Composition of Solutions

Size: px
Start display at page:

Download "Composition of Solutions"

Transcription

1 Chapter 11 Solutions The Composition of Solutions The Solution Process Factors that Affect Solubility Measuring Concentrations of Solutions Quantities for Reactions That Occur in Aqueous Solution Colligative Solutions Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Composition of Solutions A solution is: A homogeneous mixture with uniform composition throughout Composed of: Solute Substance being dissolved Usually present in the lesser amount Solvent Substance doing the dissolving Usually present in the greater amount Composition of Solutions What is the solute? What is the solvent?

2 Composition of Solutions Figure 11.5 Solubility How readily or completely a solute dissolves in a solvent A soluble ionic compound dissociates into ions when dissolved in water. Insoluble compounds remain mostly undissociated in their ionic, crystalline structure. The solubilities for ionic compounds do not follow a predictable pattern Must be recalled from experimental data Solubility rules are listed in Table Ions Rules Used to Predict the Solubility of Ionic Salts Rules Na +, K +, NH 4 + NO 3 - SO 4 2- Cl -, Br -, I - Ag + O 2-, OH - S 2- CrO 4 2- CO 3 2-, PO 4 3-, SO 3 2-, SiO 3 2- Most salts of sodium, potassium, and ammonium ions are soluble. All nitrates are soluble. Most sulfates are soluble. Exceptions: BaSO 4, SrSO 4, PbSO 4, CaSO 4, Hg 2 SO 4, & Ag 2 SO 4 Most chlorides, bromides, and iodides are soluble. Exceptions: AgX, Hg 2 X, PbX 2, & HgI 2 (X = Cl, Br, or I) Silver salts, except AgNO 3, are insoluble. Oxides and hydroxides are insoluble. Exceptions: NaOH, KOH, Ba(OH) 2, & Ca(OH) 2 (somewhat soluble) Sulfides are insoluble. Exceptions: Salts of Na +, K +, NH 4 +, and the alkaline earth metal ions Most chromates are insoluble. Exceptions: Salts of Na +, K +, NH 4+, Mg 2+, Ca 2+, Al 3+, and Ni 2+ Most carbonates, phosphates, sulfites, and silicates are insoluble. Exceptions: Na +, K +, and NH

3 Electrolytes A solution that conducts electricity Two kinds of electrolytes: Strong electrolyte A solute that dissociates completely into ions in aqueous solution Weak electrolyte A solute that dissociates partially into ions in aqueous solution Nonelectrolyte A solute that does not dissociate into ions in aqueous solution Electrolytes Practice Composition of Solutions What ions, atoms, or molecules are present when the following substances are mixed with water? Write a balanced equation to represent the process of dissolving each substance in water. ZnCl 2 (s) KNO 3 (s) C 5 H 11 OH(l)

4 Practice Solutions Composition of Solutions ZnCl 2 (s) ZnCl 2 (s) + H 2 O(l) Zn 2+ (aq) + 2 Cl - (aq) KNO 3 (s) KNO 3 (s) + H 2 O(l) K + (aq) + NO 3- (aq) C 5 H 11 OH(l) C 5 H 11 OH(l) + H 2 O(l) C 5 H 11 O - (aq) + H + (aq) Does not dissolve extensively Like Dissolves Like When the bonding in a solvent is similar to the bonding in a solute, then the solute will dissolve in the solvent. Polar covalent solvents dissolve polar covalent solutes. Nonpolar covalent solvents dissolve nonpolar covalent solutes. See Table 11.2 below: Solute Polar Solvent Nonpolar Ionic Soluble Insoluble Polar Soluble Insoluble Nonpolar Insoluble Soluble Solution Process Figure

5 Solution Process Ion-dipole force An attraction between an ion and a polar molecule When an ionic compound dissolves in water: Ionic bonds in the solute break. Hydrogen bonds between water molecules break. Ion-dipole forces form between ions and water molecules. Solution Process Heat of Solution The difference between the energy required for separation of solute and solvent and the energy released upon formation of ion-dipole interactions When the solvation process provides more energy than is needed to separate the pure solvent and solvent particles, the heat of solution is negative, and the overall dissolving process is exothermic

