A d. Par$cle size and the rate of dissolu$on. Consider the surface of the fixed amount of compound as the func$on of linear microcrystal
|
|
- Dwain Bell
- 5 years ago
- Views:
Transcription
1 Par$cle size and the rate of dissolu$on Consider the surface of the fixed amount of compound as the func$on of linear microcrystal size, d, and the total volume V For non-cubic shapes, calculate the Area as a func$on of total volume and shape. A d For simple cubic shape the total area of microcrystal surface is inversely propor$onal to the crystal size = V 6d 2 = d 3 6V d
2 Review The chemical poten$al of component J: Gas Liquid mixture ΔG and entropy of mixing. The chemical equilibrium K via concentra$ons and reac$on stoichiometry From K, to ΔG o From K at T 1 and T 2, to ΔH o, Van t Hoff K µ ln K g = µ 0 + i i µ = P c = µ 0 + i i Δ r G RT P RT ln( i P c RT ln i c a i is molar fraction x i or concentration c i or activity depending on the standard state and ideality n [ A B = ν ai i, e. g. K = i= 1 [ A][ B o ΔrH ln K = RT o ΔrS + R o K ln K 2 ΔH = R 0 0 ] ] 1 T1 T o )
3 Review Chemical poten$al of the same molecule in different phases or compartments (osmosis) must be equal Chemical poten$al of water is lower (beser) in solu$on If x solutes is small: Osmo$c pressure: P osm =MRT, where M is molarity corrected by dissocia$on, i, M=iM 0 Osmosis: semi permeable membranes. Osmolarity and Tonicity: coun$ng solutes that can not cross the membrane and taking dissocia$on into account ( i, van t Hoff s factor). Boiling point eleva$on Freezing point depression (K f does not depend on solutes!). K f = K kg/mol Water pressure reduc$on: Raoult s law Gas dissolu$on in water: Henry s law The effects are entropic and to the first approxima$on do not depend on the nature of solutes (colliga$ve proper$es) µ w _ in _ solution = µ w _ pure + RT ln(x w ) Δµ w = RT ln(1 x solutes ) RTx solutes ΔS w Rx solutes P osm = Δn sol RT = imrt V ΔT boiling = K b x solutes ΔT freezing = K f x solutes P w _ vap _ solution = P w _ vap _ pure x water P solute_in _ gas = K solute Henry x solute_in _ water
4 Review of Energy Contribu5ons to the non-covalent Binding Energy q-q: Coulomb: (+) or (-), strong in non-polar medium and weak in water. Long range (r -1 ). C=332 (kcal/mol)å(eu) -2 q-water: Ion and dipole Solva$on. Large (-):. D-H..A: Hbonds. Medium, short range. A-A: Van der Waals interac$on Weak (-0.2 km), but many. Short range (r -6 ). Apolar-Apolar Hydrophobic energy, water entropy contribu$on E el E solv w m = = C Cq 2r q q 1 ε E hb = f (r HA,α ALP HD) E vw = A r 12 B r 6 E hp = σ Area q 2 1 ε r 2 w 1 ε m
5 H.H.: a quan5ta5ve picture Most drugs are weak acids or weak bases It is not all or nothing, there are always several species at different concentra$ons [ A ] log HA [ ] [ B] log [ BH + ] = ph = ph pka pka K a pka + [H ][Base] =, [Acid] = log( K ph = log([ H a + ) ]) Drug Solu$ons (acidic and basic) ph = pk log c a ph = pk a logc
6 LogD depends on LogP of the neutral form O OH and ph-pk a pka = 4.2; LogD (ph=7.2) = water octanol O OH [ AH ] log P = log [ AH ] oct wat O O log D = [ AH ] log [ AH ] oct wat + [ A + [ A ] ] oct wat O O LogD is apparent LogP logd = logp - log( ph-pk a) for acids logp (ph pka) (for ph> pka+1, charged form dominates) logd = logp - log( (ph-pk a)) for bases logp + (ph pka) (for ph < pka-1, charged form dominates)
7 Binding Reac5on PL P + L; K d = [P][L]/[PL] ; K a = 1/K d x = [PL]; (P 0 -x)(l 0 -x) = x K d x = ½ ( P 0 + L 0 + K 0 - ((P 0 + L 0 + K 0 ) 2-4P 0 L 0 ) ½ ) P 0 << K d : [PL]/[P] L 0 /K d (50% L 0 = K d ) [PL] << P 0 (protein in excess) : [PL]/[L] P 0 /K d, frac$on_drug_bound P 0 / (P 0 +K d )
8 Kine5cs and Diffusion k = Ae G activation RT [A] = [A] o kt J = D dc dx ΔC [Drug] = Flux(J) Area(A) Time K eq = [B] [A] = k f k r [A] = [A] o e kt 1 [ A] 1 A [ ] 0 = k 2 t K bind = [PL] [P][L] = k on k off K d = [P][L] [PL] = k off k on
