Ch.16. REDOX TITRATIONS
|
|
- Shawn Hudson
- 6 years ago
- Views:
Transcription
1 Ch.16. REDX TITRATINS 16.1 redox titrations Chemistry useful in biology, environmental Science, material Sc 161. The Shape of a Redox Titration Curve Consider titration of Fe 2+ with std Ce 4+ : potentiometric detection of end point Ce 4+ + Fe 2+ Ce + Fe K ~ 10 1 in 1M HCl 4 At reference electrode : Calomel. 2Hg (l) + 2Cl Hg 2 Cl 2(s) + 2e At Pt indicator: two reactions Fe + e Fe 2+ E o = 0.6V Ce 4+ + e Ce E o = 1.0V which of the two is reduced? higher st. red. Potential Ce 4+ Ce
2 161. The Shape of a Redox Titration Curve combined possible cell reactions: 2Fe + 2Hg (l) + 2Cl 2Fe 2+ + Hg 2 Cl 2(s) or 2Ce Hg (l) + 2Cl 2Ce + Hg 2 Cl 2(s) How the cell voltage changes as Fe 2+ is titrated with Ce 4+? Reg1). Before the Equivalence point. Before eq. excess Fe 2+ exists Need to know [Fe 2+. [Fe E = E + E = = in case of the middle point of titration, [Fe 2+ = [Fe, E= Volt similar to ph = pk a at half 161. The Shape of a Redox Titration Curve Reg2). At the eq. point [Fe produced = [Ce produced very tiny amounts of [Ce 4+, [Fe 2+ present at equilibrium [Ce 4+ = [Fe 2+, [Ce = [Fe At eq. E + is the same for both half. [ Fe E + = log [ Fe 2+ [ Ce E + = log [ Ce 4+ 2E + = log [ Fe [ Fe 2+ [ Ce [ Ce E + = E + = 1.23V 2 E = E + E SCE = = 0.99V
3 161. The Shape of a Redox Titration Curve Req 3) After Eq. all [Fe 2+ [Fe = [Ce, extra [Ce 4+ remains as it is E = E + E SCE [ Ce = ( log ) [ Ce in case of V= 2V e (V e = volume at equil. point) [Ce = [Ce 4+ E + = 1.0 before after v = 2v e equili. point v The Shape of a Redox Titration Curve ex) Suppose that we titrate 100.0mL of M Fe 2+ with 0.100M Ce 4+ using the cell in Fig 161. The equivalence point occurs when V= 50.0mL, because the Ce 4+ is twice as concentrated as the Fe 2+. Calculate the cell voltage at 36.0, 50.0, and 63.0mL.
4 162. Finding the End Point 16. 1) Redox Indicators : color changes upon their oxidation and reduction state In (oxid) + ne In (red) [ In( red) E = E o log n [ In( oxid) reduced form of In. comes when vice versa o E = E ± n volts [ In( red) [ In( oxid) 10 1 for ferroin E o = 1.14 thus. Color change occur in < E < volt In case of SCE as reference, 0.84< E SCE < volt 162. Finding the End Point 16.8
5 162. Finding the End Point 16.9 Starch Iodine complex. (blue) titrations involving Indicator. Use starch as indicator Sugar amylose Starchiodine complex 164. xidation with Potassium permanganate (KMn 4 ) KMn 4 : oxidizing agent, violet color in ph < 1, self indicator, : Mn 4 + 8H + + 5e Mn H 2 E o =1.50V colorless in neutral or alkaline : Mn 4 + 4H + + 3e Mn 2(s) + 2H 2 E o = 1.692V brown solid in very strongly alkaline (2M NaH) : Mn 4 + e Mn 2 4 E o = 0.56V 1) Preparation and Standardization. KMn 4. Has trace amount of Mn 2 standardized by Na 2 C 2 4 (sodium oxalate) Mn 4 + 5H 2 C H + 2Mn C 2 + 8H 2 or by pure Fe wire put Fe in H 2 S 4 Fe 2+
6 1) pure distinctive rxn 165. xidation with Ce Ce 4+ + e Ce in acidic sol yellow colorless. Formal potential 1.0V 1F HCl V 1F HN 3 1.4V 1F HCl 1.44V 1F H 2 S 4` 166. xidation with K 2 Cr 2 (potassium dichromate) in acidic sol. Cr 2 : powerful oxidant red Cr : Cr 2 +14H + +6e 2Cr + H 2. E o =1.36V formal p. 1.00V in 1M HCl 1.11V in 2M H 2 S 4 less powerful oxidizing agent than Mn 4, Ce 4+ in basic. Cr 2 Cr 4 (yellow) converted. Cr H 2 + 3e Cr(H) 3(s) + 5H E o = 0.12V Advantages (primary std) color change self ind. can be monitored by Pt. and SCE
7 I) ii) I) (I 1. ii) 1. iii) 16. Methods involving Iodine i) Iodimetry : I 2 (titrant). actually I 3 reducing agent titrated with I 2 I Iodometry : oxidizing I to produce I 2 2 is titrated with NaS 2 3 ) thiosulfate I 2 : slightly soluble in water. to increase solubility, I 2(aq) + I I 2 3 K = 10 iodide triiodide (complex) iodine as a titrant means I Methods involving Iodine ) Use of starch indicator starch is used for iodine. Iodimetry : starch is added at just before equivalence. (titration turn dark blue. With I 3 ) since I 3 forms starch iodine complex (some iodine bounds to starch) In Iodimetry, Reasons for keeping the solution from strongly acidic i) starch hydrolyzes in strong acid. equilibrium is affected for several red. Agents H 3 As 3 + I 2 + H 2 H 3 As 4 + 2I + 2H + strong acid, reaction goes backward. produced I tends to oxidized. by 2. 4I H + 2I 2 + 2H 2