6 Endothermic Solution Process Figure 11.14B Solution Process for Nonpolar- Nonpolar Interactions Entropy A measure of the tendency for matter to become disordered or random in its distribution Matter spontaneously changes from a state of order to a state of randomness, unless energy changes oppose it. Solutions form because the makeup of the solution naturally tends toward disorganization

7 Entropy Figure Practice The Solution Process Iodine (I 2 ) dissolves in hexane (C 6 H 14 ) to form a solution. Describe the forces that must be broken for the solution to form. Practice Solutions The Solution Process Iodine (I 2 ) dissolves in hexane (C 6 H 14 ) to form a solution. Describe the forces that must be broken for the solution to form. London forces must be broken to allow I 2, the solute, to dissolve. London forces must also be broken to allow C 6 H 14, the solvent, to dissolve

8 Factors that Affect Solubility Three factors affect solubility: Structure Temperature Pressure Structure For a solid to be soluble in a given solvent, the energy released by the solvation process must compensate for all of the energy required to break up the forces at work both within the solute and the solvent. Entropy is also a factor The solubility (or miscibility) of liquids in other liquids depends largely on the polarity of the solute and solvent molecules. Temperature Affects the solubility of most substances in water Most ionic solids are more soluble in water at higher temperatures Gases are less soluble as temperature increases Figure

9 Pressure Affects gases but not liquids or solids The solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid An increase in pressure results in an increase in solubility of a gas Pressure Figure Measuring Concentrations of Solutions Concentration The relative amounts of the solutes and solvent that make up the solution Concentrat ion = amount of solute amount of solution (or solvent) Solubility The ratio that identifies the maximum amount of a solute that will dissolve in a particular solvent to form a stable solution under specified conditions A measure of maximum concentration Three types of concentrated solution: Saturated solution Unsaturated solution Supersaturated solution

10 Saturated Solution A solution that contains the maximum possible amount of solute When this type of solution forms, a dynamic equilibrium is established. Undissolved solute continues to dissolve, but at the same time, previously dissolved solute is deposited from solution. Supersaturated Solution A solution that contains more than the maximum possible amount of solute Unsaturated solution A solution that contains less than the maximum possible amount of solute Figure Table 11.3: Concentration Units Unit Percent by mass Percent by volume Mass/volume percent Parts per million Parts per billion Molarity (M) Molality (m) grams of solute x 100% grams of solution volume of solute x 100% volume of solution grams of solute x 100% volume of solution grams of solute x 10 6 grams of solution grams of solute x 10 9 grams of solution moles of solute liters of solution moles of solute kilograms of solvent Definition

11 Percent by Mass Is calculated by dividing the solute mass by the mass of the solution and multiplying it by 100% Percent by mass = mass (solute) x 100% mass (solution) To find the mass of the solution, we can add the mass of the solute to the mass of the solvent. Percent by Mass Example: What is the percent-by-mass concentration of acetic acid (CH 3 CO 2 H) in a vinegar solution that contains 2.70 g of acetic acid and g of water? Percent by mass = mass (solute) x 100% mass (solution) Percent by mass = 2.70 g x 100% (2.70 g g) Percent by mass = 2.15% Percent by Volume Is calculated by dividing the solute volume by the solution volume and multiplying by 100% Percent by volume = volume (solute) x 100% volume (solution) The volume of the solution must be measured. Volumes are not additive like masses

12 Percent by Volume Example: To prepare a solution, we dissolve 205 ml of ethanol in sufficient water to give a total volume of 235 ml. What is the percent by volume concentration of ethanol? Percent by volume = volume (solute) x 100% volume (solution) Percent by volume = 205 ml x 100% 235 ml Percent by volume = 87.2% Mass/Volume Percent Is calculated by dividing the solute mass by the volume of solution and multiplying by 100% Mass/Volume Percent = grams of solute x 100% volume of solution Example: The concentration of NaCl in a saline bag is 0.9%. Therefore, for every 100 ml of solution, the mass of NaCl present is 0.9 g. Parts per Million and per Billion Parts per million Is calculated by dividing the mass of solute by the mass of solution and multiplying by 1 million (10 6 ) Parts per million = mass (solute) x 10 6 mass (solution) Parts per billion Is calculated by dividing the mass of solute by the mass of solution and multiplying by 1 billion (10 9 ) Parts per billion = mass (solute) x 10 9 mass (solution)

