14. INORGANICS IN AQUEOUS SOLUTION
|
|
|
- Merry Warner
- 7 years ago
- Views:
Transcription
1 14. INRGANICS IN AQUEUS SLUTIN Acid-base chemistry 14.. Brønsted-Lowry or Lewis base? Ligand substitution reactions Inference from aqueous tests Inorganics aqueous solution answers Inorganics aqueous solution 14.
2 14.1. Acid-base chemistry For each of the test tube reactions described below; (a) Write a balanced symbol equation (cludg state symbols) for the reactions occurrg, (b) Describe what you would expect to observe. 1. Sodium hydroxide solution is added dropwise to an aqueous solution of copper(ii) sulfate until present. Equation... (1 mark) bservations.... Sodium hydroxide solution is added dropwise to an aqueous solution of iron(ii) sulfate until present. Equation... (1 mark) bservations Sodium carbonate solution is added dropwise to an aqueous solution of manganese(ii) sulfate until present. Equation... (1 mark) bservations Sodium carbonate solution is added dropwise to an aqueous solution of iron(iil) chloride until present. Equation... (1 mark) bservations Sodium hydroxide solution is added dropwise to an aqueous solution of chromium(iii) sulfate until present. Equation(s)... bservations... Inorganics aqueous solution 14.1.
3 14.. Brønsted-Lowry or Lewis base? A Brønsted-Lowry base is a proton acceptor. A Lewis base donates a pair of electrons. In each of the test tube reactions described below, ammonia acts either as a Brønsted-Lowry base or a Lewis base. Complete the descriptions by fillg the blanks labelled (10 marks) Aqueous alumium ions When an aqueous solution of ammonia is added dropwise to an aqueous solution of alumium sulfate, a is does not dissolve on addition of ammonia. Equation: [Al(H ) 6 ] 3+ (aq) + 3 NH 3 (aq) [Al(H ) 3 (H) 3 ](s) + 3 NHŸ(aq) In this reaction, ammonia is actg as a Aqueous cobalt ions When an aqueous solution of ammonia is added dropwise to a pk solution of aqueous cobalt(ii) chloride, a blue precipitate is formed itially. Equation: [Co(H ) 6 ] + (aq) + NH 3 (aq) In this reaction, ammonia is actg as a Brønsted-Lowry base. n addg ammonia solution, the blue precipitate re-dissolves to form a (which is oxidised by air to a dark brown mixture contag Co(III) compounds.) Equation: [Co(H ) 4 (H) ](s) + 6 NH 3 (aq) [Co(NH 3 ) 6 ] + (aq) + 4 H (l) + H (aq) In this second reaction, ammonia is actg as a Aqueous copper ions When an aqueous solution of ammonia is added dropwise to a blue solution of aqueous copper(ii) sulfate, a is itially Equation: [Cu(H ) 6 ] + (aq) + NH 3 (aq) [Cu(H ) 4 (H) ](s) + NHŸ(aq) In this reaction, ammonia is actg as a Brønsted-Lowry base. n the addition of ammonia solution, the re-dissolves to form Equation: [Cu(H ) 4 (H) ](s) + 4 NH 3 (aq) H (l) + H (aq) In this second reaction, ammonia is actg as a Inorganics aqueous solution 14..
4 14.3. Ligand substitution reactions For each of the criteria 1-5 below, identify a ligand substitution reaction startg from [Cu(H ) 6 ] + and selectg ligands from NH 3,, en (H NCH CH NH ), C Øʇ and EDTA 4 which meet the criteria required. Choose a different reaction for each set of criteria, and each case, draw a 3-dimensional representation of the fal product. 1. No either the coordation number or the overall charge on the complex....( marks). No the coordation number of the complex but a the overall charge on the complex....( marks) 3. A both the coordation number and overall charge on the complex....( marks) 4. The largest positive entropy....( marks) 5. Produces a chiral product....( marks) Inorganics aqueous solution 14.3.
