CHM-201 General Chemistry and Laboratory I Laboratory 4. Introduction to Chemical Reactions (based in part on Small Scale Chemistry methodology as
|
|
- Charlotte Shepherd
- 5 years ago
- Views:
Transcription
1 CHM-201 General Chemistry and Laboratory I Laboratory 4. Introduction to Chemical Reactions (based in part on Small Scale Chemistry methodology as described in Chemtrek by Stephen Thompson at Colorado State University) October 16, 2018 Purpose: This laboratory will introduce you to a variety of chemical reactions. You will observe precipitation reactions, acid-base reactions, oxidation-reduction reactions and reactions in which complex ions are formed. You will gather information about known compounds to help you deduce the identity of an unknown compound. Introduction: There are several types of chemical reactions. A fundamental understanding of chemical reactions is necessary to consider the other topics in this course. This laboratory is designed to give you experience with chemical reactions and to observe what is meant by a chemical change. By observing some chemical reactions, you may find it easier to understand what they are. Rather than discuss each reaction as it comes, it is easier when we group reactions into categories. We will use three categories to describe reactions in this laboratory: 1. Precipitation Reactions: reactions that result in the formation of an insoluble (solid) compound. 2. Acid-Base Reactions: reactions that result from the transfer of a hydrogen ion (H + ) from one species to another. 3. Oxidation-Reduction Reactions: reactions that result in the transfer of electrons from one species to another. To state it another way, there is a change in oxidation number for at least two elements in the reaction. Now that we have categorized reactions, we shall discuss each type of reaction in more detail and relate that to what we expect to observe in the laboratory session. 1. Precipitation Reactions In precipitation reactions, two substances, one insoluble (a precipitate) and one soluble (that you probably cannot observe) form in what is called an exchange reaction. In an exchange reaction, the cation from one solution combines with the anion in the second solution to form a precipitate. Exchange reactions have the following general form: C 1A 1(aq) + C 2A 2(aq) C1A2(s) + C2A1(aq) Where C 1 is the cation of solution 1, A 1 is the anion of solution 1, C 2 is the cation of solution 2, and A 2 is the anion of solution 2 As an example, we shall use the reaction of silver nitrate with sodium chloride to form silver chloride, a precipitate, and sodium nitrate. The silver chloride will appear as a white precipitate. The chemical reaction is written below: AgNO 3(aq) + NaCl AgCl(s) + (aq) (Note that C 1 = Ag +, A 1 = NO 3-, C 2 = Na +, A 2 = Cl - in this example) Since AgCl is an insoluble material we might suspect that the combination of AgNO 3 and NaCl would give an insoluble material (You will do this in the experiment. Check it out!). Notice that the other possible product, NaNO 3, would also be formed but remains in solution, giving you no way to observe it. The reason that this is a precipitation reaction is that it forms an observable solid, AgCl, from the combination of two solutions.
2 Being able write an exchange reaction for two ionic compounds does not necessarily mean that a chemical reaction occurs, however. When you combine sodium chloride, NaCl, and copper(ii) sulfate, CuSO 4, in the laboratory, no precipitate forms. The sodium chloride solution is colorless and the copper sulfate solution is blue. When you combine them, you get a solution that is lighter blue than the original copper sulfate solution. Nothing else seems to happen. No chemical reaction is apparent. We can write an exchange reaction as follows: 2NaCl(aq) + CuSO 4(aq) CuCl 2(aq) + Na 2SO 4(aq), but there is no precipitate (no solid formed). What ions are present on the left side of the equation? Answer: 2 sodium ions, 2 chloride ions, 1 copper ion and 1 sulfate ion. And what ions are present on the right hand side of the equation? Answer: 2 sodium ion, 2 chloride ion, 1 copper ion and 1 sulfate ion. If both sides contain the same ions in the same amounts, there is no chemical reaction. If you correctly write the net ionic equation, you will find that there is no net ionic reaction because everything cancels (prove this to yourself). There is no reaction. Sodium chloride and copper sulfate (the reactants) are both soluble, and copper(ii) chloride and sodium sulfate (the products) are also soluble. In this case, since the same ions are present in solution as reactants and as products, there was no net ionic equation. We have simply mixed two soluble ionic compounds. 2. Acid-Base Reactions We will use a very simple definition of acids and bases in order to understand them better. We will define acids as compounds that can donate hydrogen ions (H + ) to other substances. We can define bases as compounds that consume hydrogen ions (note that when we discuss acids and bases in greater detail in CHM202, the definitions of what we call acids and bases will be expanded). If an acid and a base are combined, they will react with one another such that the acid will donate a hydrogen ion and the base will consume it. A common acid used in the laboratory is hydrochloric acid (HCl). HCl is an acid because it can donate hydrogen ions to other substances. A common base is sodium hydroxide (NaOH) which can consume hydrogen ion since hydroxide ion (OH - ) combines with hydrogen ion to form water (H 2O). The chemical reaction we would write for this chemical change would be: The net ionic equation for this reaction is: HCl(aq) + NaOH(aq) H 2O(l) + NaCl(aq) H + (aq) + OH - (aq) H 2O(l) The combination of hydrogen ion (H + ) and hydroxide ion (OH - ) to form water is a very common net ionic equation for acid-base reactions (it accounts for about 80% of such reactions you will see in this course). This type of reaction can be described as, "an acid and base react to form water and a salt." Does the reaction of HCl with NaOH meet this description? Another common acid-base reaction takes place when an acid reacts with carbonate (CO 3 2- ) or hydrogen carbonate, also known as bicarbonate, (HCO 3- ) to give water and carbon dioxide. An example is given below for the reaction of sulfuric acid with potassium carbonate: H 2SO 4(aq) + K 2CO 3(aq) K 2SO 4(aq) + H 2O(l) + CO 2(g) In this case, carbon dioxide gas is formed in addition to a salt and water. The net ionic equation for this reaction is: 2H + (aq) + CO 3 2- (aq) H 2O(l) + CO 2(g) The two net ionic equations described above should apply to almost all of the acid-base reactions you will observe in this course.
