# Honors Unit 10 Notes Solutions

 To view this video please enable JavaScript, and consider upgrading to a web browser that supports HTML5 video
Save this PDF as:

Size: px
Start display at page:

## Transcription

1 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 solubility curves and to predict the effect of temperature and pressure on the solubility of solids and gases. 3. Students will be able to calculate freezing points and boiling points of solutions based on the theory and equations describing colligative properties of solutions both for electrolytes and nonelectrolytes. Vocabulary Solution o Every solution contains a solute and a solvent. Solute Solvent o The solute gets dissolved in the solvent! Colloids o Colloids may look clear when dilute enough. o Examples: Tyndall effect o Causes the beam of light to become visible o Why you can see rays from the sun sometimes!

2 2 Suspension a mixture from which the particles settle out slowly upon standing o o Suspensions can be! o Examples: Concentration Concentration of a solution = the amount of in a given quantity of o A solution contains a relatively amount of solute vs. the solvent o A solution contains a relatively amount of solute vs. the solvent Concentrated and dilute aren t very quantitative though! Quantitative Concentration Values: 1. Molarity 2. Mass Percent 3. Molality Molarity (Review from Unit 4) Molarity (M) moles of solute liters of solution Example #1: What is the molarity of a solution made by dissolving 12.5 g of oxalic acid (H2C2O4) in 456 ml of solution?

3 Example #2: How many grams of sodium carbonate (Na2CO3) are needed to prepare L of an aqueous M solution? 3 Mass Percent mass of solute percent by mass *100 mass of solution Example #3: What is the percent by mass of the solute in a solution made by adding 1.20 g of methyl alcohol (CH3OH) to 16.8 g of water? Molality (m) Why use molality if you can use molarity instead? o Molarity varies with temperature due to the exapansion or contraction in the volume of the solution o Molality does not change with temperature since it s based on the mass of solvent added (instead of a volume). molesof solute Molality ( m ) kilogramsof solvent

4 Example #4: A solution contains 15.5 g of a compound, NH2CONH2, in 74.3 g of water. Calculate the molality of the solution. 4 Dilution of Solutions Dilutions are used to the concentration (or molarity) of a soln. Example #5: How would you prepare L of M Na2CO3 starting with 1.33 M solution? Example #6: Copper sulfate is widely used as a dietary supplement for animal feed. A lab technician prepares a stock solution of CuSO4 by adding g of CuSO4 to enough water to make ml of solution. An experiment requires a M solution of CuSO4. (a) What is the molarity of the CuSO4 stock solution prepared by the technician? (b) How would you prepare L of a M solution from the stock solution?

5 Solubility 5 Vocabulary two liquids that are soluble in each other (mix in all proportions) liquids that are insoluble in each other (do not mix) contains the maximum amount of dissolved solute contains less than the maximum amount of dissolved solute contains more solute than can theoretically be dissolved at a given temperature o A supersaturated solution is created when a warm, saturated solution is allowed to cool without the precipitation of the excess solute. o Testing for Saturation: Add crystal of a solid and watch for crystallization. the maximum amount of solute that will dissolve in a given quantity of solvent at a specific temperature and pressure to produce a saturated soln. 1. Units: 2. Example: At 20 C, NaNO3 has a solubility of 74 g/100 grams of water. Factors which influence solubility: Like Dissolve Like The concentration of the solute in a saturated solution (the solubility) can be shown on a graph or curve called a solubility curve.

6 Solubility Curves Example #7: What mass of solute will dissolve in 100 g of water at the following temperatures? 6 a) KNO3 at 70 C b) NaCl at 100 C Example #8: At 20 C, if 100 grams of NaNO3 are dissolved in 100 grams of water, is this solution saturated, unsaturated, or supersaturated? Example #9: Which term - saturated, unsaturated, or supersaturated - best describes a solution that contains 70 g of NaNO3 per 50 g H2O at 30 C? Example #10: Which term - saturated, unsaturated, or supersaturated - best describes a solution that contains 70 g of dissolved KCl per 200 g H2O at 80 C? Example #11: Determine the molality of a saturated NaCl solution at 25 C.

