##What this page is about:
The WheeStat is a potentiostat, which is an instrument used to study electron transfer reactions between species in solution and electrodes. This instrument can be used to teach electrochemistry or to quantify the concentration of some analyte (such as a metal ion) in water. There is a PublicLab wiki page that discusses potentiostats [here](http://publiclab.org/wiki/potentiostat).
[](https://i.publiclab.org/system/images/photos/000/005/081/original/figure_1.png)
##Links to Public Lab Research Notes that describe the WheeStat:
The history of the project was first described [here](http://publiclab.org/notes/JSummers/11-02-2013/potentiostat-notes-1-wheestat-history).
Discussions of how to build the WheeStat hardware are described [here ](http://publiclab.org/notes/JSummers/12-30-2013/potentiostat-notes-3-wheestat-5-1-fabrication)and [here](http://publiclab.org/notes/JSummers/01-08-2014/potentiostat-notes-4-fabrication-made-easy). While the former note discusses how to build your own pcb, the latter tells how to order the pcb from OSH Park.
Some early discussion on the software and graphic user interface are [here](http://publiclab.org/notes/JSummers/12-20-2013/potentiostat-software) and [here](http://publiclab.org/notes/JSummers/01-04-2014/potentiostat-notes-3a-timing-de-bugged).
A discussion of making low cost electrodes is [here](http://publiclab.org/notes/JSummers/01-09-2014/potentiostat-notes-5-how-to-make-low-cost-electrodes).
Use of the WheeStat and low cost electrodes in monitoring airborne hydrogen sulfide is [here](http://publiclab.org/notes/JSummers/03-10-2014/quantifying-airborne-hydrogen-sulfide).
##Setup:
To run the WheeStat, you need to install the appropriate drivers on your computer and have the application file for the GUI installed.
**Drivers:** The WheeStat is based on the Stellaris or Tiva microcontroller development board from Texas Instruments. The first thing you will need to do is download and install drivers from Texas Instruments. Drivers for the In-Circuit-Debug-Interface (ICDI) can be downloaded from this web page found [here](http://www.ti.com/tool/stellaris_icdi_drivers). At the same web page is a link to instructions for installing the drivers on windows machines. I recommend you print out the instructions and have them handy when installing the drivers.
**GUI Application Files** You should be able to get this software from our GitHub page ([here](https://github.com/WheeSci). You will need the application file (.exe) and the folders containing the source code, the libraries, and the data files. These will all need to be in one folder on your computer.
##Source Code:
While the files described above can be used to run the WheeStat, some users may wish to change the functionality of the microcontroller or GUI. In addition, if you are building the potentiostat yourself, you will need to install firmware on your microcontroller board.
**Microcontroller Code:** The firmware was written using the program Energia, which can be downloaded from www.energia.nu. You will need the most recent version of the WheeStat source code and the altSPI library. As of this writing, the most recent version is WheeStat5_4a. You should be able to get this software from our GitHub page ([here](https://github.com/WheeSci) Let me know if you have trouble with this. I am a little slow on updating software.). Once you download the program, you will need to have the altSPI library (altSPI.h and altSPI.cpp files) in a folder called "libraries" inside your sketchbook folder.
**GUI Code:** The Graphic user interface (GUI) was written using a program called Processing that can be downloaded from processing.org. Source code for the GUI can be downloaded from the same GitHub page described above ([here](https://github.com/WheeSci)). As of this writing, the most current version was WheeStat5_4.
##Graphic User Interface:
The following video shows the setup of the GUI and some of it's functionality. It shows the expected behavior of the instrument, tested using a resistor of known value. The demonstration shows that Ohm's Law can be used to predict the current / voltage behavior of the voltage ramp experiment.
##Experiments:
The WheeStat is programmed to run a number of experiments that are useful for a number of tasks. These experiments are accessed by clicking on the "mode" button at the top of the GUI. Below is a quick discussion of what each does and what it is used for.
****Instrument Testing and Calibration:**** The first experiment in the dropdown list is called "ramp". It is a quick experiment that used to test how well the instrument is functioning. To run the experiment, the black lead is attached to one side of a test resistor and the other two leads are attached to the other side, as shown in Figure 1, above. The voltage / time profile is shown in Figure 2, below and the experiment is demonstrated in the video demonstrating the GUI, above. The voltammagram shows the current as a function of applied voltage. If the experiment is working correctly, this should be a linear plot extending through the origin (0 current, 0 mV) with a slope equal to 1/R.
[](https://i.publiclab.org/system/images/photos/000/005/082/original/figure2.png)
****Experiments for Teaching Electrochemistry: 1. Chronoamperometry:**** In single step chronoamperometry, the potential of the working electrode is stepped from its initial value to a final value and the current is sampled as a function of time. Typically, the initial voltage is established where the compound in question is stable and no current passes. The voltage is then stepped to a potential where the compound will either accept or lose an electron to give a second compound. To illustrate, we consider electrochemical response of the hexacyanoferrate ion (FeCN63-). In this experiment, the initial voltage was set to +600 mV, where the iron(III) compound is stable. At time = 0, the voltage was stepped to +100 mV. At this voltage, the iron(II) form of the compound is the stable species and the following half reaction occurs at the working electrode:
FeCN63- + e- <==> FeCN64- (1)
Data from such an experiment employing the iron(III) compound, FeCN63- is presented in Figure 3.
