Solutions. Chapter 14 Solutions. Ion-Ion Forces (Ionic Bonding) Attraction Between Ions and Permanent Dipoles. Covalent Bonding Forces
|
|
- Shanon Chambers
- 6 years ago
- Views:
Transcription
1 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 temperatures. NaCl,, mp = 800 o C MgO,, mp = 2800 o C Covalent Bonding Forces 3 Attraction Between Ions and Permanent Dipoles 4 C=C, 610 kj/mol C H, 413 kj/mol C C, C, 346 kj/mol CN, 887 kj/mol water -δ O dipole H H +δ Water is highly polar and can interact with positive ions to give hydrated ions in water. Attraction Between Ions and Permanent Dipoles 5 Attraction Between Ions and Permanent Dipoles 6 water -δ O dipole H H +δ Water is highly polar and can interact with positive ions to give hydrated ions in water. Many metal ions are hydrated. This is the reason metal salts dissolve in water.
2 Attraction Between Ions and Permanent Dipoles Attraction between ions and dipole depends on ion charge and ion-dipole distance. Measured by H H for M n+ + H 2 O --> > [M(H 2 O) x ] n+ 7 Dipole-Dipole Forces Such forces bind molecules having permanent dipoles to one another. 8 δ- O H δ- H O H H Mg2+ δ+ δ+ Na + Cs + δ- H O H δ kj/mol -405 kj/mol -263 kj/mol Dipole-Dipole Forces Influence of dipole-dipole forces is seen in the boiling points of simple molecules. Compd Mol. Wt. Boil Point N C CO C Br o C ICl o C 9 Hydrogen Bonding A special form of dipole-dipole attraction, which enhances dipole-dipole attractions. 10 H-bonding is strongest when X and Y are N, O, or F Hydrogen Bonding in H 2 O H-bonding is especially strong in water because the O H O H bond is very polar there are 2 lone pairs on the O atom Accounts for many of water s s unique properties. 11 FORCES INVOLVING INDUCED DIPOLES How can non-polar molecules such as O 2 and I 2 dissolve in water? The water dipole INDUCES a dipole in the O 2 electric cloud. Dipole-induced induced dipole 12
3 FORCES INVOLVING INDUCED DIPOLES 13 FORCES INVOLVING INDUCED DIPOLES 14 Solubility increases with mass the gas Process of inducing a dipole is polarization Degree to which electron cloud of an atom or molecule can be distorted in its polarizability. IM FORCES INDUCED DIPOLES Consider I 2 dissolving in ethanol, CH 3 CH 2 OH. I-I -δ O R H +δ The alcohol temporarily creates or INDUCES a dipole in I 2. I-I -δ +δ -δ O R H +δ 15 FORCES INVOLVING INDUCED DIPOLES Formation of a dipole in two nonpolar I 2 molecules. Induced dipole- induced dipole Intermolecular Forces Summary Liquids In a liquid molecules are in constant motion there are appreciable intermolecular forces molecules close together Liquids are almost incompressible Liquids do not fill the container
4 Liquids The two key properties we need to describe are EVAPORATION and its opposite CONDENSATION LIQUID evaporation > Add energy VAPOR break IM bonds make IM bonds Remove energy <---condensation 19 Liquids Evaporation To evaporate, molecules must have sufficient energy to break IM forces. Breaking IM forces requires energy. The process of evaporation is endothermic Phase Diagrams Phase Diagrams Solutions: Definitions A solution is a One constituent is usually HOMOGENEOUS regarded as the SOLVENT mixture of 2 or more and the others as SOLUTES. substances in a single phase. Definitions Solute(s): That which is dissolved, generally in lower concentration Solvent: The medium doing the dissolving of the solute 23 Dissolving An Ionic Solid 24 Solutions can be classified as unsaturated or saturated. A saturated solution contains the maximum quantity of solute that dissovles at that temperature. SUPERSATURATED SOLUTIONS contain more than is possible and are unstable. Writing Equations: NaCl(s) Na + (aq) + Cl - (aq) You do CaCl 2 and Al 2 (SO 4 ) 3
