Chapter 13. Ions in aqueous Solutions And Colligative Properties
|
|
- Abigail Turner
- 5 years ago
- Views:
Transcription
1 Chapter 13 Ions in aqueous Solutions And Colligative Properties
2 Compounds in Aqueous Solution Dissociation The separation of ions that occurs when an ionic compound dissolves H2O NaCl (s) Na+ (aq) + Cl- (aq) H2O MgCl2 (s) Mg2+ (aq) + 2 Cl- (aq)
3 Assuming 100% dissociation 1 mole NaCl in water -> 1 mole Na+ and 1 mole Cl- =2 mole of solute ions 1 mole CaCl2 -> 1 mole of Ca and 2 mol of Cl- = 3 mole of solute ions
4 Do practice page 436
5 Remember must represent the facts when writing an equation Some substances do not remain soluble in solution. Use table 437 and 860 to determine solubility
6 Net Ionic Equations Show the compounds and ions that undergo a chemical change in a reaction in an aq soln. To create an ionic equation, must convert a balanced chemical equation into an ionic eq. ALL soluble ionic compounds are shown as dissociated ions in soln.
7 Ionic equations 2HCl (aq) + Na2O (aq) -> 2NaCl (aq) + H20 (l) 2H+ (aq) + 2Cl- (aq) + 2Na+ (aq) + O2- (aq) 2 Na+ (aq) + 2 Cl- (aq) + H20 (l)
8 Spectator Ions Ions that do not take part in a chemical reaction and are found in solution both before and after the reaction To convert an ionic equation into a net ionic equation, remove the spectator ions from both sides of the equation The ions and compounds left after the spectator ions are removed is called the net ionic equation
9 See practice page 440
10 Ionization Molecular compounds can also form ions in solution Ionization means creating ions where there were none H2O HCl (g) - H+ (aq) + Cl- (aq)
11 Hydronium Ion Molecular compounds often contain Hydrogen bonded by a polar covalent bond. Some of the compounds ionize in an aq. Solution to release H+, the H+ ion has such a high reactivity that it attaches itself to water to form H3O+ or the hydronium ion (ACIDS) HCl (g) + H2O H3O+ (aq) + Cl- (aq)
12 Electrolytes Strong electrolytes Any compound whose dilute aqueous solutions conduct electricity well Caused by almost all solutes existing as ions in solution Weak electrolytes Any compound whose dilute aqueous solutions conduct electricity poorly Caused by very small amounts of solute existing as ions in solution
13 Homework: Do section review page 443 page 458 #2, 8-13
14 Colligative Properties of Soln. Properties that depend on the concentration of solute particles but not on their identity These include: freezing point, boiling point, vapor pressure, osmotic pressure,
15 Raoult's Law and Vapor Pressure Lowering Bp and Fp of soln differ from those of pure solvents When Nonvolatile solutes (a substance that has little tendency to become a gas under existing conditions) added to a liquid to form a solution, the vapor pressure above that solution decreases.
16 Liquid molecules at the surface of a liquid can escape to the gas phase when they have a sufficient amount of energy to break free of the liquid's intermolecular forces. That vaporization process is reversible. Gaseous molecules coming into contact with the surface of a liquid can be trapped by intermolecular forces in the liquid. Eventually the rate of escape will equal the rate of capture to establish a constant, equilibrium vapor pressure above the pure liquid.
17 If add a nonvolatile solute to that liquid, the amount of surface area available for the escaping solvent molecules is reduced because some of that area is occupied by solute particles. the solvent molecules will have a lower probability to escape the solution than the pure solvent.