13 Molarity The ratio of moles of solute to the volume of solution in liters Molarity (M) = moles (solute) liters (solution) Example A solution contains 117 g of potassium hydroxide (KOH) dissolved in sufficient water to give a total volume of 2.00 L. The molar mass of KOH is g/mol. What is the molarity of the aqueous potassium hydroxide solution? Molarity Example A solution contains 117 g of potassium hydroxide (KOH) dissolved in sufficient water to give a total volume of 2.00 L. The molar mass of KOH is g/mol. What is the molarity of the aqueous potassium hydroxide solution? Molarity (M) = moles (solute) liters (solution) Moles KOH = 117 g KOH x 1 mol KOH = 2.09 mol KOH g KOH Molarity (M) = 2.09 mol KOH = 1.04 M KOH 2.00 L Molality If the temperature of a solution increases, the molarity of the solution changes because the volume changes. Molality does not change with temperature because it divides moles of solute with the mass of solution. molality (m) = moles (solute) kilograms (solution)

14 Molality Example A solution contains 56.7 g of potassium hydroxide (KOH) dissolved in sufficient water to give a total mass of g. The molar mass of KOH is g/mol. What is the molality of the aqueous potassium hydroxide solution? molality (m) = moles (solute) kilograms (solution) moles (solute) = 56.7 g KOH x 1 mol KOH = 1.01 mol KOH g KOH kilograms (solvent) = g x 1 kg = kg 1000 g Molality Example A solution contains 56.7 g of potassium hydroxide (KOH) dissolved in sufficient water to give a total mass of g. The molar mass of KOH is g/mol. What is the molality of the aqueous potassium hydroxide solution? molality (m) = moles (solute) kilograms (solution) molality (m) = 1.01 mol KOH = 4.11 m KOH kg KOH Precipitation Reactions The cation from one reactant combines with the anion from another reactant to form an insoluble compound, called a precipitate. Example When a solution of lead(ii) nitrate is mixed with a solution of potassium chromate, a yellow precipitate forms according to the equation: Pb(NO 3 ) 2 (aq) + K 2 CrO 4 (aq) 2 KNO 3 (aq) + PbCrO 4 (s) What volume of M lead(ii) nitrate is required to react with ml of M potassium chromate? What mass of PbCrO 4 solid forms?

15 Precipitation Reactions Pb(NO 3 ) 2 (aq) + K 2 CrO 4 (aq) 2 KNO 3 (aq) + PbCrO 4 (s) What volume of M lead(ii) nitrate is required to react with ml of M potassium chromate? What mass of PbCrO 4 solid forms? To solve for volume of Pb(NO 3 ) 2 : M x V = moles 100.0mL K 2 CrO 4 x moles K 2 CrO 4 = moles K 2 CrO ml K 2 CrO moles K 2 CrO 4 x 1 mol Pb(NO 3 ) 2 = moles Pb(NO 3 ) 2 1 mol K 2 CrO moles Pb(NO 3 ) 2 x 1 L Pb(NO 3 ) 2 = L Pb(NO 3 ) mol Pb(NO 3 ) 2 Precipitation Reactions Pb(NO 3 ) 2 (aq) + K 2 CrO 4 (aq) 2 KNO 3 (aq) + PbCrO 4 (s) What volume of M lead(ii) nitrate is required to react with ml of M potassium chromate? What mass of PbCrO 4 solid forms? To solve for volume of Pb(NO 3 ) 2 : M x V = moles moles K 2 CrO 4 * 1 mol PbCrO 4 = moles PbCrO 4 1 mol K 2 CrO moles PbCrO 4 * g PbCrO 4 = 3.88 g PbCrO 4 1 mol PbCrO 4 Acid-Base Titrations Titration The process of determining the concentration of one substance in solution by reacting it with a solution of another substance that has a known concentration Equivalence point The point in a titration at which the moles of the acid equal the moles of the base End point The point in a titration where the indicator changes color Slightly different than the equivalence point, but a good estimation

