Simulation of Electrolyte Processes: Status and Challenges
|
|
- Hope Hopkins
- 6 years ago
- Views:
Transcription
1 Simulation of Electrolyte Processes: Status and Challenges Paul M Mathias and Chau-Chyun Chen Aspen Technology, Inc. 12 March 2002 AIChE Spring 2002 Meeting AIChE 2002 Spring Meeting.
2 Summary Opportunities/needs for electrolyte simulations Special complexities of electrolyte simulations Successes and status Future challenges AIChE 2002 Spring Meeting 2
3 Electrolyte applications are widespread in chemical technology Wastewater treatment Seawater desalination Gas scrubbing Normal and extractive crystallization Salt-effect enhanced extraction and distillation Hydrometallurgical processes Salt-added bioseparations.. AIChE 2002 Spring Meeting 3
4 Use of process simulation is standard practice, even for electrolyte processes Study process alternatives Assess feasibility and preliminary economics Interpret pilot-plant data Process design and optimization Pollution control Plant trouble-shooting Plant retrofit AIChE 2002 Spring Meeting 4
5 Finance / Planning/R&D Conceptual Design Process Engineering Detailed Engineering Construction / Start-up Operations / Asset Mgt,PSURYH&DSLWDO (IILFLHQF\ Reliable and consistent economic evaluation and project scheduling Synthesis for systematic exploration of design alternatives Modeling to accurately predict process performance AIChE 2002 Spring Meeting 5
6 Finance / Planning/R&D Conceptual Design Process Engineering,PSURYH Detailed (QJLQHHULQJ Engineering 4XDOLW\ (IILFLHQF\ Construction / Start-up Operations / Asset Mgt Concurrent engineering for error free and efficient workflow Consistent properties, models and economics throughout the life cycle Downstream integration with detail design (e.g. Intergraph) Fast evaluation of optimized alternatives AIChE 2002 Spring Meeting 6
7 Finance / Planning/R&D Conceptual Design Process Engineering Detailed Engineering Construction / Start-up Operations / Asset Mgt Consistent Models and Physical Properties for Accurate evaluation and prediction of plant performance Ability to solve large scale complex optimization problems On-line process monitoring and optimization,qfuhdvh 2SHUDWLRQDO 3URGXFWLYLW\ AIChE 2002 Spring Meeting 7
8 Special challenges of electrolyte processes Many extra species form due to ionization and complexation (e.g., aqueous FeCl 3 has 14 different species.) Solution nonideality is complex because of ionic forces and numerous species. Chemical and physical equilibrium must be solved simultaneously, causing problems for user interfaces and flash algorithms Kinetics and mass transfer often need to be included to develop an accurate model AIChE 2002 Spring Meeting 8
9 Successes and Status Aqueous FeCl 3 Sour water (aqueous CO 2 /H 2 S/NH 3 ) Scrubbing of CO 2 /Cl 2 with caustic Nitric acid AIChE 2002 Spring Meeting 9
10 FeCl 3 Aqueous Chemistry FECL3 l FECL2+ + CL- FE2OH2+4 l 2 FEIII OH- FECL2+ l FECL+2 + CL- FECL4- l FECL3 + CL- FECL+2 l FEIII+3 + CL- FEOH2+ l FEOH+2 + OH- FEIIIOH3 l FEOH2+ + OH- FEIIOH4- l FEIIIOH3 + OH- FEOH+2 l FEIII+3 + OH- H2O l H+ + OH- HCL l H+ + CL- Salt FECL3W6 l FEIII CL- + 6 H2O Salt FECL3-S l FEIII CL- Salt FEOH3-S l FEIII OH- Salt FECL3W25 l FEIII CL H2O Salt FECL3W2 l FEIII CL- + 2 H2O AIChE 2002 Spring Meeting
11 of 1 Mole FeCl 3 in Moles Water at 25qC and 1 atm Comp Moles Comp Moles H2O FECL HCL 2.634e-09 FEIII FEIIIOH e-09 FEOH e-06 FECL OH e-13 FE2OH e-07 FECL FECL e-06 FEIIOH e-16 FEOH H CL Fe complexes with OH to form FEOH+2, which shifts the water dissociation to form H+ ions. ph = 2.22 AIChE 2002 Spring Meeting
