Activities and Activity Coefficients
|
|
- Harold Flynn
- 6 years ago
- Views:
Transcription
1 CHEM 331 Physical Chemistry Fall 017 Activities and Activity Coefficients We now finish answering the question we asked during our last lecture, what is the form of the chemical potential i (T,P,x i ) for components of condensed phase (liquid/solid) solutions. Previously we determined that the chemical potential for the components of these solutions are given by: i = i * + RT ln x i (Ideal Solution) j = j ** + RT ln x j (Ideal-Dilute Solution) j = j *** + RT ln (Ideal-Dilute Solution) j = + RT ln (Ideal-Dilute Solution) provided the solution is Ideal or Ideal-Dilute. We now push toward forms for i when the solution is Real. In the case where the solution is Real, we introduce an "effective" concentration, much as we introduced the fugacity as an "effective" pressure for Real gases, which we call the Activity; denoted as a i. We also retain the previous definitions of the Reference States i *, j **, j ***, and. This then gives us: i = i * + RT ln a i I = i ** + RT ln a i
2 i = i *** + RT ln i = + RT ln It should be noted that we have really defined four different activities a * i, a ** i, a *** i and ; each denoted commonly as a i. For this reason, the Reference State being used must be identified when working with a given activity. Notice also that the distinction between the solvent i and solutes j has been dropped, as any one of these forms will work over the entire concentration range of the solution. However, having said this, it is still useful to use the Ideal Reference State * i when working with the solvent and the others when working with the solutes. We now introduce a new parameter, the Activity Coefficient i. This parameter is incorporates all the non-idealities of the solution. Depending on the Reference State chosen, it is defined according to: a i * a i ** a i *** = i * x i = i ** x i = i *** m i = c i Again, each is more generically denoted i. Because our solutions are expected to behave ideally at the limit x i 1 or as ideal-dilute in the limit x i 0, it is expected i should approach 1 in these limits. The limiting behavior of each i is given: i i * i i ** i i *** as x i 1 so a i x i and i 1 as x i 1 as x i 0 so a i x i and i 1 as x i 0 as m i 0 so a i m i and i 1 as m i 0 i as c i 0 so a i c i and i 1 as c i 0 Now, how do we determine a i or i? There are a number of methods. Some rely on colligative property data, others electrochemical cell data, etc. We will illustrate the determination of i from vapor pressure data. So, assume our condensed phase is in equilibrium with its vapor and that it is Real, therefore the vapor pressure of the i th component P i will deviate from either Raoult's or Henry's Law.
3 Now do the usual bit, equate the chemical potentials of component i across the phase boundary. i,gas (T,P i,y i ) = i,liq (T,P i,x i ) If we are working with Ideal Reference State, then: i,liq (T,P i,x i ) = i * + RT ln a i = i o + RT ln P i * + RT ln a i and: i,gas (T,P i,y i ) = i o + RT ln P i Inserting these forms into the above equation gives: RT ln a i = RT ln Or, simplifying: a i =
4 This, then, allows for the determination of i : i = = If the Reference State in use is the Ideal-Dilute Reference State, then: And so on. A couple of examples. a i = and i = For Hg(l) at 35 o C, P Hg * = kpa. An amalgam of Hg and Tl at this same temperature, composed of Hg (solvent) and 1.163g Tl (solute), has a vapor pressure of P Hg = 5.04 kpa. What is Hg for the Hg at this solution composition? Mole Fractions N Hg = 18.70g / (00.59 g/mol) = mol Hg N Tl = 1.163g / (04.37 g/mol) = mol Tl x Hg = = = 0.94 Activity a Hg = = = Activity Coefficient Hg = = = Notice that since x Hg ~ 1, Hg ~ 1. At 5 o C, K N = 8.9 x 10 9 Pa for N in Water. What is N when a partial pressure of Nitrogen P N = kpa of N is applied above the Water? At this vapor pressure, N N = 6.40 x 10-4 mol N. Mole Fraction Activity x N = = = x 10-5 a N = = = x10-5
5 Activity Coefficient N = = = Again, notice that since x N ~ 0, N ~ 1. Keep in mind, this is only one method for determining activity coefficients. Now to one last detail concerning the form of i. The behavior of Electrolyte Solutions is skewed by the fact that the electrolyte disassociates in Water. So, we now turn to deal with aqueous electrolyte solutions. First, some background. Consider reasonably dilute aqueous solutions of HCl. According to Henry's Law: P HCl should = K HCl m HCl In other words, P HCl should be linear in m HCl. However, a plot of the data demonstrates this is not the case. In fact, a plot of P HCl vs. m HCl is instead linear in the dilute limit. This suggests that Henry's Law for aqueous HCl solutions should be written as: P HCl =
