Solutions CHAPTER OUTLINE

Size: px
Start display at page:

Download "Solutions CHAPTER OUTLINE"

Transcription

1 Chapter 8A Solutions 1 CHAPTER OUTLINE Type of Solutions Electrolytes & Nonelectrolytes Equivalents of Electrolytes Solubility & Saturation Soluble & Insoluble Salts Formation of a Solid Precipitation Reactions 2 1

2 TYPE OF SOLUTIONS A solution is a homogeneous mixture of two substances: Solute: substance being dissolved Solvent: present in smaller amount substance doing the dissolving present in larger amount Solutes and solvents may be of any form of matter: solid, liquid or gas. 3 TYPE OF SOLUTIONS Type Example Solute Solvent Gas in gas Air Oxygen Nitrogen Gas in liq. Liq. in liq. Solid in liq. Soda water CO 2 Water Vinegar Acetic acid Water Seawater Salt Water 4 2

3 TYPE OF SOLUTIONS Type Example Solute Solvent Liquid in solid Dental amalgam Mercury Silver Solid in solid Brass Zinc Copper 5 SOLUBILITY Solutions form between solute and solvent molecules because of similarities between them. Like dissolves Like Ionic solids dissolve in water because the charged ions (polar) are attracted to the polar water molecules. Nonpolar molecules such as oil and grease dissolve in nonpolar solvents such as kerosene. 6 3

4 SOLUBILITY Water (polar) CH 2 Cl 2 (nonpolar) Ni(NO 3 ) 2 (polar) I 2 (nonpolar) 7 ELECTROLYTES & NONELECTROLYTES Solutions can be characterized by their ability to conduct an electric current. Solutions containing ions are conductors of electricity and those that contain molecules are nonconductors. Substances that dissolve in water to form ions are called electrolytes. The ions formed from these substances conduct electric current in solution, and can be tested using a conductivity apparatus. 8 4

5 STRONG ELECTROLYTES Electrolytes are further classified as strong electrolytes and weak electrolytes. In water, a strong electrolyte exists only as ions. Strong electrolytes Only make ions the light present bulb on the conductivity after apparatus glow brightly. solution Ionic substances such as NaCl are strong electrolytes. NaCl (s) Na (aq) Cl (aq) 9 WEAK ELECTROLYTES Solutions containing weak electrolytes contain only a few ions. These solutions make the light bulb on the conductivity Few ions apparatus glow dimly. present Weak acids and bases that after dissolve in water and produce solution few ions are weak electrolytes. HF (aq) H (aq) F (aq) 10 5

6 NON ELECTROLYTES Substances that do not form any ions in solution are called nonelectrolytes. No ions With these solutions the bulb on present the conductivity apparatus does not glow. after solution Covalent molecules that dissolve in water but do not form ions, such as sugar, are nonelectrolytes. C 12 H 22 O 11 (s) C 12 H 22 O 11 (aq) 11 ELECTROLYTES & NONELECTROLYTES 12 6

7 Example 1: Identify the predominant particles in each of the following solutions and write the equation for the formation of the solution: NH 4 Br Strong electrolyte (only ions) NH 4 Br (s) NH 4 (aq) Br (aq) 13 Example 1: Identify the predominant particles in each of the following solutions and write the equation for the formation of the solution: CH 4 N 2 O Nonelectrolyte (only molecules) CH 4 N 2 O (s) CH 4 N 2 O (aq) 14 7

8 Example 1: Identify the predominant particles in each of the following solutions and write the equation for the formation of the solution: HClO Weak electrolyte (few ions) HClO (aq) H (aq) ClO (aq) 15 EQUIVALENTS OF ELECTROLYTES Body fluids typically contain a mixture of several electrolytes, such as Na, Cl, K and Ca 2. Each individual ion is measured in terms of an equivalent (Eq), which is the amount of that ion equal to 1 mole of positive or negative electrical charge. For example, 1 mole of Na ions and 1 mole of Cl ions are each 1 equivalent (or 1000 meq) because they each contain 1 mole of charge. 16 8

9 EQUIVALENTS OF ELECTROLYTES An Some ion examples with a charge of ions of and 2 or their 2 contains equivalents 2 are equivalents shown below: per mole. Ion Electrical Charge No. of Equivalents in 1 Mole Na 1 1 Eq Ca Eq Fe Eq Cl 1 1 Eq SO Eq 17 EQUIVALENTS OF ELECTROLYTES In body, the charge of the positive ion is always balanced by the charge of the negative ion. For example, a solution containing 25 meq/l of Na and 4 meq/l of K must have 29 meq/l of Cl to balance. Shown next are examples of some common intravenous solutions and their ion concentrations. 18 9