12 FeCl 3 Aqueous Chemistry FECL3 l FECL2+ + CL- FE2OH2+4 l 2 FEIII OH- FECL2+ l FECL+2 + CL- FECL4- l FECL3 + CL- FECL+2 l FEIII+3 + CL- FEOH2+ l FEOH+2 + OH- FEIIIOH3 l FEOH2+ + OH- FEIIOH4- l FEIIIOH3 + OH- FEOH+2 l FEIII+3 + OH- H2O l H+ + OH- HCL l H+ + CL- Salt FECL3W6 l FEIII CL- + 6 H2O Salt FECL3-S l FEIII CL- Salt FEOH3-S l FEIII OH- Salt FECL3W25 l FEIII CL H2O Salt FECL3W2 l FEIII CL- + 2 H2O AIChE 2002 Spring Meeting
13 ph of Aqueous FeCl 3 Solution at 25ºC ph E-08 1.E-06 1.E-04 1.E-02 1.E+00 Molality of FeCl 3 AIChE 2002 Spring Meeting
14 Sour Water System 7HPSHUDWXUH &DQG & /LTXLG&RPSRVLWLRQ 1+ PRODO ZW &2 PRODO ZW + 6 PRODO ZW + 2 EDODQFH AIChE 2002 Spring Meeting 14
15 Sour Water System - Model Vs. Data NH 3, CO 2, H 2 S Treated as Molecular Species Calculated Partial Pressures (mmhg) NH3 CO2 H2S Calc=Exp Experimental Partial Pressures (mmhg) AIChE 2002 Spring Meeting
16 Sour Water System - Model Vs. Data Electrolyte Speciation Included Calculated Partial Pressure (mmhg) NH3 CO2 H2S Calc=Exp Experimental Partial Pressure (mmhg) AIChE 2002 Spring Meeting
17 Electrolyte Reactions in Sour Water System H 2 O H + + OH - NH 3 (aq) + H 2 O NH 4+ + OH - CO 2 (aq) + H 2 O H + + HCO - 3 HCO - 3 H + + CO 2-3 NH 2 CO 2- + H 2 O NH 3 (aq) + HCO - 3 H 2 S(aq) H + + HS - HS - H + + S 2- AIChE 2002 Spring Meeting
18 Scrubbing of Cl 2 /CO 2 Gas with Caustic Caustic 1,200 kg/hr H 2 O 100+ kg/hr NaOH Gas 2.3 kmol/hr H 2 O 0.1+ kmol/hr CO kmol/hr Cl kmol/hr N 2 25 C 1 atm Scrubbed Gas Liquid Study scrubbing capacity as a function of CO 2 level and NaOH in caustic feed AIChE 2002 Spring Meeting
19 Aqueous Chemistry in Caustic Scrubbing of Cl 2 /CO 2 Salt Dissociation HCL H+ + CL- HCLO H+ + CLO- CO2 + H2O H+ + HCO3- H2O H+ + OH- HCO3- H+ + CO3-2 CL2 + H2O H+ + CL- + HCLO NACO3- NA+ + CO3-2 NAHCO3 NA+ + HCO3- NAHCO3-S NA+ + HCO3- NAOH OH- + NA+ AIChE 2002 Spring Meeting
20 Chlorine Mole Fraction in Exit Gas Cl2 Mole Fraction in Exit Gas E-05 1E-06 1E-07 1E-08 1E-09 1E-10 The numbers in the legend refer to the CO 2 flow in kgmole/hr High CO 2 Low CO NaOH:Cl 2 Mole Ratio AIChE 2002 Spring Meeting 20
21 0.009 Precipitation of NaHCO 3 Precip of NaHCO3 (NaHCO3/NaOH) The numbers in the legend refer to the CO 2 flow in kgmole/hr High CO 2 Low CO NaOH:Cl 2 Mole Ratio AIChE 2002 Spring Meeting 21
22 Challenges of Nitric Acid Modeling Performance is flow rate and pressure sensitive Multiple reactions occur in most equipment, including pipes, gas coolers, heat exchangers and condensers Special physical properties are needed for nitric acid VLE and heat of mixing calculations Absorption tower has rate-limited and equilibrium vapor and liquid reactions, rate-limited mass transfer, and cooling coils on most trays Many recycle streams for heat and power integration AIChE 2002 Spring Meeting
23 Electrolyte NRTL and Chemistry High Accuracy for thermodynamic properties: ƒ Vapor-liquid equilibrium ƒ Enthalpy ('H mix, C p ) ƒ Density H O+HNO 2 3 H O+ 3 + NO 3 AIChE 2002 Spring Meeting
24 Excess Enthalpy of Mixing of Nitric Acid- Water Mixtures at 25 C Excess Enthalpy (Cal/g) Weight% HNO 3 AIChE 2002 Spring Meeting 24
25 Heat Capacity (Cal/gm.K) Heat Capacity of Nitric Acid-Water Mixtures at 25 C Weight% HNO 3 AIChE 2002 Spring Meeting 25
26 Txy Diagram of Nitric Acid - Water at 760 Torr Temperature ( C) Full line is calculated dew point Dashed line is calculated bubble point Points are experimental data Liquid or Vapor Mole Fraction of HNO 3 AIChE 2002 Spring Meeting 26
27 Kinetics and Mass Transfer for Absorber Three gas-phase reactions: 1. 2NO + O 2 mo 2NO 2 -- Kinetic 2. 2NO mo 2 N 2 O N 2 O 4 + 2H 2 O mo 4HNO 3 + 2NO -- N 2 O 4 (g) o N 2 O 4 (l) Implemented in user subroutines NOABS Reaction 3 rate correlated as a function of: Temperature N 2 O 4 partial pressure Tray dimensions (e.g., column diameter) Liquid-phase HNO 3 concentration AIChE 2002 Spring Meeting 27
