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Ecell = E0 - (0.0591n)log[H+]0.207 = 0.0591log[H+]1Therefore.pdf

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The document discusses the calculation of the electrochemical cell potential (ecell) in relation to hydrogen ion concentration ([h+]). It derives the pH value from the relationship between ecell and log[h+], indicating a pH of 3.5. The equations presented link the standard electrode potential (e0) and the Nernst equation.

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Ecell = E0 - (0.0591/n)log[H+] 0.207 = 0.0591*log[H+]/1 Therefore - log[H+] = pH = 3.5 Solution Ecell = E0 - (0.0591/n)log[H+] 0.207 = 0.0591*log[H+]/1 Therefore - log[H+] = pH = 3.5

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Ecell = E0 - (0.0591n)log[H+]0.207 = 0.0591log[H+]1Therefore.pdf

  • 1. Ecell = E0 - (0.0591/n)log[H+] 0.207 = 0.0591*log[H+]/1 Therefore - log[H+] = pH = 3.5 Solution Ecell = E0 - (0.0591/n)log[H+] 0.207 = 0.0591*log[H+]/1 Therefore - log[H+] = pH = 3.5