5 14.4. Inference from aqueous tests Use the results of the simple test tube reactions shown below to identify the anion and the cation each of the unknown salts A-E. Each of the tests were carried out on a small sample of the salt dissolved water. Salt A Salt B Salt C Salt D Salt E Test 1 Add NaH(aq) dropwise until present re-dissolved to form a green solution A pale blue ppt A blue ppt A brown ppt Test Add NH 3 (aq) dropwise until present re-dissolved to form a purple solution A pale blue ppt re-dissolved to form a deep blue solution A pale blue ppt re-dissolved to form a pale yellow / brown solution slowed turned orange / brown on standg. No visible with A brown ppt Test 3 Add CÕʇ(aq) dropwise until present Effervescence. with A blue green ppt with A pk ppt with with A brown ppt Effervescence. with Test 4 Add HN 3 followed by AgN 3 (aq) was observed to dissolve dil. NH 3 (aq) A cream ppt was observed to dissolve conc. NH 3 (aq) was observed to dissolve dil. NH 3 (aq) Test 5 Add H followed by Ba (aq) formed formed Salt A is... Salt B is... Salt C is... Salt D is... Salt E is......( marks)...( marks)...( marks)...( marks)...( marks) Inorganics aqueous solution 14.4.
6 14. Inorganics aqueous solution answers Acid-base chemistry (1 mark for each correct equation with state symbols; 1 mark for each correct full observation) 1. Equation: [Cu(H ) 6 ] + (aq) + H (aq) [Cu(H ) 4 (H) ](s) + H (l) bservations: Blue solution to a blue precipitate which doesn t re-dissolve NaH.. Equation: [Fe(H ) 6 ] + (aq) + H (aq) [Fe(H ) 4 (H) ](s) + H (l) bservations: Pale green solution to a murky green precipitate which is oxidised the air to orange/brown [Fe(H ) 3 (H) 3 ](s). 3. Equation: [Mn(H ) 6 ] + (aq) + CÕʇ(aq) MnC 3 (s) + 6 H (l) bservations: Very pale pk solution to a very pale pk precipitate. 4. Equation: [Fe(H ) 6 ] 3+ (aq) + 3 CÕʇ(aq) [Fe(H ) 3 (H) 3 ](s) + 3 H (l) + 3 C (g) bservations: Yellow/brown solution to a orange/brown precipitate and effervescence. 5. Equations: [Cr(H ) 6 ] 3+ (aq) + 3 H (aq) [Cr(H ) 3 (H) 3 ](s) + 3 H (l) [Cr(H ) 3 (H) 3 ](s) + 3 H (aq) [Cr(H) 6 ] 3 (aq) + 3 H (l) bservations: Ruby or green solution to a green precipitate which dissolves NaH to form a green solution Brønsted-Lowry or Lewis base? 1. white precipitate. Brønsted-Lowry base 3. [Co(H ) 4 (H) ](s) 4. NHŸ(aq) 5. pale yellow/brown solution 6. Lewis base 7. blue precipitate 8. deep blue solution 9. [Cu(NH 3 ) 4 (H ) ] Lewis base Ligand substitution reactions 1. [Cu(H ) 6 ] + (aq) + 4 NH 3 (aq) [Cu(H ) (NH 3 ) 4 ] + (aq) + 4 H (l) H H N NH 3 A 3 Cu H N NH 3 H (10 marks) + 3 Inorganics aqueous solution answers
7 14. Inorganics aqueous solution answers 4. [Cu(H ) 6 ] + (aq) + 3 C Øʇ(aq) [Cu(C 4 ) 3 ] 4 (aq) + 6 H (l) Cu A 3. [Cu(H ) 6 ] + (aq) + 4 (aq) [Cu 4 ] (aq) + 6 H (l) Cu 4. [Cu(H ) 6 ] + (aq) + EDTA 4 (aq) [CuEDTA] (aq) + 6 H (l) N + N + Cu A 5. [Cu(H ) 6 ] + (aq) + 3 en (aq) [Cu en 3 ] + (aq) + 6 H (l) H N N H HN Cu A HN NH NH + (1 mark for each correct equation, 1 mark for each correct drawg) 14.4 Inference from aqueous tests Salt A is chromium(iii) sulfate Salt B is copper(ii) chloride Salt C is cobalt(ii) bromide Salt D is iron(ii) chloride Salt E is iron(iii) sulfate ( marks) ( marks) ( marks) ( marks) ( marks) Inorganics aqueous solution answers
REACTIONS OF SOME TRANSITION METAL IONS
Transition Metals 2815 1 REACTIONS OF SOME TRANSITION METAL IONS COBALT Cobalt(II) aqueous solutions contain the pink, octahedral hexaaquacobalt(ii) ion. hexaaqua ions can also be present in solid samples
REACTIONS OF SOME TRANSITION METAL IONS COBALT
Transition Metals 1 REACTIONS OF SOME TRANSITION METAL IONS COBALT Cobalt(II) aqueous solutions contain the pink, octahedral hexaaquacobalt(ii) ion hexaaqua ions can also be present in solid samples of
This experiment involves the separation and identification of ions using
Chemistry 112: Reactions Involving Complex Ions Page 27 COMPLEX IONS AND AMPHOTERISM This experiment involves the separation and identification of ions using two important reaction types: (i) the formation
JUNIOR COLLEGE CHEMISTRY DEPARTMENT EXPERIMENT 21 SECOND YEAR PRACTICAL. Name: Group: Date: THE CHEMISTRY OF COPPER AND IRON