28 Input Variables for NOABS Integer variable: 1 sieve tray; 2 bubble-cap tray Real Variable 1 Description Column diameter (m) Suggested value From equipment 2 3 Bubble-cap slot or sieve-hole submergence (m) Factor for NO 2 formation From equipment 1 4 Factor for N 2 O 4 absorption rate 1 AIChE 2002 Spring Meeting 28
29 Tuning of Absorber Model Cooling-water flow assumed proportional to number of heaters UA: U 250 Btu/hr.ft 2. F, A from equipment measurement Vapor hold-ups from plant measurement Cooling water temperature from plant data Factor for NO 2 formation to match profile Factor for N 2 O 4 absorption to match profile Procedure gives accurate NO, NO 2 in tail gas, acid strength and temperature of tailgas compared to plant data AIChE 2002 Spring Meeting 29
30 Acid-Strength Profile in Absorber 80% 70% Acid Strength 60% 50% 40% 30% 20% 10% Plant Simulation 0% Tray AIChE 2002 Spring Meeting 30
31 Temperature Profile in Absorber Tray Temp ( F) Plant Simulation Tray AIChE 2002 Spring Meeting 31
32 Future Challenges Hands-on expertise and education Predictive methods for nonideality Mixed-solvent electrolytes Systems containing small molecules, polymers and electrolytes Ionic surfactants and micelle formation Reliable flash calculations, particularly for liquid-liquid systems New applications such as corrosion AIChE 2002 Spring Meeting 32
Chapter 2 Introduction to Aqueous Speciation
Chapter 2 Introduction to Aqueous Speciation Overview It is our belief that the predictive modeling of aqueous systems requires that the system be fully speciated. This allows for smoother extrapolation
More informationX212F Which of the following is a weak base in aqueous solution? A) H 2 CO 3 B) B(OH) 3 C) N 2 H 4 D) LiOH E) Ba(OH) 2
PX212SP14 Practice Exam II / Spring 2014 1. Which of the following statements are characteristic of acids? 1. They are proton donors. 2. They react with bases to produce a salt and water. 3. They taste
More informationMass Transfer in a Small Scale Flue Gas Absorber Experimental and Modeling
Mass Transfer in a Small Scale Flue Gas Absorber Experimental and Modeling P.J.G. Huttenhuis, E.P. van Elk, S. Van Loo, G.F. Versteeg Procede Gas Treating B.V., The Netherlands 11 th MEETING of the INTERNATIONAL
More informationOLI Simulation Conference 2010
OLI Simulation Conference 2010 Advances in OLI Simulation: Examples Wet Flue Gas Desulfurization and Amine Gas Sweetening Think Simulation! Harnessing the power of the OLI Engine James Berthold OLI Systems,
More informationThermodynamic model to study removal of Chlorine, Silicon Tetrafluoride and other uncommon materials from off gases
A publication of CHEMICAL ENGINEERING TRANSACTIONS VOL. 69, 018 Guest Editors: Elisabetta Brunazzi, Eva Sorensen Copyright 018, AIDIC Servizi S.r.l. ISBN 978-88-95608-66-; ISSN 83-916 The Italian Association
More information9.1 Water. Chapter 9 Solutions. Water. Water in Foods
Chapter 9 s 9.1 Water 9.1 Properties of Water 9.2 s 9.3 Electrolytes and Nonelectrolytes 9.6 Percent Concentration 9.7 Molarity Water is the most common solvent. The water molecule is polar. Hydrogen bonds
More informationChE 201 August 26, ChE 201. Chapter 8 Balances on Nonreactive Processes Heat of solution and mixing
ChE 201 Chapter 8 Balances on Nonreactive Processes Heat of solution and mixing Definitions A solution is a homogeneous mixture A solute is dissolved in a solvent. solute is the substance being dissolved
More informationAvailable online at Energy Procedia 00 (2008) GHGT-9
Available online at www.sciencedirect.com Energy Procedia (8) Energy Procedia www.elsevier.com/locate/xxx GHGT-9 Quantitative Evaluation of the Aqueous-Ammonia Process for CO Capture Using Fundamental
More information2. Write a balanced chemical equation which corresponds to the following equilibrium constant expression.