9 Braggs Law of Diffrac$on Methods The diffrac$on condi$on for a crystal 2d sinθ = nλ λ is the wavelength of gamma-rays ( ~ 1.5A ) d is the distance between planes, θ is the angle of diffrac$on and n is an integer known as the order of the diffracted beam F = q( E + v B) ( m / q) a = E + v ν = γb B Lorenz force mv R R = 2 = m q qvb v B
10 Waves An X-ray picture (radiograph), taken by Wilhelm Röntgen in 1896, of Albert von Kölliker's hand. Wilhelm Röntgen λ = c / f ω = 2π f = 2π / T E = hf = ω E mole = N A ω E X ray ~ ~ J / mol!
11 Two and five slit diffrac5on In a crystal millions of planes in direc$on lead to coherent rays in the Bragg direc$ons d λ/2 Minimum λ maximum 2-slit and 5-slit diffrac$on
12 Diffrac5on: Bragg s Law The path difference is 2dsinθ The diffrac$on condi$on for a crystal 2d sinθ = nλ λ is the wavelength of gamma-rays ( ~ 1.5A ) d is the distance between planes, θ is the angle of diffrac$on and n is an integer known as the order of the diffracted beam In 1915, William Henry Bragg and William Lawrence Bragg were awarded the Nobel Prize for their contribu$ons to crystal structure analysis. They were the first and (so far) the only father-son team to have jointly won the prize. Coherence will only be achieved for certain values of θ for each set of planes
13 Diffrac5on from a single crystal Each spot corresponds to a set of parallel planes 2d sinθ = nλ
14 Single Crystal Only one crystal is mounted for X-ray crystallography In this crystal all unit cells are oriented the same way
15 Waves An X-ray picture (radiograph), taken by Wilhelm Röntgen in 1896, of Albert von Kölliker's hand. Wilhelm Röntgen Waves and diffrac$on X-rays: single crystals to 3D electron density Bragg s condi$on (2dsinθ=nλ ) Unit cell, asymmetric unit, non-crys. symmetry
16 The phase problem Each spot needs: 3 coordinates, h,k,l, intensity and phase, F hkl, A hkl To get the electron density map the Fourier transforma$on is used We need spot intensi$es and phases, but we only have intensi$es. Yet another limita$on of quality Direct methods Anomalous diffrac$on (MAD) molecular replacement
17 Mass Spectrometry Analy$cal tool measuring molecular weight of molecules in chemistry, biology and pharmacology Only picomolar concentra$ons required Within 5 ppm for small organic molecules For a 40 kda protein, there is a 4Da error MS can detect amino acid subs$tu$ons, posttransla$onal modifica$ons
18 From mass to compound iden5ty MS iden$fies a mass, but does not tell you what the compound is. Many molecules will have the same mass Interpreta$on of fragmenta$on paserns may help if you choose from a small set Proteins: with a fixed human genome, it may be possible
19 Physics behind MS An ion moves in a magne$c field A neutral molecule CAN NOT BE measured with MS Magne$c field bends the trajectories according to the ra$o m/q
20 Electric (E) and Magne5c (B) Fields Field = Force on a probe charge q=1 Current (I) flowing through a wire produces a magne$c field, B [tesla] E Coulomb = C q r source 2
21 Lorenz Force When charged molecules move in electric and magne$c fields In electric fields they accelerate. F el = qe In magne$c fields their trajectories bend F mg = qvb F = q( E + v B) ( m / q) a = E + v B
22 Radius of ion trajectory The a force is perpendicular to V it causes circular mo$on with accelera$on v 2 /R If magne$c field B is perpendicular to V, then ma = qv B mv R 2 = m R = q qvb v B
23 Mass-to-charge ra5o m/q, or m/e, or m/z, z is the electronic charge of a molecular ion or fragment. If z=+1,m = m/z Mass: isotopes are detected. E.g. 12 C, 13 C, 79 Br : 81 Br, intensity 1:1 and 35 Cl : 37 Cl, intensity 3:1 Charge: in an electron impact mass spectrometer, a high energy beam of electrons displaces an electron from the organic molecule to form a radical ca5on known as the molecular ion. If the molecular ion is too unstable then it can fragment to give other smaller ions.