7 Solubility of Gases 7 A. Effect of temperature Most gases become in liquids as the temperature. o Example: B. Effect of pressure Pressure has a major effect on the solubility of a gas in a liquid, but little effect on other systems. Henry s Law at low to moderate pressure the concentration of a gas with the pressure o Colligative Properties When adding a solute to a solvent, the properties of the solvent are modified: Vapor pressure Melting point Boiling point These changes are called Colligative means. o Depends only on the of dissolved particles, not on the of the dissolved particles. o Examples of colligative properties:

8 Boiling Point Elevation Boiling occurs when equals 8 The boiling point of a is than the boiling point of the. o Dissolving substances increases ( ) the boiling point of a solvent. Example: Formula for Boiling Point Elevation: kb = i= Van t Hoff factor= # of ions in solution (1 for all nonelectrolytes) m = ΔTb = Freezing Point Depression The freezing point of a is lower than the freezing point of the. o Dissolving substances lowers ( ) the freezing point of a solvent. o Example:

9 ***Example: Antifreeze (ethylene glycol in water) prevents car s radiator from boiling over in the summer (raises boiling point of water) & prevents car s radiator from freezing in the winter (lowers freezing point of water) 9 Formula for Freezing Point Depression: kf = i= Van t Hoff factor= # of ions in solution (1 for all nonelectrolytes) m = ΔTf = Electrolytes Soluble ionic compounds. When they dissolve in solution, they dissociate completely into ions and conduct Example: NaCl (aq) Covalent (molecular) molecules in aqueous solution: o Covalent particles don t dissociate in solution, so the # of molecules = # of particles ***The greater the product of molality and number of ions, the the boiling point elevation or freezing point depression!

10 Example #12: Calculate the boiling point of solution that contains 50.0 g of glucose, C6H12O6, in 400 g of water. The molal boiling point constant of water is 0.52 o C/m. 10 Example #13: Rank the following aqueous solutions in order of lowest to highest melting point: (1) m C6H12O6 (3) m HCl (2) m MgCl2 (4) m Al2(SO4)3

### 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:

### 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,

### 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

### 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:

### Solutions. How Solutions Form

Solutions How Solutions Form Solvent substance doing the dissolving, present in greater amount Definitions Solution - homogeneous mixture Solute substance being dissolved Definitions Solute - KMnO 4 Solvent

### 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

### 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

### 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

### Chapter 13. Properties of Solutions

13.4 Ways of Expressing Concentration All methods involve quantifying the amount of solute per amount of solvent (or solution). Concentration may be expressed qualitatively or quantitatively. The terms

### 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

### Chapter 7, Reactions and Solutions

1. Classify the following reaction as precipitation, acid-base or oxidation-reduction: Ce4+(aq) + Fe2+(aq) Ce3+(aq) + Fe3+(aq) Ans. oxidation-reduction 2. Classify the following reaction as precipitation,

### 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.

### 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

### 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

### 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

### 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

### 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,

### 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.

### Colligative Properties - Freezing Point Depression

Purpose To observe freezing point depression of different solutions and calculate the molar mass of commercial antifreeze. Introduction In winter, trucks dispense dirt and salt onto the roads and antifreeze

### From the book (10, 12, 16, 18, 22, 24 52, 54, 56, 58, 62, 64, 66, 68, 74, 76, 78, 80, 82, 86, 88, 90, 92, 106 and 116)

Chem 112 Solutions From the book (10, 12, 16, 18, 22, 24 52, 54, 56, 58, 62, 64, 66, 68, 74, 76, 78, 80, 82, 86, 88, 90, 92, 106 and 116) 1. Which of the following compounds are nonelectrolytes? A. NaF

### SOLUBILITY CURVES WORKSHEET

SOLUBILITY CURVES WORKSHEET 1.) Which compound is least soluble at 20 o C? At 80 o C? 2.) Which substance is the most soluble at 10 o C? At 50 o C? At 90 o C? 3.) The solubility of which substance is most

### 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

### 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

### 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.

### 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

### 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

### 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

### 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

### 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

### 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

### 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

### 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

### 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

### 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

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

### Molarity Practice Worksheet

Molarity Practice Worksheet Find the molarity of the following solutions: 1) 0.5 moles of sodium chloride is dissolved to make 0.05 liters of solution. 2) 0.5 grams of sodium chloride is dissolved to make