Practice Problems for Chem 1B Exam 1 Chapter 14: Chemical Equilibrium 1. Which of the following statements is/are CORRECT? 1. For a chemical system, if the reaction quotient (Q) is greater than K, products
More informationOutline. Water The Life Giving Molecule. Water s Abundance. Water
Chapter 3 Water and Life Outline I. Water A. Properties of water II. Acids and Bases Water The Life Giving Molecule Water s Abundance Why are we so interested in finding evidence of water on Mars? What
More informationChapter 16 Aqueous Ionic Equilibrium Buffer Solutions
Chapter 16 Aqueous Ionic Equilibrium 16.1-16.2 Buffer Solutions Why? While a weak acid will partially ionize to produce its conjugate base, it will not produce enough conjugate base to be considered a
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 informationESP FLOWSHEET SIMULATION APPLICATION BRIEF Chlor-Alkali Simulation
ESP FLOWSHEET SIMULATION APPLICATION BRIEF Chlor-Alkali Simulation Revised April 10, 2012 1 The anode in an electrochemical cell is the strongest oxidizer known, as it is fully capable of taking an electron
More informationWater - HW. PSI Chemistry
Water - HW PSI Chemistry Name 1) In a single molecule of water, the two hydrogen atoms are bonded to a single oxygen atom by A) hydrogen bonds. B) nonpolar covalent bonds. C) polar covalent bonds. D) ionic
More informationChapter 14. Objectives
Section 1 Properties of Acids and Bases Objectives List five general properties of aqueous acids and bases. Name common binary acids and oxyacids, given their chemical formulas. List five acids commonly
More informationAcids and bases, as we use them in the lab, are usually aqueous solutions. Ex: when we talk about hydrochloric acid, it is actually hydrogen chloride
Acids and Bases Acids and bases, as we use them in the lab, are usually aqueous solutions. Ex: when we talk about hydrochloric acid, it is actually hydrogen chloride gas dissolved in water HCl (aq) Concentrated
More informationAcids. Names of Acids. Naming Some Common Acids. Solution. Learning Check Acids and Bases. Arrhenius acids Produce H + ions in water.
Chapter 10 Acids and Bases Acids 10.1 Acids and Bases Arrhenius acids Produce H + ions in water. H 2 O HCl(g) H + (aq) + Cl (aq) Are electrolytes. Have a sour taste. Turn litmus red. Neutralize bases.
More informationCHEMICAL EQUILIBRIUM -3
CHEMICAL EQUILIBRIUM -3 1. Arrhenius neutralisation involves 1. formation of dative bond. formation of water by the combination of H + with OH - 3. transfer of proton 4.all of these. NH 3 is not a base
More informationGeneral Chemistry Study Guide
General Chemistry 1311 Study Guide Name : Louise K number: Date: Oct 02006 Instructor: Jingbo Louise Liu kfjll00@tamuk.edu 1 Chapter 04 & 05 (10 questions required and 5 questions for extra credit) Credited
More information1 A. That the reaction is endothermic when proceeding in the left to right direction as written.
1 Q. If Δ r H is positive, what can you say about the reaction? 1 A. That the reaction is endothermic when proceeding in the left to right direction as written. 2 Q If Δ r H is negative, what can you say
More informationChapter 4 Outline. Electrolytic Properties
+4.1 - General Properties of Aqueous Solutions Solution = a homogeneous mixture of two or more substances Solvent = substance present in greatest quantity Solute = the other substance(s) present in a solution
More informationChapter 8 Acids, Bases, and Acid-Base Reactions. An Introduction to Chemistry by Mark Bishop
Chapter 8 Acids, Bases, and Acid-Base Reactions An Introduction to Chemistry by Mark Bishop Chapter Map Arrhenius Base Definitions A base is a substance that generates OH when added to water. A basic solution
More informationChapter 16 - Acids and Bases
Chapter 16 - Acids and Bases 16.1 Acids and Bases: The Brønsted Lowry Model 16.2 ph and the Autoionization of Water 16.3 Calculations Involving ph, K a and K b 16.4 Polyprotic Acids 16.1 Acids and Bases:
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 informationChapter 4 Electrolytes Acid-Base (Neutralization) Oxidation-Reduction (Redox) Reactions. Dr. Sapna Gupta
Chapter 4 Electrolytes Acid-Base (Neutralization) Oxidation-Reduction (Redox) Reactions Dr. Sapna Gupta Types of Reactions Two classifications: one how atoms are rearrangement and the other is chemical
More informationStation 1 ACIDS, BASES, AND NEUTRALS Classify each statement as talking about an [A]cid, [B]ase, or [N]eutral. B feels slippery
South Pasadena Honors Chemistry Name 4 Salts and Solutions Period Date / / Station 1 ACIDS, BASES, AND NEUTRALS Classify each statement as talking about an [A]cid, [B]ase, or [N]eutral. B feels slippery
More informationChem 106 Thursday, March 10, Chapter 17 Acids and Bases
Chem 106 Thursday, March 10, 2011 Chapter 17 Acids and Bases K a and acid strength Acid + base reactions: Four types (s +s, s + w, w + s, and w + w) Determining K from concentrations and ph ph of aqueous
More informationHomework #7 Chapter 8 Applications of Aqueous Equilibrium
Homework #7 Chapter 8 Applications of Aqueous Equilibrium 15. solution: A solution that resists change in ph when a small amount of acid or base is added. solutions contain a weak acid and its conjugate
