Electrolytes do conduct electricity, in proportion to the concentrations of their ions in solution.
|
|
- Evan Doyle
- 5 years ago
- Views:
Transcription
1 Chapter 4 (Hill/Petrucci/McCreary/Perry Chemical Reactions in Aqueous Solutions This chapter deals with reactions that occur in aqueous solution these solutions all use water as the solvent. We will look at some properties of these solutions and also look briefly at three different general types of reactions that occur in aqueous solutions. water is such a good solvent for so many ionic and molecular substances that it has been called the universal solvent. (Hill, p.125) Electrical Properties of Aqueous Solutions Nonelectrolytes do not conduct electricity electrical conductance requires the presence of charged particles. Electrolytes do conduct electricity, in proportion to the concentrations of their ions in solution. Strong electrolyte: almost all molecules or neutral units present form ions in aqueous solution HCl(aq) + H 2 O H 3 O + (aq) + Cl 1- (aq) (strong electrolyte) 100% ionized (converted to ions) Weak electrolyte: relatively few molecules or neutral units present form ions in aqueous solution HC 2 H 3 O 2 (l) + H 2 O H 3 O + (aq) + C 2 H 3 O 1-2 (aq) (weak electrolyte) <<100% ionized Carefully read pp in Hill! Molarities of Ions in Strong Electrolytes: to calculate the molarity of an ion in a solution of strong electrolyte, simply multiply the subscript for that ion in the compound by the given molarity of the electrolyte See Example 4.1, Hill, p.129 See Exercise 4.1A, Hill, p.129 Reactions of Acids in Aqueous Solution Recall: an acid is a proton donor in aqueous solution; a base is a proton acceptor in aqueous solution. Strong Acids Are Strong Electrolytes - Six strong acids that you should recognize: HCl hydrochloric acid HNO 3 nitric acid HBr hydrobromic acid H 2 SO 4 sulfuric acid HI hydroiodic acid HClO 4 perchloric acid See also Table 4.1, p. 131, Hill
2 Most of the other acids that you will encounter are weak acids that are weak electrolytes. Ionization of Acids in Aqueous Solution By convention, the chemical formulas for acids have their ionizable protons (H + ions) at the front of the formula. Recall the strong acids: HCl hydrochloric acid 1 ionizable proton HBr hydrobromic acid 1 ionizable proton HI hydroiodic acid 1 ionizable proton HNO 3 nitric acid 1 ionizable proton H 2 SO 4 sulfuric acid 2 ionizable protons HClO 4 perchloric acid 1 ionizable proton Ionization of Acids in Aqueous Solution 0.10 M 0 0 HCl(aq) + H 2 O H 3 O + (aq) + Cl 1- (aq) means 100% 0.0 M 0.10 M 0.10 M 100% ionization in water = strong acid 0.10 M 0 0 HC 2 H 3 O 2 (aq) + H 2 O H 3 O + (aq) + C 2 H 3 O 2 1- (aq) 0.09 M 0.01 M 0.01 M at equilibrium means <<100% ionization in water = weak acid Reactions of Bases in Aqueous Solution Recall: a base is a proton acceptor in aqueous solution. Strong Bases Are Strong Electrolytes Most strong bases are Group IA and Group IIA hydroxides: IA: LiOH, NaOH, KOH, RbOH, CsOH IIA: Mg(OH) 2, Ca(OH) 2, Sr(OH) 2, Ba(OH) 2, See also Table 4.1, p. 131, Hill Ionization of Bases in Aqueous Solution 0.10 M 0 0 NaOH(aq) (+ H 2 O) Na + (aq) + OH 1- (aq) 0.0 M 0.10 M 0.10 M 100% ionization in water = strong base
3 0.10 M 0 0 NH 3 (aq) + H 2 O(l) NH 4 + (aq) + OH 1- (aq) 0.09 M 0.01 M 0.01 M at equilibrium <<100% ionization in water = weak base Most common weak bases: NH 3 and amines Reaction of Acids with Bases: Neutralization neutralization reaction: the reaction of ionizable H + ions on acid molecules with OH 1- or other anions (such as HCO 3 1- or CO 3 2- ) on base molecules Example. We represent an acid-base reaction as a molecular equation. (no ions involved) NaOH(aq) + HCl(aq) H 2 O(l) + NaCl(aq) But, underlying reaction: H + + OH 1- H 2 O(l) Classically, acid-base reactions produce a salt and water. Molecular Equations to Ionic Equations ionic equation: all ionizable species written as ions, i.e. in their ionized or dissociated forms Example. If the molecular equation is NaOH(aq) + HCl(aq) H 2 O(l) + NaCl(aq) we must break up the aqueous ionizable species into their respective ions: NaOH(aq) ionizes to Na + (aq) + OH 1- (aq) HCl(aq) ionizes in water to H 3 O + (aq) + Cl 1- (aq) Molecular Equation: NaOH(aq) + HCl(aq) H 2 O(l) + NaCl(aq) NaOH(aq): Na + (aq) + OH 1- (aq) HCl(aq): H 3 O + (aq) + Cl 1- (aq) NaCl(aq): ionizes to Na + (aq) + Cl 1- (aq) Corresponding Ionic Equation: Na + (aq) + OH 1- (aq) + H 3 O + (aq) + Cl 1- (aq) H 2 O(l) + Na + (aq) + Cl 1- (aq) Species in bold that appear on both sides are called spectator ions and cancel out. These species do not participate in the chemical reaction.