24 Spectrum of 2-chloropropane Loss of Cl gives the main peak.
25 Separa5on of mixtures Chromotography, (greek, color- wri$ng) Chromatography exploits par$$on between a mobile phase and a sta$onary phase to separate the components in a mixture. Molecules interact with the sta$onary phase based on charge, rela$ve solubility or adsorp$on Gas, thin layer, paper, Column (liquid) ion-exchange (charge) size-exclusion (size) Affinity FPLC (proteins) and HPLC (pressure) Mikhail Semenovich Tsvet, , a Russian botanist. He used liquid - adsorp$on column chromatography Thin layer chromatography is used to separate components of chlorophyll
26 Chromatography terms Prepara5ve chromatography is used to nondestruc$vely purify sufficient quan$$es of a substance for further use, rather than analysis. Large HPLC columns. Analy5cal chromatography is used to determine the iden$ty and concentra$on of molecules in a mixture. Quan$ta$ve. Mid-size HPLC columns LC of LCMS. Small HPLC columns. The analyte is the substance which is to be purified A chromatogram is the visual output of the chromatograph. Different peaks -> different molecules The mobile phase is the analyte and solvent mixture which travels through the sta$onary phase The reten5on 5me is the characteris$c $me it takes for a par$cular molecule to pass through the system Sta5onary phase: Examples include the silica layer, or columns
27 HPLC High-performance (high pressure) LC
28 Shopping in Factory outlets The elu$on $me depends on the number and dura$on of stops
29 Approaching the Finals Friday: Next Friday: 8am, Review (IK), Exam
Waves. λ = c / f ω = 2π f = 2π / T. E = hf = ω E mole = N A. E X ray. ~ ~ J / mol! Wilhelm Röntgen
Waves An X-ray picture (radiograph), taken by Wilhelm Röntgen in 1896, of Albert von Kölliker's hand. Wilhelm Röntgen λ c / f ω 2π f 2π / T E hf ω E mole N A ω E X ray ~ 6 10 23 10 34 10 18 ~ 6 10 7 J
More informationFrom mass to compound iden3ty
Mass Spectrometry Analy&cal tool measuring molecular weight of molecules in chemistry, biology and pharmacology Only picomolar concentra&ons required Within 5 ppm for small organic molecules For a 40 kda
More informationDrug Stability & Kine1cs
Drug Stability & Kine1cs Rates of drug dissolu/on, permea/on, diffusion, metabolism, binding are controlled by the laws of chemical kine/cs Liquid (and even solid) dosage drug form is suscep/ble to: Hydrolysis
More informationDrug targets, Protein Structures and Crystallography
Drug targets, Protein Structures and Crystallography NS5B viral RNA polymerase (RNA dep) Hepa88s C drug Sofosbuvir (Sovaldi) FDA 2013 Epclusa - combina8on with Velpatasvir approved in in 2016) Prodrug
More informationBack to molecular interac/ons Quantum theory and molecular structure
Back to molecular interac/ons Quantum theory and molecular structure Atoms are arranged in 3D to cons1tute a molecule. Atoms in one molecule are connected by strong covalent bonds that are not easily broken
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 informationLECTURE 6 NON ELECTROLYTE SOLUTION
LECTURE 6 NON ELECTROLYTE SOLUTION Ch 45.5 pplied Phy Chem First Sem 2014-15 Ch 45.5 Exam II September 1/3 (Multiple Choice/Problem Solving) Coverage: Second/Third Laws of Thermodynamics Nonelectrolyte
