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A solution containing 26.40 mg of an unknown protein per 22.5 mL solution was found to have an osmotic pressure of 3.95 torr at...Asked by M
A solution containing 26.05 mg of an unknown protein per 23.5 mL solution was found to have an osmotic pressure of 3.75 torr at 44 C.
What is the molar mass of the protein?
What is the molar mass of the protein?
Answers
Answered by
DrBob222
pi=MRT
You know pi (osmotic pressure. I would convert that to atmospheres (3.75/760 = ?? although 3.75 atm sounds more like an osmotic pressure).Solve for M = molarity.
Then M = moles/L. You know M and L, calculate moles, then use moles = grams/molar mass. Knowing M and grams, calculate molar mass.
You know pi (osmotic pressure. I would convert that to atmospheres (3.75/760 = ?? although 3.75 atm sounds more like an osmotic pressure).Solve for M = molarity.
Then M = moles/L. You know M and L, calculate moles, then use moles = grams/molar mass. Knowing M and grams, calculate molar mass.
Answered by
Emmi
I don't understand how you get the M. I know that M = moles/L, but the problem gives mg and ml so how do we find the molarity?
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