10 EQUIVALENTS OF ELECTROLYTES 19 Example 1: Indicate the number of equivalents in each of the following: 2 mol K 2 mol x 1 Eq 1 mol = 2 Eq 0.5 mol Mg mol x 3 mol CO mol x 2 Eq 1 mol 2 Eq 1 mol = 1 Eq = 6 Eq 20 10

11 Example 2: A typical concentration for Ca 2 in blood is 8.8 meq/l. How many moles of Ca 2 are present in 0.50 L of blood? Liter blood meq moles Ca L x 8.8 meq 1 L x 1 Eq 10 3 meq x 1 mol 2 Eq = mol 21 Example 3: An IV solution contains 155 meq/l of Cl. If a patient received 1250 ml of the IV solution, how many moles of chloride were given to him? 1250 ml x 1 L 10 3 ml x 155 meq 1 L x 1 Eq 10 3 meq x 1 mol 1 Eq = mol 22 11

12 Example 4: A sample of Ringer s solution contains the following concentrations (meq/l) of cations: Na 147, K 4, and Ca 2 4. If Cl is the only anion in the solution, what is the concentration of Cl in meq/l? Total cation meq/l = = 155 meq/l Total cation meq/l = Total anion meq/l Total Cl meq/l = 155 meq/l 23 SOLUBILITY Solubility refers to the maximum amount of solute that can be dissolved in a given amount of solvent. Many factors affect the solubility of a solute in a solution. Type of solute Type of solvent Temperature Solubility is measured in grams of solute per 100 grams of solvent at a given temperature

13 SATURATION A solution that does not contain the maximum amount of solute in it, at a given temperature, is called an unsaturated solution. A solution that contains the maximum amount of solute in it, at a given temperature, is called a saturated solution. Undissolved solid in solution 25 SOLUBILITY Solubility of most solids in water increases as temperature increases. Using a solubility chart, the solubility of a solute at a given temperature can be determined. For example, KNO 3 has a solubility of 80 g/100 g H 2 O (80%) at 40 C

14 SOLUBILITY OF GASES Solubility of gases in water decreases as temperature increases. At higher temperatures more gas molecules have the energy to escape from solution. Henry s law states that the solubility of a gas is directly proportional to the pressure above the liquid. For example, a can of soda is carbonated at high pressures in order to increase the solubility of CO 2. Once the can is opened, the pressure is reduced and the excess gas escapes from the solution. 27 SOLUBLE & INSOLUBLE SALTS Many ionic solids dissolve in water and are called soluble. However, some ionic salts do not dissolve in water and do not form ions in solution. These salts are called insoluble salts and remain solid in solution. Chemists use a set of solubility rules to predict whether a salt is soluble or insoluble. These rules are summarized next

15 SOLUBILITY RULES S O L U B L E NO 3 Na, K NH 4 Cl, Br, I SO 4 2 No exceptions No exceptions Except those containing Ag, Pb 2 Except those containing Ba 2, Pb 2, Ca 2 29 SOLUBILITY RULES I N S O L U B L E S 2, CO 3 2 PO 4 3 OH Except those containing Na, K, NH 4 Except those containing Na, K, Ca 2, NH

16 Example 1: Use the solubility rules to determine if each of the following salts are soluble or insoluble: K 3 PO 4 soluble (all salts of K are soluble) CaCO 3 insoluble (most carbonates are insoluble) 31 Example 2: Using the solubility chart, determine if each of the following solutions is saturated or unsaturated at 20 C: 25 g NaCl in 100 g water Solubility of NaCl at 20 C is 40% Solution is unsaturated 32 16

17 Example 2: Using the solubility chart, determine if each of the following solutions is saturated or unsaturated at 20 C: 11 g NaNO 3 in 25 g water Solubility of NaNO 3 at 20 C is 85% Solution is unsaturated 33 Example 2: Using the solubility chart, determine if each of the following solutions is saturated or unsaturated at 20 C: 400. g of glucose in 125 g water Solubility of glucose at 20 C is 80% Solution is saturated 34 17

18 FORMATION OF A SOLID Solubility rules can be used to predict whether a solid, called a precipitate, can be formed when two solutions of ionic compounds are mixed. A solid is formed when two ions of an insoluble salt come in contact with one another. For example, when a solution of K 2 CrO 4 is mixed with a solution of Ba(NO 3 ) 2 a yellow insoluble salt BaCrO 4 is produced. 35 AQUEOUS REACTIONS K 2 CrO 4 (aq) Ba(NO 3 ) 2 (aq) BaCrO 4 (s) 2 KNO 3 (aq) precipitate Solid BaCrO 4 forms 36 18

19 PRECIPITATION REACTIONS Double replacement reactions in which a precipitate is formed are called precipitation reactions. To predict a precipitate, follow the steps outlined next. 37 PRECIPITATION REACTIONS 1. Write the reactant ions that form after dissolution. 2. Write the product combinations possible when reactant ions combine. 3. Use solubility rules to determine if any of the products are insoluble. 4. If a precipitate forms, write the formula for the solid. Write other ions that form soluble salts as ions. If no precipitate forms, write NO REACTION after the arrow. 5. Cancel ions that appear the same on both sides of the equation (spectator ions), to form Net Ionic Equation