16 Acid-Base Titrations Practice - Acid-Base Titrations We need ml of M HCl solution to completely titrate ml of Ba(OH) 2 solution of unknown concentration. What is the molarity of the barium hydroxide solution? Practice Solutions - Acid- Base Titrations We need ml of M HCl solution to completely titrate ml of Ba(OH) 2 solution of unknown concentration. What is the molarity of the barium hydroxide solution? First, write the balanced chemical equation: 2 HCl(aq) + Ba(OH) 2 (aq) BaCl 2 (aq) + 2 H 2 O(l) Next, find the moles of HCl: ml HCl x moles HCl 1000 ml HCl = x 10-3 moles HCl

17 Practice Solutions - Acid-Base Titrations HCl(aq) + Ba(OH) 2 (aq) BaCl 2 (aq) + H 2 O(l) Next, we need to find the volume (in L) of Ba(OH) 2 : ml Ba(OH) 1liter Ba(OH) = 2 2 x L Ba(OH) ml Ba(OH) 2 Finally, divide the moles of Ba(OH) 2 by the volume of Ba(OH) 2 : x 10 moles Ba(OH) Molarity [Ba(OH) = ] = M Ba(OH) L Ba(OH) 2 Acid-Base Titrations Volume of Reactant M reactant Moles of Reactant mole ratio Moles of Product M product Volume of Product Colligative Properties A property that does not depend on the identity of a solute in solution Vary only with the number of solute particles present in a specific quantity of solvent 4 colligative properties: Osmotic pressure Vapor pressure lowering Boiling point elevation Freezing point depression

18 Osmotic Pressure Osmosis A process in which solvent molecules diffuse through a barrier that does not allow the passage of solute particles The barrier is called a semipermeable membrane. A membrane that allows the passage of some substances but not others Osmotic Pressure Pressure that can be exerted on the solution to prevent osmosis Osmotic Pressure Figure Vapor Pressure Lowering Solutes come in 2 forms: Volatile Solutes that readily form a gas Nonvolatile Solutes that DO NOT readily form a gas Generally, the addition of a solute lowers the vapor pressure of a solution when compared to the pure solvent

19 Vapor Pressure Lowering Phase Diagram Boiling Point Elevation The addition of solute affects the boiling point because it affects the vapor pressure. The boiling point is raised with the addition of solute in comparison to the pure solvent. An equation that gives the increase in boiling point: T b = K b m Where T b is the increase in temperature from the pure solvent s boiling point, K b is the boiling point constant, which is characteristic of a particular solvent, and m is the molality (moles of solute per kg of solution)

20 Freezing Point Depression The freezing point is lowered with the addition of solute in comparison to the pure solvent. An equation that gives the decrease in freezing point: T f = K f m Where T f is the decrease in temperature from the pure solvent s freezing point, K f is the freezing point constant, which is characteristic of a particular solvent, and m is the molality (moles of solute per kg of solution) Practice Freezing Point Depression What is the change in freezing point for a 1.5 m solution of sucrose in water? Practice Solutions Freezing Point Depression What is the change in freezing point for a 1.5 m solution of sucrose in water? K f (water) = C/m T f = K f m T f = C * 1.5 m = C m