6 Physical Chemistry, nd Ed. J. Philip Bromberg What is going on? Consider a generic electrolyte that is fully soluble in Water: M p N q (aq) p M x+ (aq) + q N y- (aq) Some specific examples: HCl(aq) H + (aq) + Cl - (aq) p = 1 q = 1 CaCl (aq) Ca + (aq) + Cl - (aq) p = 1 q = Na SO 4 (aq) Na + (aq) + SO 4 - p = q = 1 If the solution molality is m, then the molality of the cations m + and molality of the anions m - is given by: m + = p m m - = q m Now, we will formally write and *** as: = p + + q - *** = p + *** + q - ***
7 where + and - are the chemical potentials of the cations and anions respectively. Also note that the subscript i has been dropped, so as to not muddy up the notation too much. Then, according to our usual forms: + = + *** + RT ln a + - = - *** + RT ln a - with a + = + m + and a - = - m -. Now, the problem is, we cannot measure + and - simultaneously. (Think about why this is!) So, instead of trying to indentify + and -, we instead introduce a Mean Ionic Chemical Potential: ± = ± *** = where s = p + q. And, we have a ± = ± m ±. The following relationships also follow: a s ± = a p q + a - m s ± = m p q + m - ± = p q + - Now we can write: = s ± = s ± *** + RT ln ± s + RT ln m ± s Further, m ± can be determined from m: m ± = (m + p m - q ) 1/s = ( (pm) p (qm) q ) 1/s = (p p q q m s ) 1/s = (p p q q ) 1/s m A single measurement of can indeed yield the single value of ±, making this form of quite useful for electrolyte solutions. Now back to the HCl problem. When dissolved in Water, HCl will dissociate completely. HCl(aq) H + (aq) + Cl - (aq)
8 with p=1, q=1, and s=. Thus, liq,hcl = ± *** + RT ln a ± ± *** + RT ln m ± (if reasonably dilute and ± ~ 1) = ± *** + RT ln m HCl Now, to consider the vapor-liquid equilibrium: HCl,liq = HCl,gas HCl,gas = o + RT ln P HCl HCl,liq = ± *** + RT ln m HCl = o + RT ln K HCl + RT ln m HCl This gives: o + RT ln K HCl + RT ln m HCl = o + RT ln P HCl resulting in a P ~ m dependence: P HCl = K HCl m HCl And, now we see why Henry's Law must be modified for the electrolyte. P HCl = Theoretical estimates of ± are extremely difficult to come by because the intermolecular interactions between the cations and anions are so extremely strong in the solution. One method for estimating ±, developed by Peter Debye and Erich Huckel, works in the extremely dilute electrolyte limit; m < 0.001m.
9 Peter Debye Erich Huckel Using a statistical mechanical model, Debye and Huckel showed that: log ± = z + z - I c 1/ where z + and z - are the charges of the cation and anion respectively and I c is the Ionic Strength. I c = c i is the concentration of each of the ionic species present in the solution. It should be noted that this form of the Debye-Huckel Law only works for aqueous solutions at 5 o C. Further note that only the charges of the ions are required to estimate ±. This model can be extended to slightly higher concentrations by including the hydrodynamic radius of each ion. We will not consider this Extended Debye-Huckel Law further. Below is a graph showing the validity of the Debye-Huckel Law for several actual electrolytes; the dashed lines are the Debye-Huckel predictions for various z + and z - values.
10 Walter J. Moore Physical Chemistry, 4 th Ed. As an example: Use the Debye-Huckel Law to estimate ± for 0.001m BaCl in 0.000m aqueous HNO 3. BaCl (aq) Ba + (aq) + Cl - (aq) I c = (c Ba+ z Ba+ + c Cl- z Cl- + c H+ z H+ + c NO3- z NO3- ) = ((0.001m)( ) + (0.00m)(1 ) + (0.000m)(1 ) + (0.000m)(1 )) = 0.003m 1/ log ± = z Ba+ z cl- I c = (+) (-1) (0.003) 1/ = ± = = 0.987
The Chemical Potential of Components of Solutions
CHEM 331 Physical Chemistry Fall 2017 The Chemical Potential of Components of Solutions We have shown that the Gibbs Free Energy for a solution at constant T and P can be determined from the chemical potential
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 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 informationChem 321 Lecture 11 - Chemical Activities 10/3/13
Student Learning Objectives Chem 321 Lecture 11 - Chemical Activities 10/3/13 One of the assumptions that has been made in equilibrium calculations thus far has been to equate K to a ratio of concentrations.
