Colligative Properties. Properties where how much solute dissolved matters not what is being dissolved. Ex: Osmosis.

Slides:

Advertisements

Similar presentations

IV. Colligative Properties of Solutions (p. 498 – 504)

Advertisements

Ch. 14: Mixtures & Solutions

Chapter 13 Preview Multiple Choice Short Answer

A positive attitude may not solve all your problems, but it will annoy enough people to make it worth the effort. Herm AlbrightHerm Albright ( )

Physical Properties of Solutions Chapter 12 Copyright © The McGraw-Hill Companies, Inc. Permission required for reproduction or display.

Colligative Properties Honors Chemistry Unit 8 Chapter 15.

Colligative Properties (solutions)

Colligative Properties of Solutions. All pure liquids have a normal freezing point. However, impure liquids (liquid solutions) always freeze at a LOWER.

Physical Properties of Solutions Unit 10 Why are some compounds more effective in melting ice than others?

Molality (these calculations are not in your book) (these calculations are not in your book) Molality is said molal and is represented by a lower case.

Colligative Properties of Solutions Colligative properties = physical properties of solutions that depend on the # of particles dissolved, not the kind.

Part 2: External Control of Solubility Temperature and Pressure Predictions: Will solubility increase or decrease with increasing temperature? Will solubility.

Concentration Units Molarity Molality Mole Fraction Weight Percent ppm ppb.

Colligative Properties of Solutions Chemistry Mrs. Coyle.

Changing Molarity to Molality

Colligative Properties Colligative properties depend only on the number of solute particles present, not on the identity of the solute particles. Among.

Why does acetone dissolve Styrofoam? 1/ both are nonpolar: “Like (nonpolar) dissolves like (nonpolar)”. 2/ Styrofoam is mostly air. acetone.

III. Particles in Solution

Ch Solutions I. How Solutions Form  Definitions  Types of Solutions  Dissolving  Rate of Dissolving.

Colligative Properties. Definition Properties that depend on the concentration of a solution no matter what the solute’s identity is.

1 Colligative Properties of Solutions Colligative properties are properties that depend only on the number of solute particles in solution and not on the.

Concentration Units Continued M = moles of solute liters of solution Molarity (M) Molality (m) m = moles of solute mass of solvent (kg) 12.3.

Colligative properties

III. Colligative Properties (p )

II III I IV. Colligative Properties of Solutions (p. 498 – 504) Ch. 14 – Mixtures & Solutions.

II III I C. Johannesson III. Colligative Properties (p ) Ch. 13 & 14 - Solutions.

Topic: Colligative Properties. Adding a non-volatile (doesn’t readily evaporate) solute affects… Conductivity (electrolytes) Freezing point Boiling point.

Colligative Properties Physical properties affected by dissolved solute particles Type of solute doesn’t matter. Number of particles does matter. Colligative.

Colligative Properties. Colligative properties Properties that depend on the TOTAL number of dissolved particles.

Colligative Properties of Solutions Chemistry Honors.

Solutions. Definitions Solution – Homogeneous mixture of two or more substances Solute – Substance that is dissolved Solvent – Substance that dissolves.

1 Solutions Why does a raw egg swell or shrink when placed in different solutions?

1.  Temperature  You can dissolve more into a warm liquid than you can into a cold liquid 2.

1 Terms Soluble Insoluble Saturated solution Unsaturated solution Supersaturated solution Concentration Molarity Dilution.

folder/flashfiles/propOfSoln/colligative.html.

II III I Colligative Properties. A. Definition  Colligative Property property that depends on the concentration of solute particles, not their identity.

III. Colligative Properties

Chapter 21 Colligative Properties: Part 2. Colligative Properties Properties determined by the number of solute particles in solution rather than the.

Chem-To-Go Lesson 37 Unit 9 COLLIGATIVE PROPERTIES.

Colligative Properties Chemistry GT 5/11/15. Drill List the four colligative properties. Give a real world example of each. What is the molality of a.

Bell Work: Colligative Properties 1.Vapor pressure goes ( up / down) with more solute added. 2.Vapor pressure is closely related to ( freezing / boiling.

Colligative Properties Colligative properties refers to properties of a solution that depend on the concentration of particles. Vapor pressure Boiling.

Calculations Involving Colligative Properties. Objectives When you complete this presentation, you will be able to o calculate the molality of a solution.

Colligative Properties. ____________ – physical properties of solutions that are affected only by the number of particles NOT the identity of the solute.

Physical Properties of Solutions Chapter 12. Objectives 1.0 Define key terms and concepts. 1.8 Explain how a solute and solvent interact to make a solution.

© 2009, Prentice-Hall, Inc. Colligative Properties Changes in colligative properties depend only on the number of solute particles present, not on the.

Solution: a homogeneous mixture of two or more substances Solution: a homogeneous mixture of two or more substances Solute: substance that is dissolved.

Name __________________________ Block_____ Chapter 17 Solutions and Molarity Some Definitions A solution is a homogeneous mixture of 2 or more substances.

Colligative Properties of Solutions Ch Definition of Colligative Properties The physical properties of solutions that are affected by the number.

1 Solutions Chapter Some Definitions A solution is a homogeneous mixture of 2 or more substances in a single phase. One constituent is usually regarded.

Solutions-3 Colligative Properties. When a solute is added to a solvent, particles get in the way of crystal formation. Freezing requires lower temperature.

Colligative Properties

Do Now: What are the units for molarity?

V. Colligative Properties

Properties of Solutions

Colligative Properties

Solutions of Electrolytes

Colligative Properties

III. Colligative Properties

Colligative Properties

Colligative Properties

Colligative Properties

Solutions Particles in Solution “Like Dissolves Like” Electrolytes

Colligative Properties

III. Colligative Properties (p )

III. Particles in Solution

Colligative Properties of Solutions

Solutions Particles in Solution “Like Dissolves Like” Electrolytes

Solutions Part II.

Aim: How does the addition of a solute affect the colligative properties of the solvent? Do Now: In pairs compare answers to HW.

Presentation transcript:

Colligative Properties

Properties where how much solute dissolved matters not what is being dissolved. Ex: Osmosis

Colligative Properties Boiling Point Elevation Ex: coolant/ethylene glycol – Lowers the boiling point of water Boiling point elevation ∆T = k b m

Colligative Properties Boiling point elevation ∆T = k b m What is the boiling point of 50. g of ethylene glycol in 50. g of water?

Colligative Properties Freezing Point Depression Ex: salt on ice – This melts ice by lowering the freezing point of the water Ex: Antifreeze/ethylene glycol Freezing point depression ∆T = k f m

Colligative Properties Freezing point depression ∆T = k f m What is the freezing point of 25 g of glucose, C 6 H 12 O 6, in 75 g of ethanol?

Colligative Properties This works well for nonelectrolytes This a problem for electrolytes Electrolytes (ionic compounds and acids) break into ions in water. Remember the definition of a colligative property – It doesn’t matter what is dissolved just how much

Colligative Properties NaCl  Na + + Cl - 1 m of NaCl is really 1 m of Na + and 1 m Cl - giving a total of 2 m K 3 PO 4  3K + + PO m of K 3 PO 4 is really.75 m of K + and.25 PO 4 -3 giving a total of 1.0 m

Colligative Properties For the following solutions what is the total concentration m CuCl m CH m H 2 CO m Al 2 (SiO 3 ) 3

Colligative Properties Which of the following would have the highest boiling point? 0.25 m KCN 1.0 m CH 3 OH 0.50 m Ca(NO 3 ) m HCl

Colligative Properties What is the boiling point of 5.0 g of CuSO 4 in 20. g of water?