5 Energy of the Solution Process 25 Energy of the Solution Process Lattice Energy E to form lattice (note negative sign) Hydration Energy E evolved when gaseous ions are dissolved Energy - KF If the enthalpy of formation of the solution is more negative that that of the solvent and solute, the enthalpy of solution is negative. The solution process is exothermic! Supersaturated Sodium Acetate Supersaturated Sodium Acetate One application of a supersaturated solution is the sodium acetate heat pack. Sodium acetate has an ENDOthermic heat of solution. Sodium acetate has an ENDOthermic heat of solution. NaCH 3 CO 2 (s) + heat ----> Na + (aq) ) + CH 3 CO - 2 (aq) Therefore, formation of solid sodium acetate from its ions is EXOTHERMIC. Na + (aq) ) + CH 3 CO - 2 (aq) ---> NaCH 3 CO 2 (s) + heat
6 Concentration Units An IDEAL SOLUTION is one where the properties depend only on the concentration of solute. Need conc. units to tell us the number of solute particles per solvent particle. The unit molarity does not do this! 31 Concentration Units X A = mol fraction A = MOLE FRACTION, X For a mixture of A, B, and C mol A mol A + mol B + mol C MOLALITY, m mol solute m of solute = kilograms solvent WEIGHT % = grams solute per 100 g solution 32 Calculating Concentrations 33 Calculating Concentrations 34 Dissolve 62.1 g (1.00 mol) of ethylene glycol in 250. g of H 2 O. Calculate mol fraction, molality,, and weight % of glycol. Consider a solution that is g of NaOH dissolved in 250 ml of total aqueous solution (the final density of solution is 1.10 g/ml) Calculate M, m, mole fraction NaOH and w% Calculating Concentrations 35 Calculating Concentrations 36 Consider a solution that is g of NaOH dissolved in 250 ml of total aqueous solution (the final density of solution is 1.10 g/ml) Consider a solution that is g of NaOH dissolved in 250 ml of total aqueous solution (the final density of solution is 1.10 g/ml) Calculate M, m, mole fraction NaOH and w% Calculate M, m, mole fraction NaOH and W%
7 What Affects Solubility?? 37 Dissolving Gases & Henry s Law 38 Pressure Inc. P over gas, increase solubility Gas + Solvent Solution Temperature Reactions are exothermic ( H = negative) or endothermic ( H = positive). Endo: NaNO 3 (s) + Heat Na + (aq) + NO 3- (aq) Increase temperature increase solubility (most salts) Gas solubility (mol/l) = k H P gas k H for H 2 = 1.07 x 10-6 M/mmHg Exo: NH 4 Cl (s) NH 4+ (aq) + Cl - (aq) + Heat Increase temperature decrease solubility When P gas drops, solubility drops. What is solubility of H 2 at 1 atm?? And 0.33 atm? Colligative Properties On adding a solute to a solvent, the props. of the solvent are modified. Vapor pressure decreases Will Melting point Boiling point decreases increases Osmosis is possible (osmotic pressure) These changes are called COLLIGATIVE PROPERTIES. They depend only on the NUMBER of solute particles relative to solvent particles, not on the KIND of solute particles. 39 To understand colligative properties, study the LIQUID-VAPOR EQUILIBRIUM for a solution. Understanding Colligative Properties 40 Understanding Colligative Properties VP of H 2 O over a solution depends on the number of H 2 O molecules per solute molecule. P solvent proportional to X solvent 41 Raoult s Law An ideal solution is one that obeys Raoult s law. P A = X A P o A 42 P solvent = X solvent P o solvent VP of solvent over solution = (Mol frac solvent) (VP pure solvent) RAOULT S S LAW Because mole fraction of solvent, X A, is always less than 1, then P A is always less than P o A. The vapor pressure of solvent over a solution is always LOWERED!
