Chapter 18 Notes, part III Colligative Properties.

Slides:

Advertisements

Similar presentations

Colligative Properties

Advertisements

Colligative Properties

Ions in aqueous Solutions And Colligative Properties

Colligative Properties Honors Chemistry Unit 8 Chapter 15.

Colligative Properties of Solutions. Colligative Properties Colligative Property: A property that depends only upon the number of solute particles (),

Molarity  Molarity = grams / molar mass / Liters  Liters = grams / molar mass/ Molarity  Grams = Molarity x Liters x molar mass.

Colligative Properties. Properties that depend upon the concentration of solute particles are called colligative properties. Generally these properties.

Colligative Properties of Solutions Chemistry Mrs. Coyle.

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

COLLIGATIVE PROPERTIES STRUCTURE MEETS FUNCTION: WHAT PROPERTIES DO SOLUTIONS HAVE AND WHY?

Notes on Solutions. Qualitative ways of describing solutions Dilute vs. concentrated Unsaturated, saturated, supersaturated Miscible/immiscible Solute,

16.1 Properties of Solutions

Chapter 21 Colligative Properties: Boiling Point & Freezing Point.

Dilution Review Take 5 minutes with your partner to solve the scenario below. Oops! I spilled 100mL of water into my 300mL of 6 M HCl. Is my solution too.

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

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

Chapter 13 Section 5: Colligative Properties

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

Colligative Properties of Solutions Chemistry Honors.

Mini-Unit: Colligative Properties Calculations with Colligative Properties Day 2 - Notes.

SOLUTIONS Chapter 13 and 14.

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

Monday Warm Up Find the molarity of a solution in which 5.5 mol of CaCl 2 is dissolved to make 2 L aqueous CaCl 2 solution. Find the molarity of a solution.

CHAPTER 15: SOLUTIONS Honors Chemistry. SOLUTIONS A solution is a The is(are) the substance(s) present in the The is the substance present in the.

Solids and Gases in Liquids.  Describe the effect of solutes on vapour pressure of solvent.  Describe the effect of solutes on boiling point of the.

Homogeneous mixture = solution Solute the substance that’s being dissolved Solvent - the substance that the solute is dissolved in.

These colligative properties are… The pressure within a solution – pushing out because it wants to evaporate! Atmospheric pressure usually prevents.

Warm Up # 4 You have a 400. mL solution with a concentration of M. How much more solvent did you add to your solution if the new concentration of.

Why do you put antifreeze in your car radiator? Can you cook spaghetti faster in salt water? Why is salt placed on roads to keep ice from forming?

1 Colligative Properties of Solutions. 2 Colligative Properties Colligative properties are physical properties of solutions that change when adding a.

Colligative Properties

Colligative Properties. Doesn’t depend on identity, but number of particles Boiling Point Elevation (BPE) – addition of solute raises Boiling Point Freezing.

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.

Colligative Properties

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

Changing melting and boiling points. Putting salt on sidewalks and roads in the winter helps because it lowers the freezing point of water by a few degrees.

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

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

Molarity and Colligative Properties Chemistry GT 5/8/15.

Unit 4: Solutions Lesson 6. C : Perform a lab to demonstrate freezing-point depression and boiling-point elevation. C : Explain freezing-point.

Colligative Properties of Solutions Section 16.3.

CH 16- Solutions. Outline Concentration % by mass Molarity Dilution Formula Colligative Properties Concept- explain how it occurs BP Elevation FP Depression.

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

Solutions. Occur in all phases u The solvent does the dissolving. u The solute is dissolved. u We will focus on aqueous solutions.

Chemistry 16.3.

COLLIGATIVE PROPERTIES

Do Now: What are the units for molarity?

Ions in Solution Chapter 14.

Colligative Properties

Unit 6: Solutions and Kinetics

Colligative Properties

Colligative Properties

Solvation, Solubility, and Colligative Properties

Colligative Properties of Solutions

8.3 Colligative Properties Objective S3

Colligative Properties

Lesson 6.1: Solutions and Concentration

Colligative Properties of Solutions

Colligative Properties

Chapter 12: Solutions Mrs. Taylor HAHS H. Chem 1B.

Colligative Properties

Section 3 – Colligative Properties of Solutions

Colligative Properties

Vapor-Pressure Lowering

Chapter 13 Section 5: Colligative Properties

Solutions Part II.

Colligative Properties

Colligative Properties of Solutions

8.2 Colligative Properties Objective 2

Presentation transcript:

Chapter 18 Notes, part III Colligative Properties

INTRO QUESTION: Why is the water boiling at a temperature other than 100 o C?

What are colligative properties? Properties that are only affected by the number of particles dissolved in a solvent.

Ionic vs. Covalent in Colligative Properties As discussed before, when a salt dissolves in water it dissociates. This means there are more particles in a solution of a salt in comparison to a solution with a covalent compound (such as sugar).

How many particles do the following break into:NaCl CaCl 2 C 6 H 12 O 6 H 3 PO 4 CO 2 KNO 3 N2ON2ON2ON2O Na 2 CO 3 AlF 3 C3H6OC3H6OC3H6OC3H6O Be 3 N 2 SO 3

Three Colligative Properties Boiling Point Elevation Freezing Point Depression Vapor Pressure

Boiling Point Elevation When a solute is added to a solution, the boiling point of the liquid is increased. It takes more kinetic energy to get the molecules out of the liquid phase and into the gas phase! Why is this?

Freezing Point Depression When a solute is added the freezing point of a solvent is decreased. Why does this occur?

Vapor Pressure There is a decrease in vapor pressure when a solute is added to a solvent. This is because the solvent’s particles are busy surrounding the solute, so less are free to escape into the air.

Calculating Change in Boiling/Freezing Point The change in boiling point can be found using the formula:  T b =K b x m The change in freezing point can be found using the formula:  T f =K f x m For water, K b =0.512 o C/m For water, K f =1.86 o C/m

Practice Problem #1 What temperature does a salt solution boil at if 95.5g of NaCl has been added to 1.5kg of water?

Practice Problem #2 At what temperature does a solution freeze if it is made by adding 52.2g of MgCl 2 to 1127g of water?

Practice Problem #3 What is the molar mass of a sugar if when 235.8g are dissolved into 515g of water, the boiling point is o C?

Practice Problem #4 What is the molar mass of a salt that breaks into two parts, if when 122.5g are dissolved into 495g of water, the boiling point is o C?