20 The reaction of K 2 CrO 4 and Ba(NO 3 ) 2 can be predicted as shown below 2 K CrO 2 Step 1: 4 Ba 2 2 NO 3??? Step 2: 2 K CrO 2 4 Ba 2 2 NO 3 BaCrO 4 (?) 2K NO 3 (?) Net Ionic Step 3: 2 K CrO 2 4 Ba 2 2 NO Equation 3 BaCrO 4 (s) 2K NO 3 (aq) Step 4: PRECIPITATION REACTIONS 2 K CrO 4 2 Ba 2 2 NO 3 BaCrO 4 (s) 2K 2NO 3 Step 5: Ba 2 CrO 4 2 BaCrO 4 (s) precipitate spectator ions 39 Example 1: Predict the products, if any, for the reaction of AgNO 3 and NaCl and write the net ionic equation. Step 1: Ag NO 3 Na Cl??? Step 2: Ag NO 3 Na Cl Ag Cl (?) Na NO Net Ionic 3 (?) Step 3: Ag NO 3 Na Cl Equation Ag Cl (s) Na NO 3 (aq) Step 4: Ag NO 3 Na Cl AgCl (s) Na NO 3 (aq) Step 5: Ag spectator Cl ions AgCl (s) precipitate spectator ions 40 20

21 Example 2: Predict the products, if any, for the reaction of Na 2 SO 4 and Pb(NO 3 ) 2 and write the net ionic equation. 2 Na SO 2 Step 1: 4 Pb 2 2 NO 3??? Step 2: 2Na SO 2 4 Pb 2 2NO 3 2Na NO 3 (?) Pb 2 SO 2 4 (?) Step 3: 2Na SO 2 4 Pb 2 2NO 3 2Na NO 3 (aq) Pb 2 SO 2 4 (s) Step 4: 2Na SO 2 4 Pb 2 2NO 3 2Na 2NO 3 (aq) PbSO 4 (s) Step 5: Pb 2 SO 4 2 PbSO 4 (s) precipitate (NIE) 41 Example 3: Predict the products, if any, for the reaction of PbCl 2 and KI and write the net ionic equation. Step 1: Pb 2 2 Cl K I??? Step 2: Pb 2 2 Cl K I Pb 2 I 2 (?) K Cl (?) Step 3: Step 4: Pb 2 2 Cl 2 K 2 I Pb 2 I 2 (s) 2 K Cl (aq) Pb 2 2 Cl 2 K 2 I PbI 2 (s) 2 K 2 Cl Step 5: Pb 2 2 I PbI 2 (s) precipitate (NIE) 42 21

22 Example 4: Predict the products, if any, for the reaction of NH 4 Cl and KNO 3 and write the net ionic equation. NH Step 1: 4 Cl K NO 3??? No Reaction Step 2: NH 4 Cl K NO 3 NH 4 NO 3 (?) K Cl (?) Step 3: NH 4 Cl K NO 3 NH 4 NO 3 (aq) K Cl (aq) Step 4: NH 4 Cl K NO 3 NH 4 NO 3 K Cl 43 THE END 44 22

Chemistry 51 Chapter 8 TYPES OF SOLUTIONS. Some Examples of Solutions. Type Example Solute Solvent Gas in gas Air Oxygen (gas) Nitrogen (gas)

Chemistry 51 Chapter 8 TYPES OF SOLUTIONS. Some Examples of Solutions. Type Example Solute Solvent Gas in gas Air Oxygen (gas) Nitrogen (gas) TYPES OF SOLUTIONS A solution is a homogeneous mixture of two substances: a solute and a solvent. Solute: substance being dissolved; present in lesser amount. Solvent: substance doing the dissolving; present

More information

IONIC CHARGES. Chemistry 51 Review

IONIC CHARGES. Chemistry 51 Review IONIC CHARGES The ionic charge of an ion is dependent on the number of electrons lost or gained to attain a noble gas configuration. For most main group elements, the ionic charges can be determined from

More information

Quick Review. - Chemical equations - Types of chemical reactions - Balancing chemical equations - Stoichiometry - Limiting reactant/reagent

Quick Review. - Chemical equations - Types of chemical reactions - Balancing chemical equations - Stoichiometry - Limiting reactant/reagent Quick Review - Chemical equations - Types of chemical reactions - Balancing chemical equations - Stoichiometry - Limiting reactant/reagent Water H 2 O Is water an ionic or a covalent compound? Covalent,

More information

Unit 3: Solubility Equilibrium

Unit 3: Solubility Equilibrium Unit 3: Chem 11 Review Preparation for Chem 11 Review Preparation for It is expected that the student understands the concept of: 1. Strong electrolytes, 2. Weak electrolytes and 3. Nonelectrolytes. CHEM