8 Raoult s Law Assume the solution containing 62.1 g of glycol in 250. g of water is ideal. What is the vapor pressure of water over the solution at 30 o C? (The VP of pure H 2 O is 31.8 mm Hg; see App. E.) 43 Changes in Freezing and Boiling Points of Solvent VP Pure solvent VP solvent after adding solute 1 atm P 44 BP solution BP pure solvent T Vapor Pressure Lowering 45 Elevation of Boiling Point Elevation in BP = T BP = K BP m (where K BP is characteristic of solvent) 46 Dissolve 62.1 g of glycol (1.00 mol) in 250. g of water. What is the BP of the solution? K BP = o C/molal for water (see Table 14.3). Figure Elevation of Boiling Point Elevation in BP = T BP = K BP (where K BP is characteristic of solvent) P VP Pure solvent 1 atm BP pure solvent VP solvent after adding solute BP solution T BP m 47 Change in Freezing Point Pure waterethylene glycol/water solution The freezing point of a solution is LOWER than that of the pure solvent. FP depression = T FP = K FP m Calculate the FP of a 4.00 molal glycol/water solution. FP = o C/molal (Table 14.4) K FP 48
9 Freezing Point Depression 49 Freezing Point Depression 50 Calculate the FP of a 4.00 molal glycol/water solution. K FP = o C/molal (Table 14.4) How much NaCl must be dissolved in 4.00 kg of water to lower FP to o C?. K FP = (-1.86( o C/molal) Freezing Point Depression 51 Freezing Point Depression 52 How much NaCl must be dissolved in 4.00 kg of water to lower FP to o C?. Solution How much NaCl must be dissolved in 4.00 kg of water to lower FP to o C?. Solution Boiling Point Elevation and Freezing Point Depression T T = K m i A general equation i = van t Hoff factor = number of particles produced per formula unit. Compound Theoretical Value of i glycol 1 NaCl 2 CaCl Osmosis Solvent Solution Semipermeable membrane The semipermeable membrane allows only the movement of solvent molecules. Solvent molecules move from pure solvent to solution in an attempt to make both have the same concentration of solute. OSMOTIC PRESSURE, = crt (c is conc. in mol/l) 54
10 Osmosis at the Particulate Level 55 Process of Osmosis 56 Figure Osmosic Pressure, Equilibrium is reached when pressure the OSMOTIC PRESSURE, produced by extra solution Osmotic counterbalances pressure of pressure solvent molecules moving thru the membrane. = crt (c is conc. in mol/l) 57 Osmosis Calculating a Molar Mass Dissolve 35.0 g of hemoglobin in enough water to make 1.00 L of solution. Π measured to be 10.0 mm Hg at 25 C. Calc. molar mass of hemoglobin. 58 Osmosis Calculating a Molar Mass 59 Osmosis 60 Dissolve 35.0 g of hemoglobin in enough water to make 1.00 L of solution. Π measured to be 10.0 mm Hg at 25 C. Calc. molar mass of hemoglobin. Osmosis of solvent from one solution to another can continue until the solutions are ISOTONIC they have the same concentration.
11 Osmosis and Living Cells 61 Reverse Osmosis Water Desalination 62 Water desalination plant in Tampa
Properties of Solutions. Chapter 13
Properties of Solutions Chapter 13 Sodium acetate crystals rapidly form when a seed crystal is added to a supersaturated solution of sodium acetate. Saturated solution: contains the maximum amount of a
More 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 informationor supersaturatedsaturated Page 1
Solutions Unit #9 Chapter #11 A solution is a HOMOGENEOUS mixture of 2 or more substances in a single phase. One constituent is usually regarded as the SOLVENT and the others as SOLUTES. 1 Definitions
More 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 informationSolutions and Their Properties
Chapter 11 Solutions and Their Properties Solutions: Definitions A solution is a homogeneous mixture. A solution is composed of a solute dissolved in a solvent. When two compounds make a solution, the
More 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 information11/4/2017. General Chemistry CHEM 101 (3+1+0) Dr. Mohamed El-Newehy. Chapter 4 Physical Properties of Solutions
General Chemistry CHEM 11 (3+1+) Dr. Mohamed El-Newehy http://fac.ksu.edu.sa/melnewehy Chapter 4 Physical Properties of Solutions 1 Types of Solutions A solution is a homogenous mixture of 2 or more substances.
