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vredina [299]
3 years ago
14

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.​
Chemistry
1 answer:
horsena [70]3 years ago
5 0

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.

​

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

For more information on this visit

brainly.com/question/1689737  

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