CHEM 200/202. Professor Jing Gu Office: EIS-210. All s are to be sent to:
|
|
- Shonda Paul
- 5 years ago
- Views:
Transcription
1 CHEM 200/202 Professor Jing Gu Office: EIS-210 All s are to be sent to: My office hours will be held in GMCS-212 on Monday from 9 am to 11 am or by appointment.
2 ANNOUNCEMENTS Chapter 2 homework due 9/14/18 Lab report Volumetric Equipment and Pre-Lab assignment and report: Qualitative Analysis is due on 9/17/18 Quiz 1 due 9/20/18. Homework Chapter 3 and 4 due 9/21/18. Exam 1 is on 9/22/18 at 2-4 pm.
3 LECTURE OBJECTIVES Chapter Balance chemical reactions. Express aqueous ionic reactions in various manners. Identify spectator ions in aqueous ionic reactions. Identify precipitates in aqueous ionic reactions.
4 BALANCING CHEMICAL EQUATIONS It is crucial to have properly balanced reactions when trying to interpret chemical reactions. The balanced reaction shows us how much of each reagent is required and how much of each product is formed. Methane (CH4) undergoes a combustion reaction with oxygen (O2), producing carbon dioxide (CO2) and water (H2O).
5 BALANCE THE REACTIONS BELOW _N2(g) + _H2(g) _NH3(g) _Pb(s) + _H2O(l) +_O2(g) _Pb(OH)2(s)
6 IONIC REACTIONS Many chemical reactions which take place in aqueous solutions involve ionic compounds. These ionic reactions can be depicted in various forms depending on how we wish to focus our attention. The various forms include: The molecular equation The complete ionic equation The net ionic equation
7 IONIC EQUATIONS Sample reaction: lead nitrate reacting with potassium iodide. The molecular equation Pb(NO 3 ) 2(aq) + 2KI (aq) PbI 2(s) + 2KNO 3(aq) The reaction depicts the molecular reactants and products, but does not show the ions present in solution.
8 IONIC EQUATIONS Pb(NO 3 ) 2(aq) + 2KI (aq) PbI 2(s) + 2KNO 3(aq) Dissociation of ionic compounds: Pb(NO 3 ) 2(aq) Pb 2+ (aq) + 2NO 3 (aq) KI (aq) K + (aq) + I (aq) KNO 3(aq) K + (aq) + NO 3 (aq) PbI 2(s) PbI 2(s) (There are no ions, lead iodide is insoluble in water.) Complete ionic equation: Pb 2+ (aq) + 2NO 3 (aq) + 2K + (aq) + 2I (aq) PbI 2(s) + 2K + (aq) + 2NO 3 (aq)
9 IONIC EQUATIONS The net ionic equation is a simplification of the complete ionic equation. The net ionic equation removes all the spectator ions. Pb 2+ (aq) + 2NO3 (aq) + 2K + (aq) + 2I (aq) PbI2(s) + 2K + (aq) + 2NO3 (aq) Net ionic equation: Pb 2+ (aq) + 2I (aq) PbI2(s)
10 REACTION CLASSIFICATIONS There are three principle aqueous chemical reactions that we will focus on in this course: Precipitations reactions Acid-base reactions Redox reactions (oxidation-reductions)
11 PRECIPITATION REACTIONS Precipitation reactions occur when pairs of insoluble ions (e.g. Ag + and Cl ) are both present in solution at the same time. A mixture of aqueous solutions may result in more than one precipitate being formed, if more than one insoluble pair is present. Knowledge of the common soluble and insoluble ions is required to predict precipitations (solubility rules).
