Why do strong oxidizers and hydroxide not react with each other?

[ShawnD]

Hydroxide is a strong reducing agent, probably the strongest that can exist in water.
Oxyacids without the hydrogen are all strong oxidizing agents, but most oxyacids (all?), without their hydrogen, can be put in a strong hydroxide solution and nothing will happen. Oxidation of organics with potassium permanganate is often done in the presence of a strong base. Potassium nitrate and sodium hydroxide don't seem to react. Sodium hypochlorite is made by bubbling chlorine gas into sodium hydroxide, so obviously hypochlorite does not react with hydroxide, or it does at a rate so slow that it's almost nonexistent.

Shouldn't something happen between oxyacids and hydroxide?

 

[lightarrow]

Hydroxide is a strong reducing agent

?

, probably the strongest that can exist in water.

$$\displaystyle {OH^-}$$

doesn't react with water to give

$$\displaystyle {H_2}$$.

Oxyacids without the hydrogen

What do you mean? Their coniugated base?

are all strong oxidizing agents

Not all.

$$\displaystyle {H_2SO_3, ~H_2CO_3, ~H_3PO_4,~H_3BO_3}$$

are not (for example) and not even their coniugated bases:

$$\displaystyle {HSO_3^-, ~SO_3^{2-},~HCO_3^-,~\displaystyle{ecc.}$$

, but most oxyacids (all?), without their hydrogen, can be put in a strong hydroxide solution and nothing will happen. Oxidation of organics with potassium permanganate is often done in the presence of a strong base. Potassium nitrate and sodium hydroxide don't seem to react. Sodium hypochlorite is made by bubbling chlorine gas into sodium hydroxide, so obviously hypochlorite does not react with hydroxide, or it does at a rate so slow that it's almost nonexistent.
Shouldn't something happen between oxyacids and hydroxide?

Yes, an acid-base reaction