8 16. Methods involving Iodine ) Use of sodium thiosulfate In Iodometry Cr 2 + 6I + 14H + 2Cr + 3I 2 + H 2 universal titrant for I 3 in neutral or acidic. I 3 + 2S 2 3 3I + S 4 6 I 2 + 2S 2 3 2I + S 4 6. each Cr 2 reacts with 6S 2 3 Why not titratig oxidizing agent directly with thiosulfute? strong ox, agent (Mn 4, Cr 2, I 3 ) oxidize S 2 3 S Methods involving Iodine 16.16
Redox Titrations. -the oxidation/reduction reaction between analyte and titrant. -the equivalence point is based upon:
Redox Titrations -the oxidation/reduction reaction between analyte and titrant -titrants are commonly oxidizing agents, although reducing titrants can be used -the equivalence point is based upon: A ox
More informationPharmaceutical Analytical Chemistry PHCM223 Lecture 9 REDOX REACTIONS (I) Dr. Nesrine El Gohary 9 th lecture
Pharmaceutical Analytical Chemistry PHCM223 Lecture 9 REDOX REACTIONS (I) Dr. Nesrine El Gohary 9 th lecture Learning outcomes Define redox reactions. Apply redox titrations. Detect the end point of redox
More informationChapter 16 Redox Titrations. In general: Determining the amount of reductant in a sample through titration with a strong oxidant.
Chapter 16 Redox Titrations In general: Determining the amount of reductant in a sample through titration with a strong oxidant. Example: Analysis of Fe 2+, titration with Ce 4+. Ce 4+ + e Ce 3+ E = 1.70
More informationCHAPTER II. POTENTIOMETRY AND REDOX TITRATIONS
CHAPTER II. POTENTIOMETRY AND REDOX TITRATIONS I. Principles of Potentiometry Potentiometric methods of analysis are based upon measurements of the potential of electrochemical cells under conditions of
More informationRedox Titration. Properties of Umass Boston
Redox Titration Redox Titration Ce 4+ + Fe 2+ Ce 3+ + Fe 3+ Redox titration is based on the redox reaction (oxidation-reduction) between analyte and titrant. Position of the end point Determine the end
More informationChapter 19. Applications of Standard Electrode Potentials
Chapter 19 Applications of Standard lectrode Potentials 1 Calculating potentials of electrochemical cells The thermodynamic potential of an electrochemical cell is the difference between the electrode
More informationElectrochemistry. Redox reactions. Half Reactions. Nernst Equation Ion selective electrodes
Electrochemistry Nernst Equation Ion selective electrodes Redox reactions oxidation - loss of electrons M n+ M n+1 + e - M is oxidized - reducing agent reduction - gain of electrons N n+ + e - N n-1 N
More informationRedox titration. KMnO 4 H 2 SO 4
Redox titration KMnO 4 H SO 4 In acid-base titrations, the change in ph during titration may be calculated, and the titration curves thus obtained can be used to ascertain the most suitable indicator to
More informationEXPERIMENT NINE Part I - The Standardization of Thiosulfate Solutions
EXPERIMENT NINE Part I - The Standardization of Thiosulfate Solutions In general, thiosulfate solutions are standardized by indirect methods, Primary-standard oxidizing agents such as KIO 3, As 2 O 3,
More informationExercise 4 Oxidation-reduction (redox) reaction oxidimetry. Theoretical part
Exercise 4 Oxidation-reduction (redox) reaction oxidimetry. Theoretical part In oxidation-reduction (or redox) reactions, the key chemical event is the net movement of electrons from one reactant to the
More informationREDUCTION - OXIDATION TITRATION REDOX TITRATION
References REDUCTION OXIDATION TITRATION REDOX TITRATION 1 Fundamentals of analytical chemistry, Skoog. 2 Analytical chemistry, Gary D. Christian. الكيمياء التحليلية الجامعية تأليف د.هادي حسن جاسم 3 Oxidation
More informationOXIDATION/REDUCTION REACTIONS