JUNIOR COLLEGE CHEMISTRY DEPARTMENT EXPERIMENT 21 SECOND YEAR PRACTICAL Name: Group: Date: COPPER THE CHEMISTRY OF COPPER AND IRON 1. To a solution of Cu 2+ ions add aqueous sodium hydroxide and heat the
Final. Mark Scheme. Chemistry CHEM5. (Specification 2420) Unit 5: Energetics, Redox and Inorganic Chemistry
Version.0 General Certificate of Education (A-level) June 203 Chemistry CHEM5 (Specification 2420) Unit 5: Energetics, Redox and Inorganic Chemistry Final Mark Scheme Mark schemes are prepared by the Principal
Chapter 16: Tests for ions and gases
The position of hydrogen in the reactivity series Hydrogen, although not a metal, is included in the reactivity series because it, like metals, can be displaced from aqueous solution, only this time the
80. Testing salts for anions and cations
Classic chemistry experiments 203 80. Testing salts for anions and cations Topic Qualitative analysis. Timing Description 12 hours. Students attempt to identify the anions and cations present in a salt
Paper 1 (7405/1): Inorganic and Physical Chemistry Mark scheme
AQA Qualifications A-level Chemistry Paper (7405/): Inorganic and Physical Chemistry Mark scheme 7405 Specimen paper Version 0.5 MARK SCHEME A-level Chemistry Specimen paper 0. This question is marked
Final. Mark Scheme. Chemistry CHEM5. (Specification 2420) Unit 5: Energetics, Redox and Inorganic Chemistry
Version.4 General Certificate of Education (A-level) January 203 Chemistry CHEM5 (Specification 2420) Unit 5: Energetics, Redox and Inorganic Chemistry Final Mark Scheme Mark schemes are prepared by the
Final. Mark Scheme. Chemistry CHEM5. (Specification 2420) Unit 5: Energetics, Redox and Inorganic Chemistry
Version.2 General Certificate of Education (A-level) January 202 Chemistry CHEM5 (Specification 2420) Unit 5: Energetics, Redox and Inorganic Chemistry Final Mark Scheme Mark schemes are prepared by the
One problem often faced in qualitative analysis is to test for one ion in a
Chemistry 112 Laboratory: Silver Group Analysis Page 11 ANALYSIS OF THE SILVER GROUP CATIONS Ag + Pb Analysis of a Mixture of Cations One problem often faced in qualitative analysis is to test for one
Chapter 14 - Acids and Bases
Chapter 14 - Acids and Bases 14.1 The Nature of Acids and Bases A. Arrhenius Model 1. Acids produce hydrogen ions in aqueous solutions 2. Bases produce hydroxide ions in aqueous solutions B. Bronsted-Lowry
Chemistry 3202. Unit 2 Acids and Bases
Chemistry 3202 Unit 2 Acids and Bases Definitions of Acids and Bases An operational definition is one that is based on the observable properties, behaviours or uses of an entity. The earliest definitions
Balancing Chemical Equations Worksheet
Balancing Chemical Equations Worksheet Student Instructions 1. Identify the reactants and products and write a word equation. 2. Write the correct chemical formula for each of the reactants and the products.
The Synthesis of trans-dichlorobis(ethylenediamine)cobalt(iii) Chloride
CHEM 122L General Chemistry Laboratory Revision 2.0 The Synthesis of trans-dichlorobis(ethylenediamine)cobalt(iii) Chloride To learn about Coordination Compounds and Complex Ions. To learn about Isomerism.
Q.1 Classify the following according to Lewis theory and Brønsted-Lowry theory.
Acid-base A4 1 Acid-base theories ACIDS & BASES - IONIC EQUILIBRIA 1. LEWIS acid electron pair acceptor H, AlCl 3 base electron pair donor NH 3, H 2 O, C 2 H 5 OH, OH e.g. H 3 N: -> BF 3 > H 3 N BF 3 see
Experiment 8 - Double Displacement Reactions
Experiment 8 - Double Displacement Reactions A double displacement reaction involves two ionic compounds that are dissolved in water. In a double displacement reaction, it appears as though the ions are
Chapter 4 Chemical Reactions
Chapter 4 Chemical Reactions I) Ions in Aqueous Solution many reactions take place in water form ions in solution aq solution = solute + solvent solute: substance being dissolved and present in lesser
Qualitative Analysis
Chemistry 201 Qualitative Analysis Introduction General comments: It is always a good idea to use as few chemicals as possible; it makes sense both from consideration of lab safety and chemical waste disposal.