More information

Unit 3: Solubility Equilibrium

Unit 3: Solubility Equilibrium Unit 3: Chem 11 Review Preparation for Chem 11 Review Preparation for It is expected that the student understands the concept of: 1. Strong electrolytes, 2. Weak electrolytes and 3. Nonelectrolytes. CHEM

More information

The solvent is the dissolving agent -- i.e., the most abundant component of the solution

The 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 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

Precipitation Reactions

Precipitation Reactions Precipitation Reactions Precipitation reactions are reactions in which a solid forms when we mix two solutions reactions between aqueous solutions of ionic compounds produce an ionic compound that is insoluble

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 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

Chapter 15. Solutions

Chapter 15. Solutions Chapter 15 Solutions Key Terms for this Chapter Make sure you know the meaning of these: Solution Solute Solvent Aqueous solution Solubility Saturated Unsaturated Supersaturated Concentrated Dilute 15-2

More information

9.1 Water. Chapter 9 Solutions. Water. Water in Foods

9.1 Water. Chapter 9 Solutions. Water. Water in Foods Chapter 9 s 9.1 Water 9.1 Properties of Water 9.2 s 9.3 Electrolytes and Nonelectrolytes 9.6 Percent Concentration 9.7 Molarity Water is the most common solvent. The water molecule is polar. Hydrogen bonds

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

Solutions. Heterogenous Mixture (Not a Solution) Ice Water (w/ Ice Cubes) Smog Oil and Water

Solutions. Heterogenous Mixture (Not a Solution) Ice Water (w/ Ice Cubes) Smog Oil and Water Solutions Unit 6 1 Solutions Homogenous Mixture (Solution) two or more substances mixed together to have a uniform composition, its components are not distinguishable from one another Heterogenous Mixture

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

Introducing Driving Force #3 - Formation of a Solid

Introducing Driving Force #3 - Formation of a Solid Introducing Driving Force #3 - Formation of a Solid A solid that forms in an aqueous reaction is called a precipitate Precipitation reactions are also known as double replacement reactions Cations trade

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

A solution is a homogeneous mixture of two or more substances.

A solution is a homogeneous mixture of two or more substances. UNIT (5) SOLUTIONS A solution is a homogeneous mixture of two or more substances. 5.1 Terminology Solute and Solvent A simple solution has two components, a solute, and a solvent. The substance in smaller

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 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

Session 8: LECTURE OUTLINE (SECTIONS I1 I4 pp F61 F67)

Session 8: LECTURE OUTLINE (SECTIONS I1 I4 pp F61 F67) Session 8: LECTURE OUTLINE (SECTIONS I1 I4 pp F61 F67) I. Elecrolytes a. Soluble substances b. Insoluble substances c. Electrolytes d. Non-Electrolytes e. Ions and electrical conductivity f. Strong and

More information

Brass, a solid solution of Zn and Cu, is used to make musical instruments and many other objects.

Brass, a solid solution of Zn and Cu, is used to make musical instruments and many other objects. Brass, a solid solution of Zn and Cu, is used to make musical instruments and many other objects. 14.1 General Properties of Solutions 14.2 Solubility 14.3 Rate of Dissolving Solids 14.4 Concentration

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 - 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

Reactions in Aqueous Solutions

Reactions in Aqueous Solutions Copyright 2004 by houghton Mifflin Company. Reactions in Aqueous Solutions Chapter 7 All rights reserved. 1 7.1 Predicting if a Rxn Will Occur When chemicals are mixed and one of these driving forces can

More information

We CAN have molecular solutions (ex. sugar in water) but we will be only working with ionic solutions for this unit.

We CAN have molecular solutions (ex. sugar in water) but we will be only working with ionic solutions for this unit. Solubility Equilibrium The Basics (should be mostly review) Solubility is defined as the maximum amount of a substance which can be dissolved in a given solute at a given temperature. The solubility of

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

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

A reaction in which a solid forms is called a precipitation reaction. Solid = precipitate

A 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 information

Name: Period: Date: solution

Name: Period: Date: solution Name: Period: Date: ID: A Solutions Test A Matching Use the choices below to answer the following 5 questions. a. Hydrogen bond d. Electrolyte b. Polar molecule e. Nonelectrolyte c. Nonpolar molecule 1.

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

Unit 10 Solution Chemistry 1. Solutions & Molarity 2. Dissolving 3. Dilution 4. Calculation Ion Concentrations in Solution 5. Precipitation 6.

