To prepare 500 micromoles of H2O2 from 6% hydrogen peroxide, you will need to make a dilution of the stock solution. Here's how you can calculate the amount of stock solution and the diluent needed:
0.5 mmol x (34.01 g/mol) = 17.005 g of H2O2
To calculate the volume of 6% hydrogen peroxide needed, use the formula:
(Volume of 6% H2O2) x (6 g/100 mL) = 17.005 g
Volume of 6% H2O2 = (17.005 g) / (6 g/100 mL) = 283.42 mL
Diluent = 500 mL - 283.42 mL = 216.58 mL
Therefore, to prepare 500 micromoles of H2O2 from 6% hydrogen peroxide, you will need to dilute 283.42 mL of the stock solution with 216.58 mL of diluent.
As for the choice of reducing agent, both ascorbic acid and hydrogen peroxide can be used to reduce hydrogen peroxide to water and oxygen. However, ascorbic acid is often preferred because it is a mild reducing agent that does not produce reactive intermediates that can damage biological samples. In addition, ascorbic acid is readily available, inexpensive, and easy to use.
Hello,
How will I calculate?
First of all I need to know the molarity of my H2O2 solution. For this I will need the density of H2O2 which is 1.11kg/L or 1111 g/L. this means that m = 1111* 0.06 (6%) = 66.66 g in 1 liter of solution.
n = m/M. M of H2O2= 34.01g/mol so n = 66.66/34.01 = 1.96 mol/L....
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