Page III-4b-1 / Chapter Four Part II Lecture Notes. Chemistry 221 Professor Michael Russell MAR. Ba(NO3)2(aq)? soluble. BaCl2(aq)?
|
|
- Garry Williamson
- 5 years ago
- Views:
Transcription
1 Page III-4b-1 / Chapter Four Part II Lecture Notes Solution Stoichiometry and Chemical Reactions Chapter 3 & Chapter 4, or Chapter 4 Part II Chemistry 221 Professor Michael Russell Terminology In solution we need to define the - SOLVENT the component whose physical state is preserved when solution forms SOLUTE the other solution component Compounds are soluble when they dissolve, insoluble when they stay as solids Water Solubility of Ionic Compounds If one ion from the Soluble Compd. list is present in a compound, the compound is water soluble. Ba(NO3)2(aq)? soluble BaCl2(aq)? soluble BaSO4(aq)? insoluble should write BaSO4(s)! Use this solubility guide in CH ! WATER SOLUBILITY OF IONIC COMPOUNDS Not all ionic compounds dissolve in water. Some are INSOLUBLE. Many ions, however, make compounds SOLUBLE all of the time. Examples: Na +, K +, Li +, NH 4 +, NO 3 -, ClO 3 -, ClO 4 -, CH 3 CO 2 -, and most SO 4 2-, Cl -, Br - and I - compounds. IONIC COMPOUNDS Compounds in Aqueous Solution Many reactions involve soluble ionic compounds, especially reactions in water - aqueous solutions. KMnO 4 in water K + (aq) + MnO 4 -(aq) Aqueous Solutions How do we know ions are present in aqueous solutions? The solutions conduct electricity! They are called ELECTROLYTES HCl, KMnO 4, MgCl 2, and NaCl are strong electrolytes. They dissociate completely (or nearly so) into ions. KMnO 4 (aq) ---> K + (aq) + MnO 4 -(aq) Page III-4b-1 / Chapter Four Part II Lecture Notes
2 Page III-4b-2 / Chapter Four Part II Lecture Notes Aqueous Solutions HCl, MgCl 2, and NaCl are strong electrolytes. They dissociate completely (or nearly so) into ions. Aqueous Solutions Acetic acid ionizes only to a small extent, so it is a weak electrolyte CH 3 CO 2 H(aq) ---> CH 3 CO 2 -(aq) + H + (aq) Aqueous Solutions Some compounds (sugar, ethanol, acetone, etc.) dissolve in water but do not conduct electricity. They are called nonelectrolytes. ACIDS Some strong acids include: HCl hydrochloric HNO 3 nitric HClO 4 perchloric H 2 SO 4 sulfuric An acid > H + in water See "Dissolve, Dissociate and Electrolyte" Guide All strong acids are strong electrolytes The Nature of Acids HCl Cl - Weak Acids All weak acids are weak electrolytes CH 3 CO 2 H acetic acid H 2 CO 3 carbonic acid H 3 PO 4 phosphoric acid H 2 O H 3 O + hydronium ion Acetic acid Page III-4b-2 / Chapter Four Part II Lecture Notes
3 Page III-4b-3 / Chapter Four Part II Lecture Notes BASES Base ---> OH - in water Ammonia, NH 3 An Important Base Bases are often metal hydroxides NaOH(aq) ---> Na + (aq) + OH - (aq) NaOH is a strong base All strong bases are strong electrolytes All weak bases are weak electrolytes Common Acids and Bases Net Ionic Equations Mg(s) + 2 HCl(aq) --> H 2 (g) + MgCl 2 (aq) Know the strong acids & bases! We really should write: Mg(s) + 2 H + (aq) + 2 Cl - (aq) ---> H 2 (g) + Mg 2+ (aq) + 2 Cl - (aq) Net Ionic Equations Mg(s) + 2 HCl(aq) H 2 (g) + MgCl 2 (aq) Aqueous solutes (HCl, MgCl2) dissociate; we really should write: Mg(s) + 2 H + (aq) + 2 Cl - (aq) H 2 (g) + Mg 2+ (aq) + 2 Cl - (aq) We leave the spectator ions (Cl - ) out in writing the NET IONIC EQUATION: Mg(s) + 2 H + (aq) H 2 (g) + Mg 2+ (aq) See Net Ionic Reactions Handout Net Ionic Equations K 2 CrO 4 (aq) + Pb(NO 3 ) 2 (aq) --> PbCrO 4 (s) + 2 KNO 3 (aq) NET IONIC EQUATION Pb 2+ (aq) + CrO 4 2-(aq) ---> PbCrO 4 (s) K + and NO 3 - are spectators See Net Ionic Reactions Handout Page III-4b-3 / Chapter Four Part II Lecture Notes