12 Soluble SOLUBILITY RULES 1. All common compounds of Group 1A(1) ions (Li +, Na +, K +...) and ammonium ions (NH4 + ) 2. All common nitrates (NO3 - ), acetates (CH3CO2 - ) and most perchlorates (ClO4 - ) 3. All common chlorides (Cl - ), bromides (Br - ) and iodides (I - ); except those of Ag +, Pb 2+, Cu + and Hg2 2+. All common fluorides (F - ) are soluble; except for Pb 2+ & Group2A(2) 4. All common sulfates (SO4 2- ); except Ca 2+, Sr 2+, Ba 2+, Ag + & Pb 2+
13 SOLUBILITY RULES Insoluble 1) All common metal hydroxides are insoluble; except those of Group 1A(1) and the larger members of Group 2A(2) - beginning with Ca 2+. 2) All common carbonates (CO3 2- ) and phosphates (PO4 3- ) are insoluble; except those from Group 1A(1) and ammonium (NH4 + ). 3) All common sulfides (S 2- ) are insoluble; except those of Groups 1A(1), 2(A)2 and NH4 +.
14 PREDICTING PRECIPITATION 1. Note the ions present in the reactants. 2. Consider the possible cation-anion combinations. 3. Decide wether any of the ion combinations is insoluble.
15 QUESTION Predict the identity of the precipitate formed when solutions of Na2CO3 and CaCl2 are mixed. Answers A B C D E Na2CO3 CaCl2 CaCO3 NaCl No ppt forms
16 PREDICTING PRECIPITATION For the following aqueous reactions, does a precipitate form? Write the net ionic equation for the reaction, if applicable. Potassium nitrate + Silver(I) acetate Sodium iodide + Copper(I) nitrate
17 PROBLEM Balance the reaction below, and provide the net ionic equation for the reaction. _Fe(NO3)3(aq) + _Na2CO3(aq) _Fe2(CO3)3(s) + _NaNO3(aq)
18 LECTURE OBJECTIVES Chapter Identify acid-base reactions and their respective products. Calculate acid-base neutralization endpoints.
19 ACIDS AND BASES Acids - produce H3O + (aq) when dissolved in water (often expressed as H + (aq)) Bases - produce OH (aq) when dissolved in water Strong acid/base - completely dissociates in water Weak acid/base - incompletely dissociates in water
20 ACID BASE THEORY H + (proton) forms H 3 O + in water (hydrogen bonding) H + is electron deficient, wants electrons, electron pair acceptor OH is electron rich, can donate a pair of electrons Water self-ionizes: 2H2O(l) H3O + (aq) + OH (aq) Acid-Base definitions: Arrhenius: Acid increases conc. of H3O + when added to water Base increases conc. of OH - when added to water Brønsted-Lowry: Acid = proton donor Base = proton acceptor Lewis: Acid: electron pair acceptor Base: electron pair donor
21 ACID-BASE THEORY Arrhenius example: NaOH (aq) + HCl (aq) H2O(l) + NaCl(aq) Net ionic equation for all Arrhenius acid-base reactions: H + (aq) + OH (aq) H2O(l) Brønstead example: HCl(benzene) + NH3(benzene) NH4Cl(s) HCl donates a proton to NH3 Lewis example: NH3(g) + BH3(g) NH3BH3
22 SELECTED ACIDS & BASES Strong Acids Hydrochloric acid, HCl Hydrobromic acid, HBr Hydroiodic acid, HI Nitric acid, HNO3 Sulfuric acid, H2SO4 Perchloric acid, HClO4 Weak Acids Hydrofluoric acid, HF Phosphoric acid, H3PO4 Acetic acid, CH3COOH (or HC2H3O2) Strong Bases Sodium hydroxide, NaOH Potassium hydroxide, KOH Calcium hydroxide, Ca(OH)2 Strontium hydroxide, Sr(OH)2 Barium hydroxide, Ba(OH)2 Weak Bases Ammonia, NH3
23 ACIDS Monoprotic: one ionizable hydrogen HCl + H 2 O H 3 O + + Cl Diprotic: two ionizable hydrogens H 2 SO 4 + H 2 O H 3 O + + HSO 4 HSO 4 + H 2 O H 3 O + + SO 4 2 Triprotic: three ionizable hydrogens Polyprotic, generic term meaning that there is more than one ionizable hydrogen on the molecule. H 3 PO 4 + H 2 O H 3 O + + H 2 PO 4 H 2 PO 4 + H 2 O H 3 O + + HPO 4 2 HPO H 2 O H 3 O + + PO 4 3
24 BASES Monobasic: yields one OH - ion KOH K + + OH NH3 +H2O NH4 + + OH Dibasic: yields two OH ions Ba(OH)2 Ba OH Ca(OH)2 Ca OH
25 ACID-BASE NEUTRALIZATION Molecular equation Acid + Base Water + Salt Total ionic equation HCl(aq) + NaOH(aq) H2O(l) + NaCl(aq) H + (aq) + Cl (aq) + Na + (aq) + OH (aq) H2O(l) + Na + (aq) + Cl (aq) Net ionic equation H + (aq) + OH (aq) H2O(l) Hint: Balance the H + with OH - the rest will work itself out.
