Chemistry 1A. Chapter 5

Size: px
Start display at page:

Download "Chemistry 1A. Chapter 5"

Transcription

1 Chemistry 1A Chapter 5

2 Water, H 2 O

3 Water Attractions

4 Liquid Water

5 Solutions A solution, also called a homogeneous mixture, is a mixture whose particles are so evenly distributed that the relative concentrations of the components are the same throughout. Water solutions are called aqueous solutions.

6 Solution (Homogeneous Mixture)

7 Solute and Solvent In solutions of solids dissolved in liquids, we call the solid the solute and the liquid the solvent. In solutions of gases in liquids, we call the gas the solute and the liquid the solvent. In other solutions, we call the minor component the solute and the major component the solvent.

8 Solution of an Ionic Compound

9 Solution of an Ionic Compound (cont.)

10 Liquid-Liquid Solution

11 Precipitation Reactions In a precipitation reaction, one product is insoluble in water. As that product forms, it emerges, or precipitates, from the solution as a solid. The solid is called a precipitate. For example, Ca(NO 3 ) 2 (aq) + Na 2 CO 3 (aq) CaCO 3 (s) + 2NaNO 3 (aq)

12 Precipitation Questions Describe the solution formed at the instant water solutions of two ionic compounds are mixed (before the reaction takes place). Describe the reaction that takes place in this mixture. Describe the final mixture. Write the complete equation for the reaction.

13 Solution of Ca(NO3)2

14 Solution of Ca(NO 3 ) 2 and Na 2 CO 3 at the time of mixing, before the reaction

15 Product Mixture for the reaction of Ca(NO 3 ) 2 and Na 2 CO 3

16 Complete Ionic Equation

17 Spectator Ions Ions that are important for delivering other ions into solution but that are not actively involved in the reaction are called spectator ions. Spectator ions can be recognized because they are separate and surrounded by water molecules both before and after the reaction.

18 Net Ionic Equations An equation written without spectator ions is called a net ionic equation. Ca 2+ (aq) + CO 3 2 (aq) CaCO 3 (s)

19 Writing Precipitation Equations Step 1: Determine the formulas for the possible products using the general double-displacement equation. AB + CD AD + CB Step 2: Predict whether either of the possible products is water insoluble. If either possible product is insoluble, a precipitation reaction takes place, and you may continue with step 3. If neither is insoluble, write No reaction.

20 Water Solubility Ionic compounds with the following ions are soluble. NH 4 +, group 1 metal ions, NO 3, and C 2 H 3 O 2 Ionic compounds with the following ions are usually soluble. Cl, Br, I except with Ag + and Pb 2+ SO 4 2 except with Ba 2+ and Pb 2+ Ionic compounds with the following ions are insoluble. CO 3 2, PO 4 3, and OH except with NH 4+ and group 1 metal cations S 2 except with NH 4+ and group 1 and 2 metal cations

21 Writing Precipitation Equations (cont) Step 3: Follow these steps to write the complete equation. Write the formulas for the reactants separated by a +. Separate the formulas for the reactants and products with a single arrow. Write the formulas for the products separated by a +. Write the physical state for each formula. The insoluble product will be followed by (s). Water-soluble ionic compounds will be followed by (aq). Balance the equation.

22 Writing Precipitation Equations (cont) Write the complete ionic equation. Describe aqueous ionic compounds as ions. Describe the solid with a complete formula. Make sure that you have correctly done the following Balanced the equation Included charges on ions Included states

23 Writing Precipitation Equations (cont) Write the net ionic equation. Eliminate ions that are in the same form on each side of the complete ionic equation. Rewrite what s left and balance.

24 Skills to Master (1) Convert between names and symbols for the common elements. Identify whether an element is a metal or a nonmetal. Determine the charges on many of the monatomic ions. Convert between the name and formula for polyatomic ions.

25 Skills to Master (2) Convert between the name and formula for ionic compounds. Balance chemical equations. Predict the products of double displacement reactions. Predict ionic solubility.

26 Arrhenius Acid Definition Anacid is a substance that generates hydronium ions, H 3 O + (often described as H + ), when added to water. An acidic solution is a solution with a significant concentration of H 3 O + ions.

27 Characteristics of Acids Acids have a sour taste. Acids turn litmus from blue to red. Acids react with bases.

28 Strong and Weak Acids Strong Acid = due to a completion reaction with water, generates close to one H 3 O + for each acid molecule added to water. Weak Acid = due to a reversible reaction with water, generates significantly less than one H 3 O + for each molecule of acid added to water.

29 Strong Acid and Water When HCl dissolves in water, hydronium ions, H 3 O +, and chloride ions, Cl, ions form.

30 Solution of a Strong Acid

31 Acetic Acid

32 Weak Acid and Water Acetic acid reacts with water in a reversible reaction, which forms hydronium and acetate ions.

33 Solution of Weak Acid

34 Strong and Weak Acids

35 Recognizing Acids From name (something) acid (metal) hydrogen sulfate (metal) dihydrogen phosphate From formula HX(aq), H a X b O c, HC 2 H 3 O 2, RCO 2 H (RCOOH) (symbol for metal)hso 4 (symbol for metal)h 2 PO 4

36 Strong and Weak Acids Strong Acids Monoprotic HCl(aq), HBr(aq), HI(aq), HNO 3, HClO 4 H 2 SO 4 Weak Acid The rest

37 Arrhenius Base Definitions A base is a substance that generates OH when added to water. A basic solution is a solution with a significant concentration of OH ions.