4 Page III-4b-4 / Chapter Four Part II Lecture Notes CHEMICAL REACTIONS IN WATER We will look at EXCHANGE REACTIONS AX + BY The "driving force" is the formation of an insoluble compound - a precipitate. Fe(NO3)3(aq) + 3 NaOH(aq) -----> 3 NaNO3(aq) + Fe(OH)3(s) AY + BX The anions exchange places between cations Precipitation Reactions Pb(NO3)2(aq) + 2 KI(aq) ----> PbI2(s) + 2 KNO3(aq) Exchange reactions often called Double Displacement Reactions Net ionic equation Fe3+(aq) + 3 OH-(aq) ---> Fe(OH)3(s) See "Five Types of Reactions" Handout Acid-Base Reactions Acids react readily with bases. The "driving force" is the formation of water. NaOH(aq) + HCl(aq) ---> NaCl(aq) + H2O(liq) Net ionic equation: OH-(aq) + H+(aq) ---> H2O(liq) This applies to ALL reactions of STRONG acids and bases. Acid-base reactions often called "neutralizations", water and "salt" created See "Five Types of Reactions" Handout Gas-Forming Reactions CaCO3(s) + 2 HCl(aq) ---> CaCl2(aq) + H2CO3(aq) Carbonic acid is unstable and forms CO2 & H2O H2CO3(aq) ---> CO2(g) + water Another gas forming species: NH4OH(aq) ---> NH3(g) + water See "Five Types of Reactions" Handout Oxidation-Reduction Reactions Combustion Reactions REDOX = reduction & oxidation 2 H2(g) + O2(g) ---> 2 H2O(liq) A special example of a gas-forming reaction Used in quantitative chemistry; high temperatures Reactants: oxygen (O2) and "something organic" (C, H, sometimes O or N) Products: water and carbon dioxide (also NO2 if N present) Examples: C2H4(g) + 3 O2(g) 2 H2O(g) + 2 CO2(g) 4 C6H5NO O2(g) 10 H2O(g) + 24 CO2(g) + 4 NO2(g) See "Five Types of Reactions" Handout See "Five Types of Reactions" Handout Page III-4b-4 / Chapter Four Part II Lecture Notes
5 Page III-4b-5 / Chapter Four Part II Lecture Notes LEO says GER LEO says GER Lose Electrons Oxidized Zn(s) Zn e- Cu e- Cu(s) Gain Electrons Reduced Oxidized Reduced Can also use "OIL RIG": OIL = "Oxidation is Losing" (electrons) RIG = "Reduction is Gaining" (electrons) REDOX REACTIONS In all reactions: if something has been oxidized then something has also been reduced: Cu(s) + 2 Ag + (aq) Cu 2+ (aq) + 2 Ag(s) Redox reactions incredibly useful (fuels, batteries, much more) Oxidation numbers help visualize electron transfer pathways Use oxidation number rules to determine redox activity: Atoms in free element have ox. no. = 0 Zn(s), O 2 (g), Br 2 (liq) In simple ions, ox. no. = charge on ion -1 for Cl -, +2 for Mg 2+ O is -2 (except peroxides (O = -1) and with F) H is +1 (except hydrides (H = -1)) Sum of oxidation numbers = 0 for a compound or equals the overall charge for an ion OXIDATION NUMBERS OXIDATION NUMBERS Determining oxidation numbers takes practice Recognizing a Redox Reaction 2 Al(s) + 3 Cu 2+ (aq) ---> 2 Al 3+ (aq) + 3 Cu(s) Al(s) --> Al 3+ (aq) + 3 e - Ox. no. of Al increases as e - are donated by the metal; Al is OXIDIZED (or the REDUCING AGENT) HF H: +1 F: -1 ClO 4 - Cl: +7 O: -2 Cu 2+ (aq) + 2 e - --> Cu(s) Page III-4b-5 / Chapter Four Part II Lecture Notes Ox. no. of Cu decreases as e - are accepted by the ion; Cu is REDUCED (or the OXIDIZING AGENT)