More informationChem 112 Dr. Kevin Moore
Chem 112 Dr. Kevin Moore Gas Liquid Solid Polar Covalent Bond Partial Separation of Charge Electronegativity: H 2.1 Cl 3.0 H Cl δ + δ - Dipole Moment measure of the net polarity in a molecule Q Q magnitude
More informationClass XI Chapter 6 Thermodynamics Chemistry
Class XI Chapter 6 Chemistry Question 6.1: Choose the correct answer. A thermodynamic state function is a quantity (i) used to determine heat changes (ii) whose value is independent of path (iii) used
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 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 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 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 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 informationThinking Like a Chemist About Solution Properties UNIT 5 DAY 4
UNIT5-DAY4-LaB1230 Page 1 UNIT5-DAY4-LaB1230 Wednesday, January 23, 2013 5:43 PM Thinking Like a Chemist About Solution Properties UNIT 5 DAY 4 What are we going to learn today? Thinking Like a Chemist
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 informationPhysiology Unit 1 CHEMISTRY REVIEW
Physiology Unit 1 CHEMISTRY REVIEW Defini7ons Types of energy Kine7c vs. poten7al Forms of energy Chemical Ex: ATP Ma0er and Energy Electrical Ex: Ac7on poten7al of an neuron Mechanical Ex: Ac7on of muscles
More informationIntroduction to Chromatography
Introduction to Chromatography Dr. Sana Mustafa Assistant Professor Department of Chemistry, Federal Urdu University of Arts, Science & Technology, Karachi. What is Chromatography? Derived from the Greek
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 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 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 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 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 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 informationSimple Mixtures. Chapter 7 of Atkins: Section
Simple Mixtures Chapter 7 of Atkins: Section 7.5-7.8 Colligative Properties Boiling point elevation Freezing point depression Solubility Osmotic Pressure Activities Solvent Activity Solute Activity Regular
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 informationProblem solving steps
Problem solving steps Determine the reaction Write the (balanced) equation ΔG K v Write the equilibrium constant v Find the equilibrium constant using v If necessary, solve for components K K = [ p ] ν
More informationMonday (March 28)- Mass spectrometry Tuesday (March 29)- Experiment 6: Separa>ons ICP-MS calcula>ons
LOOKING AHEAD Monday (March 28)- Mass spectrometry Tuesday (March 29)- Experiment 6: Separa>ons ICP-MS calcula>ons Thursday (March 31)- Poster crea>on? Hayes on travel Monday (April 4)- Chromatographic
More informationPage Chap 13: PROPERTIES of SOLUTIONS TYPES of SOLUTIONS. Degrees of Solution
Chap 13: PROPERTIES of SOLUTIONS Describe the solution process in terms of solutesolvent interactions and thermodynamics Calculate solution concentrations in terms of molarity, molality, and percentaes
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 informationEquations: q trans = 2 mkt h 2. , Q = q N, Q = qn N! , < P > = kt P = , C v = < E > V 2. e 1 e h /kt vib = h k = h k, rot = h2.
