Question

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?

Answer 1

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

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

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: brainly.com/question/2728613

#SPJ4