4 Molecular Equations to Ionic Equations Molecular Equation: NaOH(aq) + HCl(aq) H 2 O(l) + NaCl(aq) Ionic Equation: Na + (aq) + OH 1- (aq) + H 3 O + (aq) + Cl 1- (aq) H 2 O(l) + Na + (aq) + Cl 1- (aq) Net Ionic Equation: H 3 O + (aq) + OH 1- (aq) H 2 O(l) See Example 4.2 and following Exercises 4.2A and 4.2B on Hill, p. 133 Acid-Base Reactions That Form Gases 1. Carbonates (compounds that contain CO 3 2- ) CaCO 3 (s) + HCl(aq) H 2 O(l) + CaCl 2 (aq) + CO 2 (g) 2. Sulfites (compounds that contain SO 3 2- ) K 2 SO 3 (s) + H 2 SO 4 (aq) H 2 O(l) + K 2 SO 4 (aq) + SO 2 (g) 3. Sulfides (compounds that contain S 2- ) Na 2 S(aq) + 2 HCl(aq) 2 NaCl(aq) + H 2 S(g) Acid-Base Reactions: Another Example When balancing acid-base equations that have hydroxyl bases, use the lowest common denominator for the number of ionizable protons and the number of OH 1- ions per base unit. Use this number for the number of H 2 O molecules formed. Example. (unbalanced) H 3 PO 4 (aq) + Ca(OH) 2 (aq)??? 2 H 3 PO 4 (aq) + 3 Ca(OH) 2 (aq) 6 H 2 O(l) +?? 2 H 3 PO 4 (aq) + 3 Ca(OH) 2 (aq) 6 H 2 O(l) + Ca 2+ (aq) + PO 4 3- (aq) 2 H 3 PO 4 (aq) + 3 Ca(OH) 2 (aq) 6 H 2 O(l) + Ca 3 (PO 4 ) 2 (aq) Reactions That Form Precipitates precipitate: a solid product formed from the reaction of two soluble ions (a cation and an anion); a precipitate is, by definition, insoluble (not soluble) in the solvent used Example of a Precipitation Reaction: Ba 2+ (aq) + SO 4 2- (aq) BaSO 4 (s) The chemical equation above is the net ionic equation for the reaction between barium chloride and sodium sulfate: BaCl 2 (aq) + Na 2 SO 4 (aq) 2NaCl(aq) + BaSO 4 (s)
5 Can you get from this equation to the net ionic equation? Reaction of Ag+ with I 1- The reaction: AgNO 3 (aq) + KI(aq) AgI(s) + KNO 3 (aq) Net ionic reaction: Ag+(aq) + I 1- (aq) AgI(s) Silver iodide, AgI precipitates! Solubility Rules for Common Ionic Compounds 1.Group IA ions and NH 4 + are almost always SOLUBLE when paired with NO 3 1-, C 2 H 3 O 2 1- and ClO Most salts of Cl 1-, Br 1-, and I 1- are SOLUBLE; exceptions are combinations of these anions with Pb 2+, Ag + or Hg Compounds containing SO 4 2- are SOLUBLE except those with Sr 2+, Ba 2+, Pb 2+, and Hg 2 2+ ; CaSO 4 is slightly soluble. 