SYNTHESIS AND ANALYSIS OF A COORDINATION COMPOUND OF COPPER
Chemistry 111 Lab: Synthesis of a Copper Complex Page H-1 SYNTHESIS AND ANALYSIS OF A COORDINATION COMPOUND OF COPPER In this experiment you will synthesize a compound by adding NH 3 to a concentrated
Chapter 7: Chemical Reactions
Chapter 7 Page 1 Chapter 7: Chemical Reactions A chemical reaction: a process in which at least one new substance is formed as the result of a chemical change. A + B C + D Reactants Products Evidence that
An acid is a substance that produces H + (H 3 O + ) Ions in aqueous solution. A base is a substance that produces OH - ions in aqueous solution.
Chapter 8 Acids and Bases Definitions Arrhenius definitions: An acid is a substance that produces H + (H 3 O + ) Ions in aqueous solution. A base is a substance that produces OH - ions in aqueous solution.
Chapter 17. How are acids different from bases? Acid Physical properties. Base. Explaining the difference in properties of acids and bases
Chapter 17 Acids and Bases How are acids different from bases? Acid Physical properties Base Physical properties Tastes sour Tastes bitter Feels slippery or slimy Chemical properties Chemical properties
Cambridge International Examinations Cambridge International General Certificate of Secondary Education
Cambridge International Examinations Cambridge International General Certificate of Secondary Education *0123456789* CHEMISTRY 0620/04 Paper 4 Theory (Extended) For Examination from 2016 SPECIMEN PAPER
Molarity of Ions in Solution
APPENDIX A Molarity of Ions in Solution ften it is necessary to calculate not only the concentration (in molarity) of a compound in aqueous solution but also the concentration of each ion in aqueous solution.
1. Qualitative Analysis of Chromium, Iron, and Copper
1. Qualitative Analysis of Chromium, Iron, and Copper Introduction We have used copper and iron as basic materials since the Bronze and Iron Ages, but our extensive use of chromium began only after the
Q.1 Classify the following according to Lewis theory and Brønsted-Lowry theory.
Acid-base 2816 1 Acid-base theories ACIDS & BASES - IONIC EQUILIBRIA LEWIS acid electron pair acceptor H +, AlCl 3 base electron pair donor NH 3, H 2 O, C 2 H 5 OH, OH e.g. H 3 N: -> BF 3 > H 3 N + BF
Experiment 5. Chemical Reactions A + X AX AX A + X A + BX AX + B AZ + BX AX + BZ
Experiment 5 Chemical Reactions OBJECTIVES 1. To observe the various criteria that are used to indicate that a chemical reaction has occurred. 2. To convert word equations into balanced inorganic chemical
General Chemistry Lab Experiment 6 Types of Chemical Reaction
General Chemistry Lab Experiment 6 Types of Chemical Reaction Introduction Most ordinary chemical reactions can be classified as one of five basic types. The first type of reaction occurs when two or more
General Chemistry II Chapter 20
1 General Chemistry II Chapter 0 Ionic Equilibria: Principle There are many compounds that appear to be insoluble in aqueous solution (nonelectrolytes). That is, when we add a certain compound to water
6 Reactions in Aqueous Solutions
6 Reactions in Aqueous Solutions Water is by far the most common medium in which chemical reactions occur naturally. It is not hard to see this: 70% of our body mass is water and about 70% of the surface
Lab #13: Qualitative Analysis of Cations and Anions
Lab #13: Qualitative Analysis of Cations and Anions Objectives: 1. To understand the rationale and the procedure behind the separation for various cations and anions. 2. To perform qualitative analysis
CHM1 Review for Exam 12
Topics Solutions 1. Arrhenius Acids and bases a. An acid increases the H + concentration in b. A base increases the OH - concentration in 2. Strong acids and bases completely dissociate 3. Weak acids and
I N V E S T I C E D O R O Z V O J E V Z D Ě L Á V Á N Í CHEMICAL REACTIONS
Chemical reaction = process during which original substances change to new substances, reactants turn to... The bonds of reactants... and new bonds are... The classification of reactions: 1. Classification
Instructions Answer all questions in the spaces provided. Do all rough work in this book. Cross through any work you do not want to be marked.