21 Colligative Properties and Strong Electrolytes Strong electrolytes dissociate most of the time into their constituent ions. Therefore, the number of particles (in this case ions) increases with the number of ions. Colligative properties are proportional to number of particles in solution. Example: MgCl 2 (s) Mg 2+ (aq) + 2 Cl - (aq) In this case the number of particles increases to 3 particles. Therefore, we would multiply the colligative property amount by 3. Practice Strong vs. Weak Electrolytes Which of the following aqueous solutions is expected to have the lowest freezing point? 0.5 m CH 3 CH 2 OH 0.5 m Ca(NO 3 ) m KBr Practice Solutions Strong vs. Weak Electrolytes Which of the following aqueous solutions is expected to have the lowest freezing point? 0.5 m CH 3 CH 2 OH 0.5 m Ca(NO 3 ) m KBr Because the molalities are the same, we only need to concentrate on the number of particles generated by each solute. CH 3 CH 2 OH will not dissociate into ions, Ca(NO 3 ) 2 dissociates into 3 ions, and KBr dissociates into 2 ions. Therefore, the largest number of particles is generated by Ca(NO 3 ) 2 and it will have the lowest freezing point

Chapter 14 Solutions

Chapter 14 Solutions Chapter 14 Solutions 1 14.1 General properties of solutions solution a system in which one or more substances are homogeneously mixed or dissolved in another substance two components in a solution: solute

More information

Chemistry 51 Chapter 8 TYPES OF SOLUTIONS. A solution is a homogeneous mixture of two substances: a solute and a solvent.

Chemistry 51 Chapter 8 TYPES OF SOLUTIONS. A solution is a homogeneous mixture of two substances: a solute and a solvent. 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

Chemistry Ch 15 (Solutions) Study Guide Introduction

Chemistry Ch 15 (Solutions) Study Guide Introduction Chemistry Ch 15 (Solutions) Study Guide Introduction Name: Note: a word marked (?) is a vocabulary word you should know the meaning of. A homogeneous (?) mixture, or, is a mixture in which the individual

More information

Solution a homogeneous mixture = A solvent + solute(s) Aqueous solution water is the solvent

Solution a homogeneous mixture = A solvent + solute(s) Aqueous solution water is the solvent Solution a homogeneous mixture = A solvent + solute(s) Aqueous solution water is the solvent Water a polar solvent: dissolves most ionic compounds as well as many molecular compounds Aqueous solution:

More information

6 Reactions in Aqueous Solutions

6 Reactions in Aqueous Solutions 6 Reactions in Aqueous Solutions Water is by far the most common medium in which chemical reactions occur naturally. It is not hard to see this: 70% of our body mass is water and about 70% of the surface

More information

Chemistry B11 Chapter 6 Solutions and Colloids

Chemistry B11 Chapter 6 Solutions and Colloids Chemistry B11 Chapter 6 Solutions and Colloids Solutions: solutions have some properties: 1. The distribution of particles in a solution is uniform. Every part of the solution has exactly the same composition

More information

Aqueous Solutions. Water is the dissolving medium, or solvent. Some Properties of Water. A Solute. Types of Chemical Reactions.

Aqueous Solutions. Water is the dissolving medium, or solvent. Some Properties of Water. A Solute. Types of Chemical Reactions. Aqueous Solutions and Solution Stoichiometry Water is the dissolving medium, or solvent. Some Properties of Water Water is bent or V-shaped. The O-H bonds are covalent. Water is a polar molecule. Hydration

More information

stoichiometry = the numerical relationships between chemical amounts in a reaction.

stoichiometry = the numerical relationships between chemical amounts in a reaction. 1 REACTIONS AND YIELD ANSWERS stoichiometry = the numerical relationships between chemical amounts in a reaction. 2C 8 H 18 (l) + 25O 2 16CO 2 (g) + 18H 2 O(g) From the equation, 16 moles of CO 2 (a greenhouse

More information

MOLARITY = (moles solute) / (vol.solution in liter units)

MOLARITY = (moles solute) / (vol.solution in liter units) CHEM 101/105 Stoichiometry, as applied to Aqueous Solutions containing Ionic Solutes Lect-05 MOLES - a quantity of substance. Quantities of substances can be expressed as masses, as numbers, or as moles.

More information

Tutorial 4 SOLUTION STOICHIOMETRY. Solution stoichiometry calculations involve chemical reactions taking place in solution.

