A galvanic cell was prepared by immersing an anode and a cathode of the same material (of A type) in a solution containing a low solubility salt AX from the anode side and a concentration of 0.1 mol/Kg A* ion in the cathode side. The cell potential was found to be 2.50 V. The solubility product constant (ksp)of this salt is then? a. 1.85 x 10-80 b. 7.70 x 10-83

A galvanic cell was prepared by immersing an anode and a cathode of the same material (of A type) in a solution containing a low solubility salt AX from the anode side and a concentration of 0.1 mol/Kg A* ion in the cathode side. The cell potential was found to be 2.50 V. The solubility product constant (ksp)of this salt is then? a. 1.85 x 10-80 b. 7.70 x 10-83

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

1. A concentration cell is constructed using two metal (M) electrodes with M 2+ concentrations of 0.10 M and 1.00 × 10 –5 M in the two half-cells. Determine the reduction potential of M 2+ given that the potential of the cell at 25°C is 0.118 V.a. 0 Vb. +0.118 Vc. –0.118 Vd. Cannot be determined with the information given.e. None of the above.
Give the answer to the questions below: Is AuCl more soluble in pure water or in 1M aqueous solution of NaCN? Will the Pb²+ or Pb half-cell (Eºred = -0.126 V) be the cathode when coupled with the SHE in a galvanic cell? What is the oxidizing agent in the following reaction? Mg(s) | Mg2+ (aq) || Pb2+ (aq) | Pb(s).
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)
A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is a hydrogen electrode (PH, )= latm) immersed in a solution of unknown [H*]. If the cell potential is 0.216 V, what is the pH of the unknown solution at 298 K? pH =
Kindly write the sol.n
Consider the following cell reaction: Fe(s) + 2 H"(? М) —Ғе*"(1.00 М) + H-(g)(1.00 atm) →Fe? If the cell potential at 298 K is 0.164 volts, what is the pH of the hydrogen electrode? pH
A potential difference of 2.0 V is impressed across a pairof inert electrodes (e.g., platinum) that are immersed in a 0.050 M aqueous KBr solution. What are the products that form at the anode and the cathode?
Three voltaic cells can be constructed from solutions Pb(NO3)2(aq) and the corresponding metal electrodes. of Cuso (aq), ZnSOa(aq), and Reaction E Zn?daa) + 2e s zn(s) -0,7626V Pbaas + 2e 5 Pb (S) - 0.1251 V Calculate the standard cell potential for each voltaic cell combination. For a spontaneous reaction, E'cell must be positive when E'anode is subtracted from E'cathode. Use the standard potentlals from p. 119 for calculations. 1. * 2e- ニ Cucs) 0. 340 V Agčaa) e- 5 Ag(s) 0.7991 2. Identify which metal electrode serves as the cathode and which metal electrode serves as the anode. Tabulate the results from questions 1 and 2: E'cell Cell Anode Cathode Cu/Zn Cu/Pb Pb/Zn 3.a. Using the Nernst Equation, calculate the expected voltage (Etheo) for a cell which consists of 0.0300 M Pb(NOs)2(aq) and 0.0400 M CuSO (aq). b. Glve the conventional cell notation for this cell, assuming a salt bridge separates the two half- cells.
e. Calculate the cell potential Ecell of the Galvanic cell (25°C). Give your answer in volts (V).
is 0.085 correct or should it be 0.116? I got two answers and i’m not sure.
Determine the cell potential for the following cell Zn(s) | Zn2+(aq), 0.500 M || Ag+(aq), 0.010 M | Ag(s) The standard reduction potentials of Zn2+(aq) and Ag+(aq) are –0.76 V and +0.80 V, respectively. A. 1.45 V B. 1.67 V C. 1.56 V D. 1.51 V E. 1.61 V
A voltaic cell is constructed in which the cathode is a standard hydrogen electrode and the anode is a hydrogen electrode ( PH, )= latm) immersed in a solution of unknown [H*]. If the cell potential is 0.201 V, what is the pH of the unknown solution at 298 K? pH =