Unit 7. Solution Concentrations and Colligative Properties

Size: px
Start display at page:

Download "Unit 7. Solution Concentrations and Colligative Properties"

Transcription

1 Unit 7 Solution Concentrations and Colligative Properties

2 Molarity Most widely used concentration unit [HCl] means concentration of HCl in mol/l Notice volume is total volume of solution Molarity (M)= moles of solute liters of solution moles M L

3 Molarity Problems Read the problem Look for moles If you have grams of solute, convert to moles Look for the volume of the solution it must be in liters If volume is in ml or cm 3, convert to liters Once you have moles and liters, plug those numbers into the formula to get the big M

4 What is the molarity of a solution that has 84.5 grams of NaOH dissolved in a total volume of 745 ml? 1 Na O H g

5 How many grams of KCl are needed to make a 500. ml of solution that is.750 M KCl? 1 K Cl g

6 Molality Molality (m) expresses concentration in terms of the mass of the solvent. Molality is usually used with formulas revolving around colligative properties. Molality (m) = moles of solute kilograms of solvent m moles kg

7 Molarity vs Molality Molarity and molality differ in two ways: Molarity tells you about moles of solute per volume of the entire solution (solute & solvent) Molality tells you about moles of solute per mass of the solvent Keep in mind that one liter of water masses one kilogram So for a dilute solution, the amount of solution is about the same as the amount of solvent So for a dilute aqueous solution, molarity and molality are basically the same.

8 Molality Problems Read the problem Look for moles If you have grams of solute, convert to moles Look for the mass of the solvent it must be in kilograms If volume is in grams, convert to kilograms Once you have moles and kilograms, plug those numbers into the formula to get the small m

9 What is the molality of a solution that contains 46.8 grams of NaCl dissolved in 545 grams of H 2 O? 1 Na Cl

10 How many grams of KNO 3 are needed to add to 750. g of water to make.450 m KNO 3? 1 K N O

11 Mole Fraction Mole fraction equals the moles of a solute divided by total moles of solution Remember that we used mole fraction to complete one of the versions of Dalton s law X a = moles of substance a total moles of solution

12 Determine the mole fraction of MgCl 2 in a solution that contains 94.8 g MgCl 2 in 345 g of water. first find moles of each Total the moles Find the mole fraction of each

13 % Solutions % solute = mass of mass of solute solute+ mass of solvent Mass is usually in grams Make sure that you understand that the denominator is the total mass of solution.

14 Determine the percent of NaCl in a solution that contains 45.5 g NaCl dissolved in 84.3 g of water. first find the total mass of the solution Then use the formula to find %

15 Remember Density Density is the measure of mass per unit volume. Since density relates mass and volume, it is useful if you need to convert between molarity, which deals with volume, and molality, which deals with mass. D = m/v units usually g/ml or g/cm 3

16 What do you know if given 12.5 % NaCl? 12.5 g NaCl added to 87.5 g H 2 O 100 g solution 87.5 g solvent H 2 O What can you find? (must be given density) Moles solute; liters of solution; kg solvent Molarity Molality Mole fraction

17 What do you know if given 3.0 M KCl? 3.0 moles KCl in 1 liter solution What can you find? (need density again) find grams KCl find grams solvent Molality Mole fraction % solution

18 What do you know if given 2.7 m NaOH? 2.7 moles NaOH in 1 kg water What can you find? (need density) grams NaOH mole fraction % solution Molarity

19 Effect of temperature on solubility Most solids increase solubility when solution is heated some do not All gases decrease solubility when solution is heated.

20 A Solubility Curve Notice a few things: The solubility of NH 3 (a gas) decreases as temperature increases. Most of the solid substances increase in solubility as temperature increases. However, one solid, Ce 2 (SO 4 ) 3, decreases in solubility as the temperature increases. Looking at the y-axis, you can see that solubility units are usually grams of the substance dissolved in 100 grams of water.

21 Like Dissolves Like Polar or ionic solutes dissolve in polar solvents When ionic solutes dissolve they break up into ions Nonpolar solutes dissolve in nonpolar solvents. Polar and nonpolar do not mix

22 Colligative Properties Colligative properties are properties of a solution that depend on the number of solute particles in solution. The identity of the particles is not important There are four colligative properties Boiling point elevation Freezing point depression Vapor pressure lowering Osmotic pressure

23 Van t Hoff factor (i) The Van t Hoff factor needs to be taken into account when using any of the four colligative property formulas. The Van t Hoff factor tells how many ions one unit of a solute will dissociate into when placed in solution. C 6 H 12 O 6 does not dissociate, so i = 1 NaCl dissociates into Na + and Cl -, so i = 2 CaCl 2 dissociates into Ca 2+, Cl -, and Cl -, so i = 3 HF partially dissociates, so 1 < i < 2

24 Boiling Point Elevation When a solute is added to a solvent, the boiling point of the solution increases (that is, bp is higher than that of the solvent) T b = ik b m T b = change in boiling point i = Van t Hoff factor k b = boiling point elevation constant m = molality of solution

25 Boiling Point Elevation Problems You need to be able to determine i You need to be able to find the boiling point elevation constant (from a list) You might be given the temperatures (normal bp and new bp) and asked to find the molality You might be given the normal bp and the molality and asked to find the new bp

26 What is the boiling point of a 2.00 m solution of NaCl in water? Need to determine i NaCl has two ions, so the i = 2 Find the t b T b = ik b m k b = 0.52 ºC/m T b = (2)(0.52 ºC/m)(2.00 m) = 2.08 or 2.1ºC Look up the normal bp of water add the change in temp normal bp = ºC New bp = ºC ºC = ºC

27 Freezing Point Depression When a solute is added to a solvent, the freezing point of the solution decreases (that is, fp is lower than that of the solvent) T f = ik f m T f = change in freezing point i = Van t Hoff factor k f = freezing point depression constant m = molality of solution

28 Freezing Point Depression Problems You need to be able to determine i You need to be able to find the freezing point depression constant (from a list) You might be given the temperatures (normal fp and new fp) and asked to find the molality You might be given the normal fp and the molality and asked to find the new fp

29 What is the freezing point of a 2.00 m solution of CaCl 2 in water? Need to determine i CaCl 2 has three ions, so the i = 3 Find the t f T f = ik f m k f = 1.86 ºC/m T f = (3)(1.86 ºC/m)(2.00 m) = or 11.2ºC Look up the normal fp of water subtract the change in temp normal fp = 0.0 ºC New fp = 0.0 ºC 11.2 ºC = ºC

30 Vapor Pressure Lowering Called Raoult s Law when a solute is added to a solution, the vapor pressure will decrease. P = XPº P = vapor pressure of solution P º = vapor pressure of solvent X = mole fraction of solvent

31 Vapor Pressure Problems You need to determine the mole fraction of the solvent Find moles of solute, find moles of solvent Add the moles together to get total moles Then use the formula Then use the formula P = XPº Pº is the normal vapor pressure of the solvent

32 Calculate the vapor pressure of a solution made by dissolving 218 g of glucose (C 6 H 12 O 6 ) in 460. g of water. The vapor pressure of pure water at 30ºC is 31.8 mmhg. Determine the moles of solute and solvent 218 g C 6 H 12 O 6 1 mol C 6 H 12 O 6 = 1.21 mol C 6 H 12 O g C 6 H 12 O g H 2 O 1 mol H 2 O = 25.5 mol H 2 O g H 2 O Determine the mole fraction of solute total moles = 1.21 mol mol = 26.7 mol H2 O Plug values into formula P = XPº = (.955)(31.8 mmhg) = 30.4 mmhg

33 Osmotic Pressure When a pure solvent and a solution are separated by a membrane that only allows solvent to pass through, the solvent will try to pass through the membrane to dilute the solution. The greater the concentration of solute in the solution, the greater the osmotic pressure. Ώ =λ = MRTi Ώ =λ = osmotic pressure (atm) M = molarity R = gas constant =.0821 (L atm)/(mol K) T = Kelvin temperature i = Van t Hoff factor

34 What do you need to know for test? Like dissolves like Affect of temperature on solubility Molarity Molality Mole fractions % solutions Colligitave properties (math)

Molality. Molality (m) is the number of moles of solute per kilogram of solvent. mol of solute kg solvent. Molality ( m) =

Molality. Molality (m) is the number of moles of solute per kilogram of solvent. mol of solute kg solvent. Molality ( m) = Molality Molality (m) is the number of moles of solute per kilogram of solvent. Molality ( m) = mol of solute kg solvent Sample Problem Calculate the molality of a solution of 13.5g of KF dissolved in

More information

Chapter 11: Properties of Solutions

Chapter 11: Properties of Solutions Chapter 11: Properties of Solutions Apr 1 11:01 AM 11.1 Solution Composition Solve problems relating to the mass percent, mole fraction and molality. Mar 26 1:09 PM 1 Molarity (M) is defined as moles of

More information

Chapter 12.4 Colligative Properties of Solutions Objectives List and define the colligative properties of solutions. Relate the values of colligative

Chapter 12.4 Colligative Properties of Solutions Objectives List and define the colligative properties of solutions. Relate the values of colligative Chapter 12.4 Colligative Properties of Solutions Objectives List and define the colligative properties of solutions. Relate the values of colligative properties to the concentrations of solutions. Calculate

More information

Physical Properties of Solutions

Physical Properties of Solutions Physical Properties of Solutions Chapter 12 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 12.1- Types of solutions A solution is a homogenous mixture of 2 or

More information

AP Chemistry--Chapter 11: Properties of Solutions

AP Chemistry--Chapter 11: Properties of Solutions AP Chemistry--Chapter 11: Properties of Solutions I. Solution Composition (ways of expressing concentration) 1. Qualitatively, use dilute or concentrated to describe 2. Quantitatively a. Mass Percentage

More information

64 previous solution

64 previous solution 64 previous solution mole fraction (definition) 1 - Convert 29.6 grams sodium sulfate to moles. We already did this to find molality, so we can re-use the number. 2 - This is the total moles of both sodium

More information

Soluble: A solute that dissolves in a specific solvent. Insoluble: A solute that will not dissolve in a specific solvent. "Like Dissolves Like"

Soluble: A solute that dissolves in a specific solvent. Insoluble: A solute that will not dissolve in a specific solvent. Like Dissolves Like Solutions Homogeneous Mixtures Solutions: Mixtures that contain two or more substances called the solute and the solvent where the solute dissolves in the solvent so the solute and solvent are not distinguishable

More information

AP CHEMISTRY CHAPTER 8 PROBLEM SET #2. (Questions 1-3) Select the letter of the answer that best completes the statement or answers the question.

AP CHEMISTRY CHAPTER 8 PROBLEM SET #2. (Questions 1-3) Select the letter of the answer that best completes the statement or answers the question. NAME: AP CHEMISTRY CHAPTER 8 PROBLEM SET #2 (Questions 1-3) Select the letter of the answer that best completes the statement or answers the question. 1. 2. 3. According to Raoult s Law, which statement

More information

70 Example: If a solution is m citric acid, what is the molar concentration (M) of the solution? The density of the solution is 1.

70 Example: If a solution is m citric acid, what is the molar concentration (M) of the solution? The density of the solution is 1. 70 Example: If a solution is 0.688 m citric acid, what is the molar concentration (M) of the solution? The density of the solution is 1.049 g/ml molality definition molarity definition To solve the problem,

More information

Chapter 13. Ions in aqueous Solutions And Colligative Properties

Chapter 13. Ions in aqueous Solutions And Colligative Properties Chapter 13 Ions in aqueous Solutions And Colligative Properties Compounds in Aqueous Solution Dissociation The separation of ions that occurs when an ionic compound dissolves H2O NaCl (s) Na+ (aq) + Cl-

More information

SOLUTION CONCENTRATIONS

SOLUTION CONCENTRATIONS SOLUTION CONCENTRATIONS The amount of solute in a solution (concentration) is an important property of the solution. A dilute solution contains small quantities of solute relative to the solvent, while

More information

Solutions and Their Properties

Solutions and Their Properties Chapter 11 Solutions and Their Properties Solutions: Definitions A solution is a homogeneous mixture. A solution is composed of a solute dissolved in a solvent. When two compounds make a solution, the

More information

Solutions. Chapter 14 Solutions. Ion-Ion Forces (Ionic Bonding) Attraction Between Ions and Permanent Dipoles. Covalent Bonding Forces

Solutions. Chapter 14 Solutions. Ion-Ion Forces (Ionic Bonding) Attraction Between Ions and Permanent Dipoles. Covalent Bonding Forces Solutions Chapter 14 1 Brief Review of Major Topics in Chapter 13, Intermolecular forces Ion-Ion Forces (Ionic Bonding) 2 Na + Cl - in salt These are the strongest forces. Lead to solids with high melting

More information

CH 222 Chapter Eleven Concept Guide

CH 222 Chapter Eleven Concept Guide CH 222 Chapter Eleven Concept Guide 1. Molality A 4.5 M nitric acid solution contains 65.0 g of HNO 3 in 288 g of solution. What is the molality of this solution? Molality is calculated by dividing the

More information

Properties of Solutions. Chapter 13

Properties of Solutions. Chapter 13 Properties of Solutions Chapter 13 Sodium acetate crystals rapidly form when a seed crystal is added to a supersaturated solution of sodium acetate. Saturated solution: contains the maximum amount of a

More information

Intermolecular Forces

Intermolecular Forces Intermolecular Forces! When two molecules approach one another, they are attracted to some extent! Polar molecules are attracted through the electrostatic interaction of their dipole moments! Non-polar

More information

CP Chapter 15/16 Solutions What Are Solutions?

CP Chapter 15/16 Solutions What Are Solutions? CP Chapter 15/16 Solutions What Are Solutions? What is a solution? A solution is uniform that may contain solids, liquids, or gases. Known as a mixture Solution = + o Solvent The substance in abundance

More information

Chapter 11. Properties of Solutions

Chapter 11. Properties of Solutions Chapter 11 Properties of Solutions Section 11.1 Solution Composition Various Types of Solutions Copyright Cengage Learning. All rights reserved 2 Section 11.1 Solution Composition Solution Composition

More information

Big Idea Three Topics

Big Idea Three Topics Big Idea Three Topics 1. Molecular, Ionic, Net Ionic Equations 2. Stoichiometry 3. Synthesis, Decomposition Reactions 6. Chemical Change Evidence 7. Endothermic & Exothermic Reactions 8. Electrochemistry

More information

COLLIGATIVE PROPERTIES OF SOLUTIONS

COLLIGATIVE PROPERTIES OF SOLUTIONS NAME: UNIT #9: MOLARITY DILUTIONS SOLUBILITY CURVES COLLIGATIVE PROPERTIES OF SOLUTIONS 1. MOLARITY a) Molarity is a measurement of the concentration of a solution in Chemistry. b) When making solutions,

More information

Chapter 7 Solutions and Colloids

Chapter 7 Solutions and Colloids Chapter 7 Solutions and Colloids 7.1 Physical States of Solutions Solutions are homogeneous mixtures of two or more substances in which the components are present as atoms, molecules, or ions. Properties

More information

Chapter 7 Solutions and Colloids

Chapter 7 Solutions and Colloids Chapter 7 Solutions and Colloids 7.1 Physical States of Solutions Solutions are homogeneous mixtures of two or more substances in which the components are present as atoms, molecules, or ions. Properties

More information

Mixtures. Chapters 12/13: Solutions and Colligative Properties. Types of Solutions. Suspensions. The Tyndall Effect: Colloid

Mixtures. Chapters 12/13: Solutions and Colligative Properties. Types of Solutions. Suspensions. The Tyndall Effect: Colloid Mixtures Chapters 12/13: Solutions and Colligative Properties Solution - a homogeneous mixture of two or more substances in a single phase Soluble - capable of being dissolved Solutions - 2 Parts Solvent

More information

Chapter 13. Characteristics of a Solution. Example of A Homogenous Mixtures. Solutions

Chapter 13. Characteristics of a Solution. Example of A Homogenous Mixtures. Solutions Chapter 13 Solutions Characteristics of a Solution A solution is a homogeneous mixture A solution is composed of a: Solute: the substance in lesser amount Solvent: the substance in greater amount Two liquid

More information

StudyHub: AP Chemistry

StudyHub: AP Chemistry StudyHub+ 1 StudyHub: AP Chemistry Solution Composition and Energies, Boiling Point, Freezing Point, and Vapor Pressure StudyHub+ 2 Solution Composition: Mole Fraction: Formula: Mole Fraction of Component

More information

Chapter 11. General Chemistry. Chapter 11/1

Chapter 11. General Chemistry. Chapter 11/1 Chapter 11 Solutions and Their Properties Professor Sam Sawan General Chemistry 84.122 Chapter 11/1 Solutions Solution: A homogeneous mixture. Solvent: The major component. Solute: A minor component. Copyright

More information

Chapter 11 Problems: 11, 15, 18, 20-23, 30, 32-35, 39, 41, 43, 45, 47, 49-51, 53, 55-57, 59-61, 63, 65, 67, 70, 71, 74, 75, 78, 81, 85, 86, 93

Chapter 11 Problems: 11, 15, 18, 20-23, 30, 32-35, 39, 41, 43, 45, 47, 49-51, 53, 55-57, 59-61, 63, 65, 67, 70, 71, 74, 75, 78, 81, 85, 86, 93 Chapter 11 Problems: 11, 15, 18, 20-23, 30, 32-35, 39, 41, 43, 45, 47, 49-51, 53, 55-57, 59-61, 63, 65, 67, 70, 71, 74, 75, 78, 81, 85, 86, 93 Chapter 11 Properties of Solutions Types of mixtures: homogenous

More information

x =!b ± b2! 4ac 2a moles particles solution (expt) moles solute dissolved (calculated conc ) i =

x =!b ± b2! 4ac 2a moles particles solution (expt) moles solute dissolved (calculated conc ) i = Properties of Solution Practice Exam Solutions Name (last) (First) Read all questions before you start. Show all work and explain your answers. Report all numerical answers to the proper number of sig.

More information

Sample Problem. (b) Mass % H 2 SO 4 = kg H 2 SO 4 /1.046 kg total = 7.04%

Sample Problem. (b) Mass % H 2 SO 4 = kg H 2 SO 4 /1.046 kg total = 7.04% A Sample 0.750 M solution Problem of H 2 SO 4 in water has a density of 1.046 g/ml at 20ºC. What is the concentration in (a) mole fraction, (b) mass percent, (c) molality (MM = 98.086 g/mol)? (a) Since

More information

Chapter 12. Properties of Solutions

Chapter 12. Properties of Solutions Chapter 12. Properties of Solutions What we will learn: Types of solutions Solution process Interactions in solution Types of concentration Concentration units Solubility and temperature Solubility and

More information

Chapter 13. Properties of Solutions

Chapter 13. Properties of Solutions Chapter 13 Properties of Solutions Warm - Up Why doesn t salt dissolve in nonpolar solvents such as hexane? How does the orientation of water around Na + differ from the orientation of water around Cl

More information

Physical Properties of Solutions

Physical Properties of Solutions Physical Properties of Solutions Physical Properties of Solutions Types of Solutions (13.1) A Molecular View of the Solution Process (13.2) Concentration Units (13.3) Effect of Temperature on Solubility

More information

Slide 1. Slide 2. Slide 3. Colligative Properties. Compounds in Aqueous Solution. Rules for Net Ionic Equations. Rule

Slide 1. Slide 2. Slide 3. Colligative Properties. Compounds in Aqueous Solution. Rules for Net Ionic Equations. Rule Slide 1 Colligative Properties Slide 2 Compounds in Aqueous Solution Dissociation - The separation of ions that occurs when an ionic compound dissolves Precipitation Reactions - A chemical reaction in

More information

COLLIGATIVE PROPERTIES

COLLIGATIVE PROPERTIES COLLIGATIVE PROPERTIES Depend on the number of solute particles in solution but not on the identity of the solute Vapor pressure lowering Boiling point elevation Freezing point depression Osmotic pressure

More information

Soln Notes February 17, 2017

Soln Notes February 17, 2017 Chapter 15 Solutions You are responsible for reading/notes on Section 15.4 Heterogeneous Mixtures p.476-479 What is a SOLUTION? SOLUTE vs SOLVENT Characteristics of Solutions: Soluble/ Insoluble Solvation

More information

Bushra Javed Valencia College CHM 1046 Chapter 12 - Solutions

Bushra Javed Valencia College CHM 1046 Chapter 12 - Solutions Bushra Javed Valencia College CHM 1046 Chapter 12 - Solutions 1 Chapter 12 :Solutions Tentative Outline 1. Introduction to solutions. 2. Types of Solutions 3. Solubility and the Solution Process: Saturated,

More information

Warm up. 1. What is a solution? 2. What is a solute? 3. What is a solvent?

Warm up. 1. What is a solution? 2. What is a solute? 3. What is a solvent? Warm up 1. What is a solution? 2. What is a solute? 3. What is a solvent? Solutions Chapter 12.2 Solubility The amount of substance that can dissolve at a given temperature to produce a saturated solution

More information

75 A solution of 2.500g of unknown dissolved in g of benzene has a freezing point of C. What is the molecular weight of the unknown?

75 A solution of 2.500g of unknown dissolved in g of benzene has a freezing point of C. What is the molecular weight of the unknown? 75 A solution of 2.500g of unknown dissolved in 100.0 g of benzene has a freezing point of 4.880 C. What is the molecular weight of the unknown? Solving for Cm (molality) will allow us to calculate how

More information

SOLUTIONS. Chapter Test B. A. Matching. Column A. Column B. Name Date Class. 418 Core Teaching Resources

SOLUTIONS. Chapter Test B. A. Matching. Column A. Column B. Name Date Class. 418 Core Teaching Resources 16 SOLUTIONS Chapter Test B A. Matching Match each term in Column B to the correct description in Column A. Write the letter of the correct term on the line. Column A Column B 1. the number of moles of

More information

Concentration of Solutions

Concentration of Solutions Chapter 11 Textbook Assigned Problems Exercises Concentration of Solutions 25. Because the density of water is 1.00 g/ml, 100.0 ml of water has a mass of 100. g. density = = 1.06 g/ml = 1.06 g/cm 3 mol

More information

- Applications: In chemistry, this effect is often used to determine the molecular weight of an unknown molecule.

- Applications: In chemistry, this effect is often used to determine the molecular weight of an unknown molecule. 73 FREEZING POINT DEPRESSION concentration of solute (molality) Freezing point depression constant (for SOLVENT) Freezing point depression: The amount the freezing temperature is LOWERED by the solute.

More information

concentration of solute (molality) Freezing point depression constant (for SOLVENT)

concentration of solute (molality) Freezing point depression constant (for SOLVENT) 74 FREEZING POINT DEPRESSION concentration of solute (molality) Freezing point depression constant (for SOLVENT) Freezing point depression: The amount the freezing temperature is LOWERED by the solute.

More information

Freezing point depression - The freezing temperature of a SOLUTION gets lower as the CONCENTRATION of a solution increases.

Freezing point depression - The freezing temperature of a SOLUTION gets lower as the CONCENTRATION of a solution increases. 73 COLLIGATIVE PROPERTIES - properties unique to solutions. - depend only on the CONCENTRATION of a solution and not the IDENTITY of the solute** **ionic solutes: Remember that they dissociate into MULTIPLE

More information

Solutions CHAPTER Solution Formation. Ch.16 Notes with notations. April 17, 2018

Solutions CHAPTER Solution Formation. Ch.16 Notes with notations. April 17, 2018 CHAPTER 16 Solutions 16.1 Solution Formation Solutions can be either solids, liquids, or gases Solutions are homogeneous mixtures that are grouped according to physical state. (mixtures = no bonding) The

More information

1. What is a solution? and think

1. What is a solution? and think 1. What is a solution? and think Solutions Properties of Solutions Solutions: 1. Have no visible parts (particles are small) 2. They are homogeneous evenly distributed particles 3. The particles do not

More information

An aqueous solution is 8.50% ammonium chloride by mass. The density of the solution is g/ml Find: molality, mole fraction, molarity.

An aqueous solution is 8.50% ammonium chloride by mass. The density of the solution is g/ml Find: molality, mole fraction, molarity. 66 An aqueous solution is 8.50% ammonium chloride by mass. The density of the solution is 1.024 g/ml Find: molality, mole fraction, molarity. Find molality: mass percent molality Assuming 100 g solution,

More information

What are the parts of a solution? What is the solution process:

What are the parts of a solution? What is the solution process: What are the parts of a solution? o Solute: the thing that gets dissolved (usually solid) o Solvent: the thing that does the dissolving (usually liquid) What is the solution process: Ionic Compound Covalent

More information

2011, Robert Ayton. All rights reserved.

2011, Robert Ayton. All rights reserved. Solutions Outline 1. Solubility 2. Concentration Calculations 3. Colligative Properties 4. Freezing Point Depression or Boiling Point Elevation Problems 5. Graphs of Colligative Properties Review 1. Solubility

More information

SOLUTIONS. Definitions. Solvation. Hydration. Energy changes involved in solutions

SOLUTIONS. Definitions. Solvation. Hydration. Energy changes involved in solutions 1 SOLUTIONS Definitions Solvation Hydration Energy changes involved in solutions 2 Solubility Definition Unsaturated Saturated supersaturated Factors affecting solubility Interactions of solute with solvent

More information

PHYSICAL PROPERTIES OF SOLUTIONS

PHYSICAL PROPERTIES OF SOLUTIONS PHYSICAL PROPERTIES OF SOLUTIONS Do all the exercises in your study guide. PHYSICAL PROPERTIES OF SOLUTIONS A solution is a homogeneous mixture of a solute and a solvent. A solvent is a substance that

More information

Warm UP. between carbonate and lithium. following elements have? 3) Name these compounds: 1) Write the neutral compound that forms

Warm UP. between carbonate and lithium. following elements have? 3) Name these compounds: 1) Write the neutral compound that forms Warm UP 1) Write the neutral compound that forms between carbonate and lithium 2) How many valence electrons do the following elements have? a) Chlorine b) Neon c) Potassium 3) Name these compounds: a)

More information

Properties of Solutions. Overview of factors affecting solubility Ways of expressing concentration Physical properties of solutions

Properties of Solutions. Overview of factors affecting solubility Ways of expressing concentration Physical properties of solutions Properties of Solutions Overview of factors affecting solubility Ways of expressing concentration Physical properties of solutions Learning objectives Define terms solute, solvent and solution Distinguish

More information

11/4/2017. General Chemistry CHEM 101 (3+1+0) Dr. Mohamed El-Newehy. Chapter 4 Physical Properties of Solutions

11/4/2017. General Chemistry CHEM 101 (3+1+0) Dr. Mohamed El-Newehy.   Chapter 4 Physical Properties of Solutions General Chemistry CHEM 11 (3+1+) Dr. Mohamed El-Newehy http://fac.ksu.edu.sa/melnewehy Chapter 4 Physical Properties of Solutions 1 Types of Solutions A solution is a homogenous mixture of 2 or more substances.

More information

PX-III Chem 1411 Chaps 11 & 12 Ebbing

PX-III Chem 1411 Chaps 11 & 12 Ebbing PX-III Chem 1411 Chaps 11 & 12 Ebbing 1. What is the name for the following phase change? I 2 (s) I 2 (g) A) melting B) condensation C) sublimation D) freezing E) vaporization 2. Which of the following

More information

Chapter 12. Solutions and Their Behavior. Supersaturated contains more than the saturation limit (very unstable)

Chapter 12. Solutions and Their Behavior. Supersaturated contains more than the saturation limit (very unstable) Chapter 12 Solutions and Their Behavior Unsaturated holds less than maximum capacity at a given T Supersaturated contains more than the saturation limit (very unstable) Saturated maximum amount of solute

More information

- Let's look at how things dissolve into water, since aqueous solutions are quite common. sucrose (table sugar)

- Let's look at how things dissolve into water, since aqueous solutions are quite common. sucrose (table sugar) 68 HOW THINGS DISSOLVE - Let's look at how things dissolve into water, since aqueous solutions are quite common. sucrose (table sugar)... what happens? - Water molecules pull the sugar molecules out of

More information

Solutions: Formation and Properties

Solutions: Formation and Properties New Jersey Center for Teaching and Learning Slide 1 / 48 Progressive Science Initiative This material is made freely available at www.njctl.org and is intended for the non-commercial use of students and

More information

VAPOR PRESSURE LOWERING - Described by RAOULT'S LAW

VAPOR PRESSURE LOWERING - Described by RAOULT'S LAW 73 VAPOR PRESSURE LOWERING - Described by RAOULT'S LAW partial pressure of the VAPOR of solvent molecules. mole fraction of component A vapor pressure of pure component A (depends on temperature) partial

More information

10) On a solubility curve, the points on the curve indicate a solution. 11) Values on the graph a curve represent unsaturated solutions.

10) On a solubility curve, the points on the curve indicate a solution. 11) Values on the graph a curve represent unsaturated solutions. Unit 11 Solutions- Funsheets Part A: Solubility Curves- Answer the following questions using the solubility curve below. Include units! 1) What mass of each solute will dissolve in 100mL of water at the

More information

Colligative Properties

Colligative Properties Colligative Properties Vapor pressures have been defined as the pressure over a liquid in dynamic equilibrium between the liquid and gas phase in a closed system. The vapor pressure of a solution is different

More information

Classification of Solutions. Classification of Solutions. Aqueous Solution Solution in which H2O is the solvent

Classification of Solutions. Classification of Solutions. Aqueous Solution Solution in which H2O is the solvent SOLUTIONS Solution Homogeneous mixture in which one substance is dissolved in another SOLUTE: substance that is dissolved SOLVENT: substance doing the dissolving INSOLUBLE: does NOT dissolve SOLUBLE: does

More information

Colligative properties CH102 General Chemistry, Spring 2011, Boston University

Colligative properties CH102 General Chemistry, Spring 2011, Boston University Colligative properties CH12 General Chemistry, Spring 211, Boston University here are four colligative properties. vapor-pressure lowering boiling-point elevation freezing-point depression osmotic pressure

More information

Solutions. Definitions. Some Definitions. Page 1. Parts of a Solution

Solutions. Definitions. Some Definitions. Page 1. Parts of a Solution Chapter 15 s 1 Definitions 4 Why does a raw egg swell or shrink when placed in different solutions? s can be classified as saturated or unsaturated. A saturated solution contains the maximum quantity of

More information

The Water Molecule. Draw the Lewis structure. H O H. Covalent bonding. Bent shape

The Water Molecule. Draw the Lewis structure. H O H. Covalent bonding. Bent shape Water & Solutions 1 The Water Molecule Draw the Lewis structure. H O H Covalent bonding. Bent shape 2 Water What determines whether a molecule is polar? Is water a polar molecule? d- d+ d+ 1. Oxygen is

More information

TOPICS TO BE COVERED 1. WHAT ARE SOLUTIONS? 2. SOLVENTS AND SOLUTES 3. SOLUBILITY AND ITS FACTORS 4. CONCENTRATIONS 5. SOLUTION STOICHIOMETRY 6.

TOPICS TO BE COVERED 1. WHAT ARE SOLUTIONS? 2. SOLVENTS AND SOLUTES 3. SOLUBILITY AND ITS FACTORS 4. CONCENTRATIONS 5. SOLUTION STOICHIOMETRY 6. TOPICS TO BE COVERED 1. WHAT ARE SOLUTIONS? 2. SOLVENTS AND SOLUTES 3. SOLUBILITY AND ITS FACTORS 4. CONCENTRATIONS 5. SOLUTION STOICHIOMETRY 6. COLLIGATIVE PROPERTIES SOLUTIONS CHEMICALS + WATER 1. WHAT

More information

UNIT 8: SOLUTIONS. Essential Question: What kinds of properties affect a chemical s solubility?

UNIT 8: SOLUTIONS. Essential Question: What kinds of properties affect a chemical s solubility? UNIT 8: SOLUTIONS Essential Question: What kinds of properties affect a chemical s solubility? SOLUTIONS & THEIR CHARACTERISTICS (5) Most chemical reactions take place IN solutions 1. Homogeneous mixture

More information

Find molality: mass percent. molality Assume a basis of 100g solution, then find moles ammonium chloride: Find mass water: So molality is:

Find molality: mass percent. molality Assume a basis of 100g solution, then find moles ammonium chloride: Find mass water: So molality is: 66 An aqueous solution is 8.50% ammonium chloride by mass. The density of the solution is 1.024 g/ml Find: molality, mole fraction, molarity. Find molality: mass percent molality Assume a basis of 100g

More information

Solutions. Experiment 11. Various Types of Solutions. Solution: A homogenous mixture consisting of ions or molecules

Solutions. Experiment 11. Various Types of Solutions. Solution: A homogenous mixture consisting of ions or molecules Solutions Solution: A homogenous mixture consisting of ions or molecules -Assignment: Ch 15 Questions & Problems : 5, (15b,d), (17a, c), 19, 21, 23, 27, (33b,c), 39, (43c,d),45b, 47, (49b,d), (55a,b),

More information

Chapter 12. Physical Properties of Solutions. Chemistry, Raymond Chang 10th edition, 2010 McGraw-Hill