26 AN AQUEOUS STRONG ACID-BASE REACTION ON THE ATOMIC SCALE
27 ACID-BASE TITRATION
28 QUESTION What is the concentration of a sulfuric acid solution if it requires ml of a M sodium hydroxide solution to titrate ml of the sulfuric acid solution?
29 GAS FORMATION WITH AN ACID-BASE Molecular equation REACTION NaHCO3(aq) + CH3CO2H(aq) H2O(l) + CH3CO2Na(aq) + CO2(g) Total ionic equation Na + (aq) + HCO3 - (aq) + H + (aq) + CH3CO2 - (aq) H2O(l) + Na + (aq) + CH3CO2 - (aq) + CO2(g) Net ionic equation HCO3 - (aq) + CH3CO2H(aq) CH3CO2 - + H2O(l) + CO2(g)
30 An aqueous solution of H 2 SO 4 is added to an aqueous solution of Ba(OH) 2. The reaction is monitored using a conductivity meter. Predict the correct statement(s): 1. Both H 2 SO 4 & Ba(OH) 2 are strong electrolytes 2. This is a neutralization reaction 3. This is a precipitation reaction 4. The light bulb will glow at the neutralization point Answers A B C D E Statement 2 Statements 1 & 2 Statements 1, 2 & 3 All of the statements are true All of the statements are lies
CHEM 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 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 12:00 pm to 2:00 pm or by appointment.
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. FALL 2018 ROOM
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 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 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 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 informationAqueous Reactions and Solution Stoichiometry (continuation)
Aqueous Reactions and Solution Stoichiometry (continuation) 1. Electrolytes and non-electrolytes 2. Determining Moles of Ions in Aqueous Solutions of Ionic Compounds 3. Acids and Bases 4. Acid Strength
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 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 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 informationUnit Nine Notes N C U9
Unit Nine Notes N C U9 I. AcidBase Theories A. Arrhenius Acids and Bases 1. Acids contain hydronium ions (H O ) commonly referred to as hydrogen ions (H ) that dissociate in water a. Different acids release
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 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 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 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 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 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 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 informationAREA 1: WATER. Chapter 6 ACIDS AND BASES. 6.1 Properties of acids and bases
AREA 1: WATER Chapter 6 ACIDS AND BASES 6.1 Properties of acids and bases Acids are: Sour May be corrosive Dissolve in water to produce an electrolyte, Turn blue litmus red Neutralised by bases. Bases
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 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 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 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 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 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 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 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 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 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 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 informationChapter 14. Objectives
Section 1 Properties of Acids and Bases Objectives List five general properties of aqueous acids and bases. Name common binary acids and oxyacids, given their chemical formulas. List five acids commonly
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 informationAcids and Bases. Unit 10
Acids and Bases Unit 10 1 Properties of Acids and Bases Acids Bases Taste Sour Turns Litmus Dye Red Reacts with Metals to give H 2 (g) Taste Bitter Turns Litmus Dye Blue Do Not React with Metals Reacts
More informationChapter 14: Acids and Bases
Chapter 14: Acids and Bases Properties of Acids and Bases What is an acid? Some examples of common items containing acids: Vinegar contains acetic acid; lemons and citrus fruits contain citric acid; many
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 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 informationChapters 15 & 16 ACIDS & BASES ph & Titrations