Unit 10 Solution Chemistry 1. Solutions & Molarity 2. Dissolving 3. Dilution 4. Calculation Ion Concentrations in Solution 5. Precipitation 6. Unit 10 Solution Chemistry 1. Solutions & Molarity 2. Dissolving 3. Dilution 4. Calculation Ion Concentrations in Solution 5. Precipitation 6. Formula, Complete, Net Ionic Equations 7. Qualitative Analysis

More information

CHEM 12 Unit 3 Review package (solubility)

CHEM 12 Unit 3 Review package (solubility) CHEM 12 Unit 3 Review package (solubility) 1. Which of the following combinations would form an ionic solid? A. Metalloid - metal B. Metal non-metal C. Metalloid metalloid D. Non-metal non-metal 2. Which

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

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

Solutions & Solubility: Net Ionic Equations (9.1 in MHR Chemistry 11)

Solutions & Solubility: Net Ionic Equations (9.1 in MHR Chemistry 11) Solutions & Solubility: Net Ionic Equations (9.1 in MHR Chemistry 11) 1 Solubility vs. Temperature 2 Solubility Table Anions SOLUBILITY Table 8.3 page 363 in MHR Cl Br I S OH SO CO 3 PO 3 SO 3 C 2 H 3

More information

Reactions in aqueous solutions Precipitation Reactions

Reactions in aqueous solutions Precipitation Reactions Reactions in aqueous solutions Precipitation Reactions Aqueous solutions Chemical reactions that occur in water are responsible for creation of cenotes. When carbon dioxide, CO2, dissolves in water, the

More information

1. Forming a Precipitate 2. Solubility Product Constant (One Source of Ions)

1. Forming a Precipitate 2. Solubility Product Constant (One Source of Ions) Chemistry 12 Solubility Equilibrium II Name: Date: Block: 1. Forming a Precipitate 2. Solubility Product Constant (One Source of Ions) Forming a Precipitate Example: A solution may contain the ions Ca

More information

Stoichiometry. Percent composition Part / whole x 100 = %

Stoichiometry. Percent composition Part / whole x 100 = % Stoichiometry Conversion factors 1 mole = 6.02 x 10 23 atoms (element) 1 mole = 6.02 x 10 23 molecules (covalent compounds) 1 mole = 6.02 x 10 23 formula units (ionic compounds) 1 mole (any gas @ STP)

More information

Reaction Classes. Precipitation Reactions

Reaction 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 information

Unit 10 Solution Chemistry 1. Solutions & Molarity 2. Dissolving 3. Dilution 4. Calculation Ion Concentrations in Solution 5. Precipitation 6.

Unit 10 Solution Chemistry 1. Solutions & Molarity 2. Dissolving 3. Dilution 4. Calculation Ion Concentrations in Solution 5. Precipitation 6. Unit 10 Solution Chemistry 1. Solutions & Molarity 2. Dissolving 3. Dilution 4. Calculation Ion Concentrations in Solution 5. Precipitation 6. Formula, Complete, Net Ionic Equations 7. Qualitative Analysis

More information

1 of 43 Boardworks Ltd Chemistry 11. Solution Chemistry

1 of 43 Boardworks Ltd Chemistry 11. Solution Chemistry 1 of 43 Boardworks Ltd 2009 Chemistry 11 Solution Chemistry Crash Course: Solutions 2 of 43 Boardworks Ltd 2009 https://www.youtube.com/watch?v=9h2f1bjr0p4&t=39s 3 of 43 Boardworks Ltd 2009 Solubility

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

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

Section 4: Aqueous Reactions

Section 4: Aqueous Reactions Section 4: Aqueous Reactions 1. Solution composition 2. Electrolytes and nonelectrolytes 3. Acids, bases, and salts 4. Neutralization ti reactions 5. Precipitation reactions 6. Oxidation/reduction reactions

More information

Chapter 10 Solutions. Introduction Concentration Introduction

Chapter 10 Solutions. Introduction Concentration Introduction Chapter 10 Solutions Introduction Solutions are homogeneous mixtures, i.e., mixtures whose properties are uniform throughout. Solutions are all around us. We live in a solution of gases called the atmosphere.

More information

Chemistry 20 Unit 3A Solutions FITB Notes. Topic A Classification of Solutions

Chemistry 20 Unit 3A Solutions FITB Notes. Topic A Classification of Solutions Chemistry 20 Unit 3A Solutions FITB Notes General Outcome: Topic A Classification of Solutions Matter is a substance with and A substance is a type of matter with one definite formula (elements, compounds)

More information

Chemistry. Approximate Timeline. Students are expected to keep up with class work when absent.