6 Page III-4b-6 / Chapter Four Part II Lecture Notes Agents of Redox! Examples of Redox Reactions NO = reducing agent O 2 = oxidizing agent 2 NO + O 2 2 NO 2 Fe = reducing agent Cl 2 = oxidizing agent 2 Fe + 3 Cl 2 2 FeCl 3 Reduced = Oxidizing Agent Oxidized = Reducing Agent reducing agent = oxidized oxidizing agent = reduced Concentration of Solute The amount of solute in a solution is given by its concentration. PROBLEM: Dissolve 5.00 g of NiCl 2 6 H 2 O in enough water to make 250. ml of solution. Calculate molarity. Molarity (M) = moles solute liters of solution Concentration (M) = [ ] PROBLEM: Dissolve 5.00 g of NiCl 2 6 H 2 O in enough water to make 250. ml of solution. Calculate molarity. Step 1: Calculate moles of NiCl 2 6H 2 O 5.00 g 1 mol g mol L = mol Step 2: Calculate molarity = M [NiCl 2 6 H 2 O] = M The Nature of a CuCl 2 Solution Ion Concentrations CuCl 2 (aq) --> Cu 2+ (aq) + 2 Cl - (aq) If [CuCl 2 ] = 0.30 M, then [Cu 2+ ] = 0.30 M [Cl - ] = 2 x 0.30 M = 0.60 M Page III-4b-6 / Chapter Four Part II Lecture Notes
7 Page III-4b-7 / Chapter Four Part II Lecture Notes USING MOLARITY What mass of oxalic acid, H 2 C 2 O 4, is required to make 250. ml of a M solution? moles = M V Step 1: Calculate moles of acid required. ( mol/l)(0.250 L) = mol Step 2: Calculate mass of acid required. ( mol )(90.00 g/mol) = 1.13 g Preparing Solutions Weigh out a solid solute and dissolve in a given quantity of solvent or Dilute a concentrated solution to give one that is less concentrated. You have 50.0 ml of 3.0 M NaOH and you want 0.50 M NaOH. What do you do? You have 50.0 ml of 3.0 M NaOH and you want 0.50 M NaOH. What do you do? H2O But how Add much water! water do Dilute we add? the solution! How much water should be added? The important point: moles of NaOH in ORIGINAL solution = moles of NaOH in FINAL solution 3.0 M NaOH 0.50 M NaOH Concentrated Dilute You have 50.0 ml of 3.0 M NaOH and you want 0.50 M NaOH. What do you do? You have 50.0 ml of 3.0 M NaOH and you want 0.50 M NaOH. What do you do? Moles of NaOH in original solution = M * V = (3.0 mol/l)(0.050 L) = 0.15 mol NaOH Therefore, moles of NaOH in final solution must also = 0.15 mol NaOH (0.15 mol NaOH)(1 L/0.50 mol) = 0.30 L or 300 ml = volume of final solution Conclusion: H2O add 250 ml 3.0 M NaOH 0.50 M NaOH of water to 50.0 ml of 3.0 M NaOH to make 300 ml of 0.50 M NaOH. Concentrated Page III-4b-7 / Chapter Four Part II Lecture Notes Dilute
8 Page III-4b-8 / Chapter Four Part II Lecture Notes Preparing Solutions by Dilution A shortcut SOLUTION STOICHIOMETRY Zinc reacts with acids to produce H 2 gas. What volume of 2.50 M HCl is needed to convert 10.0 g of Zn? M initial * V initial = M final * V final Often abbreviated: MiVi = MfVf Zn(s) + 2 HCl(aq) --> ZnCl 2 (aq) + H 2 (g) Step 2: Use the stoichiometric factor 2 mol HCl mol Zn = mol HCl 1 mol Zn Step 3: Calculate volume of HCl required 1.00 L mol HCl = L HCl 2.50 mol Zinc reacts with acids to produce H 2 gas. What volume of 2.50 M HCl is needed to convert 10.0 g of Zn? Step 1: Calculate moles of Zn 10.0 g Zn 1.00 mol Zn g Zn = mol Zn Zn(s) + 2 HCl(aq) --> ZnCl 2 (aq) + H 2 (g) ACID-BASE REACTIONS Titrations H 2 C 2 O 4 (aq) + 2 NaOH(aq) ---> acid base Na 2 C 2 O 4 (aq) + 2 H 2 O(liq) Carry out this reaction using a TITRATION. Oxalic acid, H 2 C 2 O 4 Setup for titrating an acid with a base Setup for Titrating an acid with a base LAB PROBLEM #1: Standardize a solution of NaOH - i.e., accurately determine its concentration g of H 2 C 2 O 4 (oxalic acid) requires ml of NaOH for titration to an equivalence point. What is the concentration of the NaOH? Page III-4b-8 / Chapter Four Part II Lecture Notes H 2 C 2 O 4 (aq) + 2 NaOH(aq) ---> Na 2 C 2 O 4 (aq) + 2 H 2 O(liq)