More 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 12.4 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 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 informationOverview. Types of Solutions. Intermolecular forces in solution. Concentration terms. Colligative properties. Osmotic Pressure 2 / 46
1 / 46 2 / 46 Overview Types of Solutions. Intermolecular forces in solution Concentration terms Colligative properties Osmotic Pressure 3 / 46 Solutions and Colloids A solution is a homogeneous mixture
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 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 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 informationChapter 12. Physical Properties of Solutions. Chemistry, Raymond Chang 10th edition, 2010 McGraw-Hill
Chemistry, Raymond Chang 10th edition, 2010 McGraw-Hill Chapter 12 Physical Properties of Solutions Ahmad Aqel Ifseisi Assistant Professor of Analytical Chemistry College of Science, Department of Chemistry
More 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 informationChapter 11 Problems: 11, 15, 18, 20-23, 30, 32-35, 39, 41, 43, 45, 47, 49-51, 53, 55-57, 59-61, 63, 65, 67, 70, 71, 74, 75, 78, 81, 85, 86, 93
Chapter 11 Problems: 11, 15, 18, 20-23, 30, 32-35, 39, 41, 43, 45, 47, 49-51, 53, 55-57, 59-61, 63, 65, 67, 70, 71, 74, 75, 78, 81, 85, 86, 93 Chapter 11 Properties of Solutions Types of mixtures: homogenous
More 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 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 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 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 informationWhy is water usually a liquid and not a gas? Why does liquid water boil at such a high temperature for such a small molecule? Why does ice float on
1 Why is water usually a liquid and not a gas? Why does liquid water boil at such a high temperature for such a small molecule? Why does ice float on water? Why do snowflakes have 6 sides? Why is I 2 a
More informationChapter 12. Properties of Solutions
Chapter 12. Properties of Solutions What we will learn: Types of solutions Solution process Interactions in solution Types of concentration Concentration units Solubility and temperature Solubility and
More 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 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 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 informationCHAPTER OUTLINE. I. The Structure of Water: An Introduction to Intermolecular Forces
The Chemistry of Water and the Nature of Liquids Chapter 11 CHAPTER OUTLINE 11.2 I. The Structure of Water: An Introduction to Intermolecular Forces II. A Closer Look at Intermolecular lar Forces A. London
More informationChapter 17: Phenomena
Chapter 17: Phenomena Phenomena: Different masses of solute were added to 1 kg of either H 2 O or C 6 H 6. The boiling and freezing points of the solutions were then measured. Examine the data to determine
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 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 informationSolutions Definition and Characteristics
Solutions Solutions Definition and Characteristics Homogeneous mixtures of two or more substances Appear to be pure substances Transparency Separation by filtration is not possible Uniform distribution
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 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 informationAP CHEMISTRY NOTES 15-1 INTERMOLECULAR FORCES
AP CHEMISTRY NOTES 15-1 INTERMOLECULAR FORCES INTERMOLECULAR FORCES In addition to the covalent bonds that exist between atoms in a molecule (H2O for instance), there are also weak attractions between
More 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 informationGeneral Chemistry by Ebbing and Gammon, 9th Edition George W.J. Kenney, Jr, Professor of Chemistry Last Update: 15-May-2009
Chem 1046 General Chemistry by Ebbing and Gammon, 9th Edition George W.J. Kenney, Jr, Professor of Chemistry Last Update: 15-May-2009 Chapter 12 SOLUTIONS These Notes are to SUPPLIMENT the Text, They do
More informationChapter 13. Ions in aqueous Solutions And Colligative Properties
Chapter 13 Ions in aqueous Solutions And Colligative Properties Compounds in Aqueous Solution Dissociation The separation of ions that occurs when an ionic compound dissolves H2O NaCl (s) Na+ (aq) + Cl-
More 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 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 informationLecture outline: Chapter 13
Lecture outline: Chapter 13 Properties of solutions Why solutions form at the molecular l levell Units of solution concentration Colligative properties: effects of solutes on BP, MP, and vapor pressure
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 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 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 informationChem 124 Exam 1 Spring 2016 Version 1 Name
Chem 124 Exam 1 Spring 2016 Version 1 Name TOTAL POINTS - 116 MULTIPLE CHOICE 1.4 POINTS EACH 1) A molecule containing a central atom with sp 3 hybridization has a(n) electron geometry. A) linear B) tetrahedral
More informationChapter 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 John D. Bookstaver St. Charles Community College Cottleville, MO Chapter
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 informationChapter 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 informationName Class Date. In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question.
