11/3/09. Aqueous Solubility of Compounds. Aqueous Solubility of Ionic Compounds. Aqueous Solubility of Ionic Compounds
|
|
- Hannah Price
- 5 years ago
- Views:
Transcription
1 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 molecular compounds stay associated in water Brooks/Cole Brooks/Cole 2 Aqueous Solubility of Ionic Compounds Aqueous Solubility of Ionic Compounds 2008 Brooks/Cole Brooks/Cole 4 Aqueous Solubility of Ionic Compounds Exchange Reactions: Precipitation (a) Nitrates (soluble) (b) Hydroxides (insoluble) AgNO 3 Cu(NO 3 ) 2 Cu(OH) 2 AgOH (c) Sulfides CdS Sb 2 S 3 PbS (NH 4 ) 2 S soluble insoluble 2008 Brooks/Cole Brooks/Cole 6 1
2 Precipitation Reaction When ionic solutions mix, a precipitate may form: Not all ions react KNO 3 (aq) + NaCl(aq) No reaction A reaction occurs if a product is insoluble. Precipitation Reactions Na 2 SO 4 (aq) and Ba(NO 3 ) 2 (aq) are mixed. Will they react? Products? Na + SO 4 2 Ba 2+ NO 3 NaNO 3 and BaSO 4. Insoluble? The solubility rules help predict reactions Brooks/Cole Brooks/Cole 8 Soluble ionic compounds fully dissociate: AgNO 3 (aq) Ag + (aq) + NO 3 (aq) KCl(aq) K + (aq) + Cl (aq) On mixing: Ag + (aq) + NO 3 (aq) + K + (aq) + Cl (aq) AgCl(s) + K + (aq) + NO 3 (aq) Net ionic equation: Ag + (aq) + Cl (aq) AgCl(s) 2008 Brooks/Cole Brooks/Cole 10 (NH 4 ) 2 S(aq) + Hg(NO 3 ) 2 (aq) HgS + 2 NH 4 NO 3 Product Solubility HgS insoluble (All sulfides except group 1A, 2A and NH + 4 salts) NH 4 NO 3 soluble (All ammonium salts; all nitrates) (NH 4 ) 2 S(aq) + Hg(NO 3 ) 2 (aq) HgS + NH 4 NO 3 not balanced ammonium sulfide mercury(ii) nitrate mercury(ii) sulfide ammonium nitrate 2008 Brooks/Cole Brooks/Cole 12 2
3 Acids Increase the concentration of H + ions in water. 2 NH 4+ (aq) + S 2 (aq) + Hg 2+ (aq) + 2 NO 3 (aq) HgS(s) + 2 NH 4+ (aq) + 2 NO 3 (aq) S 2 (aq) + Hg 2+ (aq) HgS(s) Change the color of pigments (indicators) Litmus, phenolphthalein 2008 Brooks/Cole Brooks/Cole 14 Acids Bases Increase the concentration of OH (hydroxide ion) in water. Bases: Counteract an acid (neutralize an acid). Change an indicator s color (phenolphthalein ). Have a bitter taste. Feel slippery. H 2 O 2008 Brooks/Cole Brooks/Cole 16 Common Acids and Bases Neutralization Reactions acid + base salt + water. Neutralizations are exchange reactions Brooks/Cole Brooks/Cole 18 3
4 for AcidBase Reactions for AcidBase Reactions 2008 Brooks/Cole Brooks/Cole 20 GasForming Exchange Reactions GasForming Exchange Reactions Carbonic acid (unstable) Tums H 2 CO 3 (aq) H 2 O(l) + CO 2 (g) often written: CaCO 3 (s) + 2 HCl(aq) CaCl 2 (aq) + H 2 O(l) + CO 2 (g) AlkaSeltzer 2008 Brooks/Cole Brooks/Cole 22 GasForming Exchange Reactions GasForming Exchange Reactions Sulfurous acid (unstable) H 2 SO 3 (aq) H 2 O(l) + SO 2 (g) or Na 2 SO 3 (aq) + 2 HCl(aq) 2 NaCl(aq) + H 2 O(l) +SO 2 (g) 2008 Brooks/Cole Brooks/Cole 24 4
5 OxidationReduction Reactions OxidationReduction Reactions In all cases: If something is oxidized, something must be reduced. Redox reactions move e. (note: H 2 is oxidized, so CuO is an oxidizing agent) +2 e 2 Ag + (aq) + Cu(s) 2 Ag(s) + Cu 2+ (aq) 2 e Here: Cu changes to Cu 2+. Cu loses 2 e ; each Ag + gains one e Ag + is reduced (ore turned to metal) Gain of e = reduction (so, loss of e = oxidation) 2008 Brooks/Cole Brooks/Cole 26 Redox Reactions and Electron Transfer Redox Reactions and Electron Transfer e M X M loses electron(s) X gains electron(s) M is oxidized X is reduced M is a reducing agent X is an oxidizing agent 2008 Brooks/Cole Brooks/Cole 28 Common Oxidizing and Reducing Agents Oxidizing Agent Reaction Product O 2 (oxygen) O 2 (oxide ion) H 2 O 2 (hydrogen peroxide) H 2 O(l) F 2, Cl 2, Br 2, I 2 (halogen) F, Cl, Br, I (halide ion) HNO 3 (nitric acid) nitrogen oxides (NO, NO 2..) Cr 2 O 7 (dichromate ion) Cr 3+ (chromium(iii) ion) MnO 4 (permanganate ion) Mn 2+ (manganese(ii) ion) Reducing Agent Reaction Product H 2 (hydrogen) H + or H 2 O C CO and CO 2 M (metal: Na, K, Fe..) M n+ (Na +, K +, Fe 3+..) Displacement Reactions + + A XZ AZ X Redox: Fe(s) + CuSO 4 (aq) FeSO 4 (aq) + Cu(s) Cu(s) + 2 AgNO 3 (aq) Cu(NO 3 ) 2 (aq) + 2 Ag(s) Brooks/Cole Brooks/Cole 30 5