9 Page III-4b-9 / Chapter Four Part II Lecture Notes g of H 2 C 2 O 4 (oxalic acid) requires ml of NaOH for titration to an equivalence point. What is the concentration of the NaOH? g of H 2 C 2 O 4 (oxalic acid) requires ml of NaOH for titration to an equivalence point. What is the concentration of the NaOH? Step 1: Calculate moles of H 2 C 2 O g * mol acid 1 mol g 2 mol NaOH 1 mol acid = mol Step 2: Calculate moles of NaOH req d = mol NaOH H 2 C 2 O 4 (aq) + 2 NaOH(aq) ---> Na 2 C 2 O 4 (aq) + 2 H 2 O(liq) Step 1: Calculate moles of H 2 C 2 O 4 = mol acid Step 2: Calculate moles of NaOH req'd = mol NaOH Step 3: Calculate concentration of NaOH mol NaOH L [NaOH] = M = M H 2 C 2 O 4 (aq) + 2 NaOH(aq) ---> Na 2 C 2 O 4 (aq) + 2 H 2 O(liq) LAB PROBLEM #2: Use standardized NaOH to determine the amount of an acid in an unknown. Apples contain malic acid, C 4 H 6 O 5. C 4 H 6 O 5 (aq) + 2 NaOH(aq) ---> Na 2 C 4 H 4 O 5 (aq) + 2 H 2 O(liq) g of apple requires ml of M NaOH for titration. What is weight % of malic acid? g of apple requires ml of M NaOH for titration. What is weight % of malic acid? Step 1: Calculate moles of NaOH used. M * V = ( M)( L) = mol NaOH Step 2: Calculate moles of acid titrated mol NaOH = mol acid 1 mol acid 2 mol NaOH C 4 H 6 O 5 (aq) + 2 NaOH(aq) ---> Na 2 C 4 H 4 O 5 (aq) + 2 H 2 O(liq) g of apple requires ml of M NaOH for titration. What is weight % of malic acid? Step 1: moles of NaOH = Step 2: moles of acid titrated = Step 3: Calculate mass of acid titrated. ph, a Concentration Scale ph: a way to express acidity -- the concentration of H + in solution mol acid g mol = g Step 4: Calculate % malic acid. (1.539 g acid / g apple) *100 = % C 4 H 6 O 5 (aq) + 2 NaOH(aq) ---> Na 2 C 4 H 4 O 5 (aq) + 2 H 2 O(liq) Low ph: high [H + ] High ph: low [H + ] Page III-4b-9 / Chapter Four Part II Lecture Notes Acidic solution ph < 7 Neutral ph = 7 Basic solution ph > 7
10 Page III-4b-10 / Chapter Four Part II Lecture Notes The ph Scale [H+] and ph ph = - log [H+] If the [H+] of soda is 1.6 x 10-3 M, the ph is? In a neutral solution, [H+] = [OH-] = 1.00 x 10-7 M at 25 oc Because ph = - log [H+] then ph = - log [H+] = -log (1.00 x 10-7) ph= - log (1.6 x 10-3) = - (-7) = 7 ph = - (-2.80) ph = 2.80 Søren Sørensen, creator of the ph scale ph and [H+] End of Chapter Four Part 2 If the ph of Coke is 3.12, it is. See also: Chapter Four Part 2 Study Guide Chapter Four Part 2 Concept Guide Because ph = - log [H+] then log [H+] = - ph Take antilog and get [H+] = 10-pH [H+] = [H+] = 7.6 x 10-4 M more on acids, bases and ph in CH 223 Page III-4b-10 / Chapter Four Part II Lecture Notes
Compounds 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 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 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 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 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 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 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 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 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 informationThe solvent is the dissolving agent -- i.e., the most abundant component of the solution