PROPERTIES OF ACIDS Chapters 15 & 16 ACIDS & BASES ph & Titrations There are 5 main properties of acids: 1. sour taste 2. change the color of acidbase indicators 3. react with metals to produce H2 gas
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 informationChapter 6. Acids, Bases, and Acid-Base Reactions
Chapter 6 Acids, Bases, and Acid-Base Reactions Chapter Map Arrhenius Acid Definition Anacid is a substance that generates hydronium ions, H 3 O + (often described as H + ), when added to water. An acidic
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 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 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 information(Label the Conjugate Pairs) Water in the last example acted as a Bronsted-Lowry base, and here it is acting as an acid. or
Chapter 16 - Acid-Base Equilibria Arrhenius Definition produce hydrogen ions in aqueous solution. produce hydroxide ions when dissolved in water. Limits to aqueous solutions. Only one kind of base. NH
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 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 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 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 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 14 Acids and Bases
Properties of Acids and Bases Chapter 14 Acids and Bases Svante Arrhenius (1859-1927) First to develop a theory for acids and bases in aqueous solution Arrhenius Acids Compounds which dissolve (dissociate)
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 informationChemical Reaction Defn: Chemical Reaction: when starting chemical species form different chemicals.
Chemistry 11 Notes on Chemical Reactions Chemical Reaction Defn: Chemical Reaction: when starting chemical species form different chemicals. Evidence to indicate that a chemical reaction has occurred:
More informationChemistry I Notes Unit 10: Acids and Bases
Chemistry I Notes Unit 10: Acids and Bases Acids 1. Sour taste. 2. Acids change the color of acid- base indicators (turn blue litmus red). 3. Some acids react with active metals and release hydrogen gas,
More informationPage III-4b-1 / Chapter Four Part II Lecture Notes. Chemistry 221 Professor Michael Russell MAR. Ba(NO3)2(aq)? soluble. BaCl2(aq)?
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
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 informationChemical Reaction Defn: Chemical Reaction: when starting chemical species form different chemicals.
Chemical Reaction Defn: Chemical Reaction: when starting chemical species form different chemicals. Evidence to indicate that a chemical reaction has occurred: Temperature change Different coloured materials
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 informationProperties of Acids and Bases
Chapter 15 Aqueous Equilibria: Acids and Bases Properties of Acids and Bases Generally, an acid is a compound that releases hydrogen ions, H +, into water. Blue litmus is used to test for acids. Blue litmus
More informationHA(s) + H 2 O(l) = H 3 O + (aq) + A (aq) b) NH 3 (g) + H 2 O(l) = NH 4 + (aq) + OH (aq) Acid no. H + type base no. OH type
You are already familiar with some acid and base chemistry. According to the Arrhenius model, acids are substances that when dissolved in water ionize to yield hydrogen ion (H + ) and a negative ion. e.g.
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) When the following equation is balanced, the coefficients are. 1) NH3 (g) + O2 (g) NO2
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 informationAP Chemistry. Reactions in Solution
AP Chemistry Reactions in Solution S o l u t i o n s solution: a homogeneous mixture of two or more substances -- The solvent is present in greatest quantity. -- Any other substance present is called a.
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 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 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 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 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 informationMr. Storie 40S Chemistry Student Acid and bases Unit. Acids and Bases
Acids and Bases 1 UNIT 4: ACIDS & BASES OUTCOMES All important vocabulary is in Italics and bold. Outline the historical development of acid base theories. Include: Arrhenius, BronstedLowry, Lewis. Write
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 informationAcids and Bases. Bases react with acids to form water and a salt. Bases do not commonly with metals.