### Concentration of Solutions and Molarity

Concentration of Solutions and Molarity The concentration of a solution is a measure of the amount of solute that is dissolved in a given quantity of solvent. A dilute solution is one that contains a small

### 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

### 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

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

A.P. Chemistry Practice Test: Ch. 11, Solutions Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Formation of solutions where the process is

### 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

### 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

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

### 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.

### 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)

### 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:

### Colligative Properties

Colligative Properties Say Thanks to the Authors Click http://www.ck12.org/saythanks (No sign in required) To access a customizable version of this book, as well as other interactive content, visit www.ck12.org

### 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

### Chapter 13. Properties of Solutions

Sample Exercise 13.1 (p. 534) By the process illustrated below, water vapor reacts with excess solid sodium sulfate to form the hydrated form of the salt. The chemical reaction is Na 2 SO 4(s) + 10 H 2

### 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

### 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.

### 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

### Determination of Molar Mass by Freezing-Point Depression

DETERMINATION OF MOLAR MASS BY FREEZING-POINT DEPRESSION 141 Determination of Molar Mass by Freezing-Point Depression OBJECTIVES: Gain familiarity with colligative properties of nonelectrolyte solutions

### 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:

### 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

### 2. Why does the solubility of alcohols decrease with increased carbon chain length?

Colligative properties 1 1. What does the phrase like dissolves like mean. 2. Why does the solubility of alcohols decrease with increased carbon chain length? Alcohol in water (mol/100g water) Methanol

### 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.

### 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

### Colligative Properties of Nonvolatile Solutes 01. Colligative Properties of Nonvolatile Solutes 02. Colligative Properties of Nonvolatile Solutes 04

Colligative Properties of Nonvolatile Solutes 01 Colligative Properties of Nonvolatile Solutes 02 Colligative Properties: Depend on the amount not on the identity There are four main colligative properties:

### COLLIGATIVE PROPERTIES:

COLLIGATIVE PROPERTIES: A colligative property is a property that depends only on the number of solute particles present, not their identity. The properties we will look at are: lowering of vapor pressure;

### a) Consider mixing two liquids where mixing is exothermic ( Hsoln < 0). Would you expect a solution to form (yes/maybe/no)? Justify your answer.

Problems - Chapter 13 (with solutions) 1) The following question concerns mixing of liquids. a) Consider mixing two liquids where mixing is exothermic (Hsoln < 0). Would you expect a solution to form (yes/maybe/no)?

### Determination of Molar Mass by Boiling Point Elevation of Urea Solution

Determination of Molar Mass by Boiling Point Elevation of Urea Solution CHRISTIAN E. MADU, PhD AND BASSAM ATTILI, PhD COLLIN COLLEGE CHEMISTRY DEPARTMENT Purpose of the Experiment Determine the boiling

### Review of Basic Concepts, Molarity, Solutions, Dilutions and Beer s Law

Review of Basic Concepts, Molarity, Solutions, Dilutions and Beer s Law Aqueous Solutions In Chemistry, many reactions take place in water. This is also true for Biological processes. Reactions that take

### 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

### 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

### 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

### 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

### 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

### SAMPLE PROBLEM 8.1. Solutions of Electrolytes and Nonelectrolytes SOLUTION STUDY CHECK

Solutions of Electrolytes and Nonelectrolytes SAMPLE PROBLEM 8.1 Indicate whether solutions of each of the following contain only ions, only molecules, or mostly molecules and a few ions: a. Na 2 SO 4,

### Colligative Properties Discussion Chem. 1A

Colligative Properties Discussion Chem. 1A The material covered today is found in sections Chapter 12.5 12.7 This material will not be covered in lecture, you will have homework assigned. Chem. 1A Colligative

### To calculate the value of the boiling point constant for water. To use colligative properties to determine the molecular weight of a substance.

Colligative Properties of Solutions: A Study of Boiling Point Elevation Amina El-Ashmawy, Collin County Community College (With contributions by Timm Pschigoda, St. Joseph High School, St. Joseph, MI)

### 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,

### 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

### Version 001 Calculating Concentrations WKST vanden bout (51165) 1

Version 001 Calculating Concentrations WKST vanden bout (51165 1 This print-out should have 22 questions. Multiple-choice questions may continue on the next column or page find all choices before answering.