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 information6, Physical Chemistry -II (Statistical Thermodynamics, Chemical Dynamics, Electrochemistry and Macromolecules)
Subject Paper No and Title Module No and Title Module Tag 6, Physical -II (Statistical Thermodynamics, Chemical Dynamics, Electrochemistry and Macromolecules) 25, Activity and Mean Activity coefficient
More informationLecture 6. NONELECTROLYTE SOLUTONS
Lecture 6. NONELECTROLYTE SOLUTONS NONELECTROLYTE SOLUTIONS SOLUTIONS single phase homogeneous mixture of two or more components NONELECTROLYTES do not contain ionic species. CONCENTRATION UNITS percent
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 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 informationGEOL 414/514 ACTIVITY COEFFICIENTS OF DISSOLVED SPECIES
GEOL 414/514 ACTIVITY COEFFICIENTS OF DISSOLVED SPECIES Chapter 4 LANGMUIR ACTIVITY & ACTIVITY COEFFICIENTS Earlier we studied common ion effect on decreasing the solubility CaCO 3 Ca +2 + CO 3 Add Ca
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 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 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 informationChemistry 2000 Lecture 11: Chemical equilibrium
Chemistry 2000 Lecture 11: Chemical equilibrium Marc R. Roussel February 4, 2019 Marc R. Roussel Chemical equilibrium February 4, 2019 1 / 27 Equilibrium and free energy Thermodynamic criterion for equilibrium
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 informationChapter 4. Solutions and Solution Stoichiometry
Chapter 4 Solutions and Solution Stoichiometry Solutions Homogeneous mixtures are called solutions. The component of the solution that changes state is called the solute. The component that keeps its state
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 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 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 informationSolutions. Heterogenous Mixture (Not a Solution) Ice Water (w/ Ice Cubes) Smog Oil and Water
Solutions Unit 6 1 Solutions Homogenous Mixture (Solution) two or more substances mixed together to have a uniform composition, its components are not distinguishable from one another Heterogenous Mixture
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 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 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 informationExam 3: Mon, Nov. 7, 6:30 7:45 pm
Week 10: Lectures 28 30 Lecture 28: W 10/26 Lecture 29: F 10/28 Lecture 30: M 10/31 (Halloween Demo Show) Reading: BLB Ch 4.1, 4.5, 13.1 13.4 Homework: BLB 4: 3, 37, 72; Supp 4: 1 5; BLB 13: 7, 21, 23;
More informationWed Sep 5, Characteristics of Water
Wed Sep 5, 2007 Chapter 4: Types of Chemical Reactions 4.1 Water 4.2 Electrolytes 4.3 Composition of Solutions Exam #1 - Next Friday (Sep 14) Week 3 CHEM 1310 - Sections L and M 1 Characteristics of Water
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 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 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 informationChem 75 Winter, 2017 Practice Exam 3
1. The Handbook of Chemistry and Physics says that PbBr 2 is soluble in water to the tune of 8.441 g per kg of water at 25 C. The molar mass of PbBr 2 is 367 g mol 1. (a) What is the ionic strength of
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 informationChapter 11 section 6 and Chapter 8 Sections 1-4 from Atkins
Lecture Announce: Chapter 11 section 6 and Chapter 8 Sections 1-4 from Atkins Outline: osmotic pressure electrolyte solutions phase diagrams of mixtures Gibbs phase rule liquid-vapor distillation azeotropes
More informationPart A Answer all questions in this part.
Part A Directions (1-24): For each statement or question, record on your separate answer sheet the number of the word or expression that, of those given, best completes the statement or answers the question.