Chemistry. Approximate Timeline. Students are expected to keep up with class work when absent. Chemistry Name Hour Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 15 SOLUTIONS Day Plans for the day Assignment(s) for the day 1 Begin Chapter 15

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 Electrolytes and Precipitation Reactions. Dr. Sapna Gupta

Chapter 4 Electrolytes and Precipitation Reactions. Dr. Sapna Gupta Chapter 4 Electrolytes and Precipitation Reactions Dr. Sapna Gupta Aqueous Solutions Solution - a homogeneous mixture of solute + solvent Solute: the component that is dissolved Solvent: the component

More information

Solubility Equilibrium. Solutions. Dissociation Equations. April/May Chemistry 30

Solubility Equilibrium. Solutions. Dissociation Equations. April/May Chemistry 30 Solubility Equilibrium Chemistry 30 Solutions Mixture containing two or more components, but looks like one homogeneous substance Solute: dissolved substance Solvent: dissolving substance In this course:

More information

1 L = L = 434 ml

1 L = L = 434 ml CHEM 101A ARMSTRONG SOLUTIONS TO TOPIC B PROBLEMS 1) We do not need to calculate the original molarity of the solution; all we need is the number of moles of K + in 7.50 g of K 2 CO 3 : 7.50 g K 2 CO 3

More information

Net Ionic Equations. Making Sense of Chemical Reactions

Net Ionic Equations. Making Sense of Chemical Reactions Making Sense of Chemical Reactions Now that you have mastered writing balanced chemical equations it is time to take a deeper look at what is really taking place chemically in each reaction. There are

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

Solutions and Solubility. BHS Chemistry

Solutions and Solubility. BHS Chemistry Solutions and Solubility BHS Chemistry MATTER Yes Can it be separated by physical means? No MIXTURES Pure SUBSTANCES Yes Is the composition uniform? Can it be decomposed by regular chemical means? No Yes

More information

Solubility Rules and Net Ionic Equations

Solubility Rules and Net Ionic Equations Solubility Rules and Net Ionic Equations Why? Solubility of a salt depends upon the type of ions in the salt. Some salts are soluble in water and others are not. When two soluble salts are mixed together

More information

3. Liquid solutions: a. liquid - liquid Ex. vinegar b. solid - liquid Ex. salt water c. gas - liquid Ex. carbonated water in soda pop

3. Liquid solutions: a. liquid - liquid Ex. vinegar b. solid - liquid Ex. salt water c. gas - liquid Ex. carbonated water in soda pop Solution Chemistry Nature of Solutions solutions are homogeneous mixtures substances in solution are different from their solid, liquid or gas forms there should be no observable segregation of component

More information

Chapter 4. Aqueous Reactions and Solution Stoichiometry

Chapter 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 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

Solubility Reactions. objectives

Solubility Reactions. objectives Solubility Reactions objectives (#4 2) How do chemicals undergo a solubility reaction? (#4 2a) A student shall be able to identify if a reaction is a solubility reaction? (#4 2b) Students should be able

More information

CSUS Department of Chemistry Experiment 3 Chem.1A

CSUS Department of Chemistry Experiment 3 Chem.1A Experiment 3: Reactions in Aqueous Solutions: Pre lab Name: 10 points Due at the beginning of lab. Section: 1. Precipitation Reactions a. On the reverse side of this page or on a separate piece of paper,

More information

Chapter 18. Solubility and Complex- Ionic Equilibria

Chapter 18. Solubility and Complex- Ionic Equilibria Chapter 18 Solubility and Complex- Ionic Equilibria 1 The common ion effect Le Chatelier Why is AgCl less soluble in sea water than in fresh water? AgCl(s) Ag + + Cl Seawater contains NaCl 2 Problem: The

More information

Chemistry 121 Chapters 7& 8 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question.

Chemistry 121 Chapters 7& 8 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question. Chemistry 121 Chapters 7& 8 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1. A sample of carbon dioxide occupies 22.4 L at STP. Which of the

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

Solutions, Ions & Acids, Bases (Chapters 3-4) Example - Limiting Reagents. Percent Yield. Reaction Yields. Yield - example.

Solutions, Ions & Acids, Bases (Chapters 3-4) Example - Limiting Reagents. Percent Yield. Reaction Yields. Yield - example. Solutions, Ions & Acids, Bases (Chapters 3-4) Chem 107 T. Hughbanks Example - Limiting Reagents SiCl 4 is used in making computer chips. It is produced by the reaction: SiO 2 + 2 C + 2 Cl 2 SiCl 4 + 2

More information

Solutions, Ions & Acids, Bases (Chapters 3-4)

Solutions, Ions & Acids, Bases (Chapters 3-4) Solutions, Ions & Acids, Bases (Chapters 3-4) Chem 107 T. Hughbanks Example - Limiting Reagents SiCl 4 is used in making computer chips. It is produced by the reaction: SiO 2 + 2 C + 2 Cl 2 SiCl 4 + 2

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

Test bank for Chemistry An Introduction to General Organic and Biological Chemistry 12th Edition by Timberlake

Test bank for Chemistry An Introduction to General Organic and Biological Chemistry 12th Edition by Timberlake Test bank for Chemistry An Introduction to General Organic and Biological Chemistry 12th Edition by Timberlake Link download full: http://testbankair.com/download/test-bank-for-chemistry-an-introduction-to-general-organic-and-biological-chemistry-12th-edition-by-timberlak