38 Characteristics of Bases Bases have a bitter taste. Bases feel slippery on your fingers. Bases turn litmus from red to blue. Bases react with acids.

39 Strong Bases Anions in ionic compounds except Neutral anions -Cl, Br, I, NO 3, ClO 4 Acidic anions HSO 4, H 2 PO 4 Uncharged, molecular bases NH 3

40 Strong Bases Strong Base = due to a completion reaction with water, generates close to one (or more) OH for each formula unit of base added to water. Metal hydroxides (e.g. NaOH) NaOH(s) Na + (aq) + OH (aq) Metal hydrides (e.g. LiH) LiH(s) H (aq) + H 2 O(l) Li + (aq) + H (aq) Metal amides (e.g. NaNH 2 ) NaNH 2 (s) NH 2 (aq) + H 2 O(l) H 2 (aq) + OH (aq) Na + (aq) + NH 2 (aq) NH 3 (aq) + OH (aq)

41 Weak Base Weak Base = due to a reversible reaction with water, generates significantly less than one OH for each formula unit of base added to water. All other bases

42 Ammonia and Water Ammonia reacts with water in a reversible reaction, which forms ammonium and hydroxide ions.

43 Ammonia Solution

44 ph Acidic solutions have ph values less than 7, and the more acidic the solution is, the lower its ph. Basic solutions have ph values greater than 7, and the more basic the solution is, the higher its ph.

45 ph Range

46 Neutralization Reactions Reactions between Arrhenius acids and Arrhenius bases are called neutralization reactions. HNO 3 (aq) + NaOH(aq) H 2 O(l) + NaNO 3 (aq)

47 Aqueous Nitric Acid

48 Mixture of HNO 3 and NaOH Before Reaction.

49 Strong Acid and Strong Base Reaction The hydronium ion, H 3 O +, from the strong acid reacts with the hydroxide ion, OH, from the strong base to form water, H 2 O.

50 Mixture of HNO 3 and NaOH After the Reaction

51 Electrolytes Strong electrolytes ionize (strong acids) or dissociate (water-soluble ionic compounds) completely when added to water, causing the water to conduct electric currents strongly. Weak electrolytes ionize (weak acids and ammonia) incompletely when added to water, causing the water to conduct electric currents weakly. Nonelectrolytes (such as alcohols and sugars) do not form ions in solution, and therefore, do not cause water to conduct electric currents.

52 Steps to Neutralization Equations Do you have an acid and a base? If you have a strong acid or a strong base or if both are strong, write a single arrow. If both are weak, write a double arrow. Write the formulas and states for the products. If the base is ammonia, NH 3 (aq) + HX(aq) NH 4 X(aq) Otherwise, AB + CD AD + CB Balance the complete equation.

53 Steps to Neutralization Equations (2) Write the complete ionic equation. Describe strong electrolytes as ions. Describe everything else with a complete formula. Make sure that you have correctly done the following Balanced the equation Included charges on ions Included states

54 Steps to Neutralization Equations (3) Write the net ionic equation. Eliminate ions that are in the same form on each side of the complete ionic equation. Rewrite what s left and balance.

55 Steps to Neutralization Equations (4) Check to be sure the following is true. Strong acids described as H +. Weak acids described with a complete formula. H 2 SO 4 described as H + and HSO 4. Pure (s), (l), or (g) described with complete formula. Ions in strong electrolytes on both sides of the equation are eliminated.

56 Reaction between an Acid and a Hydroxide Base. The reaction has the double displacement form. AB + CD AD + CB The positive part of the acid is H +. The hydroxide base can be soluble or insoluble. The products are water and a water-soluble ionic compound.

57 Reaction between an Acid and a Carbonate Base. The reaction has the double displacement form. AB + CD AD + CB The positive part of the acid is H +. The products are water, carbon dioxide, and a water-soluble ionic compound. The H 2 O and the CO 2 come from the decomposition of the initial product H 2 CO 3.

58 Arrhenius Acid-Base Reactions? NH 3 (aq) + HF(aq) NH 4+ (aq) + F (aq) base acid H 2 O(l) + HF(aq) H 3 O + (aq) + F (aq) neutral acid NH 3 (aq) + H 2 O(l) NH 4+ (aq) + OH (aq) base neutral H 2 PO 4 (aq) + HF(aq) H 3 PO 4 (aq) + F (aq) acid acid

59 Acid and Base Definitions Acid Arrhenius: a substance that generates H 3 O + in water Brønsted-Lowry: a proton, H +, donor Base Arrhenius: a substance that generates OH - in water Brønsted-Lowry: a proton, H +, acceptor Acid-Base Reaction Arrhenius: between an Arrhenius acid and base Brønsted-Lowry: a proton (H + ) transfer

60 Brønsted-Lowry Acids and Bases NH 3 (aq) + HF(aq) NH 4+ (aq) + F (aq) base acid H 2 O(l) + HF(aq) H 3 O + (aq) + F (aq) base acid NH 3 (aq) + H 2 O(l) NH 4+ (aq) + OH (aq) base acid H 2 PO 4 (aq) + HF(aq) H 3 PO 4 (aq) + F (aq) base acid

61 Why Two Definitions for Acids and Bases? (1) Positive Aspects of Arrhenius Definitions All isolated substances can be classified as acids (generate H 3 O + in water), bases (generate OH - in water), or neither. Allows predictions, including (1) whether substances will react with a base or acid, (2) whether the ph of a solution of the substance will be less than 7 or greater than 7, and (3) whether a solution of the substance will be sour. Negative Aspects of Arrhenius Definitions Does not include similar reactions (H + transfer reactions) as acid-base reactions.