### 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

### 1) What is the overall order of the following reaction, given the rate law?

PRACTICE PROBLEMS FOR TEST 2 (March 11, 2009) 1) What is the overall order of the following reaction, given the rate law? A) 1st order B) 2nd order C) 3rd order D) 4th order E) 0th order 2NO(g) + H 2(g)

### Guide to Chapter 11. Solutions and their properties

Guide to Chapter 11. Solutions and their properties We will spend three lecture days on this chapter. You may want to start by reviewing the concepts of heterogeneous solutions (Chapter 2) Read the introductory

### Observe and measure the effect of a solute on the freezing point of a solvent. Determine the molar mass of a nonvolatile, nonelectrolyte solute

Chapter 10 Experiment: Molar Mass of a Solid OBJECTIVES: Observe and measure the effect of a solute on the freezing point of a solvent. Determine the molar mass of a nonvolatile, nonelectrolyte solute

### Calculation of Molar Masses. Molar Mass. Solutions. Solutions

Molar Mass Molar mass = Mass in grams of one mole of any element, numerically equal to its atomic weight Molar mass of molecules can be determined from the chemical formula and molar masses of elements

### 13.3 Factors Affecting Solubility Solute-Solvent Interactions Pressure Effects Temperature Effects

Week 3 Sections 13.3-13.5 13.3 Factors Affecting Solubility Solute-Solvent Interactions Pressure Effects Temperature Effects 13.4 Ways of Expressing Concentration Mass Percentage, ppm, and ppb Mole Fraction,

### Molarity is used to convert between moles of substance and liters of solution.

Appendix C Molarity C.1 MOLARITY AND THE MOLE The molar mass is the mass of a mole of a pure substance while the molarity, M, is the number of moles of a pure substance contained in a liter of a solution.

### REVIEW QUESTIONS Chapter 8

Chemistry 51 ANSWER KEY REVIEW QUESTIONS Chapter 8 1. Identify each of the diagrams below as strong electrolyte, weak electrolyte or non-electrolyte: (a) Non-electrolyte (no ions present) (b) Weak electrolyte

### Colligative Properties

CH302 LaBrake and Vanden Bout Colligative Properties PROBLEM #1: Give the molecular formula, the van t hoff factor for the following Ionic Compounds as well as guess the solubility of the compounds. If

### 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

### 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:

### Osmolality Explained. Definitions

Osmolality Explained What is osmolality? Simply put, osmolality is a measurement of the total number of solutes in a liquid solution expressed in osmoles of solute particles per kilogram of solvent. When

### Unit 3: Solubility Equilibrium

Unit 3: Chem 11 Review Preparation for Chem 11 Review Preparation for It is expected that the student understands the concept of: 1. Strong electrolytes, 2. Weak electrolytes and 3. Nonelectrolytes. CHEM

### 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

### 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

### Vapor Pressure Lowering

Colligative Properties A colligative property is a property of a solution that depends on the concentration of solute particles, but not on their chemical identity. We will study 4 colligative properties

### 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

### 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

### 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

### Molecular Mass by Freezing Point Depression

Molecular Mass by Freezing Point Depression Kyle Miller November 28, 2006 1 Purpose The purpose of this experiment is to determine the molecular mass of organic compounds which are dissolved in a solvent

### EVALUATION OF DEICER AND ANTIFREEZE PERFORMANCE

Experiment 34 EVALUATION OF DEICER AND ANTIFREEZE PERFORMANCE FV 1/11 MATERIALS: PURPOSE: beakers: 400 ml; 150 ml; 100 ml (3); 50 ml (2); 10 ml and 25 ml graduated cylinders; thermometer; 25 x 200 mm test

### 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

### Chapter 11 Properties of Solutions

Chapter 11 Properties of Solutions 11.1 Solution Composition A. Molarity moles solute 1. Molarity ( M ) = liters of solution B. Mass Percent mass of solute 1. Mass percent = 1 mass of solution C. Mole