6 Activity Series of Metals Displace H 2 from H 2 O (l), steam or acid Displace H 2 from steam or acid Displace H 2 from acid No reaction with H 2 O, steam or acid lithium potassium barium strontium calcium sodium magnesium aluminum manganese zinc chromium iron nickel tin lead hydrogen antimony copper mercury silver palladium platinum gold Ease of oxidation increases 2008 Brooks/Cole 31 Displacement Reactions Powerful reducing agents at the top. Higher elements displace lower ones: Zn(s) + CuSO 4 (aq) ZnSO 4 (aq) + Cu(s) Mg(s) + 2 HCl(aq) MgCl 2 (aq) + H 2 (g) 2008 Brooks/Cole 32 Li K Ba Sr Ca Na Mg Al Mn Zn Cr Fe Ni Sn Pb H Sb Cu Hg Ag Pd Pt Au Displacement Reactions Displacement Reactions Potassium + water 2 K(s) + 2 H 2 O(l) 2 KOH(aq) + H 2 (g) 2008 Brooks/Cole Brooks/Cole 34 Solution Concentration Relative amounts of solute and solvent. Molarity Molarity = moles solute liters of solution = mol L Shorthand: [NaOH] =1.00 M The brackets [ ] represent molarity of 2008 Brooks/Cole Brooks/Cole 36 6
7 Molarity Calculate the molarity of sodium sulfate in a solution that contains 36.0 g of Na 2 SO 4 in ml of solution. n Na2SO4 = [Na 2 SO 4 ] = 36.0 g = mol g/mol mol L Unit change! (ml to L) [Na 2 SO 4 ] = mol/l = M Molarity 6.37 g of Al(NO 3 ) 3 are dissolved to make a 250. ml aqueous solution. Calculate (a) [Al(NO 3 ) 3 ] (b) [Al 3+ ] and [NO 3 ]. (a) Al(NO 3 ) 3 FM = (14.00) + 9(16.00) = g mol 6.37 g g/mol 2008 Brooks/Cole Brooks/Cole 38 Molarity 6.37 g of Al(NO 3 ) 3 in a 250. ml aqueous solution. Calculate (a) the molarity of the Al(NO 3 ) 3, (b) the molar concentration of Al 3+ and NO 3 ions in solution. Solution Preparation Solutions are prepared either by: 1. Diluting a more concentrated solution. 1 Al(NO 3 ) 3 1 Al 3+ 1 Al(NO 3 ) 3 3 NO 3 [Al 3+ ] = M Al(NO 3 ) 1 Al 3+ 3 = M Al 3+ 1 Al(NO 3 ) 3 [NO 3 ] = M Al(NO 3 ) 3 = M NO 3 or 2. Dissolving a measured amount of solute and diluting to a fixed volume Brooks/Cole Brooks/Cole 40 Solution Preparation by Dilution M conc V conc = M dil V dil Solution Preparation from Pure Solute Prepare a M solution of potassium permanganate in a ml volumetric flask. M dil = M conc V conc = V dil 17.8 M x 75.0 ml ml = 1.34 M Mass of KMnO 4 = mol x g/mol = g 2008 Brooks/Cole Brooks/Cole 42 7
8 Solution Preparation from Pure Solute Rinse all the solid from the weighing dish into the flask. Fill the flask ⅓ full. Swirl to dissolve the solid. Fill the flask to the mark on the neck. Shake to thoroughly mix. n A = [ A ] x V [product] = n product / (total volume) Brooks/Cole Brooks/Cole 44 H 2 SO 4 (aq) + 2 NaOH(aq) Na 2 SO 4 (aq) + 2 H 2 O(l)? mol x 10 3 mol 2 NaOH 1 H 2 SO 4 H 2 SO 4 (aq) + 2 NaOH(aq) Na 2 SO 4 (aq) + 2 H 2 O(l) n NaOH = L mol L = x 10 3 mol H 2 SO 4 required = x 10 3 mol NaOH 1 H 2SO 4 2 NaOH = x 10 3 mol V acid needed: mol H V = 2 SO 4 = [H 2 SO 4 ] x 10 3 mol 1 L mol = L = 33.4 ml 2008 Brooks/Cole Brooks/Cole 46 A g mixture of oxalic acid, H 2 C 2 O 4 and NaCl was neutralized by ml of 0.550M NaOH. What was the weight % of oxalic acid in the mixture? n NaOH = L x mol/l = mol 1 H 2 C 2 O 4 2 NaOH Oxalic acid reacted = 1 H mol NaOH 2 C 2 O 4 = x10 3 mol 2 NaOH 2008 Brooks/Cole 47 A g H 2 C 2 O 4 / NaCl mixture was neutralized by ml of 0.550M NaOH. What was the weight % of oxalic acid in the mixture? Mass of acid consumed = x10 3 mol x (90.04 g/mol acid) = g of oxalic acid weight of acid Weight percent = sample weight x 100% g Weight percent = x 100% g = 16.08% 2008 Brooks/Cole 48 8