Tutorial 4 SOLUTION STOICHIOMETRY. Solution stoichiometry calculations involve chemical reactions taking place in solution. T-27 Tutorial 4 SOLUTION STOICHIOMETRY Solution stoichiometry calculations involve chemical reactions taking place in solution. Of the various methods of expressing solution concentration the most convenient

More information

SAMPLE PROBLEM 8.1. Solutions of Electrolytes and Nonelectrolytes SOLUTION STUDY CHECK

SAMPLE PROBLEM 8.1. Solutions of Electrolytes and Nonelectrolytes SOLUTION STUDY CHECK Solutions of Electrolytes and Nonelectrolytes SAMPLE PROBLEM 8.1 Indicate whether solutions of each of the following contain only ions, only molecules, or mostly molecules and a few ions: a. Na 2 SO 4,

More information

Chapter 8: Chemical Equations and Reactions

Chapter 8: Chemical Equations and Reactions Chapter 8: Chemical Equations and Reactions I. Describing Chemical Reactions A. A chemical reaction is the process by which one or more substances are changed into one or more different substances. A chemical

More information

Chapter 7: Chemical Reactions

Chapter 7: Chemical Reactions Chapter 7 Page 1 Chapter 7: Chemical Reactions A chemical reaction: a process in which at least one new substance is formed as the result of a chemical change. A + B C + D Reactants Products Evidence that

More information

Experiment 1 Chemical Reactions and Net Ionic Equations

Experiment 1 Chemical Reactions and Net Ionic Equations Experiment 1 Chemical Reactions and Net Ionic Equations I. Objective: To predict the products of some displacement reactions and write net ionic equations. II. Chemical Principles: A. Reaction Types. Chemical

More information

Chemical Equations. Chemical Equations. Chemical reactions describe processes involving chemical change

Chemical Equations. Chemical Equations. Chemical reactions describe processes involving chemical change Chemical Reactions Chemical Equations Chemical reactions describe processes involving chemical change The chemical change involves rearranging matter Converting one or more pure substances into new pure

More information

IB Chemistry 1 Mole. One atom of C-12 has a mass of 12 amu. One mole of C-12 has a mass of 12 g. Grams we can use more easily.

IB Chemistry 1 Mole. One atom of C-12 has a mass of 12 amu. One mole of C-12 has a mass of 12 g. Grams we can use more easily. The Mole Atomic mass units and atoms are not convenient units to work with. The concept of the mole was invented. This was the number of atoms of carbon-12 that were needed to make 12 g of carbon. 1 mole

More information

UNIT (4) CALCULATIONS AND CHEMICAL REACTIONS

UNIT (4) CALCULATIONS AND CHEMICAL REACTIONS UNIT (4) CALCULATIONS AND CHEMICAL REACTIONS 4.1 Formula Masses Recall that the decimal number written under the symbol of the element in the periodic table is the atomic mass of the element. 1 7 8 12

More information

Name: Class: Date: 2 4 (aq)

Name: Class: Date: 2 4 (aq) Name: Class: Date: Unit 4 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1) The balanced molecular equation for complete neutralization of

More information

Chapter 13: Properties of Solutions

Chapter 13: Properties of Solutions Chapter 13: Properties of Solutions Problems: 9-10, 13-17, 21-42, 44, 49-60, 71-72, 73 (a,c), 77-79, 84(a-c), 91 solution: homogeneous mixture of a solute dissolved in a solvent solute: solvent: component(s)

More information

Molarity of Ions in Solution

Molarity of Ions in Solution APPENDIX A Molarity of Ions in Solution ften it is necessary to calculate not only the concentration (in molarity) of a compound in aqueous solution but also the concentration of each ion in aqueous solution.

