[Guillem_dlc]

I have the solution of the redox adjustment of this equation, but why is it a basic medium?

KAsO₂+KMnO₄  AsO₃K+MnO₂

Thanks

[Borek]

I am not sot sure what your question is - what is a "basic medium" here?

Were you asked to balance the reaction assuming a high pH? Then just do so.

[chenbeier]

If you get MnO₂ as a product in a redoxreaction the enviorment is alcaline. If it is acidic normaly you get Mn²⁺. So develop the reaction by using water and Hydroxide.

[Borek]

If you get MnO₂ as a product in a redoxreaction the enviorment is alcaline.

Closer to neutral, in really alkaline solution permanganate gets reduced to MnO₄^2-.

Trick is, OP already listed MnO₂ as a product, so predicting the product was not part of the problem.

[chenbeier]

Thats true, depending on pH. Manganate Is devleoped at pH12-14, if its below 12 to neutral 7 MnO2 is developed.

I also dont think MnO2 is the problem. The hint is to develop a redox reaction in more alcaline envirement.

[Guillem_dlc]

I am not sot sure what your question is - what is a "basic medium" here?

Were you asked to balance the reaction assuming a high pH? Then just do so.

We have been taught to adjust reactions as they take place in an acidic or basic environment in one way or another. As I should do here if the problem does not specify in what way the reaction takes place.

Thanks

[chenbeier]

Read everything again. If you see MnO₂ then develop the equation in alcaline condition.