62 Why Two Definitions for Acids and Bases? (2) Positive Aspects of Brønsted-Lowry Definitions Includes similar reactions (H + transfer reactions) as acid-base reactions. Negative Aspects of Brønsted-Lowry Definitions Cannot classify isolated substances as acids (generate H 3 O + in water), bases (generate OH in water), or neither. The same substance can sometimes be an acid and sometimes a base. Does not allow predictions of (1) whether substances will react with a base or acid, (2) whether the ph of a solution of the substance will be less than 7 or greater than 7, and (3) whether a solution of the substance will be sour.

63 Conjugate Acid-Base Pairs

64 Brønsted-Lowry Acids and Bases NH 3 (aq) + HF(aq) NH 4+ (aq) + F (aq) base acid acid base H 2 O(l) + HF(aq) H 3 O + (aq) + F (aq) base acid acid base NH 3 (aq) + H 2 O(l) NH 4+ (aq) + OH (aq) base acid acid base H 2 PO 4 (aq) + HF(aq) H 3 PO 4 (aq) + F (aq) base acid acid base

65 Amphoteric Substances Can be a Brønsted-Lowry acid in one reaction and a Brønsted-Lowry base in another? HCO 3 (aq) + HF(aq) CO 2 (g) + H 2 O(l) + F (aq) base acid HCO 3 (aq) + OH (aq) CO 2 3 (aq) + H 2 O(l) acid base H 2 PO 4 (aq) + HF(aq) H 3 PO 4 (aq) + F (aq) base acid H 2 PO 4 (aq) + 2OH (aq) PO 3 4 (aq) + 2H 2 O(l) acid base

66 Oxidation Historically, oxidation meant reacting with oxygen. 2Zn(s) + O 2 (g) 2ZnO(s) Zn Zn e or 2Zn 2Zn e O + 2e O 2 or O 2 + 4e 2O 2

67 Oxidation Redefined (1) Many reactions that are similar to the reaction between zinc and oxygen were not considered oxidation. For example, both the zinc-oxygen reaction and the reaction between sodium metal and chlorine gas (described on the next slide) involve the transfer of electrons.

68 Oxidation and Formation of Binary Ionic Compounds

69 Similar to Oxidation of Zinc 2Na(s) + Cl 2 (g) 2NaCl(s) Na Na + + e or 2Na 2Na + + 2e Cl + e Cl or Cl 2 + 2e 2Cl Oxidation = Loss of Electrons

70 Oxidation Redefined (2) To include the similar reactions in the same category, oxidation was redefined as any chemical change in which at least one element loses electrons.

71 Zinc Oxide Reduction The following equation describes one of the steps in the production of metallic zinc. ZnO(s) + C(g) Zn(s) + CO(g) Because zinc is reducing the number of bonds to oxygen atoms, historically, zinc was said to be reduced. When we analyze the changes taking place, we see that zinc ions are gaining two electrons to form zinc atoms. Zn e Zn The definition of reduction was broadened to coincide with the definition of oxidation. According to the modern definition, when something gains electrons, it is reduced.

72 Reduction The loss of electrons (oxidation) by one substance is accompanied by the gain of electrons by another (reduction). Reduction is any chemical change in which at least one element gains electrons.

73 Memory Aid

74 Oxidizing and Reducing Agents A reducing agent is a substance that loses electrons, making it possible for another substance to gain electrons and be reduced. The oxidized substance is always the reducing agent. An oxidizing agent is a substance that gains electrons, making it possible for another substance to lose electrons and be oxidized. The reduced substance is always the oxidizing agent.

75 Identifying Oxidizing and Reducing Agents 2Zn(s) + O 2 (g) 2ZnO(s) Zn Zn e O + 2e O 2 Zinc atoms lose electrons, making it possible for oxygen atoms to gain electrons and be reduced, so zinc is the reducing agent. Oxygen atoms gain electrons, making it possible for zinc atoms to lose electrons and be oxidized, so O 2 is the oxidizing agent.

76 Partial Loss and Gain of Electrons N 2 (g) + O 2 (g) 2NO(g) The N-O bond is a polar covalent bond in which the oxygen atom attracts electrons more than the nitrogen atom. Thus the oxygen atoms gain electrons partially and are reduced. The nitrogen atoms lose electrons partially and are oxidized. N 2 is the reducing agent. O 2 is the oxidizing agent.

77 Redox Terms (1)

78 Redox Terms (2) Oxidation-Reduction Reaction an electron transfer reaction Oxidation complete or partial loss of electrons Reduction complete or partial gain of electrons Oxidizing Agent the substance reduced; gains electrons, making it possible for something to lose them. Reducing Agent the substance oxidized; loses electrons, making it possible for something to gain them.

79 Questions Answered by Oxidation Numbers Is the reaction redox? What s oxidized? What s reduced? What s the reducing agent? What s the oxidizing agent? If any atoms change their oxidation number, yes. The element that increases its oxidation number The element that decreases its oxidation number The substance with the element oxidized The substance with the element reduced

80 Steps for Determination of Oxidation Numbers Step 1: Assign oxidation numbers to as many atoms as you can using the guidelines described on the next slide. Step 2: To determine oxidation numbers for atoms not described on the pervious slide, use the following guideline. The sum of the oxidation numbers for each atom in the formula is equal to the overall charge on the formula. (This includes uncharged formulas where the sum of the oxidation numbers is zero.)