4. Compounds containing CO 3 2-, OH 1-, PO 4 3- and S 2- are INSOLUBLE except Group IA cations, NH 4 + ; combinations of OH 1- and S 2- with Ca 2+, Sr 2+, Ba 2+ are slightly to moderately soluble. Memorize these solubility rules! See also Table 4.3 on p. 136 (Hill) See Example 4.4 p. 137 Exercise 4.4A, p. 137 (a) MgSO 4 (aq) + KOH(aq)? (b) FeCl 3 (aq) + Na 2 S(aq)? (c) Sr(NO 3 ) 2 (aq) + Na 2 SO 4 (aq)? Oxidation-Reduction Reactions (Redox Reactions) In addition to acid-base and precipitation reactions, there is a third type of reaction: oxidationreduction or redox reactions. Oxidation-reduction reactions are electron exchange reactions (electron = e 1- ) Oxidation - loss of 1 or more electrons by an ion or molecule Reduction - gain of 1 or more electrons by an ion/molecule Example of an Oxidation Reaction. Fe 0 Fe e 1- Example of a Reduction Reaction. Cl e 1-2 Cl 1- Oxidation Numbers and the Oxidation Number Concept oxidation number: the charge on a monatomic ion or the nominal charge on an atom in a unit of a compound (oxidation number is also referred to as the oxidation state of an atom)
6 Short List of Oxidation Number Rules. 1. The oxidation number of a neutral, uncharged atom is 0 2. Ions: IA metals = +1; IIA metals = Hydrogen : H is usually +1; sometimes -1 in hydrides 4. Oxygen: O is usually -2; sometimes -1 in peroxides 5. The sum of all the oxidation numbers in a molecule or an ion is equal to the charge on the molecule (0) or ion. Examples. See Example 4.7, p. 141 (Hill) Exercise 4.7 A, p. 142 Assign known oxidation numbers and then set sum of the oxidation numbers equal to the charge and solve algebraically. Al 2 O 3 P 4 HAsO 4 3- NaMnO 4 Oxidation Numbers in Nitrogen, Sulfur and Chlorine Species (see text Figure 4.12) Identifying Oxidation and Reduction Reactions To classify a reaction as an oxidation process or as a reduction process, first assign oxidation numbers to all atoms on both sides of the equation. 1. Oxidation. If the oxidation number for an element increases (becomes more positive) from reactant to product, the process is an oxidation process 2. Reduction. If the oxidation number for an element decreases (becomes more negative) from reactant to product, the process is a reduction process Identifying Oxidation and Reduction Reactions Example. The thermite reaction: 2 Al(s) + Fe 2 O 3 (s) 2 Fe(l) + Al 2 O 3 (s) Here, Al 0 Al 3+ (oxidation) and Fe 3+ Fe 0 (reduction) We say that Al was oxidized to Al 3+ and that Fe 3+ was reduced to Fe 0 The species oxidized (Al) is the reducing agent, and the species reduced (Fe 3+ ) is the oxidizing agent. Two Other Examples. 4 HCl(aq) + O 2 (g) 2 Cl 2 (aq) + 2 H 2 O(l) Cl 1- in HCl is oxidized to Cl 0 in Cl 2, and O 2 (O 0 ) is reduced to O 2- in H 2 O Ag(s) + H + (aq) + NO 3 1- Ag+(aq) + H 2 O(l) + NO(g) Ag 0 is oxidized to Ag +, and N +5 in NO 3 1- is reduced to N +2 in NO Oxidation-Reduction Reactions (Redox Reactions) See Hill, Figure 4.14, pp. 146: HNO 3 oxidizes Cu to Cu 2+, but HCl doesn t why?
