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The active agent in many hair bleaches is hydrogen peroxide. The amount of H₂O₂ in 14.8 g of hair bleach was determined by titration with a standard potassium permanganate solution:
2MnO⁻₄ + 5H₂O₂(aq) + 6H⁺(aq) → 5O₂(g) + 2Mn²⁺(aq) + 8H₂O(l)
(b) How many moles of H₂O₂ were present in the 14.8-g sample of bleach?

Respuesta :

The 14.8-g bleach sample contained 0.113 moles of H₂O₂.

[tex]\frac{43.2 ml of MnO_{4} ^{-} }{1}[/tex] X [tex]\frac{0.105 m dos MnO^{-} _{4} }{1000 ml MnO^{-}_{4} }[/tex] X [tex]\frac{5 mol H_{2} O_{2} }{2 mol MnO^{-}_{4} }[/tex] = 0.113 moles of [tex]H_{2} O_{2}[/tex]

This is an example of the oxidation-reduction chemical reaction, which moves electrons from one species to another. The oxidation states of our species were thus altered as a result of the transfer of electrons. As we are concentrating on it in this case, the hydrogen peroxide we have weighs 14.8 g and was measured with accuracy. 0.113 moles are in question.

What is titration used for and what does it entail?

A titration can be used to figure out the concentration of an unknown solution by comparing it to one with a known concentration. Until the reaction is finished, the titrant (the known solution) is typically added from a buret to a known volume of the analyte (the unknown solution).

Learn more about titration: https://brainly.com/question/2728613

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