81 Oxidation Numbers uncharged element 0 no exceptions monatomic ions charge on ion no exceptions combined fluorine -1 no exceptions combined oxygen -2-1 in peroxides covalently bonded hydrogen +1 no exceptions

82 Single Displacement

83 Single Displacement Reaction Zn(s) + CuSO 4 (aq) ZnSO 4 (aq) + Cu(s) Zn(s) + Cu 2+ (aq) Zn 2+ (aq) + Cu(s) oxidation: reduction: Zn(s) Zn 2+ (aq) + 2e Cu 2+ (aq) + 2e Cu(s)

84 Single Displacement Reaction Example

85 Voltaic Cell The system in which two halfreactions for a redox reaction are separated allowing the electrons transferred in the reaction to be passed between them through a wire is called voltaic cell.

86 Voltaic Cell

87 Electrodes The electrical conductors placed in the half-cells are called electrodes. They can be active electrodes, which participate in the reaction, or passive electrodes, which transfer the electrons into or out of a halfcell but do not participate in the reaction.

88 Anode The anode is the site of oxidation. Because oxidation involves loss of electrons, the anode is the source of electrons. For this reason, it is described as the negative electrode. Because electrons are lost forming more positive (or less negative) species at the anode, the surroundings tend to become more positive. Thus anions are attracted to the anode.

89 Cathode The cathode is the site of reduction. By convention, the cathode is the positive electrode. Because electrons come to the cathode and substances gain these electrons to become more negative (or less positive), the surroundings tend to become more negative. Thus cations are attracted to the cathode.

90 Other Cell Components A device called a salt bridge can be used to keep the charges balanced. The portion of the electrochemical cell that allows ions to flow is called the electrolyte.

91 Leclanché Cell or Dry Cell Anode oxidation: Zn(s) Cathode reduction: Zn 2+ (aq) + 2e 2MnO 2 (s) + 2NH 4+ (aq) + 2e Mn 2 O 3 (s) + 2NH 3 (aq) + H 2 O(l) Overall reaction: Zn(s) + 2MnO 2 (s) + 2NH 4+ (aq) Zn 2+ (aq) + Mn 2 O 3 (s) + 2NH 3 (aq) + H 2 O(l)

92 Dry Cell Image

93 Alkaline Batteries Anode oxidation: Zn(s) + 2OH (aq) ZnO(s) + H 2 O(l) + 2e Cathode reduction: 2MnO 2 (s) + H 2 O(l) + 2e Mn 2 O 3 (s) + 2OH (aq) Overall reaction: Zn(s) + 2MnO 2 (s) ZnO(s) + Mn 2 O 3 (s)

94 Electrolysis Voltage, a measure of the strength of an electric current, represents the force that moves electrons from the anode to the cathode in a voltaic cell. When a greater force (voltage) is applied in the opposite direction, electrons can be pushed from what would normally be the cathode toward the voltaic cell s anode. This process is called electrolysis. In a broader sense, electrolysis is the process by which a redox reaction is made to occur in the nonspontaneous direction. 2NaCl(l) 2Na(l) + Cl 2 (g)

95 Primary and Secondary Batteries Batteries that are not rechargeable are called primary batteries. A rechargeable battery is often called a secondary battery or a storage battery.

96 Nickel-Cadmium Battery Anode reaction: Cd(s) + 2OH (aq) Cd(OH) 2 (s) + 2e Cathode reaction: NiO(OH)(s) + H 2 O(l) + e Ni(OH) 2 (s) + OH (aq) Net Reaction: Cd(s) + 2NiO(OH)(s) + 2H 2 O(l) Cd(OH) 2 (s) + 2Ni(OH) 2 (s)

97 Lead Acid Battery Pb(s) + HSO 4 (aq) + H 2 O(l) PbSO 4 (s) + H 3 O + (aq) + 2e Cathode reaction: PbO 2 (s) + HSO 4 (aq) + 3H 3 O + (aq) + 2e PbSO 4 (s) + 5H 2 O(l) Net Reaction: Pb(s) + PbO 2 (s) + 2HSO 4 (aq) + 2H 3 O + (aq) 2PbSO 4 (s) + 4H 2 O(l)

98 Conversions to Moles

99 Molarity Converts between moles of solute and volume of solution

100 Equation Stoichiometry (1)

101 Equation Stoichiometry (1) Tip-off - The calculation calls for you to convert from amount of one substance to amount of another, both of which are involved in a chemical reaction. General Steps 1. If you are not given it, write and balance the chemical equation for the reaction. 2. Start your dimensional analysis in the usual way.

102 Equation Stoichiometry (2) 3. Convert from the units that you are given for substance 1 to moles of substance 1. For pure solids and liquids, this means converting mass to moles using the molar mass of the substance. Molarity can be used to convert from volume of solution to moles of solute.

103 Equation Stoichiometry (3) 4. Convert from grams of substance 1 to moles of substance Convert from moles of substance 2 to the desired units for substance 2. For pure solids and liquids, this means converting moles to mass using the molar mass of substance 2. Molarity can be used to convert from moles of solute to volume of solution. 6. Calculate your answer and report it with the correct significant figures (in scientific notation, if necessary) and unit.

