Electrochemistry

Different metals have different reactivity and standard electrode potentials. Choose zinc, iron or carbon electrodes based on the specific reaction or cell your practical requires.

A U-tube setup suits electrolysis of a single solution, while a galvanic cell needs two separate electrode-electrolyte combinations connected by a circuit, sometimes with a salt bridge.

Carbon electrodes resist corrosion well and suit repeated use across many practicals, while reactive metal electrodes like zinc may need replacing more often as they oxidise.

A single demonstration set suits teacher-led lessons, but hands-on electrochemistry practicals need enough electrodes and glassware for every group to run the experiment themselves.

Zinc and iron are reactive metals that readily oxidise, useful for demonstrating corrosion and galvanic cells. Carbon electrodes are inert, meaning they don't react themselves, making them ideal for general-purpose electrolysis where you want to study the solution's reaction rather than the electrode.

A basic electrolysis setup needs a container for the electrolyte solution (such as a glass U-tube), two electrodes, connecting wires, and a power source such as a battery.

A galvanic cell uses the natural difference in reactivity between two metal electrodes in an electrolyte. As one metal oxidises and the other is reduced, electrons flow through the connecting wire, generating a measurable voltage.

The electrode material determines what metal gets deposited during electroplating. A copper electrode in a copper sulfate solution, for example, deposits a layer of copper onto the object being plated.

Yes. We regularly supply schools with class sets of electrodes and electrolysis apparatus. Contact us for a quote on bulk quantities for a full classroom or department.