9 25.0 ml of M FeCl 3 and 50.0 ml of M NaOH are mixed. Which reactant is limiting? How many moles of Fe(OH) 3 will form? FeCl 3 (aq) + 3 NaOH(aq) 3 NaCl (aq) + Fe(OH) 3 (s) n FeCl3 = L x mol/l = mol n NaOH = L x mol/l = mol 25.0 ml of M FeCl 3 and 50.0 ml of M NaOH are mixed. Which reactant is limiting? How many moles of Fe(OH) 3 will form? FeCl 3 (aq) + 3 NaOH(aq) 3 NaCl (aq) + Fe(OH) 3 (s) mol mol 1 Fe(OH) mol FeCl 3 3 = mol Fe(OH) 3 1 FeCl 3 1 Fe(OH) mol NaOH 3 = mol Fe(OH) 3 3 NaOH FeCl 3 is limiting; mol produced Brooks/Cole Brooks/Cole 50 Aqueous Solution Titrations Aqueous Solution Titrations Titrant: Base of known concentration Slowly add standard solution. End point: indicator changes color. Determine V titrant added. Often used to determine acid or base concentrations. Unknown acid + phenolphthalein (colorless in acid) turns pink in base 2008 Brooks/Cole Brooks/Cole 52 9
Chapter 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 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 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 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 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 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 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 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 informationReactions in aqueous solutions Redox reactions
Reactions in aqueous solutions Redox reactions Redox reactions In precipitation reactions, cations and anions come together to form an insoluble ionic compound. In neutralization reactions, H + ions and
More 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. 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 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 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 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 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 informationChem 1A Dr. White Fall Handout 4
Chem 1A Dr. White Fall 2014 1 Handout 4 4.4 Types of Chemical Reactions (Overview) A. Non-Redox Rxns B. Oxidation-Reduction (Redox) reactions 4.6. Describing Chemical Reactions in Solution A. Molecular
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 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 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 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 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. 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 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 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 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 informationWRITING CHEMICAL EQUATIONS 2002, 1989 by David A. Katz. All rights reserved. Permission for classroom used provided original copyright is included.
WRITING CHEMICAL EQUATIONS 2002, 1989 by David A. Katz. All rights reserved. Permission for classroom used provided original copyright is included. David A. Katz Chemist, Educator, Science Communicator,
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 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 informationTypes of Reactions: Reactions
1 Reactions On the A.P. Test there will be one question (question #4) that will say: Give the formulas to show the reactants and the products for the following chemical reactions. Each occurs in aqueous
More informationCHEMISTRY - CLUTCH CH.4 - CHEMICAL QUANTITIES & AQUEOUS REACTIONS
!! www.clutchprep.com CONCEPT: MOLARITY Molarity (M) can serve as the connection between the interconversion of to and vice versa. For example, a 5.8 M NaCl solution really means per. ( Molarity = MolesSolute
More informationExam 3. Objectives: Nomenclature
Exam 3 Objectives: o Nomenclature m-nm, m(vos)-nm, nm-nm o Evidence for Chemical Reactions o Writing Chemical Equations o Balancing Chemical Equations o Classifying Chemical Reactions o Combination Reactions
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 informationWhat Do You Think? Investigate GOALS
Cool Chemistry Show Activity 4 Chemical Equations GOALS In this activity you will: Represent chemical changes using word equations and chemical equations. Distinguish between different classes of chemical
More 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 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 informationelemental state. There are two different possibilities: DESCRIPTION 1. One cation (+ ion) replaces another. 2. One anion (- ion) replaces another.