More informationANSWERS CIRCLE CORRECT SECTION
CHEMISTRY 162 - EXAM I June 08, 2009 Name: SIGN: RU ID Number Choose the one best answer for each question and write the letter preceding it in the appropriate space on this answer sheet. Only the answer
More informationChemistry 51 Chapter 8 TYPES OF SOLUTIONS. Some Examples of Solutions. Type Example Solute Solvent Gas in gas Air Oxygen (gas) Nitrogen (gas)
TYPES OF SOLUTIONS A solution is a homogeneous mixture of two substances: a solute and a solvent. Solute: substance being dissolved; present in lesser amount. Solvent: substance doing the dissolving; present
More informationChapter 4. Chemical Quantities and Aqueous Reactions
Lecture Presentation Chapter 4 Chemical Quantities and Aqueous Reactions Reaction Stoichiometry: How Much Carbon Dioxide? The balanced chemical equations for fossilfuel combustion reactions provide the
More informationChapter 3: Solution Chemistry (For best results when printing these notes, use the pdf version of this file)
Chapter 3: Solution Chemistry (For best results when printing these notes, use the pdf version of this file) Section 3.1: Solubility Rules (For Ionic Compounds in Water) Section 3.1.1: Introduction Solubility
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 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 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 informationOFB Chapter 6 Condensed Phases and Phase Transitions
OFB Chapter 6 Condensed Phases and Phase Transitions 6-1 Intermolecular Forces: Why Condensed Phases Exist 6- The Kinetic Theory of Liquids and Solids 6-3 Phase Equilibrium 6-4 Phase Transitions 6-5 Phase
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 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 informationEquation Writing for a Neutralization Reaction
Equation Writing for a Neutralization Reaction An Acid-Base reaction is also called a Neutralization reaction because the acid (generates H + or H 3 O + ) and base (generates OH ) properties of the reactants
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 informationThe solvent is the dissolving agent -- i.e., the most abundant component of the solution
SOLUTIONS Definitions A solution is a system in which one or more substances are homogeneously mixed or dissolved in another substance homogeneous mixture -- uniform appearance -- similar properties throughout
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 informationLiquids and Solutions
Liquids and Solutions Introduction This course examines the properties of liquids and solutions at both the thermodynamic and the molecular level. The main topics are: Liquids, Ideal and Regular Solutions,
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 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 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. 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 informationConcentration of Solutions
Solutions We carry out many reactions in solutions Remember that in the liquid state molecules move much easier than in the solid, hence the mixing of reactants occurs faster Solute is the substance which
More informationVAPOR PRESSURE LOWERING - Described by RAOULT'S LAW
73 VAPOR PRESSURE LOWERING - Described by RAOULT'S LAW partial pressure of the VAPOR of solvent molecules. mole fraction of component A vapor pressure of pure component A (depends on temperature) partial
More informationActivity Predicting Products of Double Displacement Reactions
KEY Activity 151-6 Predicting Products of Double Displacement Reactions Directions: This GLA worksheet is focused on predicting products and writing balanced equations for double displacement reactions.
More informationCHEM N-7 November 2005
CHEM1909 2005-N-7 November 2005 Calcium chloride (3.42 g) is completely dissolved in 200 ml of water at 25.00 ºC in a coffee cup calorimeter. The temperature of the water after dissolution is 27.95 ºC.
More information1. How much work (in kj/mol) can in principle be obtained when an electron is brought to nm distance from a proton?
Thermodynamics: Examples for chapter 7. 1. How much work (in kj/mol) can in principle be obtained when an electron is brought to 0.5000 nm distance from a proton? The work is obtained by integrating the
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 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 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 informationSolutions & Solubility: Net Ionic Equations (9.1 in MHR Chemistry 11)
Solutions & Solubility: Net Ionic Equations (9.1 in MHR Chemistry 11) 1 Solubility vs. Temperature 2 Solubility Table Anions SOLUBILITY Table 8.3 page 363 in MHR Cl Br I S OH SO CO 3 PO 3 SO 3 C 2 H 3
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 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 information2011, Robert Ayton. All rights reserved.
Solutions Outline 1. Solubility 2. Concentration Calculations 3. Colligative Properties 4. Freezing Point Depression or Boiling Point Elevation Problems 5. Graphs of Colligative Properties Review 1. Solubility
More 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 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 informationChemistry 163B. Concluding Factoids. and. Comments
Chemistry 163B Concluding Factoids and Comments 1 neuron, resting potential http://projects.gw.utwente.nl/pi/sim/bovt/concep4.gif http://www.uta.edu/biology/westmoreland/classnotes/144/chapter_48_files/image009.jpg
More informationSOLUTIONS. Definitions. Solvation. Hydration. Energy changes involved in solutions
1 SOLUTIONS Definitions Solvation Hydration Energy changes involved in solutions 2 Solubility Definition Unsaturated Saturated supersaturated Factors affecting solubility Interactions of solute with solvent
More 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 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 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 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 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 4: Stoichiometry of Chemical Reactions. 4.1 Writing and Balancing Chemical Equations
Chapter 4: Stoichiometry of Chemical Reactions 4.1 Writing and Balancing Chemical Equations A chemical equation represents or symbolizes a chemical reaction. o Substances are represents by their chemical
More informationH 2 O WHAT PROPERTIES OF WATER MAKE IT ESSENTIAL TO LIFE OF EARTH? Good solvent High Surface tension Low vapor pressure High boiling point
Unit 9: Solutions H 2 O WHAT PROPERTIES OF WATER MAKE IT ESSENTIAL TO LIFE OF EARTH? Good solvent High Surface tension Low vapor pressure High boiling point Water is a polar molecule. It experiences hydrogen
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 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 4 AQUEOUS REACTIONS AND SOLUTION STOICHIOMETRY: Electrolyte-a compound that conducts electricity in the melt or in solution (water)
CHAPTER 4 AQUEOUS REACTIONS AND SOLUTION STOICHIOMETRY: Electrolyte-a compound that conducts electricity in the melt or in solution (water) STRONG ELEC. 100% Dissoc. WEAK ELEC..1-10% Dissoc. NON ELEC 0%
More informationWarm up. 1. What is a solution? 2. What is a solute? 3. What is a solvent?
