14. Solutions

Osmosis

What is Osmotic Pressure |  Extraclass.com

Osmosis Concept 3

water will flow from solution A to solution B due to higher osmotic pressure on the solution B.

water will flow from solution A to solution B due to lower osmotic pressure on solution B.

water will flow from solution B to solution A due to lower osmotic pressure on solution B.

water will flow from solution B to solution A due to lower osmotic pressure on solution A.

water will not flow because both solutions have the same osmotic pressures.

Identify the direction of water flow between 2 solutions separates by semipermeable membrane, where &nbsp;are the solute particles.<img src="https://static.studychannel.pearsonprd.tech/courses/general-chemistry/thumbnails/images/16202c8a"class="fr-fic fr-dii">

Osmosis Example 1

13 - Solutions and Colligative Properties

Four U tubes each have distilled water in the right arm, a solution in the left arm, and a semipermeable membrane between the arms. If the solute is LiF, which solution is most concentrated?<img src="https://static.studychannel.pearsonprd.tech/courses/general-chemistry/thumbnails/images/3e511daf"class="fr-fic fr-dii">

What is Osmosis? - Part 1 | Cell | Don't Memorise

Suppose you had a balloon made of some highly flexible
semipermeable membrane. The balloon is filled completely
with a 0.2 M solution of some solute and is submerged in a
0.1 M solution of the same solute:
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/fa02f4a9302cfba6-1666020240455.jpg" alt="" />
Initially, the volume of solution in the balloon is 0.25 L. Assuming the volume outside the semipermeable membrane 
is large, as the illustration shows, what would you expect for 
the solution volume inside the balloon once the system has 
come to equilibrium through osmosis? [Section 13.5]

Osmosis Concept 1

A semipermeable membrane is placed between the following solutions.<img src="https://static.studychannel.pearsonprd.tech/courses/general-chemistry/thumbnails/images/6b726a65"class="fr-fic fr-dii">Which solution will increase in volume?

45: Colligative property: Osmotic pressure

Osmosis Concept 2

Osmosis Example 2

 The total molality of particles (ions or molecules) in the solution determines the change in boiling point. 

0.150 m C6H12O6

0.050 m Al(NO3)3

Correct, the total molality of ions is 0.200 m

 Colligative properties, such as boiling point depend on the number of particles produced by the solute. 

 Which of the following aqueous solutions would have the highest boiling point? 

Important Concepts of Osmosis : Chemistry Lessons

A solution with the same osmotic pressure as the blood is

If the fluid surrounding a patient’s red blood cells is depleted in electrolytes, is crenation or hemolysis more likely to occur?

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1. Intro to General Chemistry

2. Atoms & Elements

3. Chemical Reactions

4. BONUS: Lab Techniques and Procedures

5. BONUS: Mathematical Operations and Functions

6. Chemical Quantities & Aqueous Reactions

7. Gases

8. Thermochemistry

9. Quantum Mechanics

10. Periodic Properties of the Elements

11. Bonding & Molecular Structure

12. Molecular Shapes & Valence Bond Theory

13. Liquids, Solids & Intermolecular Forces

15. Chemical Kinetics

16. Chemical Equilibrium

17. Acid and Base Equilibrium

18. Aqueous Equilibrium

19. Chemical Thermodynamics

20. Electrochemistry

21. Nuclear Chemistry

22. Organic Chemistry

23. Chemistry of the Nonmetals

24. Transition Metals and Coordination Compounds

[BOOK CHEM] Clutch Version

Types of Aqueous Solutions

When an ionic solid dissolves, ions leave the solid and become dispersed in the solvent. Three possible aqueous solutions can be formed:saturated, unsaturated and supersaturated.

Boiling Point Elevation

Boiling Point Elevation is the phenomenon when adding a solute to a pure solvent results in increased boiling point of the solvent.

Intro to Henry's Law

According to&nbsp;Henry's Law, at a constant temperature the amount of a gas dissolved in a solvent is directly proportional to its partial pressure when it is in equilibrium with its liquid phase.&nbsp;

Osmotic Pressure

Osmotic Pressure is the force that drives Osmosis from higher concentration to lower concentration.

Mole Fraction

Mole Fraction (X) relates the moles of solute and solvent within a solution.&nbsp;

The Colligative Properties

The&nbsp;Colligative Properties&nbsp;explain what happens to a pure solvent as it transitions to a solution.

Molality

Molality (m)&nbsp;represents the number of moles of solute dissolved per kilogram of solvent.&nbsp;

Freezing Point Depression

Freezing Point Depression is the phenomenon when adding a solute to a pure solvent results in decreased freezing point of the solvent.

Solutions: Solubility and Intermolecular Forces

Solutions are homogeneous mixtures that result from the dissolving of a solute by a solvent.

Vapor Pressure Lowering (Raoult's Law)

Vapor Pressure is the pressure exerted by a gas at equilibrium with its liquid phase at a specific temperature in a closed system.

Henry's Law Calculations

To calculate solubility of a dissolves gas, Henry's Law Constant and partial pressure are used.

Solutions: Mass Percent

Mass Percent represents grams of solute per grams of solution, multiplied by 100.

Osmosis is the net movement of solvent across a semipermeable membrane.

Parts per Million (ppm)

<div dir="auto"><div contenteditable="true"dir="auto"spellcheck="true">Parts per Million (ppm) and Parts per Billion (ppb) are used to express extremely dilute solution concentrations.</div></div>

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