OXIDATION/REDUCTION REACTIONS An oxidation/reduction reaction is one in which electrons are transferred from one reactant to another. An example is the oxidation of iron(ii) ions by cerium(iv) ions: Ce
More informationGeneral Information 1
General Information 1 1.1 CLEANING F VLUMETRIC GLASSWARE All the volumetric glassware (Burette, Pipette, Volumetric flasks etc) must be perfectly clean, free from dust and greasy impurities. Unreliable
More informationCHAPTER 10 Gravimetric Analysis and Precipitation Equilibria
1 CHAPTER 10 Gravimetric Analysis and Precipitation Equilibria Learning bjectives Steps of a gravimetric analysis Gravimetric calculations The solubility product, the common ion effect The diverse ion
More informationChapter 9: Polyprotic Acids and Bases
Amino acids Isoionic point Isoelectronic point 9-6 Isoelectric & Isoionic ph 9-1 Diprotic A&B Leucine: acidic & basic forms Leucine: intermediate form Monoprotic Polyprotic 9-5 Fractional compositions
More informationOxidation/reduction reaction and titration
Oxidation/reduction reaction and titration Dr. Mohammad Khanfar Oxidation/reduction reaction In an oxidation/reduction reaction, electrons are transferred from one reactant to another. An example is the
More information2] What is the difference between the end point and equivalence point for a monobasicmonoacid
4 Titrations modified October 9, 2013 1] A solution of 0.100 M AgNO 3 is used to titrate a 100.00 ml solution of 0.100 M KCl. The K sp of AgCl is 1.8e-11 a) What is pag if 50.00 ml of the titrant is added
More information[Ca 2+ ] = s (3) [IO - 3 ] = 2s (4)
E10 Chemical Equilibria: K sp of Calcium Iodate Objective! Understand the relation between the molar solubility and the solubility product constant of a sparingly soluble salt.! Measure the molar solubility
More information$ % K st. K D [ I 2 ] Aqueous. [ I 2 ] Hexane. % Aqueous
Determination of the Stability Constant of the Tri- Iodide Ion by Solvent Extraction Introduction Molecular iodine reacts with iodide to form a complex, called the tri- iodide ion, according to the reaction:
More information2. Which of the following statements best describes the movement of electrons in an electrochemical cell?
Exam 2 Chem 311 Evans Fall 2009 112: 2 pts each 1. Consider the following unbalanced redox equation: Pb (s) + PbO 2 (s) + 2 HSO 4 (aq) 2 PbSO 4 (s) Which species is being oxidized? A. HSO 4 B. Pb(s) C.
More informationElectrolysis (Determination of the Faraday constant and atomic weight of Cu)
Labs taught in Introductory University Chemistry (Chem 200). Expt # Title of Experiment (brief details of experiment) 1 Buret and Scale Operation 2 3 Hydrates (Determination of the number of waters of
More informationChapter 4 Notes Types of Chemical Reactions and Solutions Stoichiometry A Summary
Chapter 4 Notes Types of Chemical Reactions and Solutions Stoichiometry A Summary 4.1 Water, the Common Solvent A. Structure of water 1. Oxygen s electronegativity is high (3.5) and hydrogen s is low (2.1)
More informationPartner: Judy 29 March Analysis of a Commercial Bleach
Partner: Judy 29 March 2012 Analysis of a Commercial Bleach Purpose: The purpose of this lab is to determine the amount of sodium hypochlorite (NaClO) in commercial bleach. This can be done by forming
More informationAP Chemistry: Electrochemistry Multiple Choice Answers
AP Chemistry: Electrochemistry Multiple Choice Answers 14. Questions 14-17 The spontaneous reaction that occurs when the cell in the picture operates is as follows: 2Ag + + Cd (s) à 2 Ag (s) + Cd 2+ (A)
More informationDanyal Education (Contact: ) A commitment to teach and nurture
Chemistry of Reactions: Redox (#) Candidates should be able to: a) define oxidation and reduction (redox) in terms of oxygen/hydrogen gain/loss b) define redox in terms of electron transfer and changes
More informationElectrochemical Cells
Electrochemical Cells There are two types: Galvanic and Electrolytic Galvanic Cell: a cell in which a is used to produce electrical energy, i.e., Chemical energy is transformed into Electrical energy.
