Asked by Sam
What volume of 1.20 M nitric acid is needed to convert 5.5g of m-chlorophenol to 3-chloro-2,6-dinitrophenol?
I So far I have converted the 5.5g chlorophenol to mols and I got .043 mol. I know Volume * Molarity (1.2M)=moles. At this point I am stuck.
I So far I have converted the 5.5g chlorophenol to mols and I got .043 mol. I know Volume * Molarity (1.2M)=moles. At this point I am stuck.
Answers
Answered by
drwls
Writing the real subject title will usually get you answers sooner.
Answered by
DrBob222
Using the coefficients in the balanced equation, convert mols chlorophenol to mols of HNO3 need to make the product. Then you know M = moles/L; L is the only unknown.
DrWLS is right. I wouldn't click on ORGO but if you wrote chemistry there for the subject you would have obtained a quicker answer.
DrWLS is right. I wouldn't click on ORGO but if you wrote chemistry there for the subject you would have obtained a quicker answer.
Answered by
Sam
Thank you I was able to work it out:
it's a 1:1 ratio so since 5.5g chlorophenol is .043 mols, nitric acid must be .043 mols as well.
V(1.20M) = .043mol
V= .036L
it's a 1:1 ratio so since 5.5g chlorophenol is .043 mols, nitric acid must be .043 mols as well.
V(1.20M) = .043mol
V= .036L
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