104 Titration Titration involves the addition of one solution (solution 1) to another solution (solution 2) until a chemical reaction between the components in the solutions is complete. Solution 1 is called the titrant, and we say that it is used to titrate solution 2. The completeness of the reaction is usually shown by a change of color caused by a substance called an indicator.

105 Titration Apparatus

106 Steps for Titration (1) A specific volume of the solution to be titrated (solution 2) is added to an Erlenmeyer flask. For example, ml of a phosphoric acid solution of unknown concentration might be added to a 250-mL Erlenmeyer flask.

107 Steps for Titration (2) A solution of a substance that reacts with the solute in the solution in the Erlenmeyer flask is added to a buret. This solution in the buret, which has a known concentration, is the titrant. The buret is set up over the Erlenmeyer flask so the titrant can be added to the solution to be titrated. For example, a 1.02 M NaOH solution might be added to a buret, which is set up over the Erlenmeyer flask containing the phosphoric acid solution.

108 Steps for Titration (3) An indicator is added to the solution being titrated. The indicator is a substance that changes color when the reaction is complete. In our example, phenolphthalein, which is a common an acid-base indicator, is added to the phosphoric acid solution in the Erlenmeyer flask.

109 Phenolphthalein Phenolphthalein is a substance that has two forms. In acidic conditions, it is in the acid form, which is colorless. In basic conditions, an H + ion is removed from each phenolphthalein molecule, converting it to its base form, which is red.

110 Steps for Titration (4) The titrant is slowly added to the solution being titrated until the indicator changes color, showing that the reaction is complete. This stage in the procedure is called the endpoint. In our example, the NaOH solution is slowly added from the buret until the mixture in the Erlenmeyer flask changes from colorless to red. At this point, 34.2 ml of 1.02 M NaOH has been added.

111 Making Solutions From pure solids From a pure or almost pure acid (e.g. 17 M HC 2 H 3 O 2 or 18 M H 2 SO 4 ) From any other more concentrated solution

112 Making a Solution from Pure Solid

113 Making a Solution From Concentrated Acid

114 Add Concentrated Acid to Water

115 Dilution Problems mol solute concentrated = mol solute dilute --- mol solute conc --- mol solute dil --- L conc soln = --- L dil soln L conc soln L dil soln V M = V M conc conc dilute MV = MV C C D D dilute

116 Making a Solution from a More Concentrated Solution (not concentrated acid)

Chapter 7. Oxidation-Reduction Reactions

Chapter 7. Oxidation-Reduction Reactions Chapter 7 Oxidation-Reduction Reactions Chapter Map Oxidation Historically oxidation meant reacting with oxygen. 2Zn(s) + O 2 (g) 2ZnO(s) Zn Zn 2+ + 2e or 2Zn 2Zn 2+ + 4e O + 2e O 2 or O 2 + 4e 2O 2 Oxidation

More information

Chapter 9 Oxidation-Reduction Reactions. An Introduction to Chemistry by Mark Bishop

Chapter 9 Oxidation-Reduction Reactions. An Introduction to Chemistry by Mark Bishop Chapter 9 Oxidation-Reduction Reactions An Introduction to Chemistry by Mark Bishop Chapter Map Oxidation Historically, oxidation meant reacting with oxygen. 2Zn(s) + O 2 (g) 2ZnO(s) Zn Zn 2+ + 2e or 2Zn

More information

Chapter 6. Acids, Bases, and Acid-Base Reactions

Chapter 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 information

Chapter 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. 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 information

Reactions in Aqueous Solution

Reactions 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 information

ed. 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. 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 information

Chapter 4. Reactions in Aqueous Solution

Chapter 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 information

Chapter 4. Reactions in Aqueous Solution

Chapter 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 information

Chapter 4 Reactions in Aqueous Solutions. Copyright McGraw-Hill

Chapter 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 information

Reactions in Aqueous Solutions

Reactions 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 information

Chemistry 2 Summer 2008 Exam 2 Chapters 6(part), 7-10

Chemistry 2 Summer 2008 Exam 2 Chapters 6(part), 7-10 Name Chemistry 2 Summer 2008 Exam 2 Chapters 6(part), 7-10 Answer the following by writing the word, words, letter, letters or number in each blank that best completes each sentence. (1 point each) 1.

More information

9/24/12. Chemistry Second Edition Julia Burdge. Reactions in Aqueous Solutions

9/24/12. Chemistry Second Edition Julia Burdge. Reactions in Aqueous Solutions Chemistry Second Edition Julia Burdge 4 Reactions in Aqueous Solutions Copyright (c) The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 4 Reactions in Aqueous Solutions

More information

Chapter 4 Types of Chemical Reaction and Solution Stoichiometry

Chapter 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 information

CHAPTER 4 TYPES OF CHEMICAL EQUATIONS AND SOLUTION STOICHIOMETRY

CHAPTER 4 TYPES OF CHEMICAL EQUATIONS AND SOLUTION STOICHIOMETRY CHAPTER 4 TYPES OF CHEMICAL EQUATIONS AND SOLUTION STOICHIOMETRY Water, the common solvent Solution is a homogeneous mixture Solvent is the substance that does the dissolving Solute is the substance that

More information

Chapter 4. Types of Chemical Reactions and Solution Stoichiometry

Chapter 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 information

INTRODUCTORY CHEMISTRY Concepts and Critical Thinking Seventh Edition by Charles H. Corwin

INTRODUCTORY CHEMISTRY Concepts and Critical Thinking Seventh Edition by Charles H. Corwin Lecture INTRODUCTORY CHEMISTRY Concepts and Critical Thinking Seventh Edition by Charles H. Corwin Acids and Bases Properties of Acids An acid is any substance that releases hydrogen ions, H +, into water.