More informationAll Questions are to be attempted 1- Redox Titration (35 Marks)
SOHAG UNIVERSITY FACULTY OF PHARMACY PHARM. ANAL. CHEM. DEPT. Pharm. Anal. Chem-2 Second Year Students May, 31, 2016 TIME ALLOWED: TWO HOURS Total marks: 90 All Questions are to be attempted 1- Redox Titration
More informationINORGANIC CHEMISTRY (LAB MANUAL)
REDOX TITRATIONS Titrations involving oxidizing and reducing agents are termed as oxidationreduction or redox titrations. The phenomenon of oxidation and reduction plays an important role in our day-to-day
More informationAP Chemistry Unit #4. Types of Chemical Reactions & Solution Stoichiometry
AP Chemistry Unit #4 Chapter 4 Zumdahl & Zumdahl Types of Chemical Reactions & Solution Stoichiometry Students should be able to: Predict to some extent whether a substance will be a strong electrolyte,
More informationSolubility Product Constant (K sp ) and the Common-Ion Effect for Calcium Iodate, a Salt of Limited Solubility
Solubility Product Constant (K sp ) and the Common-Ion Effect for Calcium Iodate, a Salt of Limited Solubility Purpose Determine the solubility product constant (K sp ) for a sparingly soluble salt. Study
More informationName Period Date. Lab 9: Analysis of Commercial Bleach
Name Period Date Lab 9: Analysis of Commercial Bleach Introduction Many common products are effective because they contain oxidizing agents. Some products, which contain oxidizing agents, are bleaches,
More informationSafety Note: Safety glasses and laboratory coats are required when performing this experiment
The Determination of Hypochlorite in Bleach Reading assignment: Burdge, Chemistry 4 th edition, section 4.6. We will study an example of a redox titration in order to determine the concentration of sodium
More informationTYPES OF CHEMICAL REACTIONS
TYPES OF CHEMICAL REACTIONS Precipitation Reactions Compounds Soluble Ionic Compounds 1. Group 1A cations and NH 4 + 2. Nitrates (NO 3 ) Acetates (CH 3 COO ) Chlorates (ClO 3 ) Perchlorates (ClO 4 ) Solubility
More informationAP Chemistry Review Packet # form B. How many grams of water are present in 1.00 mol of copper(ii) sulfate pentahydrate?
AP Chemistry Review Packet #4 Warmup: Reaction Prediction 2010 form B (a) Solid copper(ii) sulfate pentahydrate is gently heated. How many grams of water are present in 1.00 mol of copper(ii) sulfate pentahydrate?
More informationUnit 8 REDX REACTINS I. Multiple Choice Questions (Type-I) 1. Which of the following is not an example of redox reaction? Cu Cu Fe 3 + 3C Fe + 3C K + F KF BaCl S 4 BaS 4 + HCl. The more positive the value
More informationChapter 4 Reactions in Aqueous Solution
Chapter 4 Reactions in Aqueous Solution Homework Chapter 4 11, 15, 21, 23, 27, 29, 35, 41, 45, 47, 51, 55, 57, 61, 63, 73, 75, 81, 85 1 2 Chapter Objectives Solution To understand the nature of ionic substances
More informationI. Multiple Choice Questions (Type-I) 1. Which of the following is not an example of redox reaction? Cu + H HCl. BaSO 4
Unit 8 REDX REACTINS REAC I. Multiple Choice Questions (Type-I) 1. Which of the following is not an example of redox reaction? Cu Cu Fe 2 3 + 3C 2Fe + 3C 2 2K + F 2 2KF BaCl 2 S 4 BaS 4 + 2HCl 2. The more
More informationExp. 2: The Superconductor YBa 2 Cu 3 O 7 (Text #1)
Exp. 2: The 1-2-3 Superconductor YBa 2 Cu 3 O 7 (Text #1) Last week: Performed high-temperature, solid-state reaction to prepare YBa 2 Cu 3 O x Thursday: Determine product stoichiometry ( x ) based on
More informationZinc electrode. 1M zinc sulphate solution
16. Redox Equilibria Electrochemical cells Electron flow A cell has two half cells. The two half cells have to be connected with a salt bridge. Simple half cells will consist of a metal (acts an electrode)
More informationChem 321 Lecture 16 - Potentiometry 10/22/13
Student Learning Objectives Chem 321 Lecture 16 - Potentiometry 10/22/13 In lab you will use an ion-selective electrode to determine the amount of fluoride in an unknown solution. In this approach, as
More informationChapter Four. Chapter Four. Chemical Reactions in Aqueous Solutions. Electrostatic Forces. Conduction Illustrated
1 Electrostatic Forces 2 Chemical Reactions in Aqueous Solutions Unlike charges (+ and ) attract one another. Like charges (+ and +, or and ) repel one another. Conduction Illustrated 3 Arrhenius s Theory
More informationINORGANIC CHEMISTRY (LAB MANUAL)
REDOX TITRATIONS Titrations involving oxidizing and reducing agents are termed as oxidationreduction or redox titrations. The phenomenon of oxidation and reduction plays an important role in our day-to-day
More informationScholarship 2006 Chemistry
For Supervisor s S 9 3 1 0 2 Scholarship 2006 Chemistry 2.00 pm Saturday 25 November 2006 Time allowed: Three hours Total Marks: 48 Check that the National Student Number (NSN) on your admission slip is
More information3.2.5 Group VII. Trends in oxidising abilities. 167 minutes. 167 marks. Page 1 of 19
3..5 Group VII Trends in oxidising abilities 167 minutes 167 marks Page 1 of 19 Q1. (a) Samples of solid sodium fluoride, sodium chloride, sodium bromide and sodium iodide are each warmed separately with
More informationCh 20 Electrochemistry: the study of the relationships between electricity and chemical reactions.