7 Activity Series of the Metals A metal will displace from solution the ions of any metal that lie below it in the activity series. Example. metal = Mg and ion = Ni2+ Mg 0 (s) + Ni 2+ (aq) Mg 2+ (aq) + Ni 0 (s) Read Hill, Section 4.5, pp Figure Maryland uses the Breathalyzer to determine blood alcohol levels of drivers. Cr 2 O ethanol Cr 3+ Titrations We are interested in quantitatively determining the concentration of a chemical species (called the analyte) in a sample. The sample is placed in a flask or beaker, and a solution containing a known concentration of a chemical reagent (the titrant) that will react with the analyte is added until no more analyte remains (the titration endpoint). The chemical reaction between the analyte and the titrant is known. We also know the concentration of the titrant solution and the volume of the solution required to just react with all of the analyte. A titration is carried out using a tube ( a buret) calibrated along its length, typically in 0.1 ml increments. The volume before titrant is measured and recorded; the volume after reaching the endpoint is then measured and recorded. The volume of titrant used is then: V required = V final - V initial Acid-Base Titrations See Examples and Exercises on pp (Hill) Precipitation Titrations See Examples and Exercises on pp (Hill) Redox Titrations See Examples and Exercises on pp (Hill)
Aqueous 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 informationChapter 4. Reactions in Aqueous Solution
Chapter 4. Reactions in Aqueous Solution 4.1 General Properties of Aqueous Solutions A solution is a homogeneous mixture of two or more substances. A solution is made when one substance (the solute) is
More informationChapter 4. The Major Classes of Chemical Reactions 4-1
Chapter 4 The Major Classes of Chemical Reactions 4-1 The Major Classes of Chemical Reactions 4.1 The Role of Water as a Solvent 4.2 Writing Equations for Aqueous Ionic Reactions 4.3 Precipitation Reactions
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 informationSolubility Rules See also Table 4.1 in text and Appendix G in Lab Manual
Ch 4 Chemical Reactions Ionic Theory of Solutions - Ionic substances produce freely moving ions when dissolved in water, and the ions carry electric current. (S. Arrhenius, 1884) - An electrolyte is a
More informationSession 8: LECTURE OUTLINE (SECTIONS I1 I4 pp F61 F67)
Session 8: LECTURE OUTLINE (SECTIONS I1 I4 pp F61 F67) I. Elecrolytes a. Soluble substances b. Insoluble substances c. Electrolytes d. Non-Electrolytes e. Ions and electrical conductivity f. Strong and
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 informationChapter 4: Types of Chemical reactions and Solution Stoichiometry
Chapter 4: Types of Chemical reactions and Solution Stoichiometry 4.1 Water, The Common Solvent State why water acts as a common solvent. Draw the structure of water, including partial charge. Write equations
More informationChapter 4 Suggested end-of-chapter problems with solutions
Chapter 4 Suggested end-of-chapter problems with solutions a. 5.6 g NaHCO 1 mol NaHCO 84.01 g NaHCO = 6.69 10 mol NaHCO M = 6.69 10 mol 50.0 m 1000 m = 0.677 M NaHCO b. 0.1846 g K Cr O 7 1 mol K 94.0 g
More informationChapter 4 Outline. Electrolytic Properties
+4.1 - General Properties of Aqueous Solutions Solution = a homogeneous mixture of two or more substances Solvent = substance present in greatest quantity Solute = the other substance(s) present in a solution
More informationChapter 4. Reactions In Aqueous Solution
Chapter 4 Reactions In Aqueous Solution I) General Properties of Aqueous Solutions Homogeneous mixture on a molecular level - prop. same throughout - separable by physical means - variable composition
More informationChapter 4. Concentration of Solutions. Given the molarity and the volume, the moles of solute can be determined.
Molarity Chapter 4 Concentration of Solutions Molarity (M) = moles of solute liters of solution Given the molarity and the volume, the moles of solute can be determined. Given the molarity and the moles
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 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 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 informationChapter 3 Chemical Reactions
Chapter 3 Chemical Reactions Jeffrey Mack California State University, Sacramento Chemical Reactions Reactants: Zn + I 2 Product: ZnI 2 Chemical Reactions Evidence of a chemical reaction: Gas Evolution
More informationAP Chemistry. Chapter 4
AP Chemistry Chapter 4 1 Properties of Aqueous Solution Solutions Definition: Any substance (solid, liquid or gas) EVENLY distributed throughout another substance. Solutions have 2 parts: 1) Solvent the
More informationChapter 4. Properties of Aqueous Solutions. Electrolytes in Aqueous Solutions. Strong, weak, or nonelectrolyte. Electrolytic Properties
Chapter 4 Reactions in Aqueous Solution Observing and Predicting Reactions How do we know whether a reaction occurs? What observations indicate a reaction has occurred? In your groups, make a list of changes
