Asked by CodyJinks
If exactly 14.563g of KMnO4 were dissolved to yield 750mL of solution, what is the normality? I know the equivalent weight is 31.61g. This is how much I got.
(14.563g/.750L)(1 mol KMnO4/158.03g)(5 e-/1 mol) = .615 This answer does not seem right however. If wrong, please explain
(14.563g/.750L)(1 mol KMnO4/158.03g)(5 e-/1 mol) = .615 This answer does not seem right however. If wrong, please explain
Answers
Answered by
bobpursley
The conversion for potassium permanganate, KMnO4, from Normality to Molarity is 1N = 0.2M or 1M = 5N.
Molarity= 14.563/158*.750
now, normality = 5 * molarity above
You are correct.
Molarity= 14.563/158*.750
now, normality = 5 * molarity above
You are correct.
Answered by
CodyJinks
Okay thank you Bob
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.