More information

CHEMISTRY Matter and Change

CHEMISTRY Matter and Change CHEMISTRY Matter and Change UNIT 18 Table Of Contents Section 18.1 Introduction to Acids and Bases Unit 18: Acids and Bases Section 18.2 Section 18.3 Section 18.4 Strengths of Acids and Bases Hydrogen

More information

SCHOOL YEAR CH- 13 IONS IN AQUEOUS SOLUTIONS AND COLLIGATIVE PROPERTIES SUBJECT: CHEMISTRY GRADE : 11 TEST A

SCHOOL 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 information

Chapter 4 Notes Types of Chemical Reactions and Solutions Stoichiometry A Summary

Chapter 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 information

Reactions in Aqueous Solutions

Reactions 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

Chapter 14. Objectives

Chapter 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 information

Chapter 4 Outline. Electrolytic Properties

Chapter 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 information

Chapter 6. Types of Chemical Reactions and Solution Stoichiometry

Chapter 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 information

Solubility Rules for Ionic Compounds Arrhenius Acid Base Theory

Solubility 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 information

Chapter 4 Reactions in Aqueous Solutions

Chapter 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 information

Chapter 4. Reactions in Aqueous Solution. Lecture Presentation. John D. Bookstaver St. Charles Community College Cottleville, MO

Chapter 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 information

Chapter Four: Reactions in Aqueous Solution

Chapter 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 information

Chapter 4 - Types of Chemical Reactions and Solution Chemistry

Chapter 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 information

Chemical Reactions: An Introduction

Chemical 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 information

Chap. 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. 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 information

Chapter Four. Chapter Four. Chemical Reactions in Aqueous Solutions. Electrostatic Forces. Conduction Illustrated

Chapter 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 information

Chapter 4: Chemical Quantities and Aqueous Reactions

Chapter 4: Chemical Quantities and Aqueous Reactions Chapter 4: Chemical Quantities and Aqueous Reactions C (s) + O 2 (g) CO 2 (g) CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2 H 2 0 (g) 2 C 8 H 18 (g) + 25 O 2 (g) 16 CO 2 (g) + 18 H 2 0 (g) Stoichiometry Calculations

More information

Chapter 4. The Major Classes of Chemical Reactions 4-1

Chapter 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 information

Chem II - Wed, 9/14/16

Chem II - Wed, 9/14/16 Chem II - Wed, 9/14/16 Do Now Drop off any study guides you want color coded Pull out stoich HW Homework See board Agenda Stoich Ch 4 Labish thing Chapter 4 Chemical Reactions & Solution Stoich Water Possesses

More information

15 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. 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 information

Chapter 4 Electrolytes and Aqueous Reactions. Dr. Sapna Gupta

Chapter 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 information

Solubility Rules See also Table 4.1 in text and Appendix G in Lab Manual

Solubility 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 information

Reactions in Aqueous Solution

Reactions in Aqueous Solution Reading Assignments: Reactions in Aqueous Solution Chapter 4 Chapter 4 in R. Chang, Chemistry, 9 th Ed., McGraw-Hill, 2006. or previous editions. Or related topics in other textbooks. Consultation outside

More information

Chapter 4. Reactions in Aqueous Solutions. Aqueous solutions and their chemistry. Various types of reactions.

Chapter 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 information

Acids Bases and Salts Acid

Acids 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 information

Chapter 4: Reactions in Aqueous Solutions

Chapter 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 information

CH 221 Chapter Four Part II Concept Guide

CH 221 Chapter Four Part II Concept Guide CH 221 Chapter Four Part II Concept Guide 1. Solubility Why are some compounds soluble and others insoluble? In solid potassium permanganate, KMnO 4, the potassium ions, which have a charge of +1, are

More information

Chapter 4 Reactions in Aqueous Solution

Chapter 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 information

Chapter 4. Reactions In Aqueous Solution

Chapter 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 information

Chemistry I Notes Unit 10: Acids and Bases

Chemistry 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 information

Electrolytes do conduct electricity, in proportion to the concentrations of their ions in solution.

Electrolytes 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 information

Reactions in Aqueous Solution

Reactions in Aqueous Solution Reactions in Aqueous Solution 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

4. Aqueous Solutions. Solution homogeneous mixture of two components

4. Aqueous Solutions. Solution homogeneous mixture of two components 4. Aqueous Solutions Solution homogeneous mixture of two components Many chemical reactions occur in solution Solutions in water called aqueous Definitions Solute component(s) in smaller amount 2 types:

More information

7/16/2012. Chapter Four: Like Dissolve Like. The Water Molecule. Ionic Compounds in Water. General Properties of Aqueous Solutions

7/16/2012. 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 information

Concentration Units. Solute CONCENTRATION. Solvent. g L -1. (M, molarity) concentration in. mol / litre of solution. mol L -1. molality. molality.

Concentration 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 information

Chem 110 General Principles of Chemistry

Chem 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 information

Stoichiometry: Chemical Calculations. Chemistry is concerned with the properties and the interchange of matter by reaction i.e. structure and change.