3 It is more difficult to observe an acid/base reaction than a precipitation reaction. Since there may be no immediately observable differences (for example the HCl-NaOH reaction has the combination of two colorless solutions and the product is also a colorless solution), we need a method of finding out if solutions contain a high concentration of hydrogen ions (acidic) or hydroxide ions (basic). We can do this with indicator paper (litmus paper) and/or solutions of indicators that change color depending on the concentration of H + or OH -. If we use litmus paper we can define if solutions are acids (acids turn blue litmus paper red) or bases (bases turn red litmus paper blue). In general, indicators change color depending on the acidity or basicity of a solution. One example is phenolphthalein, which is clear in acidic solution but turns pink in basic solution. The universal indicator used in this laboratory undergoes a wide range of color changes depending on the concentration of H + ions. When acids and bases react, the ph (acidity/basicity) usually changes, and there may be other indications of a chemical reaction (gas evolution for example). It may be difficult to determine when some acid-base reactions have occurred without using indicators, if the ph is different from those of the two starting solutions, it is likely that an acid-base reaction has occurred. For the HCl-NaOH example, the final reaction mixture (NaCl in water) will be neutral (no change in litmus paper) but only if equal amounts of the starting materials are combined. Why is that the case? If HCl is in excess, the resulting solution will remain acidic. If NaOH is in excess, the resulting solution will remain basic. In this laboratory, you will determine whether some solutions before and after reacting are acids or bases. Be careful to observe any other changes such as gas evolution, since that will help you identify your unknown. 3. Oxidation-Reduction Reactions Oxidation-reduction (redox) reactions are the most complex of the three. In order to describe oxidationreduction reactions we need first to understand oxidation numbers. Oxidation numbers represent the electrical charge or equivalent charge of an atom in a compound or element. The oxidation number of a pure element is always zero. You will need to know how to assign oxidation numbers in order to determine whether a reaction is an oxidation-reduction reaction. We can look at a simple case where the oxidation number is the charge of an ion (remember that a pure element has an oxidation number of zero). If we react sodium metal (an element) with chlorine gas (an element) we will obtain sodium chloride. In this reaction, the charge is equal to the oxidation number. The reaction is as follows with the oxidation number of each material below it: Oxidation # Na + Cl 2 2NaCl Any reaction in which there is a change in oxidation numbers is an oxidation-reduction reaction. One atom has to increase its oxidation number (be oxidized), and one atom has to decrease its oxidation number (be reduced). It is possible for the two atoms involve to be of the same element, but we will not see that in this laboratory. In the example above, sodium increases its oxidation number from 0 to +1 whereas chlorine decreases its oxidation number from 0 to -1. Sodium is oxidized and chlorine is reduced. When one atom undergoes an increase in oxidation number, another atom always undergoes a decrease in oxidation number. Oxidation cannot take place without a corresponding reduction and vice versa. Oxidation numbers give us a way to account for the number of electrons present. Sodium atoms and sodium ions do not have the same number of electrons. Neither do chlorine atoms and chloride ions. Oxidation-reduction reactions are reactions accompanied by a change in the number of electrons present in the materials that react. There are electrons transferred from one compound to another. In the example above, sodium transfers electrons to chlorine in order to form sodium chloride.