SOLUTIONS Definitions A solution is a system in which one or more substances are homogeneously mixed or dissolved in another substance homogeneous mixture -- uniform appearance -- similar properties throughout
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 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 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 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 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. 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 informationPrecipitation Reactions
Precipitation Reactions Precipitation Reactions Precipitation reactions are reactions in which a solid forms when we mix two solutions. 1) reactions between aqueous solutions of ionic compounds 2) produce
More informationChapter 4 Three Major Classes of Chemical Reactions
Chapter 4 Three Major Classes of Chemical Reactions Solution Stoichiometry Many reactions (biochemical, marine, etc.) take place in solution. We need to be able to express the number of moles of particles
More informationConcentration of Solutions
Solutions We carry out many reactions in solutions Remember that in the liquid state molecules move much easier than in the solid, hence the mixing of reactants occurs faster Solute is the substance which
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 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 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 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 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 informationChapter 4 Aqueous Reactions and Solution Stoichiometry
Chapter 4 Aqueous Reactions and Solution Stoichiometry 4.1 General Properties of Aqueous Solutions What is a solution? How do you identify the following two? Solvent. Solute(s). Dissociation. What is it?
More informationChapter 4. Types of Chemical Reactions
Chapter 4 Types of Chemical Reactions Classifying Chemical Reactions by What Atoms Do Classification of Reactions + Synthesis reaction + Decomposition reaction + + Single displacement reaction + + Double
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 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 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 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 informationElectrolytes do conduct electricity, in proportion to the concentrations of their ions in solution.
Chapter 4 (Hill/Petrucci/McCreary/Perry Chemical Reactions in Aqueous Solutions This chapter deals with reactions that occur in aqueous solution these solutions all use water as the solvent. We will look
More 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 informationChapter 4 - Types of Chemical Reactions and Solution Chemistry
Chapter 4 - Types of Chemical Reactions and Solution Chemistry 4.1 Water, the Common Solvent - the water molecule is bent with and H-O-H angles of approx. 105 º - O-H bonds are covalent - O is slightly
More informationChapter 4. 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 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 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 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 Solutions. Aqueous solutions and their chemistry. Various types of reactions.