Stoichiometry: Chemical Calculations. Chemistry is concerned with the properties and the interchange of matter by reaction i.e. structure and change. Chemistry is concerned with the properties and the interchange of matter by reaction i.e. structure and change. In order to do this, we need to be able to talk about numbers of atoms. The key concept is

More information

Chapter 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 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 information

Acids and Bases. Feb 28 4:40 PM

Acids and Bases. Feb 28 4:40 PM Acids and Bases H O s O Cl H O O H H N H Na O H H Feb 28 4:40 PM Properties of Acids 1. Taste sour 2. Conduct electrical current 3. Liberate H 2 gas when reacted with a metal. 4. Cause certain dyes to

More information

Chapter 7 An Introduction to Chemical Reactions. An Introduction to Chemistry by Mark Bishop

Chapter 7 An Introduction to Chemical Reactions. An Introduction to Chemistry by Mark Bishop Chapter 7 An Introduction to Chemical Reactions An Introduction to Chemistry by Mark Bishop Chapter Map Chemical Reaction A chemical change or chemical reaction is a process in which one or more pure substances

More information

Chapter Menu Chapter Menu

Chapter Menu Chapter Menu Chapter Menu Chapter Menu Section 18.1 Section 18.3 Section 18.4 Introduction to Acids and Bases Hydrogen Ions and ph Neutralization Section 18.1 Intro to Acids and Bases Objectives: Compare the Arrhenius,

More information

Chapter 9: Acids, Bases, and Salts

Chapter 9: Acids, Bases, and Salts Chapter 9: Acids, Bases, and Salts 1 ARRHENIUS ACID An Arrhenius acid is any substance that provides hydrogen ions, H +, when dissolved in water. ARRHENIUS BASE An Arrhenius base is any substance that

More information

Chem 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 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 information

Chapter 4: Types of Chemical reactions and Solution Stoichiometry

Chapter 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 information

ELECTROCHEMISTRY. Oxidation/Reduction

ELECTROCHEMISTRY. Oxidation/Reduction ELECTROCHEMISTRY Electrochemistry involves the relationship between electrical energy and chemical energy. OXIDATION-REDUCTION REACTIONS SPONTANEOUS REACTIONS Examples: voltaic cells, batteries. NON-SPONTANEOUS

More information

Lecture 4 :Aqueous Solutions

Lecture 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 information

CHEM134- 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 information

Chapter 4 Chemical Formulas, Reactions, Redox and Solutions

Chapter 4 Chemical Formulas, Reactions, Redox and Solutions Terms to Know: Solubility Solute Solvent Solution Chapter 4 the amount of substance that dissolves in a given volume of solvent at a given temperature. a substance dissolved in a liquid to form a solution

More information

Chapter 16. Acid-Base Equilibria

Chapter 16. Acid-Base Equilibria Chapter 16. Acid-Base Equilibria 16.1 Acids and Bases: A Brief Review Acids taste sour and cause certain dyes to change color. Bases taste bitter and feel soapy. Arrhenius concept of acids and bases: An

More information

Unit 4a: Solution Stoichiometry Last revised: October 19, 2011 If you are not part of the solution you are the precipitate.

Unit 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 information

How to Assign Oxidation Numbers. Chapter 18. Principles of Reactivity: Electron Transfer Reactions. What is oxidation? What is reduction?

How to Assign Oxidation Numbers. Chapter 18. Principles of Reactivity: Electron Transfer Reactions. What is oxidation? What is reduction? Chapter 18 Principles of Reactivity: Electron Transfer Reactions What is oxidation? When a molecule/ion loses electrons (becomes more positive) Whatever is oxidized is the reducing agent What is reduction?

More information

Aqueous Reactions. The products are just the cation-anion pairs reversed, or the outies (A and Y joined) and the innies (B and X joined).

Aqueous Reactions. 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 information

Unit 2 Acids and Bases

Unit 2 Acids and Bases Unit 2 Acids and Bases 1 Topics Properties / Operational Definitions Acid-Base Theories ph & poh calculations Equilibria (Kw, K a, K b ) Indicators Titrations STSE: Acids Around Us 2 Operational Definitions

More information

Chapter 4. Reactions in Aqueous Solution. Solutions. 4.1 General Properties of Aqueous Solutions

Chapter 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 information

11/3/09. Aqueous Solubility of Compounds. Aqueous Solubility of Ionic Compounds. Aqueous Solubility of Ionic Compounds

11/3/09. 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 information

BIG IDEA TWO. October 13, 2016

BIG IDEA TWO. October 13, 2016 BIG IDEA TWO October 13, 2016 Topics to Cover in Big Idea 2 1. Ionic, metallic, and covalent bonds 2. Polarity and dipole moment 3. Intermolecular forces (IMF): 4. Lewis dot structures 5. Resonance forms

More information

Chapter 8 Acids, Bases, and Acid-Base Reactions. An Introduction to Chemistry by Mark Bishop

Chapter 8 Acids, Bases, and Acid-Base Reactions. An Introduction to Chemistry by Mark Bishop Chapter 8 Acids, Bases, and Acid-Base Reactions An Introduction to Chemistry by Mark Bishop Chapter Map Arrhenius Base Definitions A base is a substance that generates OH when added to water. A basic solution

More information

AP Chemistry Note Outline Chapter 4: Reactions and Reaction Stoichiometry:

AP 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 information

Chemistry 101 Chapter 4 STOICHIOMETRY

Chemistry 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 information

Acids and bases, as we use them in the lab, are usually aqueous solutions. Ex: when we talk about hydrochloric acid, it is actually hydrogen chloride