4 In the laboratory, you may observe oxidation-reduction reactions because of some observable change, and you may be able to reverse these reactions by supplying electrons from an electrical source such as a 9V battery. If electrons are transferred when you react some materials together, you can reverse this process if you transfer the electrons back. Watch for instances of this in the laboratory. You can also connect a battery to an aqueous solution and convert the water to its constituent elements, hydrogen and oxygen. This is also an oxidation-reduction reaction. 4. Introduction to Complex Ions Finally, you will observe a few cases in which complex ions are formed in solution. Complex ions are ions in which a cation binds to one or more anions or with a molecule having lone pairs of electrons (the topic of lone pairs is covered much later in this course). For this brief introduction to the formation of complex ions in solution, you will observe the ammonia complex ions of silver and copper. The reaction of silver chloride, insoluble in water, with ammonia, results in the silver chloride dissolving. This happens because silver chloride is insoluble but silver ion reacts with ammonia to form a more soluble silver ion complex with ammonia: AgCl(s) + 2NH 3(aq) Ag(NH 3) 2+ (aq) + Cl - (aq) Similarly, blue copper ion in solution turns a much darker blue when combined with ammonia. This is due to a complex formed between copper ion and four ammonia molecules: Cu 2+ (aq) + 4NH 3(aq) Cu(NH 3) 4 2+ (aq) For this course, you do not have to predict when complex ions of this type will form, but you should be aware that this might occur. Procedure: General: Be sure to write all pertinent observations, including those you don't expect. Be sure to keep track of all precipitates, gas formations and information from litmus and indicators. Be careful not to contaminate your droppers or solutions. Poor techniques will lead to poor results, and you may not be able to identify your unknown. NOTE: You should have a graphical chart indicating the most effective order of procedures as given below. It should help clarify the procedures. 1. Precipitation reactions 1.1 Using the grid provided place one drop of AgNO 3 in each of the nine grid positions directly below it. 1.2 Repeat procedure 1.1 for each of the following: Na 2CO 3, Ba(NO 3) 2, Pb(NO 3) 2, Zn(NO 3) 2 and unknown. 1.3 Add one drop of the first compound in the left column (HCl) to the drop of silver nitrate (AgNO 3) already there. Be especially careful to keep the dropper from touching the other chemical. You may use a clean toothpick to mix the chemicals, if necessary. 1.4 Write your observations (precipitation, gas formation, color change, etc.) for any changes you observe. If there was no apparent change, write NC for no change. Use the similar chart included in your lab report. 1.5 Repeat 1.3 and 1.4 with hydrochloric acid across the top row for all the compounds on the left side under Precipitation Reactions. 1.6 Place one drop of hydrochloric acid to each of the remaining four columns under Acid/Base Reactions. 1.7 Repeat for each of the compounds in the left column (H 2SO 4, NH 4Cl, NH 3, NaOH, Na 2CO 3, Na 2HPO 4, Na 2SO 4 and NaCl, but not NH 3) one at a time, recording your observations
5 as you complete each addition. If you make a mistake, dab up the incorrect solutions and reapply. You only need one drop of each compound to make an observation. NOTE: Ammonia is a volatile solution and its fumes will affect some of the other reactions. DO NOT place any NH 3 on the sheet until all the other reactions have been observed, including Acid-base reactions. You will come back to 1.7 then. 1.8 Observe the pattern from the precipitation reactions and the acid-base reactions. Is there one pattern that is identical to that of the unknown? Use the information you have gathered to determine the identity of the unknown. (Do at home not in the lab.) 1.9 Write the number of the unknown and its identity in the space provided. The unknown is one of the five compounds across the top of the chart on the Precipitation Reactions side of the chart. (Do at home not in the lab.) 1.10 Write down your reasoning in the space provided. Your explanation need not be overly detailed or even complete, but you must articulate it. No reasoning no credit! (Do at home not in the lab.) 2. Acid-base reactions. 2.1 There should now be a drop of each solution from the left column on each space under each column on the Acid/Base Reactions side of the sheet. 2.2 Test each of the solutions with both red and blue litmus paper in the vertical columns provided. If there is a color change, record the new color (P = Pink, B = Blue). If the litmus paper does not change color, mark NC for no change. 2.3 Add one drop of phenolphthalein to each solution in the column so labeled and record the result as P for pink, or NC for no change. 2.4 Add one drop of the universal indicator to each solution in the column so labeled and record the color change (if any). NC for no change. 2.5 Now add one drop of NH 3 solution across the bottom row as in Procedure 1.7 and record your observations. 2.6 Repeat , testing the newly added ammonia solution with the indicators. 3. Complex ion formation 3.1 Place one drop of copper sulfate solution (CuSO 4) in each of the unused ovals (marked CuSO 4 and CuSO 4 + NH 3). Add a few drops of ammonia to the appropriate oval. What happens? Does the color change. Record your observations. 3.2 Rinse your acetate sheet with water over a large beaker and transfer the waste to the waste collection vessel at the instructor's desk. Wipe down your acetate sheet with a paper towel and discard the entire sheet. Be sure you have recorded all your results before you clean your sheet! 4. Oxidation-Reduction Reactions 4.1 Using the spot plate wells, add 10 drops of copper sulfate solution to the first well and 10 drops of zinc nitrate to the second well. 4.2 Place a small piece of zinc metal into the copper sulfate solution and a small piece of copper metal into the zinc nitrate solution. Let the metals sit in the solutions for 2 minutes. Remove the two metals and record your observations.