Chapter 4 Reactions in Aqueous Solutions Dr. A. AlSaadi 1 Preview Aqueous solutions and their chemistry. Various types of reactions. Precipitation reactions. Acidbase reactions. Oxidationreduction reactions.
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 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 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: 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 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 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 informationCHEM 200/202. Professor Gregory P. Holland Office: GMCS-213C. All s are to be sent to:
CHEM 200/202 Professor Gregory P. Holland Office: GMCS-213C All emails are to be sent to: chem200@mail.sdsu.edu My office hours will be held in GMCS-212 on Monday from 12 pm to 2:00 pm or by appointment.
More informationSolutions. when table salt is mixed with water, it seems to disappear, or become a liquid the mixture is homogeneous
0/4/205 25 Solutions when table salt is mixed with water, it seems to disappear, or become a liquid the mixture is homogeneous the salt is still there????, as you can tell from the taste, or simply boiling
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 informationEquation Writing for a Neutralization Reaction
Equation Writing for a Neutralization Reaction An Acid-Base reaction is also called a Neutralization reaction because the acid (generates H + or H 3 O + ) and base (generates OH ) properties of the reactants
More informationCHE 105 Spring 2018 Exam 2
CHE 105 Spring 2018 Exam 2 Your Name: Your ID: Question #: 1 A penny contains 373 x 10 2 moles of zinc How many atoms of zinc are in a penny? A 225 x 10 22 atoms B 221 x 10 23 atoms C 375 x 10 22 atoms
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 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 informationQuick Review. - Chemical equations - Types of chemical reactions - Balancing chemical equations - Stoichiometry - Limiting reactant/reagent
Quick Review - Chemical equations - Types of chemical reactions - Balancing chemical equations - Stoichiometry - Limiting reactant/reagent Water H 2 O Is water an ionic or a covalent compound? Covalent,
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 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 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 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 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 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 informationH H H H H O H O. Role of Water. Role of Water. Chapter 4. Chemical Reactions in Aqueous Solution H 2 H H H 2 O. Role of H 2 O(l) as solvent.
Role of Water Role of Water Chemical Reactions in Aqueous Solution Role of H 2 O(l) as solvent The polar nature of water molecule Two key features: 1. The distribution of bonding electrons O H covalent
More informationChapter Four: Reactions in Aqueous Solution
Chapter Four: Reactions in Aqueous Solution Learning Outcomes: Identify compounds as acids or bases, and as strong, weak, or nonelectrolytes Recognize reactions by type and be able to predict the products
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 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 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 informationRevision of Important Concepts. 1. Types of Bonding
Revision of Important Concepts 1. Types of Bonding Electronegativity (EN) often molecular often ionic compounds Bonding in chemical substances Bond energy: Is the energy that is released when a bond is
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 informationGeneral Chemistry 1 CHM201 Unit 2 Practice Test
General Chemistry 1 CHM201 Unit 2 Practice Test 1. Which statement about the combustion of propane (C 3H 8) is not correct? C 3H 8 5O 2 3CO 2 4H 2O a. For every propane molecule consumed, three molecules
More informationTypes of chemical reactions
PowerPoint to accompany Types of chemical reactions Chapters 3 & 16.1 M. Shozi CHEM110 / 2013 General Properties of Aqueous Solutions Solutions are mixtures of two or more pure substances. The solvent
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 informationChapter 4: Types of Chemical Reactions and Solution Stoichiometry
Chapter 4: Types of Chemical Reactions and Solution Stoichiometry 4.1 Water, the Common Solvent 4.2 The Nature of Aqueous Solutions: Strong and Weak Electrolytes 4.3 The Composition of Solutions (MOLARITY!)
