ag | AgCl electrodes to find the end point. (a) Write a 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 Cu+: 1.00, 12.5, 24.5, 25.0, 25.5, 30.0, and 50.0 mL. Sketch the titration curve.Consider the titration of 100.0 mL of 0.010 0 M Ce4+ in 1 M HClO4 by 0.040 0 M Cu+ to give Ce3+ and Cu2+, using Pt and Ag | AgCl electrodes (Eref = 0.197 V) to find the end point. Ce4+ + e- ↔ Ce3+ E⁰ = 1.70 Cu2+ + e- ↔ Cu+ E⁰ = 0.161 a. Write a balanced titration reaction. b. Write two different Nernst equations for the cell voltage. c. Calculate E at the following volumes of Cu+: 12.5, 25.0, and 30.0 mL.
- Consider the titration of 100.0 mL of 0.010 0 M Ce4+ in 1 M HClO4 by 0.040 0 M Cu+ to give Ce3+ and Cu2+, using Pt and Ag | AgCl electrodes (Eref = 0.197 V) to find the end point. Ce4+ + e- ↔ Ce3+ E⁰ = 1.70 Cu2+ + e- ↔ Cu+ E⁰ = 0.161 Calculate E at the following volumes of Cu+: 12.5, 25.0, and 30.0 mL.Calculate the Ecell at the equivalence point for titration of 25.0 mL of 0.100 M Fe2+ in 1.00 M HNO3 with 0.0200 M MnO4" in 1.00 M HNO3. SHE was used as the reference electrode. O A. 0.74 V O B. 0.89 V O C. 1.14 V O D. 1.39 V E. 2.28 VRedox Titration Curve Consider the titration of 100.00 mL of 0.0100 M Ce4+ in 1.00 M HClO4 by 0.0400 M Cu+ to give Ce3+ and Cu2+. Cu2+ + e- ⇄ Cu+ E° = +0.161 V Ce4+ + e- ⇄ Cu3+ E° = +1.700 V (in 1.00 M HClO4) a) What is the overall standard potential for this titration (E°cell)? b) What is the Keq for this reaction?
- Consider the titration of 25.00 mL of 0.03555 M Co2+ by 0.02784 M EDTA at pH 10.00. Kf is 1045. Calculate the pCo2+ when 35.00 mL of EDTA are added.Redox Titration Curve Consider the titration of 100.00 mL of 0.0100 M Ce4+ in 1.00 M HClO4 by 0.0400 M Cu+ to give Ce3+ and Cu2+. Cu2+ + e- ⇄ Cu+ E° = +0.161 V Ce4+ + e- ⇄ Cu3+ E° = +1.700 V (in 1.00 M HClO4) a) Which ion undergoes oxidation? b) Which ion undergoes reduction? c) Which of the following is the overall standard reaction? a. Ce3+ + Cu2+ ⇄ Ce4+ + Cu+ b. Ce4+ + Cu+ ⇄ Ce3+ + Cu2+ c. Ce4+ + Cu2+ ⇄ Ce3+ + Cu+ d. Ce3+ + Cu+ ⇄ Ce4+ + Cu2+ d) What is the overall standard potential for this titration (E°cell)?Consider the titration of 25.0 mL of 0.010 0 M Sn21 by 0.050 0 M Tl31 in 1 M HCl, using Pt and saturated 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 Tl31: 1.00, 2.50, 4.90, 5.00, 5.10, and 10.0 mL. Sketch the titration curve.