GCSE CHEMISTRY Higher Tier Chemistry 1H H Specimen 2018 Time allowed: 1 hour 45 minutes Materials For this paper you must have: a ruler a calculator the periodic table (enclosed). Instructions Answer all
Physical Changes and Chemical Reactions
Physical Changes and Chemical Reactions Gezahegn Chaka, Ph.D., and Sudha Madhugiri, Ph.D., Collin College Department of Chemistry Objectives Introduction To observe physical and chemical changes. To identify
ph: Measurement and Uses
ph: Measurement and Uses One of the most important properties of aqueous solutions is the concentration of hydrogen ion. The concentration of H + (or H 3 O + ) affects the solubility of inorganic and organic
Acids and Bases: A Brief Review
Acids and : A Brief Review Acids: taste sour and cause dyes to change color. : taste bitter and feel soapy. Arrhenius: acids increase [H ] bases increase [OH ] in solution. Arrhenius: acid base salt water.
Paper 1 (7404/1): Inorganic and Physical Chemistry Mark scheme
AQA Qualifications AS Chemistry Paper (7404/): Inorganic and Physical Chemistry Mark scheme 7404 Specimen paper Version 0.6 MARK SCHEME AS Chemistry Specimen paper Section A 0. s 2 2s 2 2p 6 3s 2 3p 6
6) Which compound is manufactured in larger quantities in the U.S. than any other industrial chemical?
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which statement concerning Arrhenius acid-base theory is not correct? A) Acid-base reactions must
EXPERIMENT 8: Activity Series (Single Displacement Reactions)
EPERIMENT 8: Activity Series (Single Displacement Reactions) PURPOSE a) Reactions of metals with acids and salt solutions b) Determine the activity of metals c) Write a balanced molecular equation, complete
Enantiomers: Synthesis, characterization, and resolution of tris(ethylenediamine)cobalt(iii) chloride Introduction:
Enantiomers: Synthesis, characterization, and resolution of tris(ethylenediamine)cobalt(iii) chloride Introduction: The development of coordination chemistry prior to 1950 involved the synthesis and characterization
Experiment 2 Qualitative Analysis
Experiment 2 Qualitative Analysis Goals To use Le Chatelier's principle, complex ion chemistry, and precipitation reactions in the determination of ions in solution. We will study two groups of ions. The
Assessment Schedule 2013 Chemistry: Demonstrate understanding of the properties of organic compounds (91391)
NCEA Level 3 Chemistry (91391) 2013 page 1 of 8 Assessment Schedule 2013 Chemistry: Demonstrate understanding of the properties of organic compounds (91391) Evidence Statement Q Evidence Achievement Achievement
Coordination Compounds with Copper (II) Prelab (Week 2)
Coordination Compounds with Copper (II) Prelab (Week 2) Name Total /10 SHOW ALL WORK NO WORK = NO CREDIT 1. What is the purpose of this experiment? 2. Write the generic chemical formula for the coordination
Solubility Product Constants
Solubility Product Constants PURPOSE To measure the solubility product constant (K sp ) of copper (II) iodate, Cu(IO 3 ) 2. GOALS 1 To measure the molar solubility of a sparingly soluble salt in water.
CHEMICAL DETERMINATION OF EVERYDAY HOUSEHOLD CHEMICALS
CHEMICAL DETERMINATION OF EVERYDAY HOUSEHOLD CHEMICALS Purpose: It is important for chemists to be able to determine the composition of unknown chemicals. This can often be done by way of chemical tests.