More informationChemistry deals with matter and its changes CHEMICAL REACTIONS
Chemistry deals with matter and its changes CHEMICAL REACTIONS CHEMICAL EQUATIONS N 2 + 3 H 2 2 NH 3 2 N 6 H 2 N 6 H reactants products balanced means equal numbers of atoms of each element on each side
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 informationCHEM134- Fall 2018 Dr. Al-Qaisi Chapter 4b: Chemical Quantities and Aqueous Rxns So far we ve used grams (mass), In lab: What about using volume in lab? Solution Concentration and Solution Stoichiometry
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 informationChapter 4. Aqueous Reactions and Solution Stoichiometry
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 dissolved in another (the solvent). The
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 informationPage 1. Exam 2 Review Summer A 2002 MULTIPLE CHOICE. 1. Consider the following reaction: CaCO (s) + HCl(aq) CaCl (aq) + CO (g) + H O(l)
Page 1 MULTIPLE CHOICE 1. Consider the following reaction: CaCO (s) + HCl(aq) CaCl (aq) + CO (g) + H O(l) The coefficient of HCl(aq) in the balanced reaction is. a) 1 b) 2 c) 3 d) 4 e) 0 2. Given the information
More informationSolution Chemistry. Chapter 4
Solution Chemistry Chapter 4 Covalent Molecule Dissolving in Water Ionic Compound Dissolving in Water Electrolytes and Nonelectrolytes Electrolytes/Nonelectrolytes Type Dissociation Electrical Conductivity
More informationChapter 4 - Types of Chemical Reactions and Solution Chemistry
Chapter 4 - Types of Chemical Reactions and Solution Chemistry 4.1 Water, the Common Solvent - the water molecule is bent with and H-O-H angles of approx. 105 º - O-H bonds are covalent - O is slightly
More informationChapter 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 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 informationChem 110 General Principles of Chemistry
Chem 110 General Principles of Chemistry Chapter 3 (Page 88) Aqueous Reactions and Solution Stoichiometry In this chapter you will study chemical reactions that take place between substances that are dissolved
More informationChapter 4. Reactions in Aqueous Solution. Solutions. 4.1 General Properties of Aqueous Solutions
Chapter 4 in Solution 4.1 General Properties of Solutions Solutions Solutions are defined as homogeneous mixtures of two or more pure substances. The solvent is present in greatest abundance. All other
More informationChapter 4. Reactions in Aqueous Solution. Lecture Presentation. John D. Bookstaver St. Charles Community College Cottleville, MO
Lecture Presentation Chapter 4 in Solution 2012 Pearson Education, Inc. John D. Bookstaver St. Charles Community College Cottleville, MO Properties of Solutions Solute: substance in lesser quantity in
More informationed. Brad Collins Aqueous Chemistry Chapter 5 Some images copyright The McGraw-Hill Companies, Inc. Sunday, August 18, 13
ed. Brad Collins Aqueous Chemistry Chapter 5 Some images copyright The McGraw-Hill Companies, Inc. A solution is a homogenous mixture of 2 or more substances at the molecular level The solute(s) is(are)
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 informationSolubility Rules for Ionic Compounds Arrhenius Acid Base Theory
Chapter 4 Reactions in Aqueous Solutions Ionic compounds dissociate in water yielding electrolyte solutions. H 2 O NaCl(s) Na + (aq) + Cl - (aq) The ions are hydrated by water. Strong & Weak Electrolytes
More informationChapter 4 Reactions in Aqueous Solutions
Chapter 4 Reactions in Aqueous Solutions Ionic compounds dissociate in water yielding electrolyte solutions. H 2 O NaCl(s) Na + (aq) + Cl - (aq) The ions are hydrated by water. The Electrical Conductivity
More informationCHEM 200/202. Professor Jing Gu Office: EIS-210. All s are to be sent to:
CHEM 200/202 Professor Jing Gu Office: EIS-210 All emails are to be sent to: chem200@mail.sdsu.edu My office hours will be held in GMCS-212 on Monday from 9 am to 11 am or by appointment. ANNOUNCEMENTS
More informationChemical reactions describe processes involving chemical change
1.1 Chemical Reactions 1.2 Chemical Equations Chemical reactions describe processes involving chemical change The chemical change involves rearranging matter Converting one or more pure substances into
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 informationChapter 7 Chemical Reactions
Chapter 7 Chemical Reactions Evidence of Chemical Change Release or Absorption of Heat Color Change Emission of Light Formation of a Gas Formation of Solid Precipitate Tro's "Introductory 2 How Do We Represent
More informationI. Properties of Aqueous Solutions A) Electrolytes and Non-Electrolytes B) Predicting Solubility* II. Reactions of Ionic Compounds in Solution*
Chapter 5 Reactions in Aqueous Solutions Titrations Kick Acid!!! 1 I. Properties of Aqueous Solutions A) Electrolytes and Non-Electrolytes B) Predicting Solubility* II. Reactions of Ionic Compounds in
More informationChapter 4: Phenomena. Electrolytes. Electrolytes. Electrolytes. Chapter 4 Types of Chemical Reactions and Solution Stoichiometry.
