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Calculate the final molarity of H2O2 if 5.5 mL of a 3.0% w/w H2O2 solution, which has a density of 1.0 g/mL, is added to 5.5 mL of a starch-iodide solution.​

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okpalawalter8

We have that the final molarity of H2O2 if 5.5 mL of a 3.0% w/w H2O2 solution, which has a density of 1.0 g/mL, is added to 5.5 mL of a starch-iodide solution.​ is

[tex]M=0.441[/tex]

From the question we are told

Calculate the final molarity of H2O2 if 5.5 mL of a 3.0% w/w H2O2 solution, which has a density of 1.0 g/mL, is added to 5.5 mL of a starch-iodide solution.

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Generally the equation for the 3\% mass  is mathematically given as

Let 3\% mass H2O2 be Hm

Therefore

[tex]3\%=\frac{Solute mass}{5.5ml*1g/ml}*1000\\\\Solute mass =X[/tex]

[tex]X=0.165g[/tex]

Generally the equation for the Molarity  is mathematically given as

[tex]M=\frac{moles of H_2O_2}{V}[/tex]

Where

[tex]moles of H_2O_2=\frac{0.165}{39}\\\\moles of H_2O_2=4.2*10^{-3}[/tex]

Therefore

[tex]M=\frac{4.2*10^{-3}}{5.5*5.5*10^{-3}}[/tex]

[tex]M=0.441[/tex]

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