Acids and bases, as we use them in the lab, are usually aqueous solutions. Ex: when we talk about hydrochloric acid, it is actually hydrogen chloride Acids and Bases Acids and bases, as we use them in the lab, are usually aqueous solutions. Ex: when we talk about hydrochloric acid, it is actually hydrogen chloride gas dissolved in water HCl (aq) Concentrated

More information

Chapter 4: Chemical Reactions in Aqueous Solutions. 4.1 Some Electronic Properties of Aqueous Solutions

Chapter 4: Chemical Reactions in Aqueous Solutions. 4.1 Some Electronic Properties of Aqueous Solutions Chapter : Chemical Reactions in Aqueous Solutions Water: the universal solvent ¾ of Earth s surface water in living organisms Some Electrical Properties of Aqueous Solutions Reactions of Acids and Bases

More information

Chapter 4 Three Major Classes of Chemical Reactions

Chapter 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 information

General Chemistry. Contents. Chapter 5: Introduction to Reactions in Aqueous Solutions. Electrolytes. 5.1 The Nature of Aqueous Solutions

General 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 information

Part One: Ions in Aqueous Solution

Part 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 information

9.1.2 AQUEOUS SOLUTIONS AND CHEMICAL REACTIONS

9.1.2 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 information

General Chemistry. Chapter 5: Introduction to Reactions in Aqueous Solutions. Principles and Modern Applications Petrucci Harwood Herring 8 th Edition

General 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 information

What are Acids and Bases? What are some common acids you know? What are some common bases you know? Where is it common to hear about ph balanced

What are Acids and Bases? What are some common acids you know? What are some common bases you know? Where is it common to hear about ph balanced What are Acids and Bases? What are some common acids you know? What are some common bases you know? Where is it common to hear about ph balanced materials? Historically, classified by their observable

More information

Acids, Bases and ph Chapter 19

Acids, Bases and ph Chapter 19 Acids, Bases and ph Chapter 19 Compounds That Become Acids When Dissolved in Water General Formula: HX H + X - monatomic or polyatomic anion Naming Acids (p. 250) Binary acids Hydro ic Acid HCl: Hydrochloric

More information

Unit 10: Acids and Bases

Unit 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 information

Chapter 4. Concentration of Solutions. Given the molarity and the volume, the moles of solute can be determined.

Chapter 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 information

Oxidation numbers are charges on each atom. Oxidation-Reduction. Oxidation Numbers. Electrochemical Reactions. Oxidation and Reduction

Oxidation numbers are charges on each atom. Oxidation-Reduction. Oxidation Numbers. Electrochemical Reactions. Oxidation and Reduction Oxidation-Reduction Oxidation numbers are charges on each atom. 1 2 Electrochemical Reactions Oxidation Numbers In electrochemical reactions, electrons are transferred from one species to another. In order

More information

Chapter Test B. Chapter: Acids and Bases

Chapter Test B. Chapter: Acids and Bases Assessment Chapter Test B Chapter: Acids and Bases PART I In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. 1. Which of the

More information

TYPES OF CHEMICAL REACTIONS

TYPES 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 information

Chapter 04. Reactions in Aqueous Solution

Chapter 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 information

Chapter 3: Solution Chemistry (For best results when printing these notes, use the pdf version of this file)

Chapter 3: Solution Chemistry (For best results when printing these notes, use the pdf version of this file) Chapter 3: Solution Chemistry (For best results when printing these notes, use the pdf version of this file) Section 3.1: Solubility Rules (For Ionic Compounds in Water) Section 3.1.1: Introduction Solubility

More information

Name: Regents Chemistry Date:

Name: Regents Chemistry Date: Name: Date: 1. The reaction CuO + CO CO 2 + Cu is an example of (A) reduction, only (B) oxidation, only (C) both oxidation and reduction (D) neither oxidation nor reduction 6. In which compound does chlorine

More information

The Major Classes of Chemical Reactions

The 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 information

AP Chemistry. Chapter 4

AP 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 information

Aqueous solutions of acids have a sour Aqueous solutions of bases taste bitter

Aqueous solutions of acids have a sour Aqueous solutions of bases taste bitter Acid and Bases Exam Review Honors Chemistry 3 April 2012 Chapter 14- Acids and Bases Section 14.1- Acid and Base Properties List five general properties of aqueous acids and bases Properties of Acids Properties

More information

Chapter 4. Aqueous Reactions and Solution Stoichiometry

Chapter 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

Chapter 4. Chemical Quantities and Aqueous Reactions

Chapter 4. Chemical Quantities and Aqueous Reactions Lecture Presentation Chapter 4 Chemical Quantities and Aqueous Reactions Reaction Stoichiometry: How Much Carbon Dioxide? The balanced chemical equations for fossilfuel combustion reactions provide the

More information

Acids and Bases. Click a hyperlink or folder tab to view the corresponding slides. Exit

Acids and Bases. Click a hyperlink or folder tab to view the corresponding slides. Exit Acids and Bases Section 18.1 Introduction to Acids and Bases Section 18.2 Strengths of Acids and Bases Section 18.3 Hydrogen Ions and ph Section 18.4 Neutralization Click a hyperlink or folder tab to view

More information

Chapter 7 Chemical Reactions

Chapter 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 information

CH 4 AP. Reactions in Aqueous Solutions

CH 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 information

Equation Writing for a Neutralization Reaction

Equation 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 information