Sketch the model representation of the first step in the dissociation of water. H 2. O (l) H + (aq) + OH- (aq) + H 2. OH - (aq) + H 3 O+ (aq)
Lesson Objectives Students will: Create a physical representation of the autoionization of water using the water kit. Describe and produce a physical representation of the dissociation of a strong acid
Writing and Balancing Chemical Equations
Name Writing and Balancing Chemical Equations Period When a substance undergoes a chemical reaction, chemical bonds are broken and new bonds are formed. This results in one or more new substances, often
Chem101: General Chemistry Lecture 9 Acids and Bases
: General Chemistry Lecture 9 Acids and Bases I. Introduction A. In chemistry, and particularly biochemistry, water is the most common solvent 1. In studying acids and bases we are going to see that water
Chapter 4: Structure and Properties of Ionic and Covalent Compounds
Chapter 4: Structure and Properties of Ionic and Covalent Compounds 4.1 Chemical Bonding o Chemical Bond - the force of attraction between any two atoms in a compound. o Interactions involving valence
Number of moles of solute = Concentration (mol. L ) x Volume of solution (litres) or n = C x V
44 CALCULATIONS INVOLVING SOLUTIONS INTRODUCTION AND DEFINITIONS Many chemical reactions take place in aqueous (water) solution. Quantities of such solutions are measured as volumes, while the amounts
Experiment 16-Acids, Bases and ph
Definitions acid-an ionic compound that releases or reacts with water to form hydrogen ion (H + ) in aqueous solution. They taste sour and turn litmus red. Acids react with certain metals such as zinc,
Work hard. Be nice. Name: Period: Date: UNIT 1: Introduction to Matter Lesson 4: A Fine Line Between Compounds and Mixtures
Name: Period: Date: UNIT 1: Introduction to Matter Lesson 4: A Fine Line Between Compounds and Mixtures Do Now: PRE-READING OPEN-NOTES QUIZ! By the end of today, you will have an answer to: How do pure
Report on the Examination
Version 1.0 General Certificate of Education (A-level) June Chemistry CHEM5 (Specification 2420) Unit 5: Energetics, Redox and Inorganic Chemistry Report on the Examination Further copies of this Report
Complexometric Titrations
Complexometric Titrations Complexometric titrations are based on the formation of a soluble complex upon the reaction of the species titrated with the titrant. M + L ML In the module Chemistry 2 you were
Molecular Models in Biology
Molecular Models in Biology Objectives: After this lab a student will be able to: 1) Understand the properties of atoms that give rise to bonds. 2) Understand how and why atoms form ions. 3) Model covalent,
Santa Monica College Chemistry 11
Types of Reactions Objectives The objectives of this laboratory are as follows: To perform and observe the results of a variety of chemical reactions. To become familiar with the observable signs of chemical
Aqueous Solutions. Water is the dissolving medium, or solvent. Some Properties of Water. A Solute. Types of Chemical Reactions.
Aqueous Solutions and Solution Stoichiometry Water is the dissolving medium, or solvent. Some Properties of Water Water is bent or V-shaped. The O-H bonds are covalent. Water is a polar molecule. Hydration
Solution. Practice Exercise. Concept Exercise
Example Exercise 8.1 Evidence for a Reaction Which of the following is experimental evidence for a chemical reaction? (a) Pouring vinegar on baking soda gives foamy bubbles. (b) Mixing two solutions produces
TOPIC 7. CHEMICAL CALCULATIONS I - atomic and formula weights.
TOPIC 7. CHEMICAL CALCULATIONS I - atomic and formula weights. Atomic structure revisited. In Topic 2, atoms were described as ranging from the simplest atom, H, containing a single proton and usually
7 theoretical problems 3 practical problems
14 14 th 7 theoretical problems 3 practical problems THE FURTEENTH INTERNATINAL CHEMISTRY LYMPIAD STCKHLM 1982 SWEDEN THERETICAL PRBLEMS PRBLEM 1 A. The IUPAC name of the compound [Co(NH 3 ) 6 ]Cl 2 is
Chapter 5. Chapter 5. Naming Ionic Compounds. Objectives. Chapter 5. Chapter 5
Objectives Name cations, anions, and ionic compounds. Write chemical formulas for ionic compounds such that an overall neutral charge is maintained. Explain how polyatomic ions and their salts are named
QUESTION (2012:3) (a) (i) Complete the table below showing the conjugate acids and bases. CO 3 H 2 O OH HCN CN -
QUESTION (2012:3) (i) Complete the table below showing the conjugate acids and bases. Conjugate acid Conjugate base - HCO 3 2 CO 3 H 2 O OH HCN CN - (ii) HPO 4 2 (aq) Write equations for the reactions
Equilibrium Constants The following equilibrium constants will be useful for some of the problems.