The electrical current passed to the electrode is presented in Figure 3 as a positive current that decays with time. To understand current response using other voltammetric techniques, it is necessary to understand the origin and nature of this decay. Just after the potential step, there is a great excess of the iron(III) compound close to the working electrode, giving rise to a large current. As time evolves, the amount of iron(III) available for reaction diminishes and subsequently, the electrical current decays. The current / time profile in chronoamperometry experiments is governed by the rates at which compounds reach the working electrode. In an unstirred electrolyte solution, the current is determined by the rate at which the compound diffuses. For a planar electrode under these conditions the current is described as a function of time by the Cottrell equation (since I cant figure out how to write equations in this format, click this [link](http://en.wikipedia.org/wiki/Cottrell_equation)).:
Note that all the terms in the Cottrell equation are constant with the exception of the current and the time. Thus, the current is expected to be proportional to one divided by the square root of time. Analysis of data (Presented in Figure 1) shows that this was the case.
**Experiment 1B. Double step chronoamperometry.** Figure 2A shows the time / voltage profile for a double potential step experiment. In this experiment, the voltage is stepped from the initial to the second
****Experiments for Teaching Electrochemistry: 2. Normal pulse voltammetry:**** . A normal pulse voltammetry experiment consists of a series of voltage pulses with varying heights. For our discussion of chronoamperometry, we assumed that the iron(III) form of the compound was the only species stable at the initial voltage and the iron(II) form was the only one stable at the second voltage. At intermediate voltages, however, both oxidation states exist at equilibrium, with their ratio determined by the Nernst equation:
E = E° + RT/nF ln([Fe3+]/[Fe2+]) (3)
Where E is the applied voltage, E° is the standard reduction potential of the couple, R is the ideal gas constant, T is the absolute temperature, n is the number of moles of electrons transferred and F is the Faraday contant. Thus, Equation 3 tells us that the applied potential (E) and the standard reduction potential (E°) determine the position of the equilibrium mixture of oxidized and reduced species. The relationship that the Nernst equation predicts for a Fe3+ / Fe2+ couple with an Eo of +300 mV is presented in Figure 3 . In this figure, the red line represents the percentage of an Fe2+ ion and the blue line represents the percentage of Fe3+. Notice that at a potential of +150 mV, nearly all the compound exists as the reduced, Fe2+ state, at +300 mV (the Eo for the couple) the mixture contains 50% of each, and at +450 mV, nearly all is in the oxidized, Fe3+ state.
[](https://i.publiclab.org/system/images/photos/000/005/085/original/Figure3.png)
If we start a single step chronoamperometry experiment at a voltage where only the iron(III) form is stable and step to a voltage where both the forms coexist, we expect the shape of the current profile to be similar to that in the above case, but at a lower total current, as the electrical current only passes to achieve the equilibrium condition, and not to total reduction of reactant. The normal pulse experiment illustrates how the chosen step potential affects the current profile. In this experiment, a series of voltage steps are generated at incrementing potentials, as shown in Figure 2A. Unlike the case for chronoamperometry, however, the current in normal pulse voltammetry is only sampled once per step, at fixed time after the step is initiated. The current sample times are illustrated as the red circles in Figure 4A. Results of this experiment are plotted as the measured current versus the voltage at which the current was measured. Figure 4B shows a screen shot of normal pulse data obtained using the same solution as that from Figures 1 and 2. Figure 4C shows an analysis of the data from figure 4B. In this figure, original data are presented as open diamonds and the model is shown as a solid blue line. The data were treated by assuming (1) a linear baseline drift (caused by uncompensated solution resistance and double layer capacitance) and (2) that Nernstian conditions were established and maintained for the duration of the pulses. Comparing the predicted and observed results indicated a good fit of the data.
[](https://i.publiclab.org/system/images/photos/000/005/098/original/figure_4.png)
****Experiments for quantifying redox active stuff: Differential Pulse Voltammetry (DPV):**** The problem with normal pulse voltammetry is that it is a very time consuming experiment if done right. This is because it is necessary to establish the initial solution conditions at the working electrode between each voltage step and also because non-Faradaic processes (double layer capacitance and solution resistance) are significant contributors to currents for these large steps. Differential Pulse Voltammetry does not suffer from these problems.
****A variation on the differential pulse theme: Stripping voltammetry**** Anodic stripping voltammetry (ASV) is a technique that can be used at very low concentrations if the product of reduction is not soluble. For example, if you reduce Cu2+ ions to Cu metal, the metal that is deposited on the electrode stays on the electrode. When this is the case, the analyte can be "pre-concentrated" on the electrode, making it easier to detect during a subsequent analysis step. The WheeStat is set up to do ASV using differential pulse voltammetry during this analysis. The difference between the ASV experiment and the DPV experiment
****Experiments for characterizing redox active stuff: Cyclic voltammetry****
The following video demonstrates some of the experiments that the WheeStat is programmed to do: