Solutions. How Solutions Form

Save this PDF as:
 WORD  PNG  TXT  JPG

Size: px
Start display at page:

Download "Solutions. How Solutions Form"

Transcription

1 Solutions How Solutions Form

2 Solvent substance doing the dissolving, present in greater amount Definitions Solution - homogeneous mixture Solute substance being dissolved

3 Definitions Solute - KMnO 4 Solvent - H 2 O

4 Types of Solutions Based on state of solvent. All solid-liquid-gas combos are possible. EX: dental amalgam (alloy of silver, mercury, etc.) liquid solute, solid solvent solid solution

5 Bell Ringer What is a solution? What is a solute? What is a solvent?

6 Types of Solutions Unsaturated not holding all the solute it can, will dissolve more. Saturated- holding all the solute it can, won t dissolve any more. Supersaturated- holding more than theoretically possible, very unstable Seed Crystal

7 Dissolving Solvation occurs at the surface of the solute solvent particles surround solute particles (+/- attraction) solute particles are pulled into solution

8 Dissolving NaCl dissolving in water

9 Rate of Solution Solids dissolve faster... more stirring small particle size (increased surface area) high temperature

10 Rate of Solution Gases dissolve faster... no shaking or stirring high pressure low temperature

11 Solutions Solubility & Concentration

12 Concentration Concentrated solution large amount of solute Dilute solution small amount of solute

13 Concentration % by Volume usually liquid in liquid EX: 10% juice = 10mL juice + 90mL water % by Mass usually solid in liquid EX: 20% NaCl = 20g NaCl + 80g water

14 Concentration UNSATURATED SOLUTION more solute dissolves SATURATED SOLUTION no more solute dissolves SUPERSATURATED SOLUTION becomes unstable, crystals form concentration

15 Solubility Solubility - maximum grams of solute that will dissolve in 100 g of solvent at a given temperature varies with temperature based on a saturated solution

16 Solubility Curve - shows the dependence of solubility on temperature Solubility

17 Solubility Solids are more soluble at... high temperatures. Gases are more soluble at... low temperatures. high pressures (Henry s Law).

18 Bell Ringer What is a saturated solution? What is a supersaturated solution? What is solubility? What factors can affect solubility?

19 Solutions Particles in Solution

20 POLAR MOLECULE A molecule that has electrically charged areas. Also called a polar substance or polar compound. + DURACELL _

21 NON-POLAR SUBSTANCES Non-polar substances do not have charged ends DURACELL

22 Aqueous (Water) Solutions Water dissolves ionic compounds and polar covalent molecules very well. Salt is ionic- makes salt water. The rule is: like dissolves like Polar dissolves polar. Nonpolar dissolves nonpolar. Oil is nonpolar. Oil and water don t mix.

23 STRUCTURE OF WATER H H O 1 molecule of water is made up of 2 hydrogen atoms bonded with 1 oxygen atom

24 Water is Very Polar + + H H O -

25 Universal Solvent Why is water so good at dissolving things? Because water is a polar molecule and is shaped like a wedge, it is able to break up substances into smaller pieces (dissolve). Water 1) breaks the + and - charged pieces apart, and 2) surrounds them.

26 H How Ionic solids dissolve in water These ions have been pulled away from the main crystal structure by water s polarity. H VTmfQUNLlMY H H H These ions have been surrounded by water, and are now dissolved!

27 Bell Ringer What is a polar molecule? Why is water called the universal solvent? Hint: 2 parts to this answer

28 Electrolytes and Nonelectrolytes Electrolytes- compounds that conduct an electric current in aqueous solution, or in the molten state all ionic compounds are electrolytes because they dissociate into ions (they are also called salts ) NaCl Na 1+ and Cl 1- Must have charged particles that can move.

29 Electrolytes and Nonelectrolytes Do not conduct? = Nonelectrolytes. Most are molecular materials, because they do not have ions Not all electrolytes conduct to the same degree there are weak electrolytes, and strong electrolytes depends on: the degree of ionization

30 Electrolytes- conduct electricity salt acetic acid sugar Electrolyte solute exists as ions only Weak Electrolyte solute exists as ions and molecules Non- Electrolyte solute exists as molecules only

31 Colligative Properties Colligative properties - properties of solutions that depend only on solute concentration Freezing Point Depression solutes lower the f.p. of a solvent Boiling Point Elevation solutes raise the b.p. of a solvent

32 Colligative Properties Freezing Point Depression

33 Colligative Properties Boiling Point Elevation Solute particles get in the way.

34 Colligative Properties Effect increases as the solute concentration increases. Uses: antifreeze making ice cream salting icy roads 8dPuuaLjXtPHzzYuWy6fYEaX9mQQ8oGr&index=23

Chapter 14. Mixtures

Chapter 14. Mixtures Chapter 14 Mixtures Warm Up What is the difference between a heterogeneous and homogeneous mixture? Give 1 example of a heterogeneous mixture and 1 example of a homogeneous mixture. Today s Agenda QOTD:

More information

Solutions & Colloids

Solutions & Colloids Chemistry 100 Bettelheim, Brown, Campbell & Farrell Ninth Edition Introduction to General, Organic and Biochemistry Chapter 6 Solutions & Colloids Solutions Components of a Solution Solvent: The substance

More information

Chapter 6. Solution, Acids and Bases

Chapter 6. Solution, Acids and Bases Chapter 6 Solution, Acids and Bases Mixtures Two or more substances Heterogeneous- different from place to place Types of heterogeneous mixtures Suspensions- Large particles that eventually settle out

More information

Honors Unit 10 Notes Solutions

Honors Unit 10 Notes Solutions Name: Honors Unit 10 Notes Solutions [Chapter 10] Objectives: 1. Students will be able to calculate solution concentration using molarity, molality, and mass percent. 2. Students will be able to interpret

More information

Chemistry 51 Chapter 8 TYPES OF SOLUTIONS. A solution is a homogeneous mixture of two substances: a solute and a solvent.

Chemistry 51 Chapter 8 TYPES OF SOLUTIONS. A solution is a homogeneous mixture of two substances: a solute and a solvent. TYPES OF SOLUTIONS A solution is a homogeneous mixture of two substances: a solute and a solvent. Solute: substance being dissolved; present in lesser amount. Solvent: substance doing the dissolving; present

More information

Chapter 7 Solutions 1

Chapter 7 Solutions 1 1 Chapter 7 Solutions Solutions: Solute and Solvent Solutions are homogeneous mixtures of two or more substances form when there is sufficient attraction between solute and solvent molecules have two components:

More information

Chapter 14 Solutions

Chapter 14 Solutions Chapter 14 Solutions 1 14.1 General properties of solutions solution a system in which one or more substances are homogeneously mixed or dissolved in another substance two components in a solution: solute

More information

A. Types of Mixtures:

A. Types of Mixtures: I. MIXTURES: SOLUTIONS 1) mixture = a blend of two or more kinds of matter, each of which retains its own identity and properties a) homogeneous mixture = a mixture that is uniform in composition throughout

More information

Chemistry B11 Chapter 6 Solutions and Colloids

Chemistry B11 Chapter 6 Solutions and Colloids Chemistry B11 Chapter 6 Solutions and Colloids Solutions: solutions have some properties: 1. The distribution of particles in a solution is uniform. Every part of the solution has exactly the same composition

More information

Properties of Ionic and Covalent Compounds. Intermolecular Forces

Properties of Ionic and Covalent Compounds. Intermolecular Forces Properties of Ionic and Covalent Compounds Intermolecular Forces Physical Properties & Bond Types Physical properties of substances are affected by the attractive forces between particles Greater attraction

More information

Unit 6 Water and Its Properties

Unit 6 Water and Its Properties Unit 6 Water and Its Properties 15.1 Water and Its Properties I. Liquid Water A. Surface Tension 1. Surface Tension a. A force that tends to pull adjacent parts of a liquid's surface together, thereby

More information

Chapter 12: Solutions

Chapter 12: Solutions Chapter 12: Solutions Problems: 3, 5, 8, 12, 14, 16, 22, 29, 32, 41-58, 61-68, 71-74 solution: homogeneous mixture of a solute dissolved in a solvent solute: solvent: component present in smaller amount

More information

Chapter Thirteen. Physical Properties Of Solutions

Chapter Thirteen. Physical Properties Of Solutions Chapter Thirteen Physical Properties Of Solutions 1 Solvent: Solute: Solution: Solubility: Types of Solutions Larger portion of a solution Smaller portion of a solution A homogeneous mixture of 2 or more

More information

Unit 13 Practice Test

Unit 13 Practice Test Name: Class: Date: Unit 13 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1) The dissolution of water in octane (C 8 H 18 ) is prevented by.

More information

Solutions. Occur in all phases. Ways of Measuring. Ways of Measuring. Page 1

Solutions. Occur in all phases. Ways of Measuring. Ways of Measuring. Page 1 Solutions Occur in all phases The solvent does the dissolving. The solute is dissolved. There are examples of all types of solvents dissolving all types of solvent. We will focus on aqueous solutions.

More information

Types of Solutions. Chapter 17 Properties of Solutions. Types of Solutions. Types of Solutions. Types of Solutions. Types of Solutions

Types of Solutions. Chapter 17 Properties of Solutions. Types of Solutions. Types of Solutions. Types of Solutions. Types of Solutions Big Idea: Liquids will mix together if both liquids are polar or both are nonpolar. The presence of a solute changes the physical properties of the system. For nonvolatile solutes the vapor pressure, boiling

More information

Colligative Properties: Freezing Point Depression and Molecular Weight

Colligative Properties: Freezing Point Depression and Molecular Weight Purpose: Colligative Properties: Freezing Point Depression and Molecular Weight The first purpose of this lab is to experimentally determine the van't Hoff (i) factor for two different substances, sucrose

More information

A) HCl C) 52 g KCl in 100 g water at 80ºC A) temperature of the solution increases B) supersaturated D) low temperature and high pressure D) KClO3

A) HCl C) 52 g KCl in 100 g water at 80ºC A) temperature of the solution increases B) supersaturated D) low temperature and high pressure D) KClO3 1. Which compound becomes less soluble in water as the temperature of the solution is increased? A) HCl B) 2. The solubility of O3(s) in water increases as the A) temperature of the solution increases

More information

Solutions. Occur in all phases. Ways of Measuring. Ways of Measuring. Energy of Making Solutions. 1. Break apart Solvent. Page 1

Solutions. Occur in all phases. Ways of Measuring. Ways of Measuring. Energy of Making Solutions. 1. Break apart Solvent. Page 1 s Occur in all phases The solvent does the dissolving. The solute is dissolved. There are examples of all types of solvents dissolving all types of solvent. We will focus on aqueous solutions. Ways of

More information

Intermolecular forces, acids, bases, electrolytes, net ionic equations, solubility, and molarity of Ions in solution:

Intermolecular forces, acids, bases, electrolytes, net ionic equations, solubility, and molarity of Ions in solution: Intermolecular forces, acids, bases, electrolytes, net ionic equations, solubility, and molarity of Ions in solution: 1. What are the different types of Intermolecular forces? Define the following terms:

More information

Chemistry Ch 15 (Solutions) Study Guide Introduction

Chemistry Ch 15 (Solutions) Study Guide Introduction Chemistry Ch 15 (Solutions) Study Guide Introduction Name: Note: a word marked (?) is a vocabulary word you should know the meaning of. A homogeneous (?) mixture, or, is a mixture in which the individual

More information

Chapter 13 Properties of Solutions. Classification of Matter

Chapter 13 Properties of Solutions. Classification of Matter Chapter 13 Properties of Solutions Learning goals and key skills: Describe how enthalpy and entropy changes affect solution formation Describe the relationship between intermolecular forces and solubility,

More information

Lecture 6: Lec4a Chemical Reactions in solutions

Lecture 6: Lec4a Chemical Reactions in solutions Lecture 6: Lec4a Chemical Reactions in solutions Zumdahl 6 th Ed, Chapter 4 Sections 1-6. 4.1 Water, the Common Solvent 4.2 The Nature of Aqueous Solutions: Strong and Weak Electrolytes 4.3 The Composition

More information

SOLUTIONS EXPERIMENT 13

SOLUTIONS EXPERIMENT 13 SOLUTIONS EXPERIMENT 13 OBJECTIVE The objective of this experiment is to demonstrate the concepts of concentrations of solutions and the properties of solution. Colloids will be demonstrated. EQUIPMENT

More information

Freezing Point Depression: Why Don t Oceans Freeze? Teacher Advanced Version

Freezing Point Depression: Why Don t Oceans Freeze? Teacher Advanced Version Freezing Point Depression: Why Don t Oceans Freeze? Teacher Advanced Version Freezing point depression describes the process where the temperature at which a liquid freezes is lowered by adding another

More information

Freezing Point Depression, the van t Hoff Factor, and Molar Mass

Freezing Point Depression, the van t Hoff Factor, and Molar Mass , the van t Hoff Factor, and Molar Mass Objectives To understand colligative properties. To find the freezing point depression of a solution. To determine the van't Hoff factor for acetic acid dissolved

More information

Chapter 13: Properties of Solutions

Chapter 13: Properties of Solutions Chapter 13: Properties of Solutions Problems: 9-10, 13-17, 21-42, 44, 49-60, 71-72, 73 (a,c), 77-79, 84(a-c), 91 solution: homogeneous mixture of a solute dissolved in a solvent solute: solvent: component(s)

More information

Experiment 15-Properties of Solutions

Experiment 15-Properties of Solutions A solution is a combination of a solvent (major component) and a solute (minor component. Solutions are heterogeneous mixtures. They may contain more than one solute. Solutes can contain solid, liquid

More information

COPYRIGHT FOUNTAINHEAD PRESS

COPYRIGHT FOUNTAINHEAD PRESS Colligative Properties of Solutions Freezing Point Depression Objectives: To investigate the colligative property of freezing point depression; to examine the relationship between freezing point depression

More information

CHEMISTRY The Molecular Nature of Matter and Change

CHEMISTRY The Molecular Nature of Matter and Change CHEMISTRY The Molecular Nature of Matter and Change Third Edition Chapter 13 The Properties of Mixtures: Solutions and Colloids Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction

More information

Sample Exercise 13.1 Predicting Solubility Patterns

Sample Exercise 13.1 Predicting Solubility Patterns Sample Exercise 13.1 Predicting Solubility Patterns Predict whether each of the following substances is more likely to dissolve in the nonpolar solvent carbon tetrachloride (CCl 4 ) or in water: C 7 H

More information

Chemistry I Study Guideline - Unit 11: Liquids + Solutions

Chemistry I Study Guideline - Unit 11: Liquids + Solutions Chemistry I Study Guideline - Unit 11: Liquids + Solutions By the end of this chapter the skills you should be able to demonstrate are: 1. Explain the properties of the different phases of matter in terms

More information

2 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.

2 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved. 16.3 Colligative of Solutions > 16.3 Colligative of Solutions > CHEMISTRY & YOU Chapter 16 Solutions 16.1 of Solutions 16.2 Concentrations of Solutions 16.3 Colligative of Solutions 16.4 Calculations Involving

More information

Names of students present in your group

Names of students present in your group Your name Names of students present in your group Lab & Table Number SCI 265: SOLUTIONS AND ELECTROLYTES IONIC AND COVALENT COMPOUNDS 1. What is an ion? 2. What is a molecule? 3. What is the difference

More information

Chapter 13 - Solutions

Chapter 13 - Solutions Chapter 13 - Solutions 13-1 Types of Mixtures I. Solutions A. Soluble 1. Capable of being dissolved B. Solution 1. A homogeneous mixture of two or more substances in a single phase C. Solvent 1. The dissolving

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

SOLUTIONS UNIT. What composition and properties characterize a true solution(five properties)?

SOLUTIONS UNIT. What composition and properties characterize a true solution(five properties)? SOLUTIONS UNIT Assignment #1 How do heterogeneous mixtures differ from homogeneous mixtures? Of the following, which are homogeneous mixtures and which are heterogeneous mixtures: black coffee, household

More information

Test Bank - Chapter 5 Multiple Choice

Test Bank - Chapter 5 Multiple Choice Test Bank - Chapter 5 The questions in the test bank cover the concepts from the lessons in Chapter 5. Select questions from any of the categories that match the content you covered with students. The

More information

Chapter 13: Physical Properties of Solutions

Chapter 13: Physical Properties of Solutions Chapter 13: Physical Properties of Solutions Key topics: Molecular Picture (interactions, enthalpy, entropy) Concentration Units Colligative Properties terminology: Solution: a homogeneous mixture Solute:

More information

5s Solubility & Conductivity

5s Solubility & Conductivity 5s Solubility & Conductivity OBJECTIVES To explore the relationship between the structures of common household substances and the kinds of solvents in which they dissolve. To demonstrate the ionic nature

More information

Chapter 13 Properties of Solutions

Chapter 13 Properties of Solutions Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 13 Properties of are homogeneous mixtures of two or more pure substances. In a solution,

More information

APS Science Curriculum Unit Planner

APS Science Curriculum Unit Planner APS Science Curriculum Unit Planner Grade Level/Subject Chemistry Stage 1: Desired Results Enduring Understanding Topic 6 Solutions: Solutions concentrations can be understood by looking at molar relationships.

More information

Chapter 4: Solution Stoichiometry Cont. Aqueous Solutions

Chapter 4: Solution Stoichiometry Cont. Aqueous Solutions Chapter 4: Solution Stoichiometry Cont. 1 Aqueous Solutions Molarity (dilution calculations, solution stoichiometry); Solubility and Solubility Rules Molecular, Ionic and Net Ionic Equations Precipitation

More information

comparing ionic and covalent bonding.notebook October 16, 2014 Bond strength IMF strength Oct 6 10:43 AM Oct 14 10:06 PM

comparing ionic and covalent bonding.notebook October 16, 2014 Bond strength IMF strength Oct 6 10:43 AM Oct 14 10:06 PM Bond strength IMF strength Oct 6 10:43 AM Oct 14 10:06 PM 1 Oct 14 10:07 PM Oct 14 10:07 PM 2 Oct 14 10:10 PM Oct 14 10:11 PM 3 comparing ionic and covalent bonding.notebook October 16, 2014 Hardness Ionic

More information

CHAPTER 4. AQUEOUS REACTION CHEMISTRY

CHAPTER 4. AQUEOUS REACTION CHEMISTRY CAPTER. AQUEOUS REACTION CEMISTRY solution - homogeneous mixture of or more substances; uniform distribution of particles and same properties throughout. A solution is composed of a solute dissolved in

More information

Chapter 14 The Chemistry of Solutes and Solutions. Solute-Solvent Interactions. Solute-Solvent Interactions. Solute-Solvent Interactions

Chapter 14 The Chemistry of Solutes and Solutions. Solute-Solvent Interactions. Solute-Solvent Interactions. Solute-Solvent Interactions John W. Moore Conrad L. Stanitski Peter C. Jurs Solubility & Intermolecular Forces Solution = homogeneous mixture of substances. It consists of: http://academic.cengage.com/chemistry/moore solvent - component

More information

Solutions. Chapter 13. Properties of Solutions. Lecture Presentation

Solutions. Chapter 13. Properties of Solutions. Lecture Presentation Lecture Presentation Chapter 13 Properties of Yonsei University homogeneous mixtures of two or more pure substances: may be gases, liquids, or solids In a solution, the solute is dispersed uniformly throughout

More information

Solute and Solvent 7.1. Solutions. Examples of Solutions. Nature of Solutes in Solutions. Learning Check. Solution. Solutions

Solute and Solvent 7.1. Solutions. Examples of Solutions. Nature of Solutes in Solutions. Learning Check. Solution. Solutions Chapter 7 s 7.1 s Solute and Solvent s are homogeneous mixtures of two or more substances. consist of a solvent and one or more solutes. 1 2 Nature of Solutes in s Examples of s Solutes spread evenly throughout

More information

Factors that Affect the Rate of Dissolving and Solubility

Factors that Affect the Rate of Dissolving and Solubility Dissolving Factors that Affect the Rate of Dissolving and Solubility One very important property of a solution is the rate of, or how quickly a solute dissolves in a solvent. When dissolving occurs, there

More information

Chapter 5 Student Reading

Chapter 5 Student Reading Chapter 5 Student Reading THE POLARITY OF THE WATER MOLECULE Wonderful water Water is an amazing substance. We drink it, cook and wash with it, swim and play in it, and use it for lots of other purposes.

More information

CHAPTER 13: ANSWERS TO ASSIGNED PROBLEMS Hauser- General Chemistry I revised 8/03/08

CHAPTER 13: ANSWERS TO ASSIGNED PROBLEMS Hauser- General Chemistry I revised 8/03/08 CHAPTER 13: ANSWERS TO ASSIGNED PROBLEMS Hauser- General Chemistry I revised 8/03/08 13.21 The solubility of Cr(NO 3 ) 3 9 H 2 O in water is 208 g per 100 g of water at 15 C. A solution of Cr(NO 3 ) 3

More information

Name Date Class. SECTION 16.1 PROPERTIES OF SOLUTIONS (pages 471 477)

Name Date Class. SECTION 16.1 PROPERTIES OF SOLUTIONS (pages 471 477) 16 SOLUTIONS SECTION 16.1 PROPERTIES OF SOLUTIONS (pages 471 477) This section identifies the factors that affect the solubility of a substance and determine the rate at which a solute dissolves. Solution

More information

EXPERIMENT 10: Electrical Conductivity Chem 111

EXPERIMENT 10: Electrical Conductivity Chem 111 EXPERIMENT 10: Electrical Conductivity Chem 111 INTRODUCTION A. Electrical Conductivity A substance can conduct an electrical current if it is made of positively and negatively charged particles that are

More information

1. Define the term colligative property and list those physical properties of a solution that can be classified as colligative properties.

1. Define the term colligative property and list those physical properties of a solution that can be classified as colligative properties. Solutions Colligative Properties DCI Name Section 1. Define the term colligative property and list those physical properties of a solution that can be classified as colligative properties. Colligative

More information

Two Ways to Form Solutions. Role of Disorder in Solutions 2/27/2012. Types of Reactions

Two Ways to Form Solutions. Role of Disorder in Solutions 2/27/2012. Types of Reactions Role of Disorder in Solutions Disorder (Entropy) is a factor Solutions mix to form maximum disorder Two Ways to Form Solutions 1. Physical Dissolving (Solvation) NaCl(s) Na + (aq) + Cl - (aq) C 12 H 22

More information

Kinetic Molecular Theory (con t) Kinetic Molecular Theory Gas Liquid Solid 1. Slightly 2. High 3. Does not expand to

Kinetic Molecular Theory (con t) Kinetic Molecular Theory Gas Liquid Solid 1. Slightly 2. High 3. Does not expand to Kinetic Energy and (Kelvin) Temperature Temperature is a Kinetic Energy and (Kelvin) Temperature(2) The Kelvin temperature scale is called the Absolute Zero - Zero degrees on the 1. Highly 2. Low 3. Fills

More information

1 Ionic and Covalent Compounds

1 Ionic and Covalent Compounds CHAPTER 3 1 Ionic and Covalent Compounds SECTION Chemical Compounds BEFORE YOU READ After you read this section, you should be able to answer these questions: What are ionic compounds? What are covalent

More information

Chemistry: The Central Science. Chapter 13: Properties of Solutions

Chemistry: The Central Science. Chapter 13: Properties of Solutions Chemistry: The Central Science Chapter 13: Properties of Solutions Homogeneous mixture is called a solution o Can be solid, liquid, or gas Each of the substances in a solution is called a component of

More information

Lab 9. Colligative Properties an Online Lab Activity

Lab 9. Colligative Properties an Online Lab Activity Prelab Assignment Before coming to lab: Lab 9. Colligative Properties an Online Lab Activity Chemistry 162 - K. Marr Revised Winter 2014 This lab exercise does not require a report in your lab notebook.

More information

Introducing Driving Force #3 - Formation of a Solid

Introducing Driving Force #3 - Formation of a Solid Introducing Driving Force #3 - Formation of a Solid In each of the next two types of chemical reactions, the reactants are aqueous solutions Reactants are ionic substances (solutes) dissolved in water

More information

The Properties of Water

The Properties of Water The Properties of Water A water molecule is made up of two hydrogen atoms bonded to an oxygen atom. Each end of a water molecule has a slight electric charge. A molecule that has electrically charged areas

More information

SCH 3UI Unit 9 Outline: Solutions, Acids and Bases

SCH 3UI Unit 9 Outline: Solutions, Acids and Bases SCH 3UI Unit 9 Outline: Solutions, Acids and Bases Lesson Topics Covered Homework Questions and Assignments 1 Note: Introduction to Solutions review of the organization of matter define: solution, solute,

More information

Review - After School Matter Name: Review - After School Matter Tuesday, April 29, 2008

Review - After School Matter Name: Review - After School Matter Tuesday, April 29, 2008 Name: Review - After School Matter Tuesday, April 29, 2008 1. Figure 1 The graph represents the relationship between temperature and time as heat was added uniformly to a substance starting at a solid

More information

Solutes, Solvents, Solutions Dr.Gergens - SD Mesa College

Solutes, Solvents, Solutions Dr.Gergens - SD Mesa College Battles over pure water or IL? ne substance with hydrate your body, the other will dehydrate (a laxative) Euphrates River Tigris River Who has the ultimate control of these waterways? Solutes, Solvents,

More information

Name Solutions Extra Credit

Name Solutions Extra Credit Name Solutions Extra Credit Page 1 1. Which compound is most soluble in water? A) silver acetate B) silver chloride C) silver nitrate D) silver sulfate 2. According to Reference Table F, which compound

More information

Chapter 14 Solutes and Solvents

Chapter 14 Solutes and Solvents Chapter 14 Solutes and Solvents A solution is a homogeneous mixture of two or more substances. The relative abundance of the substances in a solution determines which is the solute and which is the solvent.

More information

Exam 3 Chemistry 65 Summer Score:

Exam 3 Chemistry 65 Summer Score: Name: Exam 3 Chemistry 65 Summer 2015 Score: Instructions: Clearly circle the one best answer 1. The main interactions between molecules of iodine I2 are examples of A) ionic bonds. B) covalent bonds.

More information

SOLUBILITY OF A SALT IN WATER AT VARIOUS TEMPERATURES LAB

SOLUBILITY OF A SALT IN WATER AT VARIOUS TEMPERATURES LAB SOLUBILITY OF A SALT IN WATER AT VARIOUS TEMPERATURES LAB Purpose: Most ionic compounds are considered by chemists to be salts and many of these are water soluble. In this lab, you will determine the solubility,

More information

Unit 4 review for finals

Unit 4 review for finals Unit 4 review for finals These are the topics you should know and be able to answer questions about: 1. Types of compounds a. What are the four types of bonding? Describe each type of bonding. i. Ionic

More information

Solutions. ... the components of a mixture are uniformly intermingled (the mixture is homogeneous). Solution Composition. Mass percentageof solute=

Solutions. ... the components of a mixture are uniformly intermingled (the mixture is homogeneous). Solution Composition. Mass percentageof solute= Solutions Properties of Solutions... the components of a mixture are uniformly intermingled (the mixture is homogeneous). Solution Composition 1. Molarity (M) = 4. Molality (m) = moles of solute liters

More information

Experiment 9 Chem 110 Lab SOLUTIONS I. INTRODUCTION. Polar or Nonpolar? 1 ethanol (ethyl alcohol) C 2 H 6 O. 2 cyclohexane, C 6 H 12

Experiment 9 Chem 110 Lab SOLUTIONS I. INTRODUCTION. Polar or Nonpolar? 1 ethanol (ethyl alcohol) C 2 H 6 O. 2 cyclohexane, C 6 H 12 Experiment 9 Chem 110 Lab SOLUTIONS I. INTRODUCTION A solution is a homogeneous mixture of two (or more) substances. It is composed of a solvent and a dissolved material called a solute. The solute is

More information

ANSWER KEY. Acids, Bases, and Solutions. Chapter Project Worksheet 1 1. Answers will vary. Sample: cherries, blueberries,

ANSWER KEY. Acids, Bases, and Solutions. Chapter Project Worksheet 1 1. Answers will vary. Sample: cherries, blueberries, Chapter Project Worksheet 1 1. Answers will vary. Sample: cherries, blueberries, and grass 2. Answers will vary. Sample: Cut 5 g of cherries into small pieces and place in blender. Blend for two minutes,

More information

The component present in larger proportion is known as solvent.

The component present in larger proportion is known as solvent. 40 Engineering Chemistry and Environmental Studies 2 SOLUTIONS 2. DEFINITION OF SOLUTION, SOLVENT AND SOLUTE When a small amount of sugar (solute) is mixed with water, sugar uniformally dissolves in water

More information

CHAPTER 13: SOLUTIONS

CHAPTER 13: SOLUTIONS CHAPTER 13: SOLUTIONS Problems: 1-8, 11-15, 20-30, 37-88, 107-110, 131-132 13.2 SOLUTIONS: HOMOGENEOUS MIXTURES solution: homogeneous mixture of substances present as atoms, ions, and/or molecules solute:

More information

Experiment #10: Liquids, Liquid Mixtures and Solutions

Experiment #10: Liquids, Liquid Mixtures and Solutions Experiment #10: Liquids, Liquid Mixtures and Solutions Objectives: This experiment is a broad survey of the physical properties of liquids. We will investigate solvent/solute mixtures. We will study and

More information

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) All of the following statements describing solutions are true except A) Solutions are homogeneous.

More information

The Solution Process CHEMISTRY. Properties of Solutions. The Central Science. Prof. Demi Levendis Room GH807 Gate House

The Solution Process CHEMISTRY. Properties of Solutions. The Central Science. Prof. Demi Levendis Room GH807 Gate House CHEMISTRY The Central Science Properties of Solutions The Solution Process Solutions: Air; brass; body fluids; sea water When a solution forms some questions we can ask are: What happens on a molecular

More information

Heterogeneous Homogenous. Mixtures; Solutions. Phases of matter: Solid. Phases of Matter: Liquid. Phases of Matter: Gas. Solid, Liquid, Gas

Heterogeneous Homogenous. Mixtures; Solutions. Phases of matter: Solid. Phases of Matter: Liquid. Phases of Matter: Gas. Solid, Liquid, Gas Phases of matter: Solid Heterogeneous Homogenous Mixtures Solutions Phases of Matter: Liquid Atoms and molecules are more spaced out and now can move. The material can be slightly compressed into a smaller

More information

Element of same atomic number, but different atomic mass o Example: Hydrogen

Element of same atomic number, but different atomic mass o Example: Hydrogen Atomic mass: p + = protons; e - = electrons; n 0 = neutrons p + + n 0 = atomic mass o For carbon-12, 6p + + 6n 0 = atomic mass of 12.0 o For chlorine-35, 17p + + 18n 0 = atomic mass of 35.0 atomic mass

More information

CHAPTER 14 Solutions

CHAPTER 14 Solutions CHAPTER 14 Solutions The Dissolution Process 1. Effect of Temperature on Solubility 2. Molality and Mole Fraction Colligative Properties of Solutions 3. Lowering of Vapor Pressure and Raoult s Law 4. Fractional

More information

12.3 Colligative Properties

12.3 Colligative Properties 12.3 Colligative Properties Changes in solvent properties due to impurities Colloidal suspensions or dispersions scatter light, a phenomenon known as the Tyndall effect. (a) Dust in the air scatters the

More information

SOLUTE - SOLVENT SYSTEM

SOLUTE - SOLVENT SYSTEM SOLUTIONS: SOLUTE - SOLVENT SYSTEM SCH4U_08 09 Solubility The term solubility is commonly used in two senses qualitatively and quantitatively. Qualitatively, solubility is often used in a relative way

More information

Chapter 13 Solution Dynamics. An Introduction to Chemistry by Mark Bishop

Chapter 13 Solution Dynamics. An Introduction to Chemistry by Mark Bishop Chapter 13 Solution Dynamics An Introduction to Chemistry by Mark Bishop Chapter Map Why Changes Happen Consider a system that can switch freely between two states, A and B. Probability helps us to predict

More information

Solutions Review Questions

Solutions Review Questions Name: Thursday, March 06, 2008 Solutions Review Questions 1. Compared to pure water, an aqueous solution of calcium chloride has a 1. higher boiling point and higher freezing point 3. lower boiling point

More information

SAM Teachers Guide Solubility

SAM Teachers Guide Solubility SAM Teachers Guide Solubility Overview In this activity students explore solutions. They create models of solutions and discover the dissolving process involves a consideration of the intermolecular attractive

More information

What is a Colligative Property?

What is a Colligative Property? What is a Colligative Property? 0 Defined as bulk liquid properties that change when you add a solute to make a solution 0 Colligative properties are based on how much solute is added but NOT the identity

More information

Unit 1 Building Blocks

Unit 1 Building Blocks Unit 1 Building Blocks a) Substances (i) Elements Everything in the world is made from about 100 elements. Each element has a name and a symbol. Elements are classified in different ways, including naturallyoccurring/made

More information

Name Lab #3: Solubility of Organic Compounds Objectives: Introduction: soluble insoluble partially soluble miscible immiscible

Name  Lab #3: Solubility of Organic Compounds Objectives: Introduction: soluble insoluble partially soluble miscible immiscible Lab #3: Solubility of rganic Compounds bjectives: - Understanding the relative solubility of organic compounds in various solvents. - Exploration of the effect of polar groups on a nonpolar hydrocarbon

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

David A. Katz Department of Chemistry Pima Community College

David A. Katz Department of Chemistry Pima Community College Solutions David A. Katz Department of Chemistry Pima Community College A solution is a HOMOGENEOUS mixture of 2 or more substances in a single phase. One constituent t is usually regarded as the SOLVENT

More information

Chapter 3 Molecules, Moles, and Chemical Equations. Chapter Objectives. Warning!! Chapter Objectives. Chapter Objectives

Chapter 3 Molecules, Moles, and Chemical Equations. Chapter Objectives. Warning!! Chapter Objectives. Chapter Objectives Larry Brown Tom Holme www.cengage.com/chemistry/brown Chapter 3 Molecules, Moles, and Chemical Equations Jacqueline Bennett SUNY Oneonta 2 Warning!! These slides contains visual aids for learning BUT they

More information

Chapter 13: Solutions

Chapter 13: Solutions Ch 13 Page 1 Chapter 13: Solutions SOLUTION: A homogeneousmixture of two or more substances Composition can vary from one sample to another Appears to be one substance, though really contains multiple

More information

Conductivity of Electrolytes in Solution

Conductivity of Electrolytes in Solution Conductivity of Electrolytes in Solution Introduction: Electrical current can be thought of as the movement of electrons or ionic charges from an area of high potential to an area of low potential. Materials

More information

Freezing Point Depression: Why Don t Oceans Freeze? Teacher Version

Freezing Point Depression: Why Don t Oceans Freeze? Teacher Version Freezing Point Depression: Why Don t Oceans Freeze? Teacher Version Freezing point depression describes the process where the temperature at which a liquid freezes is lowered by adding another compound.

More information

Unit 10: Solutions. Student Name: Key. Class Period: _3, 5, & 10_. Page 1 of 61. Website upload

Unit 10: Solutions. Student Name: Key. Class Period: _3, 5, & 10_. Page 1 of 61. Website upload Unit 10: Solutions Student Name: Class Period: _3, 5, & 10_ Page 1 of 61 Page intentionally blank Page 2 of 61 Unit 10 Vocabulary: 1. Aqueous: A solution in which the solvent is water. 2. Colligative Property:

More information

Chemistry. Stage 1 Desired Results Kelly Clark, Kelly Puder, Sheryl Rabinowitz, Sarah Warren

Chemistry. Stage 1 Desired Results Kelly Clark, Kelly Puder, Sheryl Rabinowitz, Sarah Warren Chemistry 2013-2014 Kelly Clark, Kelly Puder, Sheryl Rabinowitz, Sarah Warren Unit 5: Solutions and Acids and Base Transfer Goal: I want you to learn that most solids, liquids, and gases are mixtures so

More information

0.279 M Change g to mol: g/mol = mol Molarity = mol L = mol 0.325L = M

0.279 M Change g to mol: g/mol = mol Molarity = mol L = mol 0.325L = M 118 ChemQuest 39 Name: Date: Hour: Information: Molarity Concentration is a term that describes the amount of solute that is dissolved in a solution. Concentrated solutions contain a lot of dissolved solute,

More information

Solutions Thermodynamics DCI

Solutions Thermodynamics DCI Solutions Thermodynamics DCI Name Section 1. The three attractive interactions which are important in solution formation are; solute-solute interactions, solvent-solvent interactions, and solute-solvent

More information

1/27/2014. Chapter 12. Solutions. Thirsty Seawater. Seawater. Seawater. Homogeneous Mixtures. Seawater. Lecture Presentation

1/27/2014. Chapter 12. Solutions. Thirsty Seawater. Seawater. Seawater. Homogeneous Mixtures. Seawater. Lecture Presentation Lecture Presentation Chapter 12 Solutions Sherril Soman, Grand Valley State University Thirsty Seawater Drinking seawater can cause dehydration. Seawater Is a homogeneous mixture of salts with water Contains

More information

Chapter 12. Solutions. Lecture Presentation

Chapter 12. Solutions. Lecture Presentation 12.1 Thirsty Solutions: Why You Shouldn t Drink Seawater 544 12.2 Types of Solutions and Solubility 546 12.3 Energetics of Solution Formation 551 12.4 Solution Equilibrium and Factors Affecting Solubility

More information