Chapter 12. Physical Properties of Solutions. Chemistry, Raymond Chang 10th edition, 2010 McGraw-Hill Chemistry, Raymond Chang 10th edition, 2010 McGraw-Hill Chapter 12 Physical Properties of Solutions Ahmad Aqel Ifseisi Assistant Professor of Analytical Chemistry College of Science, Department of Chemistry

More information

SOLVING EMPIRICAL FORMULA PROBLEMS

SOLVING EMPIRICAL FORMULA PROBLEMS SOLVING EMPIRICAL FORMULA PROBLEMS Why do we want to use Empirical Formulas? 1)Substances that do not consist of discrete units, such as in a crystal (ionic solid) of NaCl---we dont want to write Na456Cl910

More information

Colligative Properties. Vapour pressure Boiling point Freezing point Osmotic pressure

Colligative Properties. Vapour pressure Boiling point Freezing point Osmotic pressure Colligative Properties Vapour pressure Boiling point Freezing point Osmotic pressure Learning objectives Describe meaning of colligative property Use Raoult s law to determine vapor pressure of solutions

More information

1. A solution that is 9% by mass glucose contains 9 g of glucose in every g of solution.

1. A solution that is 9% by mass glucose contains 9 g of glucose in every g of solution. Solutions molarity (Homework) For answers, send email to: admin@tutor-homework.com. Include file name: Chemistry_Worksheet_0144 Price: $3 (c) 2012 www.tutor-homework.com: Tutoring, homework help, help

More information

Salting The Roads Colligative Property. B. Types. A. Definition

Salting The Roads Colligative Property. B. Types. A. Definition Salting The Roads Colligative Property A. Definition property that depends on the concentration of solute particles, not their identity Unit 11: Solutions Lesson 11.3: Colligative Properties 68 B. Types

More information

LESSON 11. Glossary: Solutions. Boiling-point elevation

LESSON 11. Glossary: Solutions. Boiling-point elevation LESSON 11 Glossary: Solutions Boiling-point elevation Colligative properties Freezing-point depression Molality Molarity (M) Mole (mol) Mole fraction Saturated solution a colligative property of a solution

More information

Aqueous Solutions (When water is the solvent)

Aqueous Solutions (When water is the solvent) Aqueous Solutions (When water is the solvent) Solvent= the dissolving medium (what the particles are put in ) Solute= dissolved portion (what we put in the solvent to make a solution) Because water is

More information

AP CHEMISTRY NOTES 15-1 INTERMOLECULAR FORCES

AP CHEMISTRY NOTES 15-1 INTERMOLECULAR FORCES AP CHEMISTRY NOTES 15-1 INTERMOLECULAR FORCES INTERMOLECULAR FORCES In addition to the covalent bonds that exist between atoms in a molecule (H2O for instance), there are also weak attractions between

More information

Ions in Aqueous Solutions and Colligative Properties

Ions in Aqueous Solutions and Colligative Properties Ions in Aqueous Solutions and Colligative Properties Section 1 Compounds in Aqueous Solutions Dissociation When compound made from ions dissolves in water, ions separate Dissociation à separation of ions

More information

Let's look at the following "reaction" Mixtures. water + salt > "salt water"

Let's look at the following reaction Mixtures. water + salt > salt water Mixtures What happens to the properties (phase changes) when we make a solution? Let's look at the following "reaction" water + salt ------> "salt water" Which has the higher entropy? A. The water + the

More information

CHAPTER OUTLINE. I. The Structure of Water: An Introduction to Intermolecular Forces

CHAPTER OUTLINE. I. The Structure of Water: An Introduction to Intermolecular Forces The Chemistry of Water and the Nature of Liquids Chapter 11 CHAPTER OUTLINE 11.2 I. The Structure of Water: An Introduction to Intermolecular Forces II. A Closer Look at Intermolecular lar Forces A. London

More information

B. Types. Salting The Roads. A. Definition 4/21/2015. Unit 11: Solutions Lesson 11.3: Colligative Properties 68. Colligative Property

B. Types. Salting The Roads. A. Definition 4/21/2015. Unit 11: Solutions Lesson 11.3: Colligative Properties 68. Colligative Property Salting The Roads Unit 11: Solutions Lesson 11.3: Colligative Properties 68 Colligative Property A. Definition property that depends on the concentration of solute particles, not their identity B. Types

More information

solubility solubilities that increase with increasing temperature

solubility solubilities that increase with increasing temperature Solubility The concentration of the solute in a saturated solution is the solubility of the solute About 95% of all ionic compounds have aqueous solubilities that increase with increasing temperature Temperature

More information

Regents Chemistry Unit 3C Solutions Text Chapter 13 Reference Tables F, G & T. Chemists have Solutions!

Regents Chemistry Unit 3C Solutions Text Chapter 13 Reference Tables F, G & T. Chemists have Solutions! Regents Chemistry Unit 3C Solutions Text Chapter 13 Reference Tables F, G & T Chemists have Solutions! SOLUTIONS homogeneous mixture (uniform composition throughout) Solute - substance being dissolved

More information

Name AP CHEM / / Chapter 11 Outline Properties of Solutions

Name AP CHEM / / Chapter 11 Outline Properties of Solutions Name AP CHEM / / Chapter 11 Outline Properties of Solutions Solution Composition Because a mixture, unlike a chemical compound, has a variable composition, the relative amounts of substances in a solution

More information

Chapter 11 Review Packet

Chapter 11 Review Packet Chapter 11 Review Packet Name Multiple Choice Portion: 1. Which of the following terms is not a quantitative description of a solution? a. molarity b. molality c. mole fraction d. supersaturation 2. Which

More information

Announcements. It is critical that you are keeping up. Ask or see me if you need help. Lecture slides updated and homework solutions posted.

