Asked by Ali
What is the osmotic pressure in torr of a 0.0155 M glucose solution at body temperature ( 35.7 °C)? What are the boiling and freezing points for the same solution?
Answers
Answered by
DrBob222
pi = MRT
Solve for pi (osmotic pressure) in atm and convert to torr. 760 torr = 1 atm.
If we assume the m = M, then
delta T = Kf*m, solve for dT and subtract from zero to obtain the new freezing point. This won't be exact since m is not quite equal to M but it will be close. There is no density listed; therefore, the assumption must be made.
delta T = Kb*m. Solve for dT and add to 100 to obtain the new boiling point.
Solve for pi (osmotic pressure) in atm and convert to torr. 760 torr = 1 atm.
If we assume the m = M, then
delta T = Kf*m, solve for dT and subtract from zero to obtain the new freezing point. This won't be exact since m is not quite equal to M but it will be close. There is no density listed; therefore, the assumption must be made.
delta T = Kb*m. Solve for dT and add to 100 to obtain the new boiling point.
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.