Assessment Chapter Test A Chapter: Solutions In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. 1. Agitation prevents settling
More 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 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 informationStrong Electrolytes - substance that dissolves almost completely in water to produce many ions to conduct electricity
I. What are Solutions A. Solution - homogeneous mixture made up of individual molecules, atoms or ions. B. Solute - the substance being C. Solvent - the substance D. Soluble - substance that in a solvent
More information(name) Place the letter of the correct answer in the place provided. Work must be shown for non-multiple choice problems
(name) Place the letter of the correct answer in the place provided. Work must be shown for non-multiple choice problems 1. According to Raoults Lab the change in the vapor pressure of a solution containing
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 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 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 informationIntermolecular Forces
Intermolecular Forces! When two molecules approach one another, they are attracted to some extent! Polar molecules are attracted through the electrostatic interaction of their dipole moments! Non-polar
More 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 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 informationClassifica,on of Solu,ons
SOLUTIONS Solu,on 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 informationSolutions. Solutions. How Does a Solution Form? Solutions. Energy Changes in Solution. How Does a Solution Form
Ummm Solutions Solutions Solutions are homogeneous mixtures of two or more pure substances. In a solution, the solute is dispersed uniformly throughout the solvent. Solutions The intermolecular forces
More informationSolution Formation. Copyright Houghton Mifflin Company.All rights reserved. Presentation of Lecture Outlines, 12 2
Solutions Solution Formation A solution is a homogeneous mixture of two or more substances, consisting of ions or molecules. (See Animation: Solution Equilibrium). A colloid, although it also appears to
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 informationChapter 11. Properties of Solutions Solutions
Chapter 11. Properties of Solutions Solutions Homogeneous Mixture 1 Solution Composition Equivalent moles of solute (mol) Acid-Base reaction Molarity (M) = liter of solution (L) 1 eq: the quantity of acid
More informationChapter 14. Physical Properties of Solutions. Concentration Units. Example: 1. Show that for dilute solutions, 1ppm is approximately equal to 1mg/L
Chapter 14 Physical Properties of Solutions alloy Concentration Units Molarity (M) = moles solute / Liters of solution Percent by Mass (weight) 1. Show that for dilute solutions, 1ppm is approximately
More informationsolubility solubilities that increase with increasing temperature
Solubility The concentration of the solute in a saturated solution is the solubility of the solute About 95% of all ionic compounds have aqueous solubilities that increase with increasing temperature Temperature
More 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 informationChemistry 201: General Chemistry II - Lecture
Chemistry 201: General Chemistry II - Lecture Dr. Namphol Sinkaset Chapter 14 Study Guide Concepts 1. Solutions are homogeneous mixtures of two or more substances. 2. solute: substance present in smaller
More 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 informationExam 2. CHEM Spring Name: Class: Date:
CHEM-112-01 Spring 2012 Name: Class: Date: 1. Record your name and ID number on the scantron form. 2. Record the test ID letter in the top right box of the scantron form. 3. Record all of your answers
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 informationSolids, Liquids and Gases
WHY? Why is water usually a liquid and not a gas? Why does liquid water boil at such a high temperature for such a small molecule? Why does ice float on water? Why do snowflakes have 6 sides? Why is I
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 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 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 informationLESSON 11. Glossary: Solutions. Boiling-point elevation
LESSON 11 Glossary: Solutions Boiling-point elevation Colligative properties Freezing-point depression Molality Molarity (M) Mole (mol) Mole fraction Saturated solution a colligative property of a solution
More informationCHAPTER 7: Solutions & Colloids 7.2 SOLUBILITY. Degrees of Solution. Page PHYSICAL STATES of SOLUTIONS SOLUTION
CHAPTER 7: Solutions & Colloids Predict the relative solubility of materials on the basis of polarity Describe solution formation in terms of solutesolvent interactions Calculate solution concentrations
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 information2. Match each liquid to its surface tension (in millinewtons per meter, mn*m -1, at 20 C).