1 CH302 Exam 4 Practice Problems (buffers, titrations, Ksp) Equilibrium Constants The following equilibrium constants will be useful for some of the problems. Substance Constant Substance Constant HCO
Cambridge International Examinations Cambridge International General Certificate of Secondary Education
ambridge International Examinations ambridge International General ertificate of Secondary Education *012345678* EMISTRY 0620/01 Paper 1 Multiple hoice (ore) For Examination from 2016 SPEIMEN PPER dditional
Properties of Acids and Bases
Properties of Acids and Bases (Adapted from Flinn Scientific Acid Base Test Kit I #AP4567) Introduction Battery acid, stomach acid, acid rain just a few acids in our everyday life! What does it mean when
EXPERIMENT 20: Determination of ph of Common Substances
Materials: ph paper and color chart (ph range 3 to 12) or ph meter distilled water white vinegar household ammonia (or baking soda) spot plate test or 3 small test tubes stirring rod solutions / fruits
Chemical Equations. Chemical Equations. Chemical reactions describe processes involving chemical change
Chemical Reactions Chemical Equations Chemical reactions describe processes involving chemical change The chemical change involves rearranging matter Converting one or more pure substances into new pure
p3 Recognizing Acid/Base Properties when p11 Recognizing Basic versus Nonbasic
General Chemistry II Jasperse Acid-Base Chemistry. Extra Practice Problems 1 General Types/Groups of problems: Conceptual Questions. Acids, Bases, and p1 K b and pk b, Base Strength, and using K b or p7-10
TRANSITION METALS AND COORDINATION CHEMISTRY
CHAPTER TWENTY-ONE TRANSITION METALS AND COORDINATION CHEMISTRY For Review 1. Chromium ([Ar]:4s 0 3d 5 ) and copper [Ar]:4s 1 3d 10 ) have electron configurations which are different from that predicted
Practical Lesson No 4 TITRATIONS
Practical Lesson No 4 TITRATIONS Reagents: 1. NaOH standard solution 0.1 mol/l 2. H 2 SO 4 solution of unknown concentration 3. Phenolphthalein 4. Na 2 S 2 O 3 standard solution 0.1 mol/l 5. Starch solution
2. DECOMPOSITION REACTION ( A couple have a heated argument and break up )
TYPES OF CHEMICAL REACTIONS Most reactions can be classified into one of five categories by examining the types of reactants and products involved in the reaction. Knowing the types of reactions can help
CHAPTERS 15 FAKE TEST QUESTIONS. 1. According to the Brønsted Lowry definition, which species can function both as an acid and as a base?
You might need to know the following K values: CHAPTERS 15 FAKE TEST QUESTIONS CH 3 COOH K a = 1.8 x 10 5 Benzoic Acid K a = 6.5 x 10 5 HNO 2 K a = 4.5 x 10 4 NH 3 K b = 1.8 x 10 5 HF K a = 7.2 x 10 4
Appendix D. Reaction Stoichiometry D.1 INTRODUCTION
Appendix D Reaction Stoichiometry D.1 INTRODUCTION In Appendix A, the stoichiometry of elements and compounds was presented. There, the relationships among grams, moles and number of atoms and molecules
Chemistry Post-Enrolment Worksheet
Name: Chemistry Post-Enrolment Worksheet The purpose of this worksheet is to get you to recap some of the fundamental concepts that you studied at GCSE and introduce some of the concepts that will be part
Chapter 16: Acid-Base and Solubility Equilibria: Reactions in Soil and Water
Chapter 16: Acid-Base and Solubility Equilibria: Reactions in Soil and Water Problems: 16.2-16.86 16.1 ACIDS AND BASES: THE BRØNSTED-LOWRY MODEL PROPERTIES OF ACIDS & BASES Acids produce hydrogen ions,
Determination of the amount of sodium carbonate and sodium hydroxide in a mixture by titration.
Module 9 : Experiments in Chemistry Lecture 38 : Titrations : Acid-Base, Redox and Complexometric Objectives In this lecture you will learn the techniques to do following Determination of the amount of
CHEM5 Energetics, Redox and Inorganic Chemistry Mark scheme
AQA Qualifications A-LEVEL CHEMISTRY CHEM5 Energetics, Redox and Inorganic Chemistry Mark scheme 2420 June 204 Version. Final Mark schemes are prepared by the Lead Assessment Writer and considered, together
Write the acid-base equilibria connecting all components in the aqueous solution. Now list all of the species present.
