# Nernst Equation

(Difference between revisions)
 Revision as of 14:53, 15 November 2010 (view source)← Older edit Revision as of 14:54, 15 November 2010 (view source)Newer edit → Line 26: Line 26: == Membrane Potential
== == Membrane Potential
== + + ''Main article: ''[[Membrane Potential]] Nernst equation is also can be used to calculate the potential of an [[Ion|ion]] across the membrane. For potential difference of a membrane, we can manipulate the Nernst Equation as follows:
Nernst equation is also can be used to calculate the potential of an [[Ion|ion]] across the membrane. For potential difference of a membrane, we can manipulate the Nernst Equation as follows:
Line 49: Line 51: [A-] is the concentration of ion outside the membrane (in this case is anion, negative charge ion)
[A-] is the concentration of ion outside the membrane (in this case is anion, negative charge ion)
− [A-] is the concentration of ion inside the membrane (in this case is anion, negative charge ion) + [A-] is the concentration of ion inside the membrane (in this case is anion, negative charge ion) == Application  == == Application  ==

## Revision as of 14:54, 15 November 2010

Nernst Equation is an equation used to calculate the electrical potential of a chemical reaction. In its equilibrium state, the Nernst equation should be zero. It also shows the direct relation between energy or potential of a cell and its participating ions. The equation is proposed by a German chemist, Walther H. Nernst (1864-1941).

## Equation

Nernst equation can be expressed as follows:

where

Ecell is the half-cell potential difference

Eθcell is the standard half-cell potential

R is the universal gas constant; R = 8.314471 J K-1 mol-1

T is the thermodynamics temperature, in Kelvin; 0 K = -273.15oC

z is the number of moles of electrons transferred between cells (defined by the valency of ions)

F is the Faraday's constant; F = 96,485.3415 C mol-1

[red] is the concentration of ion that gained electrons (reduction)

[oxi] is the concentration of ion that lost electrons (oxidation)

## Membrane Potential

Main article: Membrane Potential

Nernst equation is also can be used to calculate the potential of an ion across the membrane. For potential difference of a membrane, we can manipulate the Nernst Equation as follows:

or

where

Em is the potential difference of an ion between membranes

R is the universal gas constant; R = 8.314471 J mol-1

T is the thermodynamics temperature, in Kelvin; 0 K = -273.15oC

z is the number of moles of electrons transferred between membranes (defined by the valency of ion)

F is the Faraday's constant; F = 96,485.3415 C mol-1

[A-] is the concentration of ion outside the membrane (in this case is anion, negative charge ion)

[A-] is the concentration of ion inside the membrane (in this case is anion, negative charge ion)

## Application

### Ussing Study of Frog Skin

In biochemistry, Nernst equation can be used to calculate the potential difference of ion between membranes. Hans H. Ussing, a Danish scientist, used a frog skin to measure the potential difference of sodium and potassium ions across the membranes with his famous invention, the Ussing chamber.

Ussing model of transepithelial ions absorption.

For example at the standard condition and temperature of 25oC (298K), the above sodium ion membrane potential can be calculated as:

## References & Notes

1. http://nobelprize.org/nobel_prizes/chemistry/laureates/1920/nernst-bio.html, The Nobel Prize in Chemistry 1920; Walther Nernst
2. Diagram based on CMB2003: Cell and Membrane Transport lecture note (2010).