1. Using your knowledge of the types of intermolecular forces present in CO 2, CH 3 CN, Ne, and CH 4 gases, assign each gas to its van der Waals a parameter. a ( ) 17.58 3.392 2.253 0.2107 gas 2. Match
More informationCHM 1046 FINAL REVIEW
CHM 1046 FINAL REVIEW Prepared & Presented By: Marian Ayoub PART I Chapter Description 6 Thermochemistry 11 States of Matter; Liquids and Solids 12 Solutions 13 Rates of Reactions 18 Thermodynamics and
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 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 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 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 informationChap 10 Part 4Ta.notebook December 08, 2017
Chapter 10 Section 1 Intermolecular Forces the forces between molecules or between ions and molecules in the liquid or solid state Stronger Intermolecular forces cause higher melting points and boiling
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 informationDATA THAT YOU MAY USE UNITS Conventional Volume ml or cm 3 = cm 3 or 10-3 dm 3 Liter (L) = dm 3 Pressure atm = 760 torr = Pa CONSTANTS
DATA THAT YOU MAY USE UNITS Conventional S.I. Volume ml or cm 3 = cm 3 or 0-3 dm 3 Liter (L) = dm 3 Pressure atm = 760 torr =.03 0 5 Pa torr = 33.3 Pa Temperature C 0 C = 73.5 K PV L-atm =.03 0 5 dm 3
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 informationChapter 7 Solutions and Colloids
Chapter 7 Solutions and Colloids 7.1 Physical States of Solutions Solutions are homogeneous mixtures of two or more substances in which the components are present as atoms, molecules, or ions. Properties
More informationChapter 7 Solutions and Colloids
Chapter 7 Solutions and Colloids 7.1 Physical States of Solutions Solutions are homogeneous mixtures of two or more substances in which the components are present as atoms, molecules, or ions. Properties
More 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 informationChapter 13. Properties of Solutions
Chapter 13. Properties of Solutions Common Student Misconceptions Students often confuse dilute and concentrated with weak and strong. Students do not realize that crystallization is the reverse of dissolution.
More informationChapter 12 Intermolecular Forces and Liquids
Chapter 12 Intermolecular Forces and Liquids Jeffrey Mack California State University, Sacramento Why? Why is water usually a liquid and not a gas? Why does liquid water boil at such a high temperature
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 informationChapter 13 Study Questions
Class Copy - Do Not Write On This Test!!! ID: A Chapter 13 Study Questions True/False Indicate whether the statement is true or false. 1. A solution with a solute concentration greater than the solubility
More informationCHEMISTRY XL-14A PHYSICAL EQUILIBRIUM. August 13, 2011 Robert Iafe
CHEMISTRY XL-14A PHYSICAL EQUILIBRIUM August 13, 2011 Robert Iafe Chapter Overview 2 Phases and Phase Transitions Solubility Colligative Properties Binary Liquid Mixtures Phases and Phase Transitions 3
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 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 informationUNIT 8: SOLUTIONS. Essential Question: What kinds of properties affect a chemical s solubility?
UNIT 8: SOLUTIONS Essential Question: What kinds of properties affect a chemical s solubility? SOLUTIONS & THEIR CHARACTERISTICS (5) Most chemical reactions take place IN solutions 1. Homogeneous mixture
More 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 informationChapter 17 - Properties of Solutions
Chapter 17 - Properties of Solutions 17.1 Solution Composition 17.2 Thermodynamics of Solution Formation 17.3 Factors Affecting Solubility 17.4 Vapor Pressures of Solutions 17.5 Boiling-Point Elevation
More information