More information

Solutions. Experiment 11. Various Types of Solutions. Solution: A homogenous mixture consisting of ions or molecules

Solutions. Experiment 11. Various Types of Solutions. Solution: A homogenous mixture consisting of ions or molecules Solutions Solution: A homogenous mixture consisting of ions or molecules -Assignment: Ch 15 Questions & Problems : 5, (15b,d), (17a, c), 19, 21, 23, 27, (33b,c), 39, (43c,d),45b, 47, (49b,d), (55a,b),

More information

Chapter 4. Properties of Aqueous Solutions. Electrolytes in Aqueous Solutions. Strong, weak, or nonelectrolyte. Electrolytic Properties

Chapter 4. Properties of Aqueous Solutions. Electrolytes in Aqueous Solutions. Strong, weak, or nonelectrolyte. Electrolytic Properties Chapter 4 Reactions in Aqueous Solution Observing and Predicting Reactions How do we know whether a reaction occurs? What observations indicate a reaction has occurred? In your groups, make a list of changes

More information

insoluble partial very soluble (< 0.1 g/100ml) solubility (> 1 g/100ml) Factors Affecting Solubility in Water

insoluble 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 information

Reactions in Aqueous Solutions

Reactions 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 information

SOLUBILITY REVIEW QUESTIONS

SOLUBILITY REVIEW QUESTIONS Solubility Problem Set 1 SOLUBILITY REVIEW QUESTIONS 1. What is the solubility of calcium sulphate in M, g/l, and g/100 ml? 2. What is the solubility of silver chromate? In a saturated solution of silver

More information

UNIT III: SOLUBILITY EQUILIBRIUM YEAR END REVIEW (Chemistry 12)

UNIT III: SOLUBILITY EQUILIBRIUM YEAR END REVIEW (Chemistry 12) I. Multiple Choice UNIT III: SOLUBILITY EQUILIBRIUM YEAR END REVIEW (Chemistry 12) 1) Which one of the following would form an ionic solution when dissolved in water? A. I 2 C. Ca(NO 3 ) 2 B. CH 3 OH D.

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

Solution Chemistry. Chapter 4

Solution Chemistry. Chapter 4 Solution Chemistry Chapter 4 Covalent Molecule Dissolving in Water Ionic Compound Dissolving in Water Electrolytes and Nonelectrolytes Electrolytes/Nonelectrolytes Type Dissociation Electrical Conductivity

More information

11.3 Reactions in Aqueous Essential Understanding Reactions that occur in aqueous solutions are double-replacement

11.3 Reactions in Aqueous Essential Understanding Reactions that occur in aqueous solutions are double-replacement 13. Is the following sentence true or false? Hydrocarbons, compounds of hydrogen and carbon, are often the reactants in combustion reactions. 14. Circle the letter of each compound that can be produced

More information

Describe the formation of an aqueous LiBr solution, when solid LiBr dissolves in water.

Describe the formation of an aqueous LiBr solution, when solid LiBr dissolves in water. Chapter 9 Solutions Practice Problems Section 9.1 Solutions Goal: Identify the solute and solvent in a solution; describe the formation of a solution. Summary: A solution forms when a solute dissolves

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

Chapter 15 Solutions

Chapter 15 Solutions Chapter 15 Solutions 1. A homogeneous mixture is a combination of two (or more) pure substances that is uniform in composition and appearance throughout. Examples of homogeneous mixtures in the real world

More information

Homework #3 Chapter 4 Types of Chemical Reactions and Solution Stoichiometry

Homework #3 Chapter 4 Types of Chemical Reactions and Solution Stoichiometry Homework #3 Chapter 4 Types of Chemical Reactions and Solution Stoichiometry 13. Determine the concentrations of the solutions Solution A 4 particles 1.0 L Solution B 6 paticles 4.0 L Solution C 4 particles

More information

SI session Grue 207A

SI session Grue 207A Chem 105 Wednesday 21 Sept 2011 1. Precipitation and Solubility 2. Solubility Rules 3. Precipitation reaction equations 4. Net ionic equations 5. OWL 6. Acids and bases SI session Grue 207A TR, 12:001:30

More information

October 19, 1999 Page 1. Chapter 4 Practice Worksheet Dr. Palmer Graves, Instructor MULTIPLE CHOICE

October 19, 1999 Page 1. Chapter 4 Practice Worksheet Dr. Palmer Graves, Instructor MULTIPLE CHOICE October 19, 1999 Page 1 MULTIPLE CHOICE Section 4.1 Some Ways that Chemical Reactions Occur 1. The reaction of HNO (aq) + KOH(aq) KNO (aq) + H O(l) is best classified as a(n) a) acid-base neutralization