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 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 informationSI session Grue 207A
Chem 105 Wednesday 21 Sept 2011 1. Precipitation and Solubility 2. Solubility Rules 3. Precipitation reaction equations 4. Net ionic equations 5. OWL 6. Acids and bases SI session Grue 207A TR, 12:001:30
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 informationElectrolytes solutions
Chapter 4 Types of Chemical Reactions and Solution Stoichiometry Water has a high surface tension due to hydrogen-bonding molecules attract each other more than the air. Electrolytes solutions which conduct
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 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 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 informationThe photograph in the textbook provides evidence that an exothermic chemical reaction is occurring.
Preview Lesson Starter Objectives Indications of a Chemical Reaction Characteristics of Chemical Equations Significance of a Chemical Equation Balancing Chemical Equations Section 1 Describing Chemical
More informationUnit 4a: Solution Stoichiometry Last revised: October 19, 2011 If you are not part of the solution you are the precipitate.
1 Unit 4a: Solution Stoichiometry Last revised: October 19, 2011 If you are not part of the solution you are the precipitate. You should be able to: Vocabulary of water solubility Differentiate between
More informationAnnouncements. Exam 1 is on Thursday, September 23 from 7-8:10pm; Conflict exam is from 5:35-6:45pm
Announcements Print worksheet #6 prior to your Tuesday discussion section LON-CAPA assignment 4 is now available Don t forget to bring your Clicker to class EVERY day The points from last week have been
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 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 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 informationChemistry 1A. Chapter 5
Chemistry 1A Chapter 5 Water, H 2 O Water Attractions Liquid Water Solutions A solution, also called a homogeneous mixture, is a mixture whose particles are so evenly distributed that the relative concentrations
More informationReactions in Aqueous Solutions
Chapter 4 Reactions in Aqueous Solutions Some typical kinds of chemical reactions: 1. Precipitation reactions: the formation of a salt of lower solubility causes the precipitation to occur. precipr 2.
More informationSolubility & Net Ionic review
Solubility & Net Ionic review Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Which of the following statements is/are correct? 1. All ionic compounds
More informationLecture 4 :Aqueous Solutions
LOGO Lecture 4 :Aqueous Solutions International University of Sarajevo Chemistry - SPRING 2014 Course lecturer : Jasmin Šutković 11 th March 2014 Contents International University of Sarajevo 1. Aqueous
More informationCHEMICAL REACTIONS. There are three ways we write chemical equations. 1. Molecular Equations 2. Full Ionic Equations 3. Net Ionic Equations
CHEMICAL REACTIONS Reactants: Zn + I 2 Product: Zn I 2 Unit 2 Chemical Reactions The unit 2 exam will cover material from multiple chapters. You are responsible for the following from your text on exam
More 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 information1. Hydrochloric acid is mixed with aqueous sodium bicarbonate Molecular Equation
NAME Hr Chapter 4 Aqueous Reactions and Solution Chemistry Practice A (Part 1 = Obj. 1-3) (Part 2 = Obj. 4-6) Objective 1: Electrolytes, Acids, and Bases a. Indicate whether each of the following is 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 informationChapter 4. Aqueous Reactions and Solution Stoichiometry
Sample Exercise 4.1 (p. 127) The diagram below represents an aqueous solution of one of the following compounds: MgCl 2, KCl, or K 2 SO 4. Which solution does it best represent? Practice Exercise 1 (4.1)
More information4. Chemical reactions
4. Chemical reactions Chemical reactions types: Dissociation Precipitation Acid base or salification Redox Displacement Gas forming reaction Decomposition Synthesis Dr.ssa Rossana Galassi 320 4381420 rossana.galassi@unicam.it
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 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 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 informationAP Chemistry Campbell
11. The molar mass of magnesium carbonate is (A) 80.0 g mol 1 (B) 84.3 g mol 1 (C) 88.2 g mol 1 (D) 82.0 g mol 1 12. When the equation below is written and balanced, what is the coefficient for the hydrochloric
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 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 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 information