Ch 20 Electrochemistry: the study of the relationships between electricity and chemical reactions. In electrochemical reactions, electrons are transferred from one species to another. Learning goals and
More information1 Three redox systems, C, D and E are shown in Table 6.1. C Ag(NH 3. ) 2 + (aq) + e Ag(s) + 2NH 3. (aq) D Ag + (aq) + e Ag(s)
1 Three redox systems, C, D and E are shown in Table 6.1. C Ag(NH 3 ) 2 + (aq) + e Ag(s) + 2NH 3 (aq) D Ag + (aq) + e Ag(s) E Ag(CN) 2 (aq) + e Ag(s) + 2CN (aq) Table 6.1 The two cells below were set up
More informationFind this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site.
Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site. Still having trouble understanding the material? Check
More informationOxidation, Reduction, Red-ox reactions, Types
Oxidation, Reduction, Red-ox reactions, Types 1) Oxidation number is the charge which an atom appears to acquire in a molecule, when all the bonding electrons are counted to more electro negative element.
More information7.00 Let the Titrations Begin
7.00 Let the Titrations Begin Dr. Fred Omega Garces Analytical Chemistry 251 Miramar College, SDCCD 1 Let the Titration Technique Titration A technique of chemical analysis to determine the amount of a
More informationCHEM 101 LECTURE NOTES Fall 2003 Dr. Joy Heising S Chapter 11 lecture notes Ch. 11 Aqueous solution reactions
Ch. 11 Aqueous solution reactions Ch. 3 review: Molarity = moles solute Liters solution If 500. ml of a 2.80 M solution of NaOH is added to 75.0 ml of a 3.68 M solution of H 3 PO 4, the resulting solution
More informationChapter 20 Electrochemistry
Chapter 20 Electrochemistry Learning goals and key skills: Identify oxidation, reduction, oxidizing agent, and reducing agent in a chemical equation Complete and balance redox equations using the method
More informationOxidation/reduction reaction and titration
Oxidation/reduction reaction and titration Dr. Mohammad Khanfar Oxidation/reduction reaction In an oxidation/reduction reaction, electrons are transferred from one reactant to another. An example is the
More informationChapter 18 Electrochemistry. Electrochemical Cells
Chapter 18 Electrochemistry Chapter 18 1 Electrochemical Cells Electrochemical Cells are of two basic types: Galvanic Cells a spontaneous chemical reaction generates an electric current Electrolytic Cells
More informationChem II - Wed, 9/14/16
Chem II - Wed, 9/14/16 Do Now Drop off any study guides you want color coded Pull out stoich HW Homework See board Agenda Stoich Ch 4 Labish thing Chapter 4 Chemical Reactions & Solution Stoich Water Possesses
More informationTitration Curves. What is in the beaker at each stage of a titration? Beaker A Beaker B Beaker C Beaker D. 20 ml NaOH Added
Why? Titration Curves What is in the beaker at each stage of a titration? Titration is a very useful technique for determining the properties of an unknown solution. The unknown is reacted with a known
More informationExperiment Three. Lab two: Parts 2B and 3. Halogens used in Parts 2 and 3. Lab one: Parts 1 and 2A. Halogens (Family VIIA) used in Parts 2 and 3
Experiment Three Lab one: Parts 1 and 2A Lab two: Parts 2B and 3 1 1A 1 H 1s 1 2 IIA 3 Li 2s 1 1 1 Na 3s 1 1 9 K 4s 1 3 7 Rb 5s 1 5 5 Cs 6s 1 8 7 Fr 7s 1 4 Be 2s 2 1 2 Mg 3s 2 3 IIIB 4 IVB 5 VB 6 VIB 7
More informationEXPERIMENT #9 PRELAB EXERCISES. Redox Titration (Molarity Version) Name Section. 1. Balance the following redox reaction under acidic conditions.