Chapter 4: Phenomena Phenomena: Many different reactions are known to occur. Scientists wondered if these reactions could be separated into groups based on their properties. Look at the reactions below
More informationChapter 4: Phenomena. Electrolytes. Electrolytes. Electrolytes. Chapter 4 Types of Chemical Reactions and Solution Stoichiometry
Chapter 4: Phenomena Phenomena: Many different reactions are known to occur. Scientists wondered if these reactions could be separated into groups based on their properties. Look at the reactions below
More informationChapter 4: Phenomena. (aq)+ 4H + (aq)+ 2e - Chapter 4: Types of Chemical Reactions and Solution Stoichiometry
Chapter 4: Phenomena Phenomena: Many different reactions are known to occur. Scientists wondered if these reactions could be separated into groups based on their properties. Look at the reactions below
More informationChap. 4 AQUEOUS RXNS. O H δ+ 4.1 WATER AS A SOLVENT 4.2 AQUEOUS IONIC REACTIONS. Page 4-1. NaOH(aq) + HCl(g) NaCl(aq) +H 2 O
Chap. AQUEOUS RXNS.1 WATER AS A SOLVENT Describe solution composition in terms of molarity Describe strong and weak electrolyte solutions, including acids and bases Use ionic equations to describe neutralization
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 informationChapter 4 Electrolytes Acid-Base (Neutralization) Oxidation-Reduction (Redox) Reactions. Dr. Sapna Gupta
Chapter 4 Electrolytes Acid-Base (Neutralization) Oxidation-Reduction (Redox) Reactions Dr. Sapna Gupta Types of Reactions Two classifications: one how atoms are rearrangement and the other is chemical
More informationCHAPTER 4 AQUEOUS REACTIONS AND SOLUTION STOICHIOMETRY: Electrolyte-a compound that conducts electricity in the melt or in solution (water)
CHAPTER 4 AQUEOUS REACTIONS AND SOLUTION STOICHIOMETRY: Electrolyte-a compound that conducts electricity in the melt or in solution (water) STRONG ELEC. 100% Dissoc. WEAK ELEC..1-10% Dissoc. NON ELEC 0%
More 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 informationSection 4: Aqueous Reactions
Section 4: Aqueous Reactions 1. Solution composition 2. Electrolytes and nonelectrolytes 3. Acids, bases, and salts 4. Neutralization ti reactions 5. Precipitation reactions 6. Oxidation/reduction reactions
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 informationCompounds in Aqueous Solution
1 Compounds in Aqueous Solution Many reactions involve ionic compounds, especially reactions in water KMnO 4 in water K + (aq) ) + MnO 4- (aq) 2 CCR, page 149 3 How do we know ions are present in aqueous
More informationAnnouncements. There are 3-classes of chemical reactions that occur in aqueous solution.
Announcements Exam 1 Results: Mean: 71% Range: 39.5%-93.5% Median: 72% Other Bio-LS Class Mean 72% Please read Chapter 4 and complete problems. Please see me for help. There are 3-classes of chemical reactions
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 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 informationReactions in Aqueous Solutions
Reactions in Aqueous Solutions Chapter 4 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. A solution is a homogenous mixture of 2 or more substances. The solute
More informationChapter 4: Chemical Reactions in Aqueous Solutions. 4.1 Some Electronic Properties of Aqueous Solutions
Chapter : Chemical Reactions in Aqueous Solutions Water: the universal solvent ¾ of Earth s surface water in living organisms Some Electrical Properties of Aqueous Solutions Reactions of Acids and Bases
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 informationNet Ionic Reactions. The reaction between strong acids and strong bases is one example:
Net Ionic Reactions Model 1 Net Ionic Reactions. Net ionic reactions are frequently used when strong electrolytes react in solution to form nonelectrolytes or weak electrolytes. These equations let you
More informationChapter 5 Classification and Balancing of Chemical Reactions
Chapter 5 Classification and Balancing of Chemical Reactions 5.1 Chemical Equations Chemical equations describe chemical reactions. - As words: hydrogen plus oxygen combine to form water - As a chemical
More informationCH 221 Chapter Four Part II Concept Guide
CH 221 Chapter Four Part II Concept Guide 1. Solubility Why are some compounds soluble and others insoluble? In solid potassium permanganate, KMnO 4, the potassium ions, which have a charge of +1, are
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 information**The partially (-) oxygen pulls apart and surrounds the (+) cation. The partially (+) hydrogen pulls apart and surrounds the (-) anion.
#19 Notes Unit 3: Reactions in Solutions Ch. Reactions in Solutions I. Solvation -the act of dissolving (solute (salt) dissolves in the solvent (water)) Hydration: dissolving in water, the universal solvent.
