www.nextnano.com/manual/nextnano3/tutorials/electrolyte_GouyChapman.html

Author: Stefan Birner

If you want to obtain the input file that is used within this tutorial, please contact stefan.birner@nextnano.de.

`-> 1DGouyChapman_template.in`

2DGouyChapman_template.in

3DGouyChapman_template.in

- We solve the Poisson-Boltzmann equation for a monovalent salt, i.e. NaCl
(Na
^{+}Cl^{-}).

For this particular case, our numerical solution of the Poisson-Boltzmann equation can be compared to the analytical one-dimensional Gouy-Chapman solution for a monovalent and symmetric salt.

- The temperature is set to 298.15 K = 25°C, the static dielectric constant
of water is set to 78.

- The electrolyte region (0 nm - 200 nm) contains the following ions:

`!---------------------------------------------------------------------------!`

singly charged cations

! The electrolyte (NaCl) contains two types of ions:

! 1) 100 mM singly charged cations (Na^{+}) <- 100 mM NaCl

! 2) 100 mM singly charged anions (Cl^{-}) <- 100 mM NaCl

!---------------------------------------------------------------------------!

$electrolyte-ion-content

ion-number = 1 !

charge of the ion:

ion-valency = 1d0 !`Na`

Input in units of:^{+}

ion-concentration = 100d-3 !`[M] = [mol/l] = 1d-3 [mol/cm³]`

refers to region where the electrolyte has to be applied to

ion-region = 0d0 200d0 !

singly charged anions

ion-number = 2 !

charge of the ion:

ion-valency = -1d0 !`Cl`

Input in units of:^{-}

ion-concentration = 100d-3 !`[M] = [mol/l] = 1d-3 [mol/cm³]`

refers to region where the electrolyte has to be applied to

ion-region = 0d0 200d0 !

We vary the NaCl concentration from

`- 1 M NaCl`

Consequently, we have to vary

- 0.1 M NaCl

- 10 mM NaCl

- 1 mM NaCl

- 0.1 mM NaCl

`ion-concentration = 100d-3 ! [M]`

.

- We assume an interface charge between the oxide and the electrolyte of
`-`

0.2 C/m^{2}= -124.83 x 10^{12}|e|/cm^{2}.

`$interface-states`

...

state-number = 1 ! between contact / electrolyte at 0 nm

state-type = fixed-charge ! sigma

interface-density = -124.830193d12 ! -0.2 [C/m^2] = -124.830193 x 10^12 [|e|/cm^2]

- The pH value is 7, i.e. neutral.

`$interface-states`

concentration in

...

state-number = 2 ! between contact / electrolyte at 0 nm

state-type = electrolyte !

$electrolyte

...

pH-value = 7d0 ! pH = -lg(concentration) = 7 ->`[M]=[mol/l]`

- The following figure shows the electrostatic potential for different salt
concentrations (0.1 mM, 1 mM, 10 mM, 0.1 M and 1 M) at a fixed surface charge of
`-`

0.2 C/m^{2}.

The potential at the surface at 0 nm, that arises due to the fixed surface charge density that is in contact with the electrolyte, is screened by the ions in the solution and the resulting distribution of the ions depends on the value of the spatially varying electrostatic potential.

The Debye screening lengths (`DebyeScreeningLength.txt`

) are indicated by the squares and the values are:

`- 1 M NaCl: 0.303 nm`

(Here, the concentrations of the H3O

- 0.1 M NaCl: 0.959 nm

- 10 mM NaCl: 3.032 nm

- 1 mM NaCl: 9.589 nm

- 0.1 mM NaCl: 30.308 nm^{+}and OH

ions slighly influence the Debye screening length (last two digits) because in the next^{-}**nano**³ simulations these ions are always present and their concentrations depend on the pH value.)

For a definiton of the Debye screening length, have a look here:

`$electrolyte`

The following figure shows the Debye screening length for a monovalent salt such as NaCl as a function of the salt concentration.

For a monovalent salt the nominal value of the salt concentration is equal to the ionic strength which is a measure for the screening of charges in a solution.

- The surface potential can be found in this file:
`InterfacePotentialDensity_vs_pH1D.dat`

It reads for a salt concentration of 0.1 M NaCl:

`pH value interface potential [V] interface density (1*10^12 [e/cm^2])`

7.000000 -0.123478240580906 -124.830193000000

- The following figure shows the ion distribution for a 0.1 M NaCl
electrolyte. The multiples of the Debye screening lengths (kappa
^{-1}= 0.959 nm) are indicated by the vertical lines.

The negative surface charge is screened by the**positive Na**whereas the^{+}ions**negatively charged Cl**ions are repelled from the surface.^{-}

At about 5 nm both ions reach their equilibrium concentration of 0.1 M.

**Linearization of the Gouy-Chapman model**

In this approximation (only for high salt concentrations or small surface charges), the surface charge and the surface potential can be related through the basic capacitor equation:

sigma_{s}= phi_{s}C_{DL}

where C_{DL}is the capacitance per unit area of the electric double layer.

The following figure shows the surface potential at the solid/electrolyte interface as a function of interface charge for a monovalent salt such as NaCl at different salt concentrations calculated with the Poisson-Boltzmann equation (symbols).

The solid lines are the solutions of the analytical Grahame equation for a monovalent salt which relates surface potential to surface charge.

The dotted lines are the solutions of the Debye-Hückel approximation for a monovalent salt which relates surface potential to surface charge.

It can be clearly seen, that only for high salt concentrations or small surface charges the linearization is valid.

The linearization of the Poisson-Boltzmann equation is called "Debye-Hückel approximation".

It can be switched on using:

`! electrolyte-equation = Poisson-Boltzmann !`

Poisson-Boltzmann equation (default)`electrolyte-equation = Debye-Hueckel-approximation !`

Debye-Hückel approximation

**Capacitance**

The numerical Poisson-Boltzmann calculations for the capacitance (using the same data as in the previous figure are shown next.

The capacitance increases rapidly for higher potentials but at very small surface potentials, the capacitance is equal to the approximation of parallel plate capacitor model of the electric double layer.

This is expected because in the limit of low potentials, the solution of the Poisson-Boltzmann equation must converge to the solution of the Debye-Hückel equation.

- Please help us to improve our tutorial. Send comments to
`support [at] nextnano.com`

.