6 4.3 Connect the zinc metal that was dipped in the CuSO 4 solution to the positive post of a 9V battery using an alligator clip. Connect the graphite pencil lead to the negative post and place both solids into the copper sulfate solution without touching the solids together. Take the solids out of the solution after 1 minute. Record your observations. 4.4 Repeat 4.3 connecting the copper metal to the negative post and the graphite pencil lead to the positive post and place both solids in the zinc nitrate solution without touching. Take the solids out of the solution after 1 minute and record your observations. 4.5 See me to help with the following procedure. I will perform the preparation for your group to complete this part in the hood for safety Pierce a disposable pipette bulb with two needles, making sure the needles do not touch each other Fill the pipette with 1M sulfuric acid solution Place the pipette in an small Erlenmeyer flask with the bulb out of the flask Connect one needle to the positive terminal and one to the negative terminal of a 9V battery and observe what happens When the bulb is full of gas, ignite the gaseous mixture as instructed Record your observations.
EXPERIMENT A5: TYPES OF REACTIONS. Learning Outcomes. Introduction. Upon completion of this lab, the student will be able to:
1 Learning Outcomes EXPERIMENT A5: TYPES OF REACTIONS Upon completion of this lab, the student will be able to: 1) Examine different types of chemical reactions. 2) Express chemical equations in molecular,
More informationExperiment 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
More informationThe Copper Cycle. HCl(aq) H + (aq) + Cl (aq) HCl(aq) + H 2 O(l) H 3 O + (aq) + Cl (aq)
The Copper Cycle Introduction Many aspects of our lives involve chemical reactions from the batteries that power our cars and cell phones to the thousands of processes occurring within our bodies. We cannot
More informationChapter 4 Reactions in Aqueous Solutions. Copyright McGraw-Hill
Chapter 4 Reactions in Aqueous Solutions Copyright McGraw-Hill 2009 1 4.1 General Properties of Aqueous Solutions Solution - a homogeneous mixture Solute: the component that is dissolved Solvent: the component
More informationWhat Do You Think? Investigate GOALS
Cool Chemistry Show Activity 4 Chemical Equations GOALS In this activity you will: Represent chemical changes using word equations and chemical equations. Distinguish between different classes of chemical
More informationChapter 4 Types of Chemical Reaction and Solution Stoichiometry
Chapter 4 Types of Chemical Reaction and Solution Stoichiometry Water, the Common Solvent One of the most important substances on Earth. Can dissolve many different substances. A polar molecule because
More informationChemistry 141 Samuel A. Abrash Chemical Reactions Lab Lecture 9/5/2011
Chemistry 141 Samuel A. Abrash Chemical Reactions Lab Lecture 9/5/2011 Q: Before we start discussing this week s lab, can we talk about our lab notebooks? Sure. Q: What makes a lab notebook a good notebook?
More informationChapter 4. Types of Chemical Reactions and Solution Stoichiometry
Chapter 4 Types of Chemical Reactions and Solution Stoichiometry Chapter 4 Table of Contents 4.1 Water, the Common Solvent 4.2 The Nature of Aqueous Solutions: Strong and Weak Electrolytes 4.3 The Composition
More informationSanta Monica College Chemistry 11
Types of Reactions Objectives The objectives of this laboratory are as follows: To perform several types of simple chemical reactions, To become familiar with some common observable signs of chemical reactions,
More informationAqueous Chemical Reactions
Aqueous Chemical Reactions Introduction Many chemical reactions occur in water and therefore they are considered aqueous chemical reactions. The reagents are typically dissolved or diluted in water and
More informationExperiment 5E BOTTLES WITHOUT LABELS: STUDIES OF CHEMICAL REACTIONS
Experiment 5E BOTTLES WITHOUT LABELS: STUDIES OF CHEMICAL REACTIONS FV 1-21-16 MATERIALS: Eight 50 ml beakers, distilled water bottle, two 250 ml beakers, conductivity meter, ph paper (A/B/N), stirring
More informationEXPERIMENT 7 Precipitation and Complex Formation
EXPERIMENT 7 Precipitation and Complex Formation Introduction Precipitation is the formation of a solid in a solution as the result of either a chemical reaction, or supersaturating a solution with a salt
More informationNET IONIC REACTIONS in AQUEOUS SOLUTIONS AB + CD AD + CB
NET IONIC REACTIONS in AQUEOUS SOLUTIONS Double replacements are among the most common of the simple chemical reactions. Consider the hypothetical reaction: AB + CD AD + CB where AB exists as A + and B
More informationCHM 130LL: Double Replacement Reactions
CHM 130LL: Double Replacement Reactions One of the main purposes of chemistry is to transform one set of chemicals (the reactants) into another set of chemicals (the products) via a chemical reaction:
More informationName CHEMISTRY / / Oxide Reactions & Net Ionic Reactions
Name CHEMISTRY / / Oxide Reactions & Net Ionic Reactions The first type of reactions we will look at today are reactions between an oxide (a compound with oxygen as its anion) and water. There are two
More informationCSUS Department of Chemistry Experiment 3 Chem.1A
Experiment 3: Reactions in Aqueous Solutions: Pre lab Name: 10 points Due at the beginning of lab. Section: 1. Precipitation Reactions a. On the reverse side of this page or on a separate piece of paper,