EXPERIMENT #9 PRELAB EXERCISES Redox Titration (Molarity Version) Name Section 1. Balance the following redox reaction under acidic conditions. C 2 O 2-4 (aq) + MnO - 4 (aq) CO 2 (g) + Mn 2+ (aq) 2. A
More information5) do sample calculations 1) In electrogravimetry, analyte deposited as a solid ("plated") onto one of the electrodes.
Page 1 of 1 Chem 201 Lecture 8b Summer 09 Return tests Last time: 0) Intro to Electrochemistry 1) E, Galvanic cells Today: Potentiometry Lecture: GALVANIC CELLS: -spontaneous reaction is utilized. ; voltaic
More information5.2.3 Electrode Potentials and Fuel Cells Redox
5.2.3 Electrode Potentials and Fuel Cells Redox oxidation is the process of electron loss: Zn Zn 2+ + 2e It involves an increase in oxidation number reduction is the process of electron gain: Cl 2 + 2e
More informationName Period Date. Ch. 19: Oxidation-Reduction Reactions Homework
Name Period Date Ch. 19: OxidationReduction Reactions Homework Answer each of the following questions in as much detail as you can. Be sure to show all your work for any calculations and follow all rules
More informationPotentiometry fixes one of the half cells as a reference.
Page 1 of 1 Chem 201 Lecture 9a Summer 09 Return tests Last time: Potentiometry Today: 1. finish Potentiometry 2. Start analytical separations Potentiometry: cell potential represented by Nernst equation
More informationQuiz 1 Scores. Chapter 4: Chemical Reactions F D C- C C+ B- B B+ A- A A+ Chem 6A Michael J. Sailor, UC San Diego
Chapter 4: Chemical Reactions 1 1 80 Quiz 1 Scores 70 60 50 40 30 20 10 0 F D C- C C+ B- B B+ A- A A+ 2 Grade Projection Quiz 1 (data from 2010) score on quiz #1 F D C- C C+ B- B B+ A- A + final grade
More informationAcid-Base Equilibria. And the beat goes on Buffer solutions Titrations
Acid-Base Equilibria And the beat goes on Buffer solutions Titrations 1 Common Ion Effect The shift in equilibrium due to addition of a compound having an ion in common with the dissolved substance. 2
More informationOxidation Numbers, ox #
Oxidation Numbers, ox # are or numbers assigned to each or assuming that the are transferred from the electronegative element to the electronegative element. now mimic systems. ox # are written followed
More informationTitration of a Weak Acid with a Strong Base
Titration of a Weak Acid with a Strong Base Weak Acid w/ Strong Base Overall: INITIAL ph: Weak acids do not fully dissociate we need to do an ICE table to determine initial ph. We expect it to be weakly
More informationSCH4U: EXAM REVIEW. 2. Which of the following has a standard enthalpy of formation of 0 kj mol -1 at 25ºC and 1.00 atm?
SCH4U_08-09 SCH4U: EXAM REVIEW 1. The heat of a reaction is equal to: a. enthalpy (products) + enthalpy (reactants) b. enthalpy (reactants) enthalpy (products) c. enthalpy (products) enthalpy (reactants)
More informationChemistry 12. Resource Exam B. Exam Booklet
Chemistry 12 Resource Exam B Exam Booklet Contents: 21 pages Examination: 2 hours 50 multiple-choice questions in the Exam Booklet Additional Time Permitted: 60 minutes Province of British Columbia PART
More informationREVIEW QUESTIONS Chapter 19
Chemistry 10 ANSWER KEY REVIEW QUESTIONS Chapter 19 1. For each of the following unbalanced equations, (i) write the half-reactions for oxidation and reduction, and (ii) balance the overall equation in
More informationChem Practice Exam Two (Chapters 19, 20 and 21)
Chem 203 - Practice Exam Two (Chapters 19, 20 and 21) 1. Consider the dissolution of MnS in water (K sp = 3.0 10 14 ). MnS(s) + H 2O(l) Mn 2+ (aq) + HS (aq) + OH (aq) How is the solubility of manganese(ii)
More informationELECTROCHEMISTRY. Electrons are transferred from Al to Cu 2+. We can re write this equation as two separate half reactions:
ELECTROCHEMISTRY A. INTRODUCTION 1. Electrochemistry is the branch of chemistry which is concerned with the conversion of chemical energy to electrical energy, and vice versa. Electrochemical reactions
More informationScholarship 2015 Chemistry
93102 931020 S SUPERVISOR S Scholarship 2015 Chemistry 9.30 a.m. Friday 27 November 2015 Time allowed: Three hours Total marks: 32 Check that the National Student Number (NSN) on your admission slip is
