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Hydrogen Peroxide + NaHSO4 (aq) -> ?

ercdndrs
in Inorganic Chemistry

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Hi, I have some 3% hydrogen peroxide (H2O2) and I'd like to concentrate it to a more useful concentration. Right now I'm thinking of boiling off the extra water. I've read that at high concentrations of H2O2 decompose extremely exothermically when they're heated (resulting in a steam and very hot O2 explosion), and I've also heard that the peroxide is stabilised somewhat in an acidic environment. My three questions are:

 

-What is a safe concentration to boil the peroxide to?

 

-How will an acid affect the stability of the peroxide?

 

-The only pure acid I have around is sodium bisulphate (NaHSO4). However, when I mix the peroxide and acid, I see bubbles. Do hydrogen peroxide and sodium bisulphate react, and what is the equation?

 

- Does the acid serve to decompose the peroxide?

 

2 H2O2 + NaHSO4 (aq) -> NaHSO4 + 2 H2O + O2

 

- Or, does it produce sulphur dioxide gas and oxygen gas?

 

H2O2 + 2 NaHSO4 (aq) -> Na2SO4 + 2 H2O + O2 + SO2

 

 

Thanks for the help :)

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