18 The Vapor Pressure of a Solution is Lower than that of the Pure Solvent
19 The French chemist Francois Raoult discovered the law that mathematically describes the vapor pressure lowering phenomenon. Raoult's law states: the vapor pressure of an ideal solution is dependent on the vapor pressure of each chemical component and the mole fraction of the component present in the solution. Once the components in the solution have reached equilibrium, the total vapor pressure p of the solution is:
20 and the individual vapor pressure for each component is: Where p* is the vapor pressure of the pure component x is the mole fraction of the component in solution
21 Solutions that obey Raoult's law are called ideal solutions because they behave exactly as we would predict. Solutions that show a deviation from Raoult's law are called non-ideal solutions because they deviate from the expected behavior. Very few solutions actually approach ideality, but Raoult's law for the ideal solution is a good enough approximation for the non- ideal solutions
22 Freezing Point Depression describes the phenomenon that the freezing point of a liquid (a solvent) is depressed when another compound is added, meaning that a solution has a lower freezing point than a pure solvent. This happens whenever a solute is added to a pure solvent, such as water. The phenomenon may be observed in sea water, which due to its salt content remains liquid at temperatures below 0 C, the freezing point of pure water. The freezing point depression happens both when the solute is an electrolyte, such as various salts, and a nonelectrolyte
23 ΔT f = K f m B ΔT f, the freezing point depression, is defined as T f (pure solvent) T f (solution), the difference between the freezing point of the pure solvent and the solution. It is defined to assume positive values when the freezing point depression takes place. K f, the cryoscopic constant, which is dependent on the properties of the solvent. It can be calculated as K f = RT m2 M/ΔH f, where R is the gas constant, T m is the melting point of the pure solvent in kelvin, M is the molar mass of the solvent, and ΔH f is the heat of fusion per mole of the solvent. (LOOK THESE UP) m B is the molality of the solution, van 't Hoff factor i as m B = m solute i. The factor i accounts for the number of individual particles (typically ions) formed by a compound in solution. Examples: i = 1 for sugar in water i = 2 for sodium chloride in water, due to dissociation of NaCl into Na + and Cl - i = 3 for calcium chloride in water, due to dissociation of CaCl 2 into Ca 2+ and 2 Cl - i = 2 for hydrogen chloride in water, due to complete dissociation of HCl into H + and Cl -
24 Kf of nonelectrolytes is *C/m *C is celsius degree m is mol solute/kg solvent Kf of electrolytes may be looked up See page 448 for examples
25 Boiling Point Elevation Nonvolatile solutes elevate the bp of the solvent Molal boiling point constant is the boiling point elevation of the solvent in a 1-molal solution of a nonvolatile, nonelectrolyte solute Water is.51 *C/m
26 ΔT b = K b m B ΔT b, the boiling point elevation, is defined as T b (solution) - T b (pure solvent). K b, the ebullioscopic constant, which is dependent on the properties of the solvent. It can be calculated as K b = RT b2 M/ΔH v, where R is the gas constant, and T b is the boiling temperature of the pure solvent, M is the molar mass of the solvent, and ΔH v is the heat of vaporization per mole of the solvent. m B is the molality of the solution, calculated by taking dissociation into account since the boiling point elevation is a colligative property, dependent on the number of particles in solution. This is most easily done by using the van 't Hoff factor i as m B = m solute i. The factor i accounts for the number of individual particles (typically ions) formed by a compound in solution. Examples: i = 1 for sugar in water i = 2 for sodium chloride in water, due to the full dissociation of NaCl into Na + and Cl - i = 3 for calcium chloride in water, due to dissociation of CaCl 2 into Ca 2+ and 2Cl -
27 Do practice page 450 and 451
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 informationIons 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 informationSlide 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 informationPhysical 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 informationProperties 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 informationStudyHub: 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 informationSoluble: 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 informationMixtures. 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 informationBig 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 informationChapter 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 informationChapter 10: CHM 2045 (Dr. Capps)
Phase Diagram Phase diagrams for CO 2 and H 2 O Chapter 13. Solutions and Their Physical Properties Shows pressures and temperatures at which gaseous, liquid, and solid phases can exist. Allows us to predict
More informationChapter 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 informationChapter 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 informationPHYSICAL 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 informationChapter 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 informationColligative 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 informationHonors Chemistry Unit 4 Exam Study Guide Solutions, Equilibrium & Reaction Rates
Honors Chemistry Unit 4 Exam Study Guide Solutions, Equilibrium & Reaction Rates Define the following vocabulary terms. Solute Solvent Solution Molarity Molality Colligative property Electrolyte Non-electrolyte
More informationCP 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 informationUnit 7. Solution Concentrations and Colligative Properties
Unit 7 Solution Concentrations and Colligative Properties Molarity Most widely used concentration unit [HCl] means concentration of HCl in mol/l Notice volume is total volume of solution Molarity (M)=
More informationColligative Properties