More informationExperiment 2: Analysis of Commercial Bleach Solutions
Experiment 2: Analysis of Commercial Bleach Solutions I. Introduction The ability of household bleach to remove stains is related to the amount of oxidizing agent in it. The oxidizing agent in bleach is
More information11/3/09. Aqueous Solubility of Compounds. Aqueous Solubility of Ionic Compounds. Aqueous Solubility of Ionic Compounds
Aqueous Solubility of Compounds Not all compounds dissolve in water. Solubility varies from compound to compound. Chapter 5: Chemical Reactions Soluble ionic compounds dissociate. Ions are solvated Most
More informationCh 4-5 Practice Problems - KEY
Ch 4-5 Practice Problems - KEY The following problems are intended to provide you with additional practice in preparing for the exam. Questions come from the textbook, previous quizzes, previous exams,
More information5 ELECTRON TRANSFER REACTIONS
5 ELECTRON TRANSFER REACTIONS 5.1 TERMINOLOGY In a reaction between an acid and a base, a proton is transferred from acid to base. When an electron (or a number of electrons) is transferred from one species
More information2. Using Half Cell Potentials and Latimer Diagrams. 100 measured half cell potentials generate 10,000 full reactions
Electrochemistry 1. Balancing Redox Reactions 2. Using Half Cell Potentials and Latimer Diagrams 100 measured half cell potentials generate 10,000 full reactions 3. E as a Thermodynamic state function
More informationChapter 20 Electrochemistry
Chapter 20 Electrochemistry Electrochemical Cell Consists of electrodes which dip into an electrolyte & in which a chem. rxn. uses or generates an electric current Voltaic (Galvanic) Cell Spont. rxn. -
More informationE o cell = E o red - E o ox. **Oxidizing agent must be higher on the table than the reducing agent in order for the reaction to be spontaneous**
Chemistry 12 Electrochemistry III Name: Date: Block: 1. SRP Table Standard Reduction Potential (SRP) Table This table is used to predict whether a chemical species will spontaneously give electrons to
More informationANALYTICAL CHEMISTRY LABORATORY MANUAL 2
ANALYTICAL CHEMISTRY LABORATORY MANUAL 2 Ankara University Faculty of Pharmacy Department of Analytical Chemistry Analytical Chemistry Practices Contents INTRODUCTION TO QUANTITATIVE ANALYSIS... 2 VOLUMETRIC
More informationANSWER KEY CHEMISTRY F14O4 FIRST EXAM 2/16/00 PROFESSOR J. MORROW EACH QUESTION IS WORTH 1O POINTS O. 16.
discard 1 2 ANSWER KEY CHEMISTRY F14O4 FIRST EXAM 2/16/00 PROFESSOR J. MORROW PRINT NAME, LAST: FIRST: I.D.# : EACH QUESTION IS WORTH 1O POINTS 1. 7. 13. 2. 8. 14. 3. 9. 15. 4. 1O. 16. 5. 11. 17. 6. 12.
More informationBasic Concepts of Chemistry and Chemical Calculations. The ratio of the average mass factor to one twelfth of the mass of an atom of carbon-12
Basic Concepts of Chemistry and Chemical Calculations Relative Atomic mass: The relative atomic mass is defined as the ratio of the average atomic mass factor to the unified atomic mass unit. (Or) The
More informationPrecipitation Titrations;
Precipitation Titrations; ANALYTICAL CHEMISTRY Precipitation Titrations; Precipitation Titrations are generally famous due to their unique ability to form an insoluble precipitate during the reaction.
More informationHigher Chemistry. Chemistry In Society
Higher Chemistry Chemistry In Society Homework Oxidising and Reducing Agents, Ion-Electron and Redox Equations and Chemical Analysis 1 1. Potassium permanganate solution, acidified with dilute sulphuric
More informationCHEM N-12 November In the electrolytic production of Al, what mass of Al can be deposited in 2.00 hours by a current of 1.8 A?
CHEM161 014-N-1 November 014 In the electrolytic production of Al, what mass of Al can be deposited in.00 hours by a current of 1.8 A? What products would you expect at the anode and the cathode on electrolysis
More informationChem 115 POGIL Worksheet - Week #6 Oxidation Numbers, Redox Reactions, Solution Concentration, and Titrations
Chem 115 POGIL Worksheet - Week #6 Oxidation Numbers, Redox Reactions, Solution Concentration, and Titrations Why? In addition to metathetical reactions, electron transfer reactions often occur in solutions.
