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Ch.19 - Electrochemistry
Chapter 19, Problem 111

The cell potential of this electrochemical cell depends on the pH of the solution in the anode half-cell. Pt(s) | H2(g, 1 atm) | H+(aq, ? M) || Cu2+(aq, 1.0 M) | Cu(s) What is the pH of the solution if Ecell is 355 mV?

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Nernst Equation

The Nernst Equation relates the cell potential (E) of an electrochemical cell to the concentrations of the reactants and products. It is expressed as E = E° - (RT/nF)ln(Q), where E° is the standard cell potential, R is the gas constant, T is the temperature in Kelvin, n is the number of moles of electrons transferred, F is Faraday's constant, and Q is the reaction quotient. This equation allows us to calculate the effect of concentration changes on the cell potential.
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pH and Hydrogen Ion Concentration

pH is a measure of the acidity or basicity of a solution, defined as the negative logarithm of the hydrogen ion concentration: pH = -log[H+]. In electrochemical cells, the pH can influence the concentration of H+ ions, which in turn affects the cell potential. A lower pH indicates a higher concentration of H+ ions, which is crucial for determining the conditions in the anode half-cell.
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Electrochemical Cell Components

An electrochemical cell consists of two half-cells: the anode, where oxidation occurs, and the cathode, where reduction takes place. In the given cell, the anode involves hydrogen gas and protons, while the cathode involves copper ions and solid copper. Understanding the roles of these components and their reactions is essential for analyzing how changes in conditions, such as pH, affect the overall cell potential.
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