Question

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.​

Answer 1

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

$M=0.441$

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

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

$X=0.165g$

Generally the equation for the Molarity  is mathematically given as

$M=\frac{moles of H_2O_2}{V}$

Where

$moles of H_2O_2=\frac{0.165}{39}\\\\moles of H_2O_2=4.2*10^{-3}$

Therefore

$M=\frac{4.2*10^{-3}}{5.5*5.5*10^{-3}}$

$M=0.441$

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