More informationChemical Equilibria: Coordination Compounds
E11 Chemical Equilibria: Coordination Compounds Objective Ø Illustrate the tendency of metal ions to form metal coordination complexes with ions and neutral polar molecules that act as electron-pair donors
More informationTYPES OF CHEMICAL REACTIONS
EXPERIMENT 11 (2 Weeks) Chemistry 110 Laboratory TYPES OF CHEMICAL REACTIONS PURPOSE: The purpose of this experiment is perform, balance and classify chemical reactions based on observations. Students
More informationAqueous Chemical Reactions
Aqueous Chemical Reactions Introduction Many chemical reactions occur in water and therefore they are considered aqueous chemical reactions. The reagents are typically dissolved or diluted in water and
More informationReaction Types and Chemical Equations
Cool Chemistry Show Section 4 Reaction Types and Chemical Equations What Do You See? Learning Outcomes In this section you will Represent chemical changes using word equations and chemical equations. Distinguish
More informationTypes of Chemical Reactions
Types of Chemical Reactions Objectives Perform and observe the results of a variety of chemical reactions. Become familiar with the observable signs of chemical reactions. Identify the products formed
More informationNaming salts. Metal Acid Salt. Sodium hydroxide reacts with Hydrochloric acid to make Sodium chloride
Naming salts A salt is any compound formed by the neutralisation of an acid by a base. The name of a salt has two parts. The first part comes from the metal, metal oxide or metal carbonate. The second
More informationExperiment Nine Acids and Bases
Name: Lab Section: Experiment Nine Acids and Bases Objective Identifying and understanding the nature of acids and bases is an important part of the laboratory toolbox, the purpose of this lab is to help
More informationChapter 4. Reactions in Aqueous Solution
Chapter 4 Reactions in Aqueous Solution Topics General properties of aqueous solutions Precipitation reactions Acid base reactions Oxidation reduction reactions Concentration of solutions Aqueous reactions
More informationExperiment Eight Acids and Bases
Name: Lab Section: Experiment Eight Acids and Bases Objective Identifying and understanding the nature of acids and bases is an important part of the laboratory toolbox, the purpose of this lab is to help
More informationSingle Replacement Reactions
Single Replacement Reactions Name: Period: PURPOSE: To observe and practice writing down molecular, complete ionic, and net ionic equations for single replacement reactions. THEORY: Most reactions in chemistry
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 informationCh. 8 Chemical Reactions
Ch. 8 Chemical Reactions Intro to Reactions I II III IV V Signs of a Chemical Reaction Evolution of heat and light Formation of a gas Formation of a precipitate Color change Law of Conservation of Mass
More informationAqueous Chemical Reactions
Aqueous Chemical Reactions Introduction Many chemical reactions occur in water and therefore they are considered aqueous chemical reactions. The reagents are typically dissolved or diluted in water and
More informationChapter 6. Chemical Reactions. Sodium reacts violently with bromine to form sodium bromide.
Chapter 6 Chemical Reactions Sodium reacts violently with bromine to form sodium bromide. Evidence of Chemical Reactions Chemical Equations Reactants Products Reactant(s): Substance(s) present before the
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 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 informationChemical Change. Section 9.1. Chapter 9. Electrolytes and Solution Conductivity. Goal 1. Electrical Conductivity
Chapter 9 Chemical Change Section 9.1 Electrolytes and Solution Conductivity Goal 1 Electrical Conductivity Distinguish among strong electrolytes, weak electrolytes, and nonelectrolytes. Strong Electrolyte:
More informationChemical Reaction Types
Chemical Reactions Chemical Reaction Types There are 5 types of chemical reactions that you need to know Combination reaction Decomposition reaction Combustion reaction Single replacement (redox) reaction
More information4.6 Describing Reactions in Solution
4.6 Describing Reactions in Solution The overall or formula equation for this reaction: K 2 CrO(aq) Ba(NO 3 ) 2 (aq) BaCrO 4 (s) 2KNO 3 (aq) Although the formula equation shows the reactants and products
More informationTypes of Chemical Reactions and Equations
Types of Chemical Reactions and Equations v051413_7pm Objectives: You will be able to identify a reaction according to the chemical changes that occur. You will be able to write balanced chemical equations
More informationClassifying Chemical Reactions
1 Classifying Chemical Reactions Analyzing and Predicting Products Introduction The power of chemical reactions to transform our lives is visible all around us-in our cars, even in our bodies. Chemists
More informationEIGHT BOTTLES. H H H O Na + O Cl O H H H. Hydrated sodium ion and chloride ion
EIGHT BOTTLES 1 Chemists often do "detective work" in the lab. In order to figure out the answer to a question or to solve a mystery, chemists perform a variety of tests and analyses, then interpret the
More informationChemistry: Lab Ions in Aqueous Solution
KEY Chemistry: Lab Ions in Aqueous Solution Introduction: Many ionic solids dissolve in water to form clear, aqueous solutions that conduct electricity. It is the ions that conduct the electric current.