More information

4.6 Describing Reactions in Solution

4.6 Describing Reactions in Solution 4.6 Describing Reactions in Solution The overall or formula equation for this reaction: K 2 CrO(aq) Ba(NO 3 ) 2 (aq) BaCrO 4 (s) 2KNO 3 (aq) Although the formula equation shows the reactants and products

More information

SOLUTIONS. Homogeneous mixture uniformly mixed on the molecular level. Solvent & Solute. we will focus on aqueous solutions

SOLUTIONS. Homogeneous mixture uniformly mixed on the molecular level. Solvent & Solute. we will focus on aqueous solutions SOLUTIONS Homogeneous mixture uniformly mixed on the molecular level Solvent & Solute we will focus on aqueous solutions SOLUTE-SOLVENT SOLVENT INTERACTIONS Why do solutions form? Processes occur spontaneously

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

CP Chapter 15/16 Solutions What Are Solutions?

CP Chapter 15/16 Solutions What Are Solutions? CP Chapter 15/16 Solutions What Are Solutions? What is a solution? A solution is uniform that may contain solids, liquids, or gases. Known as a mixture Solution = + o Solvent The substance in abundance

More information

Solutions. LiCl (s) + H2O (l) LiCl (aq) 3/12/2013. Definitions. Aqueous Solution. Solutions. How Does a Solution Form? Solute Solvent solution

Solutions. LiCl (s) + H2O (l) LiCl (aq) 3/12/2013. Definitions. Aqueous Solution. Solutions. How Does a Solution Form? Solute Solvent solution Solutions Definitions A solution is a homogeneous mixture A solute is dissolved in a solvent. solute is the substance being dissolved solvent is the liquid in which the solute is dissolved an aqueous solution

More information

5. Pb(IO 3) BaCO 3 8. (NH 4) 2SO 3

5. Pb(IO 3) BaCO 3 8. (NH 4) 2SO 3 Chemistry 11 Solution Chemistry II Name: Date: Block: 1. Ions in Solutions 2. Solubility Table 3. Separating Ions Ions in Solutions Ionization Equation - Represents the salt breaking apart into ions. Practice:

More information

Name Chemistry Pre-AP. Notes: Solutions

Name Chemistry Pre-AP. Notes: Solutions Name Chemistry Pre-AP Notes: Solutions Period I. Intermolecular Forces (IMFs) A. Attractions Between Molecules Attractions between molecules are called and are very important in determining the properties

More information

Review 7: Solubility Equilibria

Review 7: Solubility Equilibria Review 7: Solubility Equilibria Objectives: 1. Be able to write dissociation equations for ionic compounds dissolving in water. 2. Given Ksp, be able to determine the solubility of a substance in both

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

Settling? Filterable? Tyndall Effect? * 1 N N Y nm

Settling? Filterable? Tyndall Effect? * 1 N N Y nm Types of Mixtures Notes *What is the Tyndall Effect? When a light shines through a mixture, the beams of light scatter. Homogeneous or Heterogeneous # of visible phases Settling? Filterable? Tyndall Effect?

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

Reactions in Aqueous Solutions Chang & Goldsby modified by Dr. Hahn

Reactions in Aqueous Solutions Chang & Goldsby modified by Dr. Hahn Reactions in Aqueous Solutions Chang & Goldsby modified by Dr. Hahn Chapter 4 Copyright McGraw-Hill Education. All rights reserved. No reproduction or distribution without the prior written consent of

More information

Unit 1 - Foundations of Chemistry

Unit 1 - Foundations of Chemistry Unit 1 - Foundations of Chemistry Chapter 2 - Chemical Reactions Unit 1 - Foundations of Chemistry 1 / 42 2.1 - Chemical Equations Physical and Chemical Changes Physical change: A substance changes its

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 Collision A bag of mostly water - Star Trek - Rareness No mobility Solution is the solution. Water, the Common Solvent A bag of mostly

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

UNIT 8: SOLUTIONS. Essential Question: What kinds of properties affect a chemical s solubility?

UNIT 8: SOLUTIONS. Essential Question: What kinds of properties affect a chemical s solubility? UNIT 8: SOLUTIONS Essential Question: What kinds of properties affect a chemical s solubility? SOLUTIONS & THEIR CHARACTERISTICS (5) Most chemical reactions take place IN solutions 1. Homogeneous mixture

More information

INTRODUCTION TO SOLUBILITY UNIT 3A SOLUBILITY THEORY. There are three classes of compounds which can form ionic solutions:

INTRODUCTION TO SOLUBILITY UNIT 3A SOLUBILITY THEORY. There are three classes of compounds which can form ionic solutions: INTRODUCTION TO SOLUBILITY There are three classes of compounds which can form ionic solutions: Acids: HCl, H 2 SO 4, HNO 3 Bases: NaOH, KOH, NH 3 Chemistry 12 UNIT 3A SOLUBILITY THEORY Salts: NaCl, KMnO

More information