More information9.1.2 AQUEOUS SOLUTIONS AND CHEMICAL REACTIONS
9.1.2 AQUEOUS SOLUTIONS AND CHEMICAL REACTIONS Work directly from Zumdahl (Chapter 4). Work through exercises as required, then summarise the essentials of the section when complete. To understand the
More informationGeneral Chemistry. Contents. Chapter 5: Introduction to Reactions in Aqueous Solutions. Electrolytes. 5.1 The Nature of Aqueous Solutions
General Chemistry Principles and Modern Applications Petrucci Harwood Herring 8 th Edition Chapter 5: Introduction to Reactions in Aqueous Solutions Philip Dutton University of Windsor, Canada N9B 3P4
More informationChapter 7: Chemical Reactions
C h a p t e r 7, C h a p t e r 1 6 ( 2-5 ) : C h e m i c a l R e a c t i o n s P a g e 1 Chapter 7: Chemical Reactions Read Chapter 7 and Check MasteringChemistry due dates. Evidence of Chemical Reactions:
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 informationChemical Reactions: An Introduction
Chemical Reactions: An Introduction Ions in Aqueous Solution Ionic Theory of Solutions Many ionic compounds dissociate into independent ions when dissolved in water H 2O NaCl(s) Na Cl These compounds that
More informationChapter 5 Chemical Reactions
Aqueous Solubility of Ionic Compounds John W. Moore Conrad L. Stanitski Peter C. Jurs Not all compounds dissolve in water. Solubility varies from compound to compound. http://academic.cengage.com/chemistry/moore
More informationGeneral Chemistry. Chapter 5: Introduction to Reactions in Aqueous Solutions. Principles and Modern Applications Petrucci Harwood Herring 8 th Edition
General Chemistry Principles and Modern Applications Petrucci Harwood Herring 8 th Edition Chapter 5: Introduction to Reactions in Aqueous Solutions Philip Dutton University of Windsor, Canada N9B 3P4
More informationChapter 3 & 4: Reactions Part 1
Chapter 3 & 4: Reactions Part 1 Read: BLB 3.1 3.2; 4.2 4.4 HW: BLB 3:1, 11a, b, e, 13 4:19, 24, 39, 49a, c, e, f, 51b, d Supplemental: Rxns:1, 2, 6 11 Know: Chapter 3 Reactions Combustion Decomposition
More informationAP Chemistry Note Outline Chapter 4: Reactions and Reaction Stoichiometry:
AP Chemistry Note Outline Chapter 4: Reactions and Reaction Stoichiometry: Water as a solvent Strong and Weak Electrolytes Solution Concentrations How to Make up a solution Types of Reactions Introduction
More informationChem 30A. Ch 7. Chemical Reactions
Chem 30A Ch 7. Chemical Reactions Chemical Equations Chemical Reactions Chemical reac+on: a process that involves the rearrangement of the ways atoms are grouped together Evidence for Chemical Reactions
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 informationSCHOOL YEAR CH- 13 IONS IN AQUEOUS SOLUTIONS AND COLLIGATIVE PROPERTIES SUBJECT: CHEMISTRY GRADE : 11 TEST A
SCHOOL YEAR 2017-18 NAME: CH- 13 IONS IN AQUEOUS SOLUTIONS AND COLLIGATIVE PROPERTIES SUBJECT: CHEMISTRY GRADE : 11 TEST A Choose the best answer from the options that follow each question. 1. A solute
More informationThe Major Classes of Chemical Reactions
Chapter 4 The Major Classes of Chemical Reactions 5.1 Properties of compounds in Aqueous Solution 5.2 Precipitation Reaction 5.3 Acids and Bases 5.4 Reactions of Acid and Bases 5.5 Gas-forming Reactions
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 informationReactions in aqueous solutions Precipitation Reactions
Reactions in aqueous solutions Precipitation Reactions Aqueous solutions Chemical reactions that occur in water are responsible for creation of cenotes. When carbon dioxide, CO2, dissolves in water, the
More informationCH 4 AP. Reactions in Aqueous Solutions
CH 4 AP Reactions in Aqueous Solutions Water Aqueous means dissolved in H 2 O Moderates the Earth s temperature because of high specific heat H-bonds cause strong cohesive and adhesive properties Polar,
More information2. The reaction of carbon monoxide and diiodine pentoxide as represented by the equation
1. The complete combustion of phenylhydrazine, C 6 H 5 NHNH 2, with the oxidizer dinitrogen tetraoxide is shown in the equation C 6 H 5 NHNH 2 + N 2 O 4 CO 2 + H 2 O + N 2 When balanced, the sum of all
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 information3.1 Chemical Equations. 3: Chemical Reactions. Chemical Equations. Chemical Equations. Chemical Equations. Types of Chemical Reactions.