Constants: R = 8.314 J mol -1 K -1 = 0.08206 L atm mol -1 K -1 k B = 0.697 cm -1 /K = 1.38 x 10-23 J/K 1 a.m.u. = 1.672 x 10-27 kg 1 atm = 1.0133 x 10 5 Nm -2 = 760 Torr h = 6.626 x 10-34 Js For H 2 O
More information5.4 Liquid Mixtures. G i. + n B. = n A. )+ n B. + RT ln x A. + RT ln x B. G = nrt ( x A. ln x A. Δ mix. + x B S = nr( x A
5.4 Liquid Mixtures Key points 1. The Gibbs energy of mixing of two liquids to form an ideal solution is calculated in the same way as for two perfect gases 2. A regular solution is one in which the entropy
More informationCHEM 102 Final Mock Exam
CHEM 102 Final Mock Exam 1. A system releases 300 J of heat and does 650 J of work on the surroundings. What is the change in internal energy of the system? a. -950 J b. 350 J c. 950 J d. -350 J 2. Which
More informationCHAPTER 11: INTERMOLECULAR FORCES AND LIQUIDS AND SOLIDS. Chemistry 1411 Joanna Sabey
CHAPTER 11: INTERMOLECULAR FORCES AND LIQUIDS AND SOLIDS Chemistry 1411 Joanna Sabey Forces Phase: homogeneous part of the system in contact with other parts of the system but separated from them by a
More informationThe change in free energy on transferring an ion from a medium of low dielectric constantε1 to one of high dielectric constant ε2:
The Born Energy of an Ion The free energy density of an electric field E arising from a charge is ½(ε 0 ε E 2 ) per unit volume Integrating the energy density of an ion over all of space = Born energy:
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 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 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 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 informationGeneral Physical Chemistry I
General Physical Chemistry I Lecture 14 Aleksey Kocherzhenko April 9, 2015" Last time " Chemical potential " Partial molar property the contribution per mole that a substance makes to an overall property
More informationChem 1A, Fall 2015, Midterm Exam 3. Version A November 17, 2015 (Prof. Head-Gordon) 2. Student ID: TA:
Chem 1A, Fall 2015, Midterm Exam 3. Version A November 17, 2015 (Prof. Head-Gordon) 2 Name: Student ID: TA: Contents: 6 pages A. Multiple choice (10 points) B. Thermochemistry and Equilibria (12 points)
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 informationPhysical Chemistry Chapter 4 The Properties of Mixtures
Physical Chemistry Chapter 4 The Properties of Mixtures by Izirwan Bin Izhab FKKSA izirwan@ump.edu.my Chapter Description Aims Determine the fugacity and fugacity coefficients for pure species using generic
More informationQuantum Condensed Matter Physics Lecture 5
Quantum Condensed Matter Physics Lecture 5 detector sample X-ray source monochromator David Ritchie http://www.sp.phy.cam.ac.uk/drp2/home QCMP Lent/Easter 2019 5.1 Quantum Condensed Matter Physics 1. Classical
More informationCHROMATOGRAPHY AND MASS SPECTROMETER
22 CHROMATOGRAPHY AND MASS SPECTROMETER 22.1 INTRODUCTION We know that the biochemistry or biological chemistry deals with the study of molecules present in organisms. These molecules are called as biomolecules
More informationPrac%ce, Week 1. Therapeu%c substance Gases
Prac%ce, Week 1 Therapeu%c substance Gases Metric prefixes Prefix Symbol Factor Factor (sci. nota8on) peta P 1,000,000,000,000,000 10 15 tera T 1,000,000,000,000 10 12 giga G 1,000,000,000 10 9 mega M
More informationsolutes solvent solu)on dissolved
Solu%ons Liquids can make weak intermolecular bonds to chemically different molecules called solutes. The solutes enter the liquid (called a solvent) as individual par%cles and the mixture is called a solu)on.
More informationMixtures, Equilibrium & Chemical Poten/al µ
Mixtures, Equilibrium & Chemical Poten/al µ Single compartment Total G -> minumum A (gas) A (liquid) equlibrium Solu9ons Suspensions Colloids (milk, nanopar/cles, colloidal silver, sulphur, gold) Two compartments
More informationOpen Column Chromatography, GC, TLC, and HPLC
Open Column Chromatography, GC, TLC, and HPLC Murphy, B. (2017). Introduction to Chromatography: Lecture 1. Lecture presented at PHAR 423 Lecture in UIC College of Pharmacy, Chicago. USES OF CHROMATOGRAPHY
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 informationSchool of Chemical & Biological Engineering, Konkuk University
School of Chemical & iological Engineering, Konkuk University Lecture 7 Ch. 5 Simple Mixtures Colligative properties Prof. Yo-Sep Min Physical Chemistry I, Spring 2009 Ch. 5-2 he presence of a solute in
More informationIntermolecular Forces and Liquids and Solids
PowerPoint Lecture Presentation by J. David Robertson University of Missouri Intermolecular Forces and Liquids and Solids Chapter 11 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction
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 informationIntermolecular Forces and Liquids and Solids. Chapter 11. Copyright The McGraw Hill Companies, Inc. Permission required for
Intermolecular Forces and Liquids and Solids Chapter 11 Copyright The McGraw Hill Companies, Inc. Permission required for 1 A phase is a homogeneous part of the system in contact with other parts of the
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 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. 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 informationNANOLCMS SOLUTIONS HPLC BASICS
NANOLCMS SOLUTIONS HPLC BASICS Main Course Topics This course is designed to provide a basic founda@on to HPLC principles. It includes a wealth of informa@on regarding HPLC instrumenta@on and HPLC columns.