More informationSolubility Rules and Net Ionic Equations
Solubility Rules and Net Ionic Equations Why? Solubility of a salt depends upon the type of ions in the salt. Some salts are soluble in water and others are not. When two soluble salts are mixed together
More informationScientific Observations and Reaction Stoichiometry: The Qualitative Analysis and Chemical Reactivity of Five White Powders
Scientific Observations and Reaction Stoichiometry: The Qualitative Analysis and Chemical Reactivity of Five White Powders Objectives Part 1: To determine the limiting reagent and percent yield of CuCO
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 informationDuring photosynthesis, plants convert carbon dioxide and water into glucose (C 6 H 12 O 6 ) according to the reaction:
Example 4.1 Stoichiometry During photosynthesis, plants convert carbon dioxide and water into glucose (C 6 H 12 O 6 ) according to the reaction: Suppose that a particular plant consumes 37.8 g of CO 2
More informationTo observe trends in solubility and exceptions to these trends. To write chemical formulas based on cation/anion charges.
Solubility Rules PURPOSE To develop a set of solubility rules. GOALS To observe trends in solubility and exceptions to these trends. To write chemical formulas based on cation/anion charges. To learn to
More informationConcentration Units. Solute CONCENTRATION. Solvent. g L -1. (M, molarity) concentration in. mol / litre of solution. mol L -1. molality. molality.
CHAPTER 4 REACTIONS IN AQUEOUS SOLUTION CONCENTRATION Solute Solvent Concentration Units mass NaCl / unit volume of solution g L -1 (M, molarity) concentration in moles per litre of solution c NaCl c B
More informationLab #14: Qualitative Analysis of Cations and Anions
Lab #14: 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
More informationChem 2115 Experiment #10. Acids, Bases, Salts, and Buffers
Chem 2115 Experiment #10 Acids, Bases, Salts, and Buffers OBJECTIVE: The goal of this series of experiments is to investigate the characteristics of acidic and basic solutions. We will explore the neutralization
More informationChemical Equations. Chemical Reactions. The Hindenburg Reaction 5/25/11
Chemical Reactions CHM 1032C Chemical Equations Chemical change involves a reorganization of the atoms in one or more substances. The Hindenburg Reaction Reactants are on left, products to the right. Arrow
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 informationDOUBLE DISPLACEMENT REACTIONS. Double your pleasure, double your fun
DOUBLE DISPLACEMENT REACTIONS Double your pleasure, double your fun Industrial processes produce unwanted by-products. Dissolved toxic metal ions-copper, mercury, and cadmium-are common leftovers in the
More informationExperiment 7: SIMULTANEOUS EQUILIBRIA
Experiment 7: SIMULTANEOUS EQUILIBRIA Purpose: A qualitative view of chemical equilibrium is explored based on the reaction of iron(iii) ion and thiocyanate ion to form the iron(iii) thiocyanate complex
More informationChemical Reactions: Introduction to Reaction Types
Chemical Reactions: Introduction to Reaction Types **Lab Notebook** Record observations for all of the chemical reactions carried out during the lab in your lab book. These observations should include:
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 informationLab: Types of Chemical Reactions
Name: Date: Period: Lab: Types of Chemical Reactions ESSENTIAL QUESTION: How do we represent chemical reactions as a chemical equation? BACKGROUND- See class handout. PRELAB: 1. What is a chemical reaction
More informationChapter 6. Types of Chemical Reactions and Solution Stoichiometry
Chapter 6 Types of Chemical Reactions and Solution Stoichiometry Chapter 6 Table of Contents (6.1) (6.2) (6.3) (6.4) (6.5) (6.6) (6.7) (6.8) Water, the common solvent The nature of aqueous solutions: Strong
More informationWhich of the following answers is correct and has the correct number of significant figures?
Avogadro s Number, N A = 6.022 10 23 1. [7 points] Carry out the following mathematical operation: 6.06 10 3 + 1.1 10 2 Which of the following answers is correct and has the correct number of significant
More informationStresses Applied to Chemical Equilibrium
Stresses Applied to Chemical Equilibrium Objective Many chemical reactions do not go to completion. Rather, they come to a point of chemical equilibrium before the reactants are fully converted to products.
