I am studying the reaction of dissolved dioxygen with manganese(II) hydroxide for the Winkler method:


The data I have been given is Mn(OH)2's pKs=12.7, as well as the standard potential for MnO2(s)/Mn(OH)2(s), which is 1.23V, and the one of O2/H2O, which is also 1.23V; nothing more. Using Gibbs free energy for each half reaction, I have managed to calculate the quilibrium constant for the reaction at 298K, which I found to be 10^-25.4, making it dramatically unfavorable to products.

Does anyone find the same thing for this constant, or have I made a mistake? If it is the right constant, how come the reaction takes place?

I am aware that it is not the commonly used reaction when it comes to the Winkler method, but its the only one I can propose when it comes to having the dioxygen react with manganese hydroxide owing to what few data I have. Also sorry for my shaky English, I'm french.

Thanks in advance for your answers!


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