More informationChem 127, Final Exam December 14, 2001
I. (55 points) This part of the final corresponds to Exam I. It covers the material in Chapters 1, 2 and 3. A. (8 points) Fill in the empty boxes with the appropriate symbol, number, word or charge. Nuclear
More informationGas Laws. Bonding. Solutions M= moles solute Mass %= mass solute x 100. Acids and Bases. Thermochemistry q = mc T
Name Period Teacher Practice Test: OTHS Academic Chemistry Spring Semester 2017 The exam will have 100 multiple choice questions (1 point each) Formula sheet (see below) and Periodic table will be provided
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 informationFormation of a salt (ionic compound): Neutralization reaction. molecular. Full ionic. Eliminate spect ions to yield net ionic
Formation of a salt (ionic compound): Neutralization reaction molecular Full ionic Eliminate spect ions to yield net ionic Hydrolysis/ reaction with water Anions of Weak Acids Consider the weak acid HF
More informationSOLUTIONS. Dissolution of sugar in water. General Chemistry I. General Chemistry I CHAPTER
11 CHAPTER SOLUTIONS 11.1 Composition of Solutions 11.2 Nature of Dissolved Species 11.3 Reaction Stoichiometry in Solutions: Acid-Base Titrations 11.4 Reaction Stoichiometry in Solutions: Oxidation-Reduction
More informationStation 1 ACIDS, BASES, AND NEUTRALS Classify each statement as talking about an [A]cid, [B]ase, or [N]eutral. feels slippery.
Name Period Date / / Station 1 ACIDS, BASES, AND NEUTRALS Classify each statement as talking about an [A]cid, [B]ase, or [N]eutral. feels slippery CH3OH tastes sour H + donor KOH increases [OH - ] turns
More informationElectrolytes do conduct electricity, in proportion to the concentrations of their ions in solution.
Chapter 4 (Hill/Petrucci/McCreary/Perry Chemical Reactions in Aqueous Solutions This chapter deals with reactions that occur in aqueous solution these solutions all use water as the solvent. We will look
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 State why water acts as a common solvent. Draw the structure of water, including partial charge. Write equations
More informationChapter 4 - Types of Chemical Reactions and Solution Chemistry
Chapter 4 - Types of Chemical Reactions and Solution Chemistry 4.1 Water, the Common Solvent - the water molecule is bent with and H-O-H angles of approx. 105 º - O-H bonds are covalent - O is slightly
More informationChapter 4. Reactions in Aqueous Solution
Chapter 4. Reactions in Aqueous Solution 4.1 General Properties of Aqueous Solutions A solution is a homogeneous mixture of two or more substances. A solution is made when one substance (the solute) is
More informationChapter Four Learning Objectives. Ions in Aqueous Solution: Electrolytes
Chapter Four Learning Objectives understand the nature of ions dissolved in water determine the products of and write chemical equations for precipitation, acid-base, and oxidation-reduction reactions
More informationPy x P P P. Py x P. sat. dq du PdV. abs Q S. An Innovative Approach in the G U TS PV P P G U TS PV T H U PV H U PV. abs. Py x P. sat.
E a 1 1 sat sat ln Py x P Py x P K H k Ae R E sat a Py x P 1 1 sat ln K1 R Py x P K H k Ae R 1 CO P H 1 1 abs ln K H H 1/ R Q C 1 1 CO P ln S K H K1 R 1 P H abs H P K1 R CP 1 K1 R 1/ R S Q P 1 E a E du
More informationSolutions. LiCl (s) + H2O (l) LiCl (aq) 3/12/2013. Definitions. Aqueous Solution. Solutions. How Does a Solution Form? Solute Solvent solution
Solutions Definitions A solution is a homogeneous mixture A solute is dissolved in a solvent. solute is the substance being dissolved solvent is the liquid in which the solute is dissolved an aqueous solution
More informationF.Y.B.Sc BIOTECH TOPIC: ACID BASE
F.Y.B.Sc BIOTECH TOPIC: ACID BASE 2016-17 Q.1) Define the following terms: 1)Electrolyte: A substance which forms a conducting solution when dissolved in water is called an electrolyte. 2) Strong electrolyte:
More informationChapter 15 - Acids and Bases Fundamental Concepts
Chapter 15 - Acids and Bases Fundamental Concepts Acids and Bases: Basic Definitions Properties of Acids Sour Taste React with active metals (Al, Zn, Fe) to yield H 2 gas: Corrosive React with carbonates
More informationChapter 4. Reactions in Aqueous Solution. Solutions. 4.1 General Properties of Aqueous Solutions
Chapter 4 in Solution 4.1 General Properties of Solutions Solutions Solutions are defined as homogeneous mixtures of two or more pure substances. The solvent is present in greatest abundance. All other
More informationShifting Equilibrium. Section 2. Equilibrium shifts to relieve stress on the system. > Virginia standards. Main Idea. Changes in Pressure
Section 2 Main Ideas Equilibrium shifts to relieve stress on the system. Some ionic reactions seem to go to completion. Common ions often produce precipitates. > Virginia standards CH.3.f The student will
More informationPage 1. Spring 2002 Final Exam Review Palmer Graves, Instructor MULTIPLE CHOICE
