Log in
Chemistry
1
answer
0
watching
122
views
11 Dec 2019

An isotonic solution of glucose contains 5.31 g of glucose (C6H12O6, Molar Mass = 180.16 g/mol) in 100.0 mL of solution. Imagine this solution is separated from pure water by a semi-permeable membrane. What would the osmotic pressure of the solution be at 293.2 K? Enter your answer in the unit of atmospheres.

Watch
1
answer
0
watching
122
views

For unlimited access to Homework Help, a Homework+ subscription is required.

Tod Thiel
Tod ThielLv2
13 Dec 2019

Unlock all answers

Get 1 free homework help answer.
Already have an account? Log in
Share
discord banner image
Join us on Discord
Chemistry Study Group
Join now

Related textbook solutions

Basic Chemistry
5 Edition,
Timberlake
ISBN: 9780134138046
Principles of Chemistry Molecular Approach
4th Edition,
Tro
ISBN: 9780134112831
Principles of Chemistry Molecular Approach
3rd Edition, 2014
Tro
ISBN: 9780321971944
Chemistry: Structure and Properties
2nd Edition,
Tro
ISBN: 9780134293936
Chemistry: A Molecular Approach
3rd Edition,
Tro
ISBN: 9780321809247
Chemistry: A Molecular Approach
5th Edition,
Tro
ISBN: 9780134874371
Principles of Chemistry: A Molecular Approach
4th Edition,
Tro
ISBN: 9780134895741
Chemistry: The Central Science
14th Edition, 2017
Brown
ISBN: 9780134414232

Related questions

Part #1:

Imagine a red blood cell with a low concentration (~0.9%) of solutes dissolved in the water in the cell. The cell membrane acts as a semi-permeable membrane. If this cell is placed in brine (a highly concentrated solution of sodium chloride) which describes what will occur?

A Nothing will occur

B Sodium chloride will flow from the cell into the brine

C Water will flow from the brine into the cell

D Sodium chloride will flow from the brine into the cell

E Water will flow from the cell into the brine

Part #2:

An isotonic solution of glucose contains 4.82 g of glucose (C6H12O6, Molar Mass = 180.16 g/mol) in 100.0 mL of solution. Imagine this solution is separated from pure water by a semi-permeable membrane. What would the osmotic pressure of the solution be at 297.0 K? Enter your answer in the unit of atmospheres.

Part #1:

30.0 g of glucose (C6H12O6, molar mass = 180.16 g/mol) are dissolved in 100. grams of water (molar mass 18.02). What is the mole fraction of water in solution? Note: glucose is a non-volatile solute.

Part #2:

At 25.0 oC, pure water has a vapor pressure of 24.2 torr. What would the vapor pressure of the solution in part one be (in torr)?

Part #3:

A liquid is a mixture of benzene and toluene. The sample contains 0.225 moles of benzene and 0.775 moles of toluene. At a given temperature, pure benzene has a vapor pressure of 38.02 torr, while pure toluene has a vapor pressure of 8.73 torr. What is the total combined vapor pressure of the two liquids (in torr?)?

A solution of glucose (C6H12O6) is prepared by dissolving 100.0 g of glucose in 1000. g of water. The density of the resultant solution is 1.050 g/mL. Kb for water is 0.52 oC/m and kf for water is รขย€ย“1.86 oC/m.

What is the vapor pressure of the solution at 100.0oC?

What is the boiling point of the solution?

please i really need a clear explanation for this

What is the osmotic pressure of the solution at 25oC?

Weekly leaderboard

Home
Homework Help 3,900,000
Chemistry 830,000
Start filling in the gaps now
Log in