The final molarity of H₂O₂ is 0.135 if 1.4 ml of the 3.0% w/w H₂O₂ solution is diluted with 3.6 ml water, then added to 5.0 ml of a starch-iodide solution.
A amount of a substance in a specific volume of solution is known as its molarity (M). The amount of moles of the a solute per litre of a solution is known as molarity. The molecular concentration of a solution is another name for molarity.
Generally the equation for the 3% mass is mathematically given as
Let 3% mass H₂O₂ be
Therefore
3% = solute mass/1.4ml * 3.6g/ml * 1000
Solute mass = X
X = 0.1512
M=moles of H₂O₂ = 0.1512/39
moles of H₂O₂ = 0.0038 = 3.8 * 10⁻³
M = 3.8 * 10⁻³/1.4 * 5.0 *10⁻³
M =0.135
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