Slide 1 Colligative Properties Practical uses of solutions Slide 2 Units of Concentration Whatever units you use, the goal is the same: specify the quantity of 1 component (the solute s ) relative to the
More informationMolality. 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 informationSOLUTION 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 informationCOLLIGATIVE 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- 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 informationName 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 informationAnnouncements. 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 informationSample 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 informationDATE: POGIL: Colligative Properties Part 1
NAME: AP Chemistry DATE: POGIL: Colligative Properties Part 1 Why? There is a general misconception that adding sodium chloride to cooking water for pasta increases the temperature of the boiling water
More informationSolutions. 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 informationAP 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 information70 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 informationA.% by mass (like % composition)
Solutions; Colloids Key Words Solute Solvent Solubility effervescence Miscible saturated Supersaturated (metastable system)- a cooled solution contains more solute than it would at equilibrium, desolvation=
More informationconcentration 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- 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 informationFreezing 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 information7.02 Colligative Properties
7.02 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 informationSoln 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 informationAP 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 informationPhysical 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 informationFind 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 informationBushra 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 informationColligative Properties
Colligative Properties! Consider three beakers: " 50.0 g of ice " 50.0 g of ice + 0.15 moles NaCl " 50.0 g of ice + 0.15 moles sugar (sucrose)! What will the freezing temperature of each beaker be? " Beaker
More informationPhysical 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 informationWarm 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 informationChapter 11: Properties of Solutions - Their Concentrations and Colligative Properties. Chapter Outline
Chapter 11: Properties of Solutions - Their Concentrations and Colligative Properties Chapter Outline 11.1 Energy Changes when Substances Dissolve 11.2 Vapor Pressure 11.3 Mixtures of Volatile Substances
More informationChapter 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 informationSolutions. Solution Formation - Types of Solutions - Solubility and the Solution Process - Effects of Temperature and Pressure on Solubility
Solutions Solutions Solution Formation - Types of Solutions - Solubility and the Solution Process - Effects of Temperature and Pressure on Solubility Colligative Properties - Ways of Expressing Concentration
More informationChapter 11: Properties of Solutions - Their Concentrations and Colligative Properties. Chapter Outline
Chapter 11: Properties of Solutions - Their Concentrations and Colligative Properties Chapter Outline 11.1 Energy Changes when Substances Dissolve 11.2 Vapor Pressure 11.3 Mixtures of Volatile Substances
More informationChapter 11 Properties of Solutions
Chapter 11 Properties of Solutions Solutions Homogeneous mixtures of two or more substances Composition is uniform throughout the sample No chemical reaction between the components of the mixture Solvents
More informationSOLUTIONS. Dissolution of sugar in water. General Chemistry I. General Chemistry I CHAPTER
11 CHAPTER SOLUTIONS 11.1 Composition of Solutions 11.2 Nature of Dissolved Species 11.3 Reaction Stoichiometry in Solutions: Acid-Base Titrations 11.4 Reaction Stoichiometry in Solutions: Oxidation-Reduction
More informationLesson 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 informationCOLLIGATIVE 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 information2 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 informationSolutions: Physical Properties and Behavior
Solutions: Physical Properties and Behavior In the previous chapter you were exposed to a great deal of information about the forces present in and the properties of individual pure substances (for example,
More informationProperties 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 informationAn 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 information15 Acids, Bases, and Salts. Lemons and limes are examples of foods that contain acidic solutions.
15 Acids, Bases, and Salts Lemons and limes are examples of foods that contain acidic solutions. Chapter Outline 15.1 Acids and Bases 15.2 Reactions of Acids and Bases 15.3 Salts 15.4 Electrolytes and
More information- 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 informationColligative Properties
Slide 1 Colligative Properties Practical uses of solutions Slide 2 Solution homogeneous mixtures composition may vary from one sample to another appears to be one substance, though really contains multiple
More information75 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 informationRegents 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 informationLet'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 informationSolutions: 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 informationAqueous 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(for tutoring, homework help, or help with online classes)
www.tutor-homework.com (for tutoring, homework help, or help with online classes) 1. If heat is added to ice and liquid water in a closed container and, after the addition of the heat, ice and liquid water
More informationProperties of Solutions
Properties of Solutions The Solution Process A solution is a homogeneous mixture of solute and solvent. Solutions may be gases, liquids, or solids. Each substance present is a component of the solution.