Warm up 1. What is a solution? 2. What is a solute? 3. What is a solvent? Solutions Chapter 12.2 Solubility The amount of substance that can dissolve at a given temperature to produce a saturated solution
More informationBrass, a solid solution of Zn and Cu, is used to make musical instruments and many other objects.
Brass, a solid solution of Zn and Cu, is used to make musical instruments and many other objects. 14.1 General Properties of Solutions 14.2 Solubility 14.3 Rate of Dissolving Solids 14.4 Concentration
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 informationUnit 2: Matter as Solutions and Gases
Selected Honour Chemistry Assignment Answers pg. 3 Unit 2: Matter as Solutions and Gases Chapter 4: Reactions in Aqueous Solutions (pg. 124 to 129) 1. Solute is the substance being dissolved. Solvent is
More information3. Liquid solutions: a. liquid - liquid Ex. vinegar b. solid - liquid Ex. salt water c. gas - liquid Ex. carbonated water in soda pop
Solution Chemistry Nature of Solutions solutions are homogeneous mixtures substances in solution are different from their solid, liquid or gas forms there should be no observable segregation of component
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 informationSolutions. π = n RT = M RT V
Solutions Factors that affect solubility intermolecular interactions (like dissolves like) temperature pressure Colligative Properties vapor pressure lowering Raoult s Law: P A = X A P A boiling point
More informationCHEMISTRY CP Name: Period:
CHEMISTRY CP Name: Period: CHEMISTRY SPRING FINAL REVIEW SHEET NOTE: Below are concepts that we have covered in class throughout the second semester. Questions are organized by chapter/concept to help
More informationBrief reminder of the previous lecture
Brief reminder of the previous lecture partial molar quantities: contribution of each component to the properties of mixtures V j V = G µ = j n j n j pt,, n pt,, n dg = Vdp SdT + µ dn + µ dn +... A A B
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 informationSubject : Chemistry Class : XII Chapter-2.Solutions Work Sheet ( WS 2. 1) Topic- 2.1 Henry s & Raoult s Laws
Work Sheet ( WS 2. 1) Topic- 2.1 Henry s & Raoult s Laws Name -. Class/ sec.. Roll No.. A. Fill in the blanks: 1. Solutions are mixtures of two or more than two components. 2. Generally, the component
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 informationCHEM 116 Colligative Properties and Intro to Rates of Reaction
CHEM 116 Colligative Properties and Intro to Rates of Reaction Note: Some of the slides here were in Lecture 10 but we didn t get to them, so we will begin with those. They are repeated here, but if you
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 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 informationChemistry 121 Chapters 7& 8 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question.
Chemistry 121 Chapters 7& 8 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1. A sample of carbon dioxide occupies 22.4 L at STP. Which of the
More informationChem 260 Quiz - Chapter 4 (11/19/99)
Chem 260 Quiz - Chapter 4 (11/19/99) Name (print) Signature Terms in bold: phase transitions transition temperature phase diagram phase boundaries vapor pressure thermal analysis dynamic equilibrium boiling
More informationHONORS CHEMISTRY Putting It All Together II
NAME: SECTION: HONORS CHEMISTRY Putting It All Together II Calculations in Chemistry It s time to pull out your calculators! In the first review sheet, you were able to write formulas of compounds when
More informationChapter 4: Types of Chemical Reactions and Solution Stoichiometry
Chapter 4: Types of Chemical Reactions and Solution Stoichiometry 4.1 Water, the Common Solvent 4.2 The Nature of Aqueous Solutions: Strong and Weak Electrolytes 4.3 The Composition of Solutions (MOLARITY!)
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 informationCHEMISTRY 110 EXAM 3 April 2, 2012 FORM A 1. Which plot depicts the correct relationship between the volume and number of moles of an ideal gas at constant pressure and temperature? 2. The height of the
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 information