Chapter 16 Acids and Bases Concept Check 16.1 Chemists in the seventeenth century discovered that the substance that gives red ants their irritating bite is an acid with the formula HCHO 2. They called
Chapter 17. The best buffer choice for ph 7 is NaH 2 PO 4 /Na 2 HPO 4. 19)
Chapter 17 2) a) HCl and CH 3 COOH are both acids. A buffer must have an acid/base conjugate pair. b) NaH 2 PO 4 and Na 2 HPO 4 are an acid/base conjugate pair. They will make an excellent buffer. c) H
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
CHE 1400 - Spring 2015 - Chapter 7 Homework 7 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1)According to Arrhenius, an acid and a base will react
W1 WORKSHOP ON STOICHIOMETRY
INTRODUCTION W1 WORKSHOP ON STOICHIOMETRY These notes and exercises are designed to introduce you to the basic concepts required to understand a chemical formula or equation. Relative atomic masses of
Acids and Bases. Chapter 16
Acids and Bases Chapter 16 The Arrhenius Model An acid is any substance that produces hydrogen ions, H +, in an aqueous solution. Example: when hydrogen chloride gas is dissolved in water, the following
Balancing Chemical Equations Practice
Science Objectives Students will describe what reactants and products in a chemical equation mean. Students will explain the difference between coefficients and subscripts in chemical equations. Students
Brønsted-Lowry Acids and Bases
Brønsted-Lowry Acids and Bases 1 According to Brønsted and Lowry, an acid-base reaction is defined in terms of a proton transfer. By this definition, the reaction of Cl in water is: Cl(aq) + Cl (aq) +
Copyright 2009 by Pearson Education, Inc. Upper Saddle River, New Jersey 07458 All rights reserved.
Sample Exercise 17.1 Calculating the ph When a Common Ion is Involved What is the ph of a solution made by adding 0.30 mol of acetic acid and 0.30 mol of sodium acetate to enough water to make 1.0 L of
Chapter 19: Acids and Bases Homework Packet (50 pts) Name: Score: / 50
Chapter 19: Acids and Bases Homework Packet (50 pts) Topic pg Section 19.1 1-3 Section 19.2 3-6 Section 19.3 6-7 Section 19.4 8 Naming Acids 9 Properties of Acids/Bases 10-11 Conjugate Acid/Base Pairs
Question Bank Electrolysis
Question Bank Electrolysis 1. (a) What do you understand by the terms (i) electrolytes (ii) non-electrolytes? (b) Arrange electrolytes and non-electrolytes from the following substances (i) sugar solution
Version 1. General Certificate of Education June 2011. Energetics, Redox and Inorganic Chemistry. Final. Mark Scheme
Version General Certificate of Education June 20 Chemistry CHEM5 Energetics, Redox and Inorganic Chemistry Final Mark Scheme Mark schemes are prepared by the Principal Examiner and considered, together
hij Teacher Resource Bank GCE Chemistry PSA10: A2 Inorganic Chemistry Carry out a redox titration
hij Teacher Resource Bank GCE Chemistry : A2 Inorganic Chemistry Copyright 2009 AQA and its licensors. All rights reserved. The Assessment and Qualifications Alliance (AQA) is a company limited by guarantee
MOLARITY = (moles solute) / (vol.solution in liter units)
CHEM 101/105 Stoichiometry, as applied to Aqueous Solutions containing Ionic Solutes Lect-05 MOLES - a quantity of substance. Quantities of substances can be expressed as masses, as numbers, or as moles.
Chapter 14: Acids and Bases
Ch 14 Page 1 Chapter 14: Acids and Bases Properties of Acids Sour taste React with some metals Turns blue litmus paper red React with bases Some Common Acids HCl, hydrochloric acid H 2 SO 4, sulfuric acid
Experiment 1 Chemical Reactions and Net Ionic Equations
Experiment 1 Chemical Reactions and Net Ionic Equations I. Objective: To predict the products of some displacement reactions and write net ionic equations. II. Chemical Principles: A. Reaction Types. Chemical
UNIT (6) ACIDS AND BASES
UNIT (6) ACIDS AND BASES 6.1 Arrhenius Definition of Acids and Bases Definitions for acids and bases were proposed by the Swedish chemist Savante Arrhenius in 1884. Acids were defined as compounds that
Chapter 8: Chemical Equations and Reactions
Chapter 8: Chemical Equations and Reactions I. Describing Chemical Reactions A. A chemical reaction is the process by which one or more substances are changed into one or more different substances. A chemical
Chemical Reactions in Water Ron Robertson
Chemical Reactions in Water Ron Robertson r2 f:\files\courses\1110-20\2010 possible slides for web\waterchemtrans.doc Properties of Compounds in Water Electrolytes and nonelectrolytes Water soluble compounds
Properties of Acids and Bases
Lab 22 Properties of Acids and Bases TN Standard 4.2: The student will investigate the characteristics of acids and bases. Have you ever brushed your teeth and then drank a glass of orange juice? What
Solubility Product Constant
Solubility Product Constant Page 1 In general, when ionic compounds dissolve in water, they go into solution as ions. When the solution becomes saturated with ions, that is, unable to hold any more, the