More informationMixtures. 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 informationClassification 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 informationChapter 11: Properties of Solutions - Their Concentrations and Colligative Properties. Chapter Outline
Chapter 11: Properties of Solutions - Their Concentrations and Colligative Properties Chapter Outline 11.1 Energy Changes when Substances Dissolve 11.2 Vapor Pressure 11.3 Mixtures of Volatile Substances
More informationChapter 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 informationx =!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 informationProperties of Solutions
Properties of Solutions Reading: Ch 11, section 8 Ch 12, sections 1-8 * = important homework question Homework: Chapter 11: 85*, 87 Chapter 12: 29, 33, 35, 41, 51*, 53, 55, 63*, 65, 67*, 69, 71, 75*, 79*,
More informationColligative 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 informationChapter 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 John D. Bookstaver St. Charles Community College St. Peters, MO 2006,
More information1. 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 informationDownloaded from
: Bhubaneswar Region CHAPTER 2-SOLUTIONS 1 MARK QUESTIONS 1 What is molarity? 2 What do you understand by saying that molality of a solution is 0.2? 3 Why is the vapour pressure of a liquid remains constant
More informationChemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten Chapter 13 Properties of Solutions
Chemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten Chapter 13 Properties of Dr. Ayman Nafady John D. Bookstaver St. Charles Community College Cottleville,
More informationColligative Properties
Colligative Properties Some physical properties of solutions differ in important ways from those of the pure solvent. For example, pure water freezes at 0 C, but aqueous solutions freeze at lower temperatures.
More informationSolutions. 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 informationConcentration 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 informationColligative 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 informationLecture Presentation. Chapter 12. Solutions. Sherril Soman, Grand Valley State University Pearson Education, Inc.
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 informationWays 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 informationWater & Solutions Chapter 17 & 18 Assignment & Problem Set
Water & Solutions Chapter 17 & 18 Assignment & Problem Set Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Water & Solutions 2 Vocabulary (know
More informationChapter 13. Properties of Solutions. Lecture Presentation. John D. Bookstaver St. Charles Community College Cottleville, MO
Lecture Presentation Chapter 13 Properties of John D. Bookstaver St. Charles Community College Cottleville, MO are homogeneous mixtures of two or more pure substances. In a solution, the solute is dispersed
More informationSalting 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 informationChapter 12: Solutions. Mrs. Brayfield
Chapter 12: Solutions Mrs. Brayfield 12.1: Solutions Solution a homogeneous mixture of two or more substances Solvent the majority component Solute the minority component What is the solute and solvent
More informationChemistry 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 informationSCHOOL YEAR CH- 13 IONS IN AQUEOUS SOLUTIONS AND COLLIGATIVE PROPERTIES SUBJECT: CHEMISTRY GRADE : 11 TEST A
SCHOOL YEAR 2017-18 NAME: CH- 13 IONS IN AQUEOUS SOLUTIONS AND COLLIGATIVE PROPERTIES SUBJECT: CHEMISTRY GRADE : 11 TEST A Choose the best answer from the options that follow each question. 1. A solute
More informationChapter 13 Properties of Solutions
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 informationUnit - 2 SOLUTIONS VSA QUESTIONS (1 - MARK QUESTIONS) 1. Give an example of liquid in solid type solution.
Unit - 2 SOLUTIONS VSA QUESTIONS (1 - MARK QUESTIONS) 1. Give an example of liquid in solid type solution. 2. Which type of solid solution will result by mixing two solid components with large difference
More informationThe 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 informationA) 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 informationChapter 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 informationCHAPTER 9 SOLUTIONS SHORT QUESTIONS WITH ANSWER Q.1 Binary solution can be homogenous or heterogeneous explain? The solutions which contain two components only are called as binary solution. If binary
More informationCHEM1109 Answers to Problem Sheet Isotonic solutions have the same osmotic pressure. The osmotic pressure, Π, is given by:
CHEM1109 Answers to Problem Sheet 5 1. Isotonic solutions have the same osmotic pressure. The osmotic pressure, Π, is given by: Π = MRT where M is the molarity of the solution. Hence, M = Π 5 (8.3 10 atm)
More informationB. 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 information1) Define the following terms: a) solution, b) miscible, c) hydration, d) percent by mass (solute), e) colligative property, f) hypotonic.
Problems - Chapter 13 (with solutions) 1) Define the following terms: a) solution, b) miscible, c) hydration, d) percent by mass (solute), e) colligative property, f) hypotonic. a) solution - A homogeneous
More information3 (4 + 3x6 +2)e- = 24e -
Chemical Bonds Atomic radii increase right to left across the period, and top to bottom down the group pposite is true for ionization energy Covalent bonds are made when difference in electronegativity
More informationGilbert Kirss Foster. Chapter 11. Properties of Solutions. Their Concentrations and Colligative Properties
Gilbert Kirss Foster Chapter 11 Properties of Solutions Their Concentrations and Colligative Properties Chapter Outline 11.1 Energy Changes when Substances Dissolve 11.2 Vapor Pressure 11.3 Mixtures of
More information