Page 1 MULTIPLE CHOICE 1. Which one of the following exhibits dipole-dipole attraction between molecules? a) XeF b) AsH c) CO d) BCl e) Cl 2. What is the predominant intermolecular force in AsH? a) London-dispersion
More informationCHEMISTRY Matter and Change
CHEMISTRY Matter and Change UNIT 18 Table Of Contents Section 18.1 Introduction to Acids and Bases Unit 18: Acids and Bases Section 18.2 Section 18.3 Section 18.4 Strengths of Acids and Bases Hydrogen
More informationACID BASE EQUILIBRIUM
ACID BASE EQUILIBRIUM Part one: Acid/Base Theories Learning Goals: to identify acids and bases and their conjugates according to Arrhenius and Bronstead Lowry Theories. to be able to identify amphoteric
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 informationQuiz name: Equilibria + Acids/Bases
Name: Quiz name: Equilibria + Acids/Bases Date: 1. 2. At 450 C, 2.0 moles each of H 2(g), I 2(g), and HI are combined in a 1.0 L rigid container. The value of K c at 450 C is 50. Which of the following
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Oxidation is the and reduction is the. A) loss of oxygen, gain of electrons B) gain of
More informationAcids and Bases. Click a hyperlink or folder tab to view the corresponding slides. Exit
Acids and Bases Section 18.1 Introduction to Acids and Bases Section 18.2 Strengths of Acids and Bases Section 18.3 Hydrogen Ions and ph Section 18.4 Neutralization Click a hyperlink or folder tab to view
More informationStoichiometry. Percent composition Part / whole x 100 = %
Stoichiometry Conversion factors 1 mole = 6.02 x 10 23 atoms (element) 1 mole = 6.02 x 10 23 molecules (covalent compounds) 1 mole = 6.02 x 10 23 formula units (ionic compounds) 1 mole (any gas @ STP)
More informationCHEMISTRY - TRO 4E CH.6 - THERMOCHEMISTRY.
!! www.clutchprep.com CONCEPT: ENERGY CHANGES AND ENERGY CONSERVATION is the branch of physical science concerned with heat and its transformations to and from other forms of energy. is the branch of chemistry
More information2. If a gas is released in a reaction (ex: Hydrogen gas bubbles off), is it written as a reactant or a product?
PRE-AP CHEMISTRY SPRING FINAL EXAM REVIEW Name _ Period Exam Date 100% COMPLETION OF THIS REVIEW BY THE DAY OF YOUR FINAL EXAM WILL COUNT AS A 5 POINT BONUS ADDED TO YOUR FINAL EXAM SCORE. THERE WILL BE
More information10. Calculate the mass percent nitrogen in (NH 4 ) 2 CO 3 (molar mass = g/mol). a % c % e % b % d % f. 96.
Chem 1721/1821: Final Exam Review Multiple Choice Problems 1. What is the molar mass of barium perchlorate, Ba(ClO 4 ) 2? a. 189.90 g/mol c. 272.24 g/mol e. 336.20 g/mol b. 240.24 g/mol d. 304.24 g/mol
More informationChapters 15 & 16 ACIDS & BASES ph & Titrations
PROPERTIES OF ACIDS Chapters 15 & 16 ACIDS & BASES ph & Titrations There are 5 main properties of acids: 1. sour taste 2. change the color of acidbase indicators 3. react with metals to produce H2 gas
More informationHOMEWORK 1C. (d) 2D + E 2F K eq = 1 x 10 9 I C E
HOMEWORK 1A 1. Write the correct equilibriumconstant expressions for the following reactions. (a) 4NH 3 (g) + 7O 2 (g) 4NO 2 (g) + 6H 2 O (g) (b) 2NO 2 (g) + 7H 2 (g) 2NH 3 (g) + 4H 2 O (g) (c) NH 4 Cl
More informationEquations. M = n/v. M 1 V 1 = M 2 V 2 if the moles are the same n 1 n 2 you can cancel out the n s. ph = -log [H + ] poh = -log [OH - ] ph + poh = 14
Equations M = n/v M 1 V 1 = M 2 V 2 if the moles are the same n 1 n 2 you can cancel out the n s. ph = -log [H + ] poh = -log [OH - ] ph + poh = 14 [H 3 O + ] = 10^-pH [OH - ] = 10^-pOH [H 3 O + ] [OH
More informationChapter 4 Electrolytes and Aqueous Reactions. Dr. Sapna Gupta
Chapter 4 Electrolytes and Aqueous Reactions Dr. Sapna Gupta Aqueous Solutions Solution - a homogeneous mixture of solute + solvent Solute: the component that is dissolved Solvent: the component that does
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 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 informationAcids and Bases. Unit 10
Acids and Bases Unit 10 1 Properties of Acids and Bases Acids Bases Taste Sour Turns Litmus Dye Red Reacts with Metals to give H 2 (g) Taste Bitter Turns Litmus Dye Blue Do Not React with Metals Reacts
More informationH = Hydrogen atoms O = Oxygen atoms
CHEMISTRY CP Name: KEY Period: TEST DATE: Unit 8 Review Sheet KEY: Properties of Water, Solutions, Concentration, Acids and Bases PROPERTIES OF WATER 1. Define the following terms: polarity, surface tension,
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 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 informationChapter 15. Acid-Base Equilibria
Chapter 15 Acid-Base Equilibria The Common Ion Effect The common-ion effect is the shift in an ionic equilibrium caused by the addition of a solute that provides an ion already involved in the equilibrium
More informationLiquids, Solids and Solutions
1 Liquids, Solids and Solutions This is a broad topic that will be spread out over several questions. This is section that will have lots of conceptual problems, but mathematical ones can also happen as
More informationChemical Equilibrium. What is the standard state for solutes? a) 1.00 b) 1 M c) 100% What is the standard state for gases? a) 1 bar b) 1.
