Redox titrations are used to determine the amounts of oxidizing and reducing agents in solution. For example, a solution of hydr
ogen peroxide, H2O2, can be titrated against a solution of potassium permanganate, KMnO4. The following equation represents the reaction: 2 KMnO4 (aq) + H2O2 (aq) + 3 H2SO4 (aq) → 3 O2 (g) + 2 MnSO4 (aq) + K2SO4 (aq) + 4 H2O (l) A certain amount of hydrogen peroxide was dissolved in 100. mL of water and then titrated with 1.66 M KMnO4. What mass of H2O2 was dissolved if the titration required 13.2 mL of the KMnO4 solution?
1 answer:
Answer:
0.374 g
Explanation:
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Since both the molarity and the volume allows us to know the moles of potassium permanganate, and we already have the balanced chemical reaction, the stoichiometric procedure that is attached in the picture, is developed to substantiate the the titrated mass of hydrogen peroxide was 0.374 g.
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Answer:
Explanation:
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In this case, according to the given information, it turns out necessary for us remember that the first-order kinetics is given by:
Whereas the 27.5% complete means A/Ao=0.275, and thus, we solve for the rate constant as follows:
Then, we plug in the variables to obtain:
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