You claim that the formation of, for example, droplets of hydrochloric acid with a concentration of hydrogen ions of 0.15 mol / l is not possible and ask for an explanation. Such a microemulsion can be obtained if strong electrolytes are used as surfactants, that is, those that are not affected by pH.

Thank you for your response Dr. Mirgorod. I need to study the rate constant of oxidation for this complex of cobalt(III) [(NH3)5 Co S2O3]Cl to form [(NH3)5 Co S2O5]Cl inside the reverse micelle at different pHs.

Below pH=1 and also above pH=12 it was fell apart and I couldnt form any reverse micelle. I am looking for a reason. Why it is impossible to form any reverse micelle in this rage of pH?

You yourself write that the complex decomposes in the range of pH = 1-12. And what about reverse micelles? Maybe they do not change. In addition, you do not write about the structure of surfactants that you use. pH can affect amphoteric surfactants, sodium carboxylic acid salts and others.

The complex does not decompose in this pHs, It is possible to prepare the complex in water at pHs below 1 and above 12. But reverse micelle preparation was impossible at very high and very low pHs. I used AOT (Dioctyl sulfosuccinate sodium) and CTAC (Cetyltrimethylammonium chloride) as a surfactant.

Between pH = 1-12 inside the droplets of special water in the reverse micelles your complexes are formed. Below pH =1 and above 12 decompsition of the complex is possible under the action of an excess of protons or decomposition of micelles nder the influence of AOT-

Dioctyl sulfosuccinate - + [(NH3)5 Co S2O3] + = Dioctyl sulfosuccinate [(NH3)5 Co S2O3]

Special water see

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