A student wishes to determine the chloride ion concentration in a water sample at 25 °C using a galvanic cell constructed with a graphite electrode and a half-cell of AgCI(s) + e Ag(s) + CI (aq) E°red = 0.2223 V %3D And a copper electrode with 0.500 M Cu²* as the second half cell Cu2*(aq) + 2 e → Cu(s) E°red%3D 0.337 V The measured cell potential when the water sample was placed into the silver side of the cell was 0.0549 V. Given the standard cell potential for this cell is 0.115 V, and the measured cell potential is 0.0549, what is the concentration of chloride ions in the solution?

A student wishes to determine the chloride ion concentration in a water sample at 25 °C using a galvanic cell constructed with a graphite electrode and a half-cell of AgCI(s) + e Ag(s) + CI (aq) E°red = 0.2223 V %3D And a copper electrode with 0.500 M Cu²* as the second half cell Cu2*(aq) + 2 e → Cu(s) E°red%3D 0.337 V The measured cell potential when the water sample was placed into the silver side of the cell was 0.0549 V. Given the standard cell potential for this cell is 0.115 V, and the measured cell potential is 0.0549, what is the concentration of chloride ions in the solution?

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter17: Electrochemistry

Section: Chapter Questions

Problem 76AP

See similar textbooks

Similar questions

The half-cells Ag+(aq. 1.0 M)|Ag(s) and H+(aq, ? M)|H2(1.0 bar) are linked by a salt bridge to create a voltaic cell. With the silver electrode as the cathode, a value of 0.902 V is recorded tor kcell at 298 K. Determine the concentration of H+ and the pH of the solution.
Calculate the electrode potentials of the following half-cells. (a) Ag+(0.0436 M)|Ag (b) Fe3+ (5.34 10-4M),Fe2+ (0.090 M)|Pt (c) AgBr(sat’d),Br- (0.037 M)|Ag
The saturated calomel electrode. abbreviated SCE. is often used as a reference electrode in making electrochemica1 measurements. The SCE is composed of mercury in contact with a saturated solution of calomel (Hg2Cl2). The electrolyte solution is saturated KCI. is +0.242 V relative to the standard hydrogen electrode. Calculate the potential for each of the following galvanic cells containing a saturated calomel electrode and the given half-cell components at standard conditions. In each case. indicate whether the SCE is the cathode or the anode. Standard reduction potentials are found in Table 17.1. a. Cu2++2eCu b. Fe3++e-Fe2+ c. AgCl+e-Ag+Cl- d. Al3++3eAl e. Ni2++2eNi
What is the voltage of a concentration cell of Fe2+ ions where the concentrations are 0.0025 and 0.750 M? What is the spontaneous reaction?
Consider the following galvanic cell: A 15 0-mole sample of NH is added to the Ag compartment (assume 1.00 L of total solution after the addition). The silver ion reacts with ammonia to form complex ions as shown: Ag+(aq)+NH3(aq)AgNH3+(aq)K1=2.1103AgNH3+(aq)+NH3(aq)Ag(NH3)2+(aq)K2=8.2103 Calculate the cell potential after the addition of 15.0 moles of NH3.
Halide ions can he deposited at a silver anode, the reaction being Ag(s) + X- AgX(s) +e- Suppose that a cell was formed by immersing a silver anode in an analyte solution that was 0.0250 M Cl-,Br-, and I -ions and connecting the half-cell to a saturated calomel cathode via a salt bridge. (a) Which halide would form first and at what potential? Is the cell galvanic or electrolytic? (b) Could I- and Br- be separated quantitatively? (Take 1.00 l0-5 M as the criterion for quantitative removal of an ion.) If a separation is feasible, what range of cell potential could he used? (c) Repeat part (b) for I- and Cl-. (d) Repeat part (b) for Br- and Cl-.
An electrolysis experiment is performed to determine the value of the Faraday constant (number of coulombs per mole of electrons). In this experiment, 28.8 g of gold is plated out from a AuCN solution by running an electrolytic cell for two hours with a current of 2.00 A. What is the experimental value obtained for the Faraday Constant?