More informationLiquid in liquid: ethanol in water. Solid in liquid: any salt in water. Solid in solid: brass, bronze, and all alloys
1 of 6 I. The solution process Solutions, colloids, and suspensions Solution: homogeneous mixture, equally dispersed at the molecular level, uniform throughout in its physical and chemical properties Colloid:
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 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 informationKEMS448 Physical Chemistry Advanced Laboratory Work. Freezing Point Depression
KEMS448 Physical Chemistry Advanced Laboratory Work Freezing Point Depression 1 Introduction Colligative properties are properties of liquids that depend only on the amount of dissolved matter (concentration),
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 informationCRYSTAL STRUCTURE, PHASE CHANGES, AND PHASE DIAGRAMS
CRYSTAL STRUCTURE, PHASE CHANGES, AND PHASE DIAGRAMS CRYSTAL STRUCTURE CRYSTALLINE AND AMORPHOUS SOLIDS Crystalline solids have an ordered arrangement. The long range order comes about from an underlying
More informationMixtures of Compounds. The nature of solu5ons and concentra5on in g/ml, percents and molar units.
Mixtures of Compounds The nature of solu5ons and concentra5on in g/ml, percents and molar units. 9.1 Mixtures and Solu5ons Heterogeneous mixture: A nonuniform mixture that has regions of different composi5on.
More informationln K = Δ reactiong o RT
Review: concentra%ons and energies Rela%onship between Gibbs free energy of reac%on and the equilibrium concentra%ons is defined by constant K K = C ν D ν D C E E.. ν C A ν A C B B.. ln K = Δ reactiong
More informationHow to study minerals?!
How to study minerals?! ü What tools did scientists have from pre-history to Renaissance? Eyes and measuring devices Calcite Crystal faces! ü One of the most spectacular aspect of minerals ü NOTE: No mention
More informationChapter 9. Solutions
Chapter 9 Solutions Water Properties Polar O more electronegative, partial negative charge H less electronegative, partial positive charge Bent structure, 2 lone pairs on oxygen Participates in HYDROGEN
More informationChem 75 February, 2017 Practice Exam 2
As before, here is last year s Exam 2 in two forms: just the questions, and then the questions followed by their solutions. 1. (2 + 6 + 8 points) At high temperature, aluminum nitride, AlN(s), decomposes
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 informationPhysical Biochemistry. Kwan Hee Lee, Ph.D. Handong Global University
Physical Biochemistry Kwan Hee Lee, Ph.D. Handong Global University Week 9 CHAPTER 4 Physical Equilibria Basic Concepts Biological organisms are highly inhomogeneous. Different regions of each cell have
More informationBasic Mathema,cs. Rende Steerenberg BE/OP. CERN Accelerator School Basic Accelerator Science & Technology at CERN 3 7 February 2014 Chavannes de Bogis
Basic Mathema,cs Rende Steerenberg BE/OP CERN Accelerator School Basic Accelerator Science & Technolog at CERN 3 7 Februar 014 Chavannes de Bogis Contents Vectors & Matrices Differen,al Equa,ons Some Units
More informationPure Liquid with solute. Pure Liquid
Colligative properties are physical properties of solutions that arise because of the number of solute molecules dissolved in solution and not on the kind of solute particles dissolved in solution. Pure
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 informationCh 13 The Properties of Mixtures: Solutions and Colloids
Ch 13 The Properties of Mixtures: Solutions and Colloids Key equations: Concentration Unit - Quantitative Ways of Expressing Concentration Principles of Solubility Colligative Properties of Solutions nonelectrolyte
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 informationCH 302 Unit 3 Exam Review NUCLEAR, KINETICS, INORGANIC
CH 302 Unit 3 Exam Review NUCLEAR, KINETICS, INORGANIC Learning ObjecDves - Nuclear Explain the macroscopic observables associated with Understand and explain the concept of isotopic stability nuclear
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 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 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 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 informationWhat is the ph of a 1.0 L 1M HCl solu7on that has reacted with 1.0L of a 1M NaOH solu7on?