CHEMICAL TYPES HANDOUT In these reactions, a free element reacts with a compound to form another compound and release one of the elements of the original compound in the elemental state. There are two
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 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 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 informationCHEMISTRY - ZUMDAHL 2E CH.6 - TYPES OF CHEMICAL REACTIONS AND SOLUTION STOICHIOMETRY
!! www.clutchprep.com CONCEPT: MOLARITY Molarity (M) can serve as the connection between the interconversion of to and vice versa. For example, a 5.8 M NaCl solution really means per. ( Molarity = MolesSolute
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 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 informationMultiple Choice Identify the letter of the choice that best completes the statement or answers the question.
Chapter 8 Prep Test Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. General Solubility Guidelines 1. Most sodium, potassium, and ammonium compounds
More informationTypes of Reactions: Reactions
1 Reactions On the A.P. Test there will be one question (question #4) that will say: Give the formulas to show the reactants and the products for the following chemical reactions. Each occurs in aqueous
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 informationSolution Stoichiometry
Chapter 8 Solution Stoichiometry Note to teacher: You will notice that there are two different formats for the Sample Problems in the student textbook. Where appropriate, the Sample Problem contains the
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 informationChemical Equations. Chemical Reactions. The Hindenburg Reaction 5/25/11
Chemical Reactions CHM 1032C Chemical Equations Chemical change involves a reorganization of the atoms in one or more substances. The Hindenburg Reaction Reactants are on left, products to the right. Arrow
More informationAP Chemistry Unit #4. Types of Chemical Reactions & Solution Stoichiometry
AP Chemistry Unit #4 Chapter 4 Zumdahl & Zumdahl Types of Chemical Reactions & Solution Stoichiometry Students should be able to: Predict to some extent whether a substance will be a strong electrolyte,
More informationElectrodeposition. - Worksheet - Envisioning Chemistry. 1. Write half reactions for the following processes under electrical current.
Electrodeposition 1. Write half reactions for the following processes under electrical current. (1). Formation of copper from copper (II) ion Example: Cu 2+ + 2e --> Cu (2). Formation of tin from tin ion
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 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 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 informationChapter 5. Chemical reactions
Chapter 5 Chemical reactions Chemical equations CaO(s) + CO 2 (g) CaCO 3 (s) + CO(g) Chemical equation - representation of a chemical reaction; uses the symbols of the elements and formulae of the compounds
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 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 informationName. Practice Test 2 Chemistry 111
Name Practice Test 2 Chemistry 111 1) In the aqueous reaction of K 2 SO 4 (aq) + Ba(NO 3 ) 2 (aq) BaSO 4 (s) + 2KNO 3 (aq), which ions are the spectator ions? A) Ba 2+ 2- and SO 4 B) Ba 2+ and K + C) Ba
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 informationinsoluble partial very soluble (< 0.1 g/100ml) solubility (> 1 g/100ml) Factors Affecting Solubility in Water
Aqueous Solutions Solubility is a relative term since all solutes will have some solubility in water. Insoluble substances simply have extremely low solubility. The solubility rules are a general set of
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 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 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 informationReaction Writing Sheet #1 Key
Reaction Writing Sheet #1 Key Write and balance each of the following reactions and indicate the reaction type(s) present: 1. zinc + sulfur zinc sulfide 8 Zn (s) + S 8 (s) 8 ZnS (s) synthesis 2. potassium
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 informationAP Chemistry Honors Unit Chemistry #4 2 Unit 3. Types of Chemical Reactions & Solution Stoichiometry
HO AP Chemistry Honors Unit Chemistry #4 2 Unit 3 Chapter 4 Zumdahl & Zumdahl Types of Chemical Reactions & Solution Stoichiometry Students should be able to:! Predict to some extent whether a substance
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 informationClassifying Chemical Reactions
Chem 101 Classifying Chemical Reactions Lectures 17 and 18 Classifying Chemical Reactions Chemical reactions can be divided into five categories: I. Combination or Synthesis Reactions II. Decomposition