3: Chemical Reactions 1. Chemical Equations 2. Types of Chemical Equations 3. Balancing Chemical Equation 4. Aqueous Reactions 4. Acid-Base Reactions 6. Redox Reactions 3.1 Chemical Equations How Do Chemists
More informationChapter 10. Acids, Bases, and Salts
Chapter 10 Acids, Bases, and Salts Topics we ll be looking at in this chapter Arrhenius theory of acids and bases Bronsted-Lowry acid-base theory Mono-, di- and tri-protic acids Strengths of acids and
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 informationAcids and Bases Unit 11
Mr. B s Chemistry Acids and Bases Unit 11 Name Block Let s start our discussion of acids and bases by defining some terms that are essential to the topics that follow. Arrhenius acids and bases are: acid
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 informationChapter 8 Chemical Reactions
Chemistry/ PEP Name: Date: Chapter 8 Chemical Reactions Chapter 8: 1 7, 9 18, 20, 21, 24 26, 29 31, 46, 55, 69 Practice Problems 1. Write a skeleton equation for each chemical reaction. Include the appropriate
More informationCHAPTER 4 TYPES OF CHEMICAL REACTIONS & SOLUTION STOICHIOMETRY
Advanced Chemistry Name Hour Advanced Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 4 TYPES OF CHEMICAL REACTIONS & SOLUTION STOICHIOMETRY Day Plans
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 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 informationArrhenius Acid-Base Concept Svante Arrhenius, 1884
Arrhenius Acid-Base Concept Svante Arrhenius, 1884 O Acids and bases are electrolytes. O Acids are substances that produce hydrogen ion, H + (aq), in solution. O Bases are substances that produce hydroxide
More informationChapter 4. Chemical Quantities and Aqueous Reactions
Lecture Presentation Chapter 4 Chemical Quantities and Aqueous Reactions Reaction Stoichiometry: How Much Carbon Dioxide? The balanced chemical equations for fossilfuel combustion reactions provide the
More informationChemistry 101 Chapter 4 STOICHIOMETRY
STOICHIOMETRY Stoichiometry is the quantitative relationship between the reactants and products in a balanced chemical equation. Stoichiometry allows chemists to predict how much of a reactant is necessary
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 informationPractice questions for Chapter 4
Practice questions for Chapter 4 1. An unknown substance dissolves readily in water but not in benzene (a nonpolar solvent). Molecules of what type are present in the substance? A) neither polar nor nonpolar
More informationCHEM 200/202. Professor Jing Gu Office: EIS-210. All s are to be sent to:
CHEM 200/202 Professor Jing Gu Office: EIS-210 All emails are to be sent to: chem200@mail.sdsu.edu My office hours will be held in GMCS-212 on Monday from 9 am to 11 am or by appointment. ANNOUNCEMENTS
More informationPart One: Ions in Aqueous Solution
A. Electrolytes and Non-electrolytes. CHAPTER FOUR: CHEMICAL REACTIONS Part One: Ions in Aqueous Solution 1. Pure water does not conduct electric current appreciably. It is the ions dissolved in the water
More informationChapter 4; Reactions in Aqueous Solutions. Chapter 4; Reactions in Aqueous Solutions. V. Molarity VI. Acid-Base Titrations VII. Dilution of Solutions
Chapter 4; Reactions in Aqueous Solutions I. Electrolytes vs. NonElectrolytes II. Precipitation Reaction a) Solubility Rules III. Reactions of Acids a) Neutralization b) Acid and Carbonate c) Acid and
More informationOctober 19, 1999 Page 1. Chapter 4 Practice Worksheet Dr. Palmer Graves, Instructor MULTIPLE CHOICE
October 19, 1999 Page 1 MULTIPLE CHOICE Section 4.1 Some Ways that Chemical Reactions Occur 1. The reaction of HNO (aq) + KOH(aq) KNO (aq) + H O(l) is best classified as a(n) a) acid-base neutralization
More informationHomework #3 Chapter 4 Types of Chemical Reactions and Solution Stoichiometry
Homework #3 Chapter 4 Types of Chemical Reactions and Solution Stoichiometry 13. Determine the concentrations of the solutions Solution A 4 particles 1.0 L Solution B 6 paticles 4.0 L Solution C 4 particles
More information