With my DIY potentiostat/galvanostat, I can perform many types of experiments. One of the most useful – especially for its link to battery chemistry – is the cyclic voltammetry (CV). In a CV experiment, the potential between a working and reference electrode is changed within a range and the current at each potential measured. The shape of the plot measured, gives important information about the chemistry in the solution. You can tell if anything is oxidized or reduced, at which potentials these processes happen and you can also get an idea about the reversibility of the reactions taking place.

A CV setup has several components. The experiment is carried out in an electrochemical cell, which is a glass vessel that can hold all of the electrodes in place, without any risk of the electrodes ever touching each other and causing a short. Although such setups can be built at home, relatively low cost high quality solutions are indeed available.

The cell has a three electrode setup. The first is the working electrode (WE) which is the electrode where the relevant electrochemical processes will happen. This electrode is usually made of an inert material – glassy carbon, platinum and gold are most common – with a high polish and a limited surface area. This is because we want the surface of the electrode to be reproducible and to always provide us with the same measurements.

The reference electrode (RE) provides us with a potential based on a chemical reaction that is always happening at a very defined potential. For best results, these are usually 1 electron reactions that happen at a very small scale – which means a current draw below pico amps – and normally involve an equilibrium with an insoluble solid. Popular choices are calomel and Ag/AgCl electrodes.

Finally the counter electrode (CE) is the electrode that is connected to ground and has a polarity opposite to that of the working electrode. It is meant to complete the circuit. This is generally made of an inert material and should have a very high surface area compared with the WE, such that reactions are never limited by it. Popular material choices are graphite rods and palladium and platinum wires.

Although the above might all sound complex and expensive – I got quotes of over 1000 EUR for the above with some EU supplier companies – I was able to find everything on ebay for relatively low prices from Chinese suppliers:

• High purity graphite rod CE (3mmx95mm)
• Professional 112 Type silver chloride reference electrode (Ag/AgCl)
• Sealed electrolytic cell (C001)
• Glassy carbon WE (3mm)

The total price for the entire setup including shipping – not counting the DIY potentiostat – was around 162 USD. I am very satisfied with the quality of all the components that I have received. I have also successfully performed my first CV experiment (showed above).

My first idea with this CV setup is to explore manganese chemistry and measure the reversibility of Mn²⁺ oxidation reactions in concentrated sulfuric acid solutions. Highly reversible Mn⁺²/M⁺³ reactions are very important for Mn based flow batteries.

I’ve done a lot of experiments during the last two years around the construction of Zinc halide batteries, in particular, Zn-Br and Zn-I batteries. So far, I have been unable to find a battery setup that provides high energy and coulombic efficiencies, high capacity and high stability.

Zinc-Bromine batteries suffers from problems related with Br₂ diffusion, zinc dendrites, hydrogen evolution and other problems that arise when you try to resolve these issues. Trying to add complexing agents, increase electrode distance or add physical barriers, will often increase coulombic efficiency at the expense of energy efficiency, such that batteries with low self-discharge or high capacity will tend to have extremely low energy efficiency values (often below 20%). Having a battery where you need to put 20kWh in to take 2kWh out is just not a viable strategy for most people. Hydrogen evolution reactions are also inevitable with Zn-Br batteries, and these irreversibly destroy the electrolyte as a function of time.

Zn-Br batteries might be easy to show in online videos and tout as a great chemistry with lots of possibilities, but the reality of constructing a >60Wh/L static Zn-Br battery with a long cycle life shows that this is extremely hard to achieve. This is why you will find no one showing proper testing – charge/discharge curves with CE and EE numbers for many cycles – of such DIY static batteries. You can read other posts in my blog and this forum thread, for more information about my journey in Zn-Br batteries.

The above were the reasons why – after doing a lot of experiments to get to know these batteries quantitatively – I decided to move to the Zinc-Iodine chemistry.

Zinc-Iodine batteries do not suffer from hydrogen evolution issues – due to the lower potential needed to charge the battery – but they also have strong problems dealing with I₂ migration, especially due to the very iodide rich electrolyte, which generated a lot of readily soluble triiodide (I₃^–). Although many solutions to these problems have been tried and published in peer reviewed journals, most are extremely hard to apply in practice and out of reach for someone with limited equipment and resources.

However, there is some hope. A paper published in 2019 got around the problem of the triiodide ion by using a “water in salt” approach (WiS). That is, they create a very highly concentrated solution of zinc chloride and potassium iodide, where water is a very minor component by mass. In this case, they add around 2g of ZnCl₂ and 0.8g of KI to only 1mL of distilled water. In such a concentrated salt solution, iodide prefers to bond to Zn to form complexes, as the formation of the triiodide ions is strongly disfavored by the environment. This is proven extensively in the paper by the use of Raman spectroscopy, supported by computational chemistry calculations.

Thankfully, both ZnCl₂ and KI are readily available chemicals plus, the electrode and separator material used by the researchers are also easy to get. The cathode is made out of carbon paper, the anode is zinc metal and the separator is cellulose filter paper. I purchased the salts for around 4 USD/kg (ZnCl₂) and 40 USD/kg (KI).

Note that ZnCl₂ is extremely hygroscopic, so it needs to be kept under airtight conditions. Solutions of ZnCl₂ are also extremely acidic (pH < 1) so you need to be very careful when handling ZnCl₂ solutions that are this concentrated. Zinc chloride also heats solutions aggressively when dissolved.

The results of trying to reproduce their research were quite astonishing. I prepared the electrolyte as published and used my Swagelok cell for testing. I used a Whatman 42 filter paper as separator and an HCB-1071 carbon cloth as cathode (note the variety kit has the 15mil, which is the one I used). For the anode, I used the surface of the graphite electrode of my Swagelok cell. In total, the thickness of my battery was just 350 microns (0.0350cm).

The above image shows you the results from the first charge/discharge cycle of this device. The capacity in this first cycle was 1.77mAh. Given the volume of this battery, the energy density is currently at 58Wh/L, the best energy density I have been able to create for any device.

I am now going to study the cycling characteristics of these devices further. I want to determine how the CE and EE change as a function of time and how the capacity changes as well. Taking this device apart confirms that elemental iodine is deposited on the carbon cloth and no appreciable triiodide – which has an orange color – is formed. This is also confirmed by the massive jump in CE and EE in these devices.

The above chemistry finally points to a path for a DIY battery that can be easy to build with readily available chemicals and materials. My hope is that this can lead to practical capacities in the >50Wh/L, with reasonable costs and hopefully low self-discharge and a long cycle life.