Announcements. It is critical that you are keeping up. Ask or see me if you need help. Lecture slides updated and homework solutions posted. Announcements Dec. 18 Hour Exam 1 C-109 Start time 6PM Coverage is Chapter 12 and 13. 10-multiple choice 3-fairly short problems 3-longer problem solving 100 point Exam Lecture slides updated and homework

More information

Name Class Date. In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question.

Name Class Date. In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. Assessment Chapter Test A Chapter: Solutions In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. 1. Agitation prevents settling

More information

Solution Concentration. Solute Solvent Concentration Molarity Molality ph

Solution Concentration. Solute Solvent Concentration Molarity Molality ph Solution Concentration Solute Solvent Concentration Molarity Molality ph http://en.wikipedia.org/wiki/homogeneou Lets Review Mixture: A mixture is a chemical substance which is a homogeneous or heterogeneous

More information

Mixtures. What happens to the properties (phase changes) when we make a solution? Principles of Chemistry II. Vanden Bout

Mixtures. What happens to the properties (phase changes) when we make a solution? Principles of Chemistry II. Vanden Bout Mixtures What happens to the properties (phase changes) when we make a solution? Let's look at the following "reaction" water + salt ------> "salt water" Which has the higher entropy? A. The water + the

More information

Ways of Expressing Concentrations of Solutions. Solutions

Ways of Expressing Concentrations of Solutions. Solutions Ways of Expressing Concentrations of Mole Fraction (X) X A = moles of A total moles in solution In some applications, one needs the mole fraction of solvent, not solute make sure you find the quantity

More information

Chapter 13 Properties of Solutions

Chapter 13 Properties of Solutions Chapter 13 Properties of Solutions 13.1 The Solution Process - Solutions are homogeneous mixtures of two or more pure substances. - In a solution, the solute is dispersed uniformly throughout the solvent.

More information

- Let's look at how things dissolve into water, since aqueous solutions are quite common. sucrose (table sugar)

- Let's look at how things dissolve into water, since aqueous solutions are quite common. sucrose (table sugar) 68 HOW THINGS DISSOLVE - Let's look at how things dissolve into water, since aqueous solutions are quite common. sucrose (table sugar)... what happens? - Water molecules pull the sugar molecules out of

More information

Chemistry 103 Spring 2010

Chemistry 103 Spring 2010 Today 1. Factors affecting solubility. 2. Colligative properties. Announcements 1. OWL homework for Ch. 14 due next week. 2. DROP deadline on Apr. 6, Tuesday. 3. ADD deadline on Apr. 12, Monday. 4. First

More information

or supersaturatedsaturated Page 1

or supersaturatedsaturated Page 1 Solutions Unit #9 Chapter #11 A solution is a HOMOGENEOUS mixture of 2 or more substances in a single phase. One constituent is usually regarded as the SOLVENT and the others as SOLUTES. 1 Definitions

More information

Solution Concentrations CHAPTER OUTLINE

Solution Concentrations CHAPTER OUTLINE Chapter 8B Solution Concentrations CHAPTER OUTLINE Concentration Units Mass Percent Using Percent Concentration Molarity Using Molarity Dilution Osmolarity Tonicity of Solutions 2 CONCENTRATION UNITS The

More information

Name: Regents Chemistry: Dr. Shanzer. Practice Packet. Chapter 11: Solutions

Name: Regents Chemistry: Dr. Shanzer. Practice Packet. Chapter 11: Solutions Name: Regents Chemistry: Dr. Shanzer Practice Packet Chapter 11: Solutions What are Solutions? Objective: How do we recognize the parts of a solution, its characteristics and the difference between dissolving

More information

CHEM 121b Exam 1 Spring 1999

CHEM 121b Exam 1 Spring 1999 Name SSN CHEM 121b Exam 1 Spring 1999 This exam consists of 15 multiple choice questions (each worth 2 points), and 5 written problems (points noted below for each). There are a total of 100 possible points.

More information

A) sublimation. B) liquefaction. C) evaporation. D) condensation. E) freezing. 11. Below is a phase diagram for a substance.

A) sublimation. B) liquefaction. C) evaporation. D) condensation. E) freezing. 11. Below is a phase diagram for a substance. PX0411-1112 1. Which of the following statements concerning liquids is incorrect? A) The volume of a liquid changes very little with pressure. B) Liquids are relatively incompressible. C) Liquid molecules

More information

Lesson Plans Chapter 15: Solutions & Solution Chemistry

Lesson Plans Chapter 15: Solutions & Solution Chemistry Lesson Plans Chapter 15: Solutions & Solution Chemistry I. Solutions a. A solution is simply a homogeneous mixture i. Homogeneous: same throughout (it does not mean one ) ex: water + sugar, air, alloys,

More information

Physical Pharmacy. Solutions. Khalid T Maaroof MSc. Pharmaceutical sciences School of pharmacy Pharmaceutics department

Physical Pharmacy. Solutions. Khalid T Maaroof MSc. Pharmaceutical sciences School of pharmacy Pharmaceutics department Physical Pharmacy Solutions Khalid T Maaroof MSc. Pharmaceutical sciences School of pharmacy Pharmaceutics department 10/31/2015 Online access: bit.ly/physicalpharmacy 1 Mixtures a combination of two or

More information

Chemistry 201: General Chemistry II - Lecture

Chemistry 201: General Chemistry II - Lecture Chemistry 201: General Chemistry II - Lecture Dr. Namphol Sinkaset Chapter 14 Study Guide Concepts 1. Solutions are homogeneous mixtures of two or more substances. 2. solute: substance present in smaller

More information