The thickness is a matter of exposure time and bleach concentration and whatever surface active compounds are also present in the bleach. Frankly, you would need to evaluate the thickness of the layer on a case-by-case basis.

Assuming that you want to produce such electrodes for electrochemical application, you should have some kind of stabilised voltage source and the ability to measure current (e.g. using a potentiostat/galvanostat). In that case, it would be far simpler and more accurate in terms of layer thickness (easy to calculate from Faraday's law) to electrochemically generate AgCl by oxidising the silver electrode in saline.

I would expect the reaction to be self-limiting, as AgCl has a specific volume roughly two times larger than silver (density of Ag is approx. 10 g/cm3, density of AgCl is approx 5.5g/cm3). This, the precipitating AgCl will tightly cover the surface of the electrode and act as ain insulating layer. As such, a limited AgCl layer thickness should be achievable at a given applied potential (or a given redox potential of the oxidising agent in your bleach).

Dear Afiq ,

domestic HOCl is highly alkaline, pH>11, so you will probably first form Ag2O (solubility in water 0.025 g/L ) which will dissociate and form low soluble AgCl on the bottom of the beaker. HOCl is also strong corrosion oxidizing species, and on the end you will completely dissolve your silver electrode via corrosion. If you need AgCl for reference electrode it is better to use electrochemical method of oxidizing silver in HCl.

Gretings