More informationA reaction in which a solid forms is called a precipitation reaction. Solid = precipitate
Chapter 7 Reactions in Aqueous Solutions 1 Section 7.1 Predicting Whether a Reaction Will Occur Four Driving Forces Favor Chemical Change 1. Formation of a solid 2. Formation of water 3. Transfer of electrons
More informationAP Chemistry Unit 2 Test (Chapters 3 and 4)
AP Chemistry Unit 2 Test (Chapters 3 and 4) NAME: 1. A student is assigned the task of determining the mass percent of silver in an alloy of copper and silver by dissolving a sample of the alloy in excess
More informationPhysical 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
More informationWhat Do You Think? Investigate GOALS
Activity 2 More Chemical Changes GOALS In this activity you will: Observe several typical examples of evidence that a chemical change is occurring. Make generalizations about the combinations of materials
More informationCh 7 Chemical Reactions Study Guide Accelerated Chemistry SCANTRON
Ch 7 Chemical Reactions Study Guide Accelerated Chemistry SCANTRON Name /80 TRUE/FALSE. Write 'T' if the statement is true and 'F' if the statement is false. Correct the False statments by changing the
More informationExperiment Six Precipitation Reactions
Experiment Six Precipitation Reactions Objective Identify the ions present in various aqueous solutions. Systematically combine solutions and identify the reactions that form precipitates and gases. Write
More informationName HONORS CHEMISTRY / / Oxide Reactions & Net Ionic Reactions
Name HONORS CHEMISTRY / / Oxide Reactions & Net Ionic Reactions The first type of reactions we will look at today are reactions between an oxide (a compound with oxygen as its anion) and water. There are
More informationReactions in Aqueous Solution
1 Reactions in Aqueous Solution Chapter 4 For test 3: Sections 3.7 and 4.1 to 4.5 Copyright The McGrawHill Companies, Inc. Permission required for reproduction or display. 2 A solution is a homogenous
More informationAcids Bases and Salts Acid
Acids Bases and Salts Acid ph less than 7.0 Sour taste Electrolyte Names of Acids Binary acids Contain only 2 elements Begin with hydro; end with ic Ternary acids Ex: H 2 S = hydrosulfuric Contain a polyatomic
More informationSeparation and Qualitative Determination of Cations
Separation and Qualitative Determination of Cations Introduction Much of laboratory chemistry is focused on the question of how much of a given substance is contained in a sample. Sometimes, however, the
More informationEXPERIMENT Identification of Unknown Solutions
EXPERIMENT Identification of Unknown Solutions PURPOSE As you work through this exercise you will learn how to: Make careful observations of chemical reactions. Develop logical testing procedures for performing
More informationChapter 04. Reactions in Aqueous Solution
Chapter 04 Reactions in Aqueous Solution Composition Matter Homogeneous mixture Contains One visible distinct phase Uniform properties throughout Two or more substances that are mixed together Substances
More informationChemical Reactions CHAPTER Reactions and Equations
CHAPTER 9 Chemical Reactions 9.1 Reactions and Equations The process by which atoms of one or more substances are rearranged to form different substances is called a chemical reaction. There are a number
More informationAqueous Reactions. The products are just the cation-anion pairs reversed, or the outies (A and Y joined) and the innies (B and X joined).
Aqueous Reactions Defining Aqueous Reactions Aqueous reactions are reactions that take place in water. To understand them, it is important to understand how compounds behave in water. Some compounds are
More informationEXPERIMENT 10: Precipitation Reactions
EXPERIMENT 10: Precipitation Reactions Metathesis Reactions in Aqueous Solutions (Double Displacement Reactions) Purpose a) Identify the ions present in various aqueous solutions. b) Systematically combine
More informationCharacteristics of Chemical Change
Section 2 Characteristics of Chemical Change What Do You See? Learning Outcomes In this section you will Observe several typical examples of evidence that a chemical change is occurring. Make generalizations
More informationChapter 4: Chemical Quantities and Aqueous Reactions
Chapter 4: Chemical Quantities and Aqueous Reactions C (s) + O 2 (g) CO 2 (g) CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2 H 2 0 (g) 2 C 8 H 18 (g) + 25 O 2 (g) 16 CO 2 (g) + 18 H 2 0 (g) Stoichiometry Calculations
More informationDraw one line from each solution to the ph value of the solution. Solution ph value of the solution
1 The ph scale is a measure of the acidity or alkalinity of a solution. (a) Draw one line from each solution to the ph value of the solution. Solution ph value of the solution 5 Acid 7 9 Neutral 11 13
More informationReactions in aqueous solutions Redox reactions
Reactions in aqueous solutions Redox reactions Redox reactions In precipitation reactions, cations and anions come together to form an insoluble ionic compound. In neutralization reactions, H + ions and
More informationReactions in Aqueous Solutions
Reactions in Aqueous Solutions 1 Chapter 4 General Properties of Aqueous Solutions (4.1) Precipitation Reactions (4.2) Acid-Base Reactions (4.3) Oxidation-Reduction Reactions (4.4) Concentration of Solutions
More informationChemical Reactions and Equations
Chemical Reactions and Equations 5-1 5.1 What is a Chemical Reaction? A chemical reaction is a chemical change. A chemical reaction occurs when one or more substances is converted into one or more new
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 9: Acids, Bases, and Salts
Chapter 9: Acids, Bases, and Salts 1 ARRHENIUS ACID An Arrhenius acid is any substance that provides hydrogen ions, H +, when dissolved in water. ARRHENIUS BASE An Arrhenius base is any substance that
More informationA general statement governing all systems in a state of dynamic equilibrium follows:
Chapter 20 Experiment: LeChâtelier s Principle: Buffers OBJECTIVES: Study the effects of concentration and temperature changes on the position of equilibrium in a chemical system. Study the effect of strong
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 informationSection I: Synthesis reactions Synthesis reactions occur when two or more substances come together to form a single new substance.
