Ag/A9CI is a commonly used reference electrode in a laboratory, which can be represented as Ag/AgCl /XM KCI. The potential of this electrode is governed by the Nernst equation. Based on the following standard reduction potential (Eº) and Ksp Values (T = 25 °C), Ag* + e' = Ag (E° = 0.799 V vs SHE) AgCl = Ag* + CI (Ksp = 1.77 x 10ʻ1º) (a) Calculate the E° value for the Ag/AgCl reference electrode. E° = V (b) If the concentration of the internal filling KCI solution for the Ag/AgCl electrode is 3 M, calculate the potential of this reference electrode.

Ag/A9CI is a commonly used reference electrode in a laboratory, which can be represented as Ag/AgCl /XM KCI. The potential of this electrode is governed by the Nernst equation. Based on the following standard reduction potential (Eº) and Ksp Values (T = 25 °C), Ag* + e' = Ag (E° = 0.799 V vs SHE) AgCl = Ag* + CI (Ksp = 1.77 x 10ʻ1º) (a) Calculate the E° value for the Ag/AgCl reference electrode. E° = V (b) If the concentration of the internal filling KCI solution for the Ag/AgCl electrode is 3 M, calculate the potential of this reference electrode.

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...

See similar textbooks

Similar questions

[References] Calculate the cell potential of a cell operating with the following reaction at 25°C in which Cr2 O,=0.025 M, I=0.035 M, [Cr]= 0.15 M, and H]= 0.30 M. Cr2 O, (ag) +61 (ag) + 14H (ag) -→ 20r (aq) + 312 (s) + 7H,0(1) Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Standard Cathode (Reduction) Half-Reaction Potential, E (V) 0.54 L(s) +2e 21 (ag) Cr20, (ag) +14H" (ag) + 6e 2Cr (aq) +7H,0(1) 1.33 Cell potential = V
The following half-cells are on the left and coupled with the standard hydrogen electrode on the right to form a galvanic Calculate the cell potential. If the cell were shorted, indicate whether the electrodes shown would act as an anode or a cathode. a. Cu Cu²+ (0.0567 M), (Cu²+/Cu = 0.337 V) V Potential = b. Cu | Cul (sat'd), KI (0.0939 M), (ECul/Cu = -0.185 V) Potential = V 3+ c. Pt | Fe³+ (0.160 M), Fe²+ (0.08340 M), (E Potential = V Fe³+/Fe²+ = = 0.771 V)
When the oxidation-reduction reaction was balanced in acidic solution. If the [H2O2] = 0.352 M, partial pressure of Oz is 2.21 atm, [K2Cr2O7) = 0.642 M, the [Cr3+] = 0.963 M, and the pH was measured to be 8.42 then what is the cell potential at 25°C? O2(g) + Cr3+ *(aq) → H202(aq) + Cr20-2" (aq)
+|| Σ D. For the cell shown, the measured cell potential, Ecell, is-0.3621 V at 25 °C. Pt(s) | H, (g, 0.853 atm) | H* (aq, ? M) || Cd²+(aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, E°, are 2H*(aq) + 2 e¯ – H, (g) A 00'0 = 07 24, Cd2+ (aq) + 2 e Cd(s) E° = -0.403 V %3D Calculate the Ht concentration. M. = [,H] 10:23 AM M. 11/9/2021 7734 F4 F5 F7 F8 F10 F11 F12 PrtScr Insert Delete Eゴ #3 Backspace 2$ ) 4. 5. 9. 7. R } 1 Enter F. K. H. Sh
9) At 25°C, what is the potential and the cell reaction for the following cell: Ni | Ni2+ (aq, 0010 M) || Cl(aq, 0.20M) | Cl2 (g, 1 atm) | Pt? What is the Keg at 298K?
John makes a galvanic cell with the half-reactions Mt3+(aq) + 3e1- -->Mt(s), and R2+(aq) + 2e1- --> R(s), with standard reduction potentials of 1.09 V and 0.34 V respectively. Would the value of the Gibbs free energy decrease, increase, or remain the same, if he changes the concentrations in the galvanic cell to 0.15 M Mt3+, and 0.45 M R2+?
For the galvanic cell at 298 K 2X(s) + 3Y2*(aq) –→ 2x3*(aq) + 3Y(s) E° cell = 0.39 V What is the measured cell potential (Ecell) when [Y2*] = 1.0 M and [X3+] = 0.01 M? Periodic Table and Datasheet O 0.39 V O 0.35 V O 0.43 V O 0.51 V
Calculațe Eo cell from the tabulated standard reduction potentials for each of the following reactions in aqueous solution. Then calculate AG° and K at 25°C from E° cell' F = 9.65 x 10 J/V•mol e R = 8.314 J/mol•K Acidic solution Standard reduction potential, E (Volts) Cu2" (ag) + e Cu'(ag) + e Cu(s) Mno, (aq) + 8H"(aq) + 5e Mn?"(aq) + 4H,0 Fe (aq) + e – Fe? (aq) Cu*(aq) 0.153 0.521 1.507 0.771 Basic solution Zn(OH) (s) + 2e → Zn(s) + 40H (aq) Mno, (aq) + 2H,O + 3e MnO,(s) + 4OH(aq) -1.22 0.588
3. At 298 K, the EMF of the cell shown below is +0.84 V. Pt(s)|Fe²*(aq, a = 1), Fe³*(aq, 1)|| Ce**(aq, a = 1), Ce³*(aq, a = 1)|Pt(s) a = (i) Define what is meant by the standard EMF of the cell. (ii) Write down the cell reaction and the Nernst equation for the cell. (iii) Calculate the equilibrium constant for the cell reaction at 298 K.
At a temperature of 25 ° C the galvanic element Pt | MnO4- 0,10M, Mn2 + 0,1M, pH = 1 | Ag + 0.0001M | Ag has the electromotive force 0,80V. Calculate the standard electrode potential of Ag + if E ° (MnO4 -, H + | Mn2 +) = 1.50V
The cell potential of the following electrochemical cell depends on the gold concentration in the cathode half- cell: Pt(s) | H2 (g, 1.0 bar) | H+(aq, 1.0 mol L-1) | Au3+(aq, ? mol L-1) | Au(s) What is the concentration of Au3+ in the solution if is Ecell is 1.24 ? Express your answer using two significant figures and don't include the exponent (e.g. if your answer is 2.5×10-4, only write 2.5)