More informationנושא 5. 1 Prof. Zvi C. Koren
נושא 5 סטויכיאומטריה: כימות כימי 1 Prof. Zvi C. Koren Stoichiometry Stoicheion + (element) metron (measure) Weight relations in chemical rxns. based on conservation of matter For any rxn., The absolute
More informationReactions (Chapter 4) Notes 2016.notebook. October 14, Chemical Reactions. Chapter 4 Notes. Oct 21 8:44 AM. Oct 22 10:14 AM
Chemical Reactions Chapter 4 Notes Oct 21 8:44 AM Oct 22 10:14 AM 1 There are several things to keep in mind writing reactions and predicting products: 1. States of matter of elements/compounds 2. Diatomics
More informationDirected by Ph. Sadeel Shanshal
University of Mosul College of Pharmacy Practical Laboratory Dept. of Pharmaceutical Chemistry Head of dept. Dr. ؤىوىست Nohad Al.Omari Directed by Ph. Sadeel Shanshal 0 Syllabus : No. Lab. Title Hours
More informationAP Chapter 4: Reactions in Aqueous Solution Name
AP Chapter 4: Reactions in Aqueous Solution Name WarmUps (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. AP Chapter 4: Reactions in Aqueous Solution 2 WarmUps
More informationChemistry 222 Exam 4: Chapters 11, 13, 14 Spring Points
Chemistry 222 Name Exam 4: Chapters 11, 13, 14 Spring 2014 80 Points Complete five (5) of the following problems. Each problem is worth 16 points. CLEARLY mark the problems you do not want graded. You
More informationEXPERIMENT C3: SOLUBILITY PRODUCT & COMMON ION EFFECT. Learning Outcomes. Introduction. Upon completion of this lab, the student will be able to:
1 EXPERIMENT C3: SOLUBILITY PRODUCT & COMMON ION EFFECT Learning Outcomes Upon completion of this lab, the student will be able to: 1) Measure the solubility product constant for a sparingly soluble salt.
More information(aq) 5VO2 + (aq) + Mn 2+ (aq) + 10H + + 4H 2 O. (aq) 5VO2 + (aq) + Mn 2+ (aq) + 2H + (aq) basic solution. MnO2 + 2H 2 O) 3H 2 O + I IO 3
Chem 1515 Section 2 Problem Set #15 Spring 1998 Name ALL work must be shown to receive full credit. Due Due in lecture at 1:30 p.m. Friday, May 1st. PS15.1. Balance the following oxidation-reduction reactions
More informationEXPERIMENT 23 Lab Report Guidelines
EXPERIMENT 23 Listed below are some guidelines for completing the lab report for Experiment 23: For each part, follow the procedure outlined in the lab manual. Observe all safety rules, including wearing
More informationExam 2 Chem 311 Fall 2002 You must do (1 or 2), (3 or 4), (5 or 6), (7 or 8), and one other problem!!! All problems are worth 20 points
Exam 2 Chem 311 Fall 2002 You must do (1 or 2), (3 or 4), (5 or 6), (7 or 8), and one other problem!!! All problems are worth 20 points 1) A 100.0 ml solution containing 0.0100 M (NH 4 ) 2 Ce(NO 3 ) 6,
More informationName AP CHEM / / Collected Essays Chapter 17
Name AP CHEM / / Collected Essays Chapter 17 1980 - #2 M(s) + Cu 2+ (aq) M 2+ (aq) + Cu(s) For the reaction above, E = 0.740 volt at 25 C. (a) Determine the standard electrode potential for the reaction
More informationМЕТОДИЧЕСКИЕ УКАЗАНИЯ СТУДЕНТАМ
МЕТОДИЧЕСКИЕ УКАЗАНИЯ СТУДЕНТАМ CLASS 1. TPIC: Introduction in a subject. Safety regularions in a chemical laboratory. 1. Introduction in a subject. (0 min.). 1.1. Control of a student s initial level
More informationChapter 19: Oxidation - Reduction Reactions
Chapter 19: Oxidation - Reduction Reactions 19-1 Oxidation and Reduction I. Oxidation States A. The oxidation rules (as summarized by Mr. Allan) 1. In compounds, hydrogen has an oxidation # of +1. In compounds,
More informationUnit The mw of Na 2 CO 3 is : Na=23, O=16, C=12 A) 140 B) 106 C) 96 D) 100 E) 60
Unit 2 1- The mw of Na 2 CO 3 is : Na=23, O=16, C=12 A) 140 B) 106 C) 96 D) 100 E) 60 2- How many grams of Na 2 CO 3 (mw = 106 ) A) 318 B) 0.028 C) 134 D) 201 E) 67 in 3 moles, 3- Calculate the normal
More informationOxidation-Reduction Reactions. (Redox) Redox Reactions. Types of Redox Rxn s. Not Redox Reactions. Combustion of methane
Oxidation-Reduction Reactions Redox Reactions Reactions in which one or more electrons are transferred 2Na (s) + Cl 2(g) 2NaCl (s) (Redox) Species loosing electrons is said to be oxidized and the species
More informationChemistry 12 APRIL Course Code = CH. Student Instructions
MINISTRY USE ONLY MINISTRY USE ONLY Place Personal Education Number (PEN) here. Place Personal Education Number (PEN) here. MINISTRY USE ONLY Chemistry 12 2002 Ministry of Education APRIL 2002 Course Code
More information