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 informationWhat is one of the spectator ions (with correct coefficient)? A)
Chem 101 Exam Fall 01 Section 001 1. Based on the solubility rules Mg (PO 4 ) is A) soluble B) insoluble. An aqueous solution of potassium sulfate is allowed to react with an aqueous solution of What is
More informationChapter 4: Reactions in Aqueous Solutions
Chapter 4: Reactions in Aqueous Solutions Water 60 % of our bodies heat modulator solvent for reactions covers 70% of Earth Chapter 4 3 types of reactions that occur in H 2 O 1. precipitation 2. acid-base
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 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 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 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 informationChemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten. Unit 4 (Chapter 4): Aqueous Reactions &
Chemistry, The Central Science, 10th edition Theodore L. Brown;. Eugene LeMay, Jr.; and Bruce E. Bursten Unit 4 (Chapter 4): Aqueous Reactions & Solution Stoichiometry John D. Bookstaver St. Charles Community
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 7. Chemical Equations and Reactions
Chemical Equations and Reactions Chemical and Physical Changes In a physical change, the chemical composition of the substance remains constant. Examples of physical changes are the melting of ice or the
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 informationCHEM 1413 Chapter 4 Homework Questions TEXTBOOK HOMEWORK
CHEM 1413 Chapter 4 Homework Questions TEXTBOOK HOMEWORK Chapter 3 3.68 Calculate each of the following quantities: (a) Mass (g) of solute in 185.8 ml of 0.267 M calcium acetate (b) Molarity of 500. ml
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 information1) What is the volume of a tank that can hold Kg of methanol whose density is 0.788g/cm 3?
1) Convert the following 1) 125 g to Kg 6) 26.9 dm 3 to cm 3 11) 1.8µL to cm 3 16) 4.8 lb to Kg 21) 23 F to K 2) 21.3 Km to cm 7) 18.2 ml to cm 3 12) 2.45 L to µm 3 17) 1.2 m to inches 22) 180 ºC to K
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 informationChemical Reactions CHAPTER Reactions and Equations
CHAPTER 9 Chemical Reactions 9.1 Reactions and Equations The process by which atoms of one or more substances are rearranged to form different substances is called a chemical reaction. There are a number
More information8 Chemical Equations. Flames and sparks result when aluminum foil is dropped into liquid bromine.
8 Chemical Equations Flames and sparks result when aluminum foil is dropped into liquid bromine. Chapter Outline 8.1 The Chemical Equation 8.2 Writing and Balancing Chemical Equations 8.3 Types of Chemical
More informationQuestion 8 Chemical properties of metals and nonmetals. 1) magnesium 2) sulfur trioxide 3) iron (II) hydroxide 4) sodium nitrate
Question 8 Chemical properties of metals and nonmetals 1. Calcium oxide doesn t react with 1) NaNO 3 2) HCl 3) CO 2 4) H 2 O 2. Calcium oxide reacts with both of the following 1) SO 2 and O 2 2) H 2 O
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 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 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 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 informationCheck Your Solution The net ionic equation is balanced, including the charges on the ions.
Ba 2+ (aq) + 2PO (aq) Ba (PO ) 2 (s) 2. Practice Problem (page 10) Write the net ionic equation for this reaction: Na 2 SO (aq) + Sr(OH) 2 (aq) SrSO (s) + NaOH(aq) You need to write the net ionic equation
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 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 informationStudy Guide: Stoichiometry
Name: Study Guide: Stoichiometry Period: **YOUR ANSWERS MUST INCLUDE THE PROPER NUMBER OF SIG FIGS AND COMPLETE UNITS IN ORDER TO RECEIVE CREDIT FOR THE PROBLEM.** BALANCE THE FOLLOWING EQUATIONS TO USE
More informationDefinition: the process by which one or more substances are rearranged to form different substances. Another name for a chemical change.
Chemical Reactions I. What is a chemical reaction? Definition: the process by which one or more substances are rearranged to form different substances. Another name for a chemical change. A. How can you
More informationIB Topics 9 & 19 Multiple Choice Practice
IB Topics 9 & 19 Multiple Choice Practice 1. What are the oxidation states of chromium in (NH 4) 2Cr 2O 7 (s) and Cr 2O 3 (s)? 2. Which of the following is a redox reaction? 3Mg (s) + 2AlCl 3 (aq) 2Al
More informationChemistry 150/151 Review Worksheet
Chemistry 150/151 Review Worksheet This worksheet serves to review concepts and calculations from first semester General Chemistry (CHM 150/151). Brief descriptions of concepts are included here. If you
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 information