Chemical Equilibrium Equilibrium constant for the reaction: aa + bb + cc + dd + [C ] c [D ] d... equilibrium constant K = [ A] a [B ] b... [] = concentration relative to standard state molarity (M): for
More information7/16/2012. Chapter Four: Like Dissolve Like. The Water Molecule. Ionic Compounds in Water. General Properties of Aqueous Solutions
General Properties of Aqueous Solutions Chapter Four: TYPES OF CHEMICAL REACTIONS AND SOLUTION STOICHIOMETRY A solution is a homogeneous mixture of two or more substances. A solution is made when one substance
More informationAccelerated Chemistry Semester 2 Review Sheet
Accelerated Chemistry Semester 2 Review Sheet The semester test will be given in two parts. The first part is a performance assessment and will be given the day before the semester test. This will include
More information3 Chemical Equilibrium
Aubrey High School AP Chemistry 3 Chemical Equilibrium Name Period Date / / 3.1 Problems Chemical Analysis 1. Write the equilibrium constant expressions for the following reactions. How are they related
More informationChapter 12 & 13 Test Review. Bond, Ionic Bond
Chapter 12 & 13 Test Review A solid solute dissolved in a solid solvent is an Alloy What is happening in a solution at equilibrium? The Ionic rate of Bond dissolving is equal to the rate of crystallization.
More informationUnit 6 Solids, Liquids and Solutions
Unit 6 Solids, Liquids and Solutions 12-1 Liquids I. Properties of Liquids and the Kinetic Molecular Theory A. Fluids 1. Substances that can flow and therefore take the shape of their container B. Relative
More informationACIDS, BASES & SALTS DR. RUCHIKA YADU
ACIDS, BASES & SALTS DR. RUCHIKA YADU Properties of Acids Acid is a compound which yields hydrogen ion (H+), when dissolved in water. Acid is sour to the taste and corrosive in nature. The ph value of
More informationChemistry Spring 2018 Final Exam Review
Name Date Period Chemistry Spring 2018 Final Exam Review TURN THIS COMPLETED REVIEW IN TO YOUR TEACHER BY DAY OF YOUR FINAL FOR A 5 point FINAL EXAM BONUS Unit #7 Moles 1. What is a mole? 2. What is molar
More informationUnit 4a Acids, Bases, and Salts Theory
Unit 4a Acids, Bases, and Salts Theory Chemistry 12 Arrhenius Theory of Acids and Bases The first theory that was proposed to explain the actions of acids and bases was by Svante Arrhenius. It is still
More informationCHEMICAL REACTIONS. There are three ways we write chemical equations. 1. Molecular Equations 2. Full Ionic Equations 3. Net Ionic Equations
CHEMICAL REACTIONS Reactants: Zn + I 2 Product: Zn I 2 Unit 2 Chemical Reactions The unit 2 exam will cover material from multiple chapters. You are responsible for the following from your text on exam
More informationPhysicochemical Processes
Lecture 3 Physicochemical Processes Physicochemical Processes Air stripping Carbon adsorption Steam stripping Chemical oxidation Supercritical fluids Membrane processes 1 1. Air Stripping A mass transfer
More informationLecture 4 :Aqueous Solutions
LOGO Lecture 4 :Aqueous Solutions International University of Sarajevo Chemistry - SPRING 2014 Course lecturer : Jasmin Šutković 11 th March 2014 Contents International University of Sarajevo 1. Aqueous
More informationUnit 12: Acids & Bases. Aim: What are the definitions and properties of an acid and a base? Properties of an Acid. Taste Sour.
