It is not titration, but you can get an indication of the strength of
the H2O2 solution using Manganese
Dioxide, even the impure stuff from dry cell batteries. You're just
trying to determine if the freezing increased the concentration,
right?
To do so, add a specific quantity of your reference solution to a
test tube. Make a small "cigarette" of the manganese dioxide in
paper and gingerly push-pin it to a one-hole rubber stopper.
Connect the stopper to a hose and the hose into the underside of
an inverted water-filled graduated cylinder. When everything is
tight and snug, rap the test tube until the cigarette falls in the
reference solution.
Record the results, clean up, and repeat the experiment with the
"concentrated" solution. Repeat a few more times to establish a
margin of error.
As long as the temperature and atmospheric pressure remain
relatively constant, the runs have consistent quantities of
Manganese Dioxide and you use an excess compared to the
Peroxide then you should get some decent comparative results.
You could Maths the volume of 02 produced to get a
more quantitative estimate of the concentration, but remember to
attach a healthy margin of error to that. The limitations here are
numerous, off the top of my head: the reaction produces heat.
Oxygen is soluble in the water in the gas trap. The Gas trap will
contained other dissolved gases, errors will occur in repositioning
the gas tube in the trap, etc.)
I was able to purchase Potassium Permanganate from a Well
Drilling company locally for twice the eBay Price. 2 lbs for
$30.00. It is used to regenerate filters that remove iron from well
water.
Cheers,
Greene
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