5.1.12 What is the ph of a 1.0 L 1M HCl solu7on that has reacted with 1.0L of a 1M NaOH solu7on? Today fundamentals of 7tra7on Calculate expected ph resul7ng from 7tra7on of a strong acid with a strong
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 18. Redox Reac)on. Oxida)on & Reduc)on 4/8/08. Electrochemistry
Chapter 18 Electrochemistry Redox Reac)on One or more elements change oxida)on number all single displacement, and combus)on, some synthesis and decomposi)on Always have both oxida)on and reduc)on split
More informationCOLLIGATIVE PROPERTIES. Engr. Yvonne Ligaya F. Musico 1
COLLIGATIVE PROPERTIES Engr. Yvonne Ligaya F. Musico 1 Colligative Properties Properties that depend on the collective effect of the number of solute particles. Engr. Yvonne Ligaya F. Musico 2 COLLEGATIVE
More informationVERSION A White. perm. version. name. Chem 1C - Spring exam 2
Chem 1C - Spring 2010 - exam 2 VERSION A White ON YOUR SCANTRON: BUBBLE IN YOUR 7 DIDGIT PERM (Leaving the last three digits blank) BUBBLE IN THE VERSION: A WRITE YOUR NAME AT THE END, HAND IN ONLY THE
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 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 informationCHEM 121a Exam 4 Fall 1998
Name SSN CHEM 121a Exam 4 Fall 1998 This exam consists of 8 true-false questions (each worth 2 pts), 20 multiple choice questions (each worth 3 pts), and 3 short problems (each worth 8 pts). There are
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 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 informationDO NOT OPEN UNTIL INSTRUCTED TO DO SO. CHEM 111 Dr. McCorkle Exam #1. While you wait, please complete the following information:
DO NOT OPEN UNTIL INSTRUCTED TO DO SO CHEM 111 Dr. McCorkle Exam #1 While you wait, please complete the following information: Name: Student ID: Turn off cellphones and stow them away. No headphones, mp3
More informationFailures and successes of the free electron model
Failures and successes of the free electron model Temperature dependence on the electric conduc1vity j e = E = ne2 m electron gas electron- phonon coupling Drude s model predicts that σ is independent
More informationChemistry 112 ACS Final
Chemistry 112 ACS Final Exam at 4 pm in ECTR 118 and you will be done by 6 pm Stop at question 56 Topics covered are below.honestly, the best way to study is to read through your notes multiple times making
More informationFACULTY OF SCIENCE MID-TERM EXAMINATION 2 MARCH 18, :30 TO 8:30 PM CHEMISTRY 120 GENERAL CHEMISTRY
FACULTY OF SCIENCE MID-TERM EXAMINATION 2 MARCH 18, 2011. 6:30 TO 8:30 PM CHEMISTRY 120 GENERAL CHEMISTRY Examiners: Prof. B. Siwick Prof. A. Mittermaier Dr. A. Fenster Name: Associate Examiner: A. Fenster
More informationVERSION B Yellow. perm. version. name. Chem 1C - Spring exam 2
Chem 1C - Spring 2010 - exam 2 VERSION B Yellow ON YOUR SCANTRON: BUBBLE IN YOUR 7 DIDGIT PERM (Leaving the last three digits blank) BUBBLE IN THE VERSION: B WRITE YOUR NAME AT THE END, HAND IN ONLY THE
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 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 informationSolutions. Making sense of the aqueous world
Solutions Making sense of the aqueous world 2012-01-24 13:13:55 1/42 Notessolutionsroessler (#2) Solution 2012-01-24 13:13:55 2/42 Notessolutionsroessler (2/42) Solutions They are homogenous Homogenous-
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 information