Unit 12: Acids & Bases Aim: What are the definitions and properties of an acid and a base? Mar 23 12:08 PM Properties of an Acid 3. Are electrolytes. (Dissociate and conduct electricity when aq) 2. Turns
More informationNotes: Acids and Bases
Name Chemistry Pre-AP Notes: Acids and Bases Period I. Describing Acids and Bases A. Properties of Acids taste ph 7 Acids change color of an (e.g. blue litmus paper turns in the presence of an acid) React
More informationSolutions, Ions & Acids, Bases (Chapters 3-4) Example - Limiting Reagents. Percent Yield. Reaction Yields. Yield - example.
Solutions, Ions & Acids, Bases (Chapters 3-4) Chem 107 T. Hughbanks Example - Limiting Reagents SiCl 4 is used in making computer chips. It is produced by the reaction: SiO 2 + 2 C + 2 Cl 2 SiCl 4 + 2
More informationSolutions, Ions & Acids, Bases (Chapters 3-4)
Solutions, Ions & Acids, Bases (Chapters 3-4) Chem 107 T. Hughbanks Example - Limiting Reagents SiCl 4 is used in making computer chips. It is produced by the reaction: SiO 2 + 2 C + 2 Cl 2 SiCl 4 + 2
More informationCHAPTER 4 TYPES OF CHEMICAL EQUATIONS AND SOLUTION STOICHIOMETRY
CHAPTER 4 TYPES OF CHEMICAL EQUATIONS AND SOLUTION STOICHIOMETRY Water, the common solvent Solution is a homogeneous mixture Solvent is the substance that does the dissolving Solute is the substance that
More informationCHEM Exam 2 March 3, 2016
CHEM 123 - Exam 2 March 3, 2016 Constants and Conversion Factors R = 0.082 L-atm/mol-K R = 8.31 J/mol-K 1 atm. = 760 torr Molar Masses: C6H12O6-180. C12H22O11-32. C2H6O - 6. H2O - 18. Al(NO3)3-213. NaOH
More informationAREA 1: WATER. Chapter 6 ACIDS AND BASES. 6.1 Properties of acids and bases
AREA 1: WATER Chapter 6 ACIDS AND BASES 6.1 Properties of acids and bases Acids are: Sour May be corrosive Dissolve in water to produce an electrolyte, Turn blue litmus red Neutralised by bases. Bases
More informationDefinition of Acid. HCl + H 2 O H 3 O + + Cl
Acids Definition of Acid Acids are substances that contain H + ions that ionize when dissolved in water. Arrhenius acid: a compound that increases the concentration of H + ions that are present when added
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 informationMoorpark College Chemistry 11 Fall 2011 Instructor: Professor Gopal. Examination #2: Section Two October 17, Name: (print)
Moorpark College Chemistry 11 Fall 2011 Instructor: Professor Gopal Examination #2: Section Two October 17, 2011 Name: (print) Directions: Make sure your examination contains ELEVEN total pages (including
More informationAcid Base Equilibria
Acid Base Equilibria Acid Ionization, also known as acid dissociation, is the process in where an acid reacts with water to produce a hydrogen ion and the conjugate base ion. HC 2 H 3 O 2(aq) H + (aq)
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 informationChemistry 12 Unit 4 Topic A Hand-in Assignment
1 Chemistry 12 Unit 4 Topic A Handin Assignment Answer the following multiplechoice and written response problems on your own paper. Submit your answers for marking. You do not need to show your work for
More informationD O UBLE DISPL Ac EMENT REACTIONS
Experiment 8 Name: D O UBLE DISPL Ac EMENT REACTIONS In this experiment, you will observe double displacement reactions and write the corresponding balanced chemical equation and ionic equations. Double
More information11/14/10. Properties of Acids! CHAPTER 15 Acids and Bases. Table 18.1
11/14/10 CHAPTER 15 Acids and Bases 15-1 Properties of Acids! Sour taste React with active metals i.e., Al, Zn, Fe, but not Cu, Ag, or Au 2 Al + 6 HCl 2 AlCl3 + 3 H2 corrosive React with carbonates, producing
More informationAcids - Bases in Water
more equilibrium Dr. Fred Omega Garces Chemistry, Miramar College 1 Acids-Bases Characteristics Acids (Properties) Taste Sour Dehydrate Substances Neutralizes bases Dissolves metals Examples: Juices: TJ,
More informationph calculations MUDr. Jan Pláteník, PhD Brønsted-Lowry concept of acids and bases Acid is a proton donor Base is a proton acceptor
ph calculations MUDr. Jan Pláteník, PhD Brønsted-Lowry concept of acids and bases Acid is a proton donor Base is a proton acceptor HCl(aq) + H 2 O(l) H 3 O + (aq) + Cl - (aq) Acid Base Conjugate acid Conjugate
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 informationChapter 9 Acids & Bases
Chapter 9 Acids & Bases 9.1 Arrhenius Acids and Bases o Arrhenius Acid: substance that produces H + ions in aqueous solutions. HCl (aq) H + (aq) + Cl - (aq) o Arrhenius Base: substance that produces OH
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 information