TYPES OF CHEMICAL REACTIONS A Laboratory Investigation Purpose: Observe the five major types of reactions. Record observations for these reactions. Complete balanced equations for these reactions. Introduction:
More informationIndicators of chemical reactions
Indicators of chemical reactions Emission of light or heat Formation of a gas Formation of a precipitate Color change Emission of odor All chemical reactions: have two parts Reactants - the substances
More informationReaction Classes. Precipitation Reactions
Reaction Classes Precipitation: synthesis of an ionic solid a solid precipitate forms when aqueous solutions of certain ions are mixed AcidBase: proton transfer reactions acid donates a proton to a base,
More information11-1 Notes. Chemical Reactions
11-1 Notes Chemical Reactions Chemical Reactions In a chemical reaction 1 or more substances (the reactants) change into 1 or more new substances (the products). Reactants are always written on the left
More informationReactions in Aqueous Solutions
Copyright 2004 by houghton Mifflin Company. Reactions in Aqueous Solutions Chapter 7 All rights reserved. 1 7.1 Predicting if a Rxn Will Occur When chemicals are mixed and one of these driving forces can
More informationTo determine relative oxidizing and reducing strengths of a series of metals and ions.
Redox Reactions PURPOSE To determine relative oxidizing and reducing strengths of a series of metals and ions. GOALS 1 To explore the relative oxidizing and reducing strengths of different metals. 2 To
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 informationExperiment 6. Investigating Chemical Reactions
In this experiment you will: Experiment 6. Investigating Chemical Reactions Perform and observe the results of a variety of chemical reactions. Become familiar with the observable signs of chemical reactions.
More information9/24/12. Chemistry Second Edition Julia Burdge. Reactions in Aqueous Solutions
Chemistry Second Edition Julia Burdge 4 Reactions in Aqueous Solutions Copyright (c) The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 4 Reactions in Aqueous Solutions
More information(A) Composition (B) Decomposition (C) Single replacement (D) Double replacement: Acid-base (E) Combustion
AP Chemistry - Problem Drill 08: Chemical Reactions No. 1 of 10 1. What type is the following reaction: H 2 CO 3 (aq) + Ca(OH) 2 (aq) CaCO 3 (aq) + 2 H 2 O (l)? (A) Composition (B) Decomposition (C) Single
More informationUnit 1 - Foundations of Chemistry
Unit 1 - Foundations of Chemistry Chapter 2 - Chemical Reactions Unit 1 - Foundations of Chemistry 1 / 42 2.1 - Chemical Equations Physical and Chemical Changes Physical change: A substance changes its
More informationCHEMICAL REACTIONS. The process by which one or more substances are changed into one or more different substances
CHEMICAL REACTIONS The process by which one or more substances are changed into one or more different substances Equations Reactions are represented by a chemical equation Reactants Products Must have
More informationChapter 9. Vocabulary Ch Kick Off Activity. Objectives. Interpreting Formulas. Interpreting Formulas
Chapter 9 Chemical Vocabulary Ch. 9.1 Chemical reaction Reactant Product Word Equation Skeleton Equation Chemical equation Coefficient 1 2 Objectives Write chemical equations to describe chemical reactions
More informationTypes of Reactions. There are five main types of chemical reactions we will talk about:
Chemical Reactions Types of Reactions There are five main types of chemical reactions we will talk about: 1. Synthesis reactions 2. Decomposition reactions 3. Single displacement reactions 4. Double displacement
More informationUnit 4: Reactions and Stoichiometry
Unit 4: Reactions and Stoichiometry Reactions Chemical equation Expression representing a chemical reaction Formulas of reactants on the left side Formulas of products on the right side Arrow(s) connect(s)
More information11. Introduction to Acids, Bases, ph, and Buffers
11. Introduction to Acids, Bases, ph, and Buffers What you will accomplish in this experiment You ll use an acid-base indicating paper to: Determine the acidity or basicity of some common household substances
More informationNCEA Chemistry 2.2 Identify Ions AS 91162
NCEA Chemistry 2.2 Identify Ions AS 91162 What is this NCEA Achievement Standard? When a student achieves a standard, they gain a number of credits. Students must achieve a certain number of credits to
More informationie) HCl (aq) H + (aq) + Cl - (aq) *Like all equations, dissociation equations are written in balanced form
Acids and Bases Acids - substances which dissolve in water to form H + ions in solution ie) HCl (aq) H + (aq) + Cl - (aq) *Like all equations, dissociation equations are written in balanced form a) contain
More information