Acids and Bases Properties of Acids and Bases Acids taste. Lemon juice and, for example, are both aqueous solutions of acids. Acids conduct electricity; they are. Some are strong electrolytes, while others
More information8.1 Theories of acids and bases
8. Acids and bases 8.1 Theories of acids and bases Sour-tasting substances (acids) have been known for thousands of years. Lavoisiers early theory: Acid= a compound of oxygen and a nonmetal. Arrhenius
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 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 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 12:00 pm to 2:00 pm or by appointment.
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 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 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 informationAcid Base Reactions. Reading: Ch 4 section 8 Homework: Chapter 4: 79, 81*, 83*, 108 (optional)
Acid Base Reactions Reading: Ch 4 section 8 Homework: Chapter 4: 79, 81*, 83*, 108 (optional) * = important homework question Background Recall: Acids and bases are special in two ways: What is special
More informationAcids and Bases. Properties, Reactions, ph, and Titration
Acids and Bases Properties, Reactions, ph, and Titration C-19 2017 Properties of acids 1. Taste Sour (don t try this except with foods). 2. Are electrolytes (conduct electricity). Some are strong, some
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 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 informationObj: Observe and describe neutralization reactions. Copy: Write the balanced chemical equation for the neutralization of HCl with KOH.
Do Now Date: April 13, 2015 Obj: Observe and describe neutralization reactions. Copy: Write the balanced chemical equation for the neutralization of HCl with KOH. HCl + KOH KCl(aq) + H 2 O(l) Practice
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: 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 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 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 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 information15 Acids, Bases, and Salts. Lemons and limes are examples of foods that contain acidic solutions.
15 Acids, Bases, and Salts Lemons and limes are examples of foods that contain acidic solutions. Chapter Outline 15.1 Acids and Bases 15.2 Reactions of Acids and Bases 15.3 Salts 15.4 Electrolytes and
More informationElectrolytes, Acids and Bases ) 3
Chapter 15 Acid (Latin acidus - sour): sour taste; turns plant dye litmus red; dissolves metals producing H 2 gas. Substances that are neither acids nor bases were called neutral substances. Electrolytes,
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 information4. What is the mass of a mol sample of sodium hydroxide? A) g B) g C) g D) g E) g
Chem 101A Study Questions, Chapters 3 & 4 Name: Review Tues 10/4/16 Due 10/6/16 (Exam 2 date) This is a homework assignment. Please show your work for full credit. If you do work on separate paper, attach
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 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 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 informationUnit 10: Acids and Bases
Unit 10: Acids and Bases PROPERTIES OF ACIDS & BASES Properties of an Acid: a Tastes sour substance which dissociates (ionizes, breaks apart in solution) in water to form hydrogen ions Turns blue litmus
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 information9/24/09 Chem 111 Experiment #7 Solutions and Reactions Brown, LeMay, and Bursten Chapter
Chem 111 Experiment #7 Solutions and Reactions Brown, LeMay, and Bursten Chapter 4.1-4.4 KEY VOCABULARY: 1. Ionic compound a compound composed of cations (+) and anions (-). Many ionic compounds dissociate
More informationPart 01 - Assignment: Introduction to Acids &Bases
Part 01 - Assignment: Introduction to Acids &Bases Classify the following acids are monoprotic, diprotic, or triprotic by writing M, D, or T, respectively. 1. HCl 2. HClO4 3. H3As 4. H2SO4 5. H2S 6. H3PO4
More informationEXAM 3 CHEM 1310 WS09 Key Version #2
EXAM 3 CHEM 1310 WS09 Key Version #2 1. (p. 116) Select the correct name and chemical formula for the precipitate that forms when the following reactants are mixed. CuCl 2 (aq) + Na 2 CO 3 (aq) A. copper(ii)
More informationis considered acid 1, identify the other three terms as acid 2, base 1, and base 2 to indicate the conjugate acid-base pairs.
18.1 Introduction to Acids and Bases 1. Name the following compounds as acids: a. H2SO4 d. HClO4 b. H2SO3 e. HCN c. H2S 2. Which (if any) of the acids mentioned in item 1 are binary acids? 3. Write formulas
More information