More information

General Chemistry II Chapter 20

General Chemistry II Chapter 20 1 General Chemistry II Chapter 0 Ionic Equilibria: Principle There are many compounds that appear to be insoluble in aqueous solution (nonelectrolytes). That is, when we add a certain compound to water

More information

Solubility Product Constant

Solubility Product Constant Solubility Product Constant Page 1 In general, when ionic compounds dissolve in water, they go into solution as ions. When the solution becomes saturated with ions, that is, unable to hold any more, the

More information

Answers and Solutions to Text Problems

Answers and Solutions to Text Problems 9 Answers and Solutions to Text Problems 9.1 a. δ O δ + δ + H H In a water molecule, the oxygen has a partial negative charge and the hydrogens have partial positive charges. b. δ δ + O H δ + δ + δ H H

More information

Sample Test 1 SAMPLE TEST 1. CHAPTER 12

Sample Test 1 SAMPLE TEST 1. CHAPTER 12 13 Sample Test 1 SAMPLE TEST 1. CHAPTER 12 1. The molality of a solution is defined as a. moles of solute per liter of solution. b. grams of solute per liter of solution. c. moles of solute per kilogram

More information

Chemistry: Chemical Equations

Chemistry: Chemical Equations Chemistry: Chemical Equations Write a balanced chemical equation for each word equation. Include the phase of each substance in the equation. Classify the reaction as synthesis, decomposition, single replacement,

More information

Aqueous Ions and Reactions

Aqueous Ions and Reactions Aqueous Ions and Reactions (ions, acids, and bases) Demo NaCl(aq) + AgNO 3 (aq) AgCl (s) Two clear and colorless solutions turn to a cloudy white when mixed Demo Special Light bulb in water can test for

More information

Balancing Chemical Equations Worksheet

Balancing Chemical Equations Worksheet Balancing Chemical Equations Worksheet Student Instructions 1. Identify the reactants and products and write a word equation. 2. Write the correct chemical formula for each of the reactants and the products.

More information

REVIEW QUESTIONS Chapter 8

REVIEW QUESTIONS Chapter 8 Chemistry 51 ANSWER KEY REVIEW QUESTIONS Chapter 8 1. Identify each of the diagrams below as strong electrolyte, weak electrolyte or non-electrolyte: (a) Non-electrolyte (no ions present) (b) Weak electrolyte

More information

Chapter 13 & 14 Practice Exam

Chapter 13 & 14 Practice Exam Name: Class: Date: Chapter 13 & 14 Practice Exam Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Acids generally release H 2 gas when they react with a.

More information

W1 WORKSHOP ON STOICHIOMETRY

W1 WORKSHOP ON STOICHIOMETRY INTRODUCTION W1 WORKSHOP ON STOICHIOMETRY These notes and exercises are designed to introduce you to the basic concepts required to understand a chemical formula or equation. Relative atomic masses of

More information

Steps for balancing a chemical equation

Steps for balancing a chemical equation The Chemical Equation: A Chemical Recipe Dr. Gergens - SD Mesa College A. Learn the meaning of these arrows. B. The chemical equation is the shorthand notation for a chemical reaction. A chemical equation

More information

13.3 Factors Affecting Solubility Solute-Solvent Interactions Pressure Effects Temperature Effects

13.3 Factors Affecting Solubility Solute-Solvent Interactions Pressure Effects Temperature Effects Week 3 Sections 13.3-13.5 13.3 Factors Affecting Solubility Solute-Solvent Interactions Pressure Effects Temperature Effects 13.4 Ways of Expressing Concentration Mass Percentage, ppm, and ppb Mole Fraction,

More information

Experiment 5. Chemical Reactions A + X AX AX A + X A + BX AX + B AZ + BX AX + BZ

Experiment 5. Chemical Reactions A + X AX AX A + X A + BX AX + B AZ + BX AX + BZ Experiment 5 Chemical Reactions OBJECTIVES 1. To observe the various criteria that are used to indicate that a chemical reaction has occurred. 2. To convert word equations into balanced inorganic chemical

More information

1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) 3 (s) + H 2 (g)

1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) 3 (s) + H 2 (g) 1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) (s) + H 2 (g) A) 1 B) 2 C) 4 D) 5 E) Al (s) + H 2 O (l)? Al(OH) (s) + H 2 (g) Al (s) + H 2 O (l)? Al(OH)

More information

1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436 #1, 7, 8, 11

1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436 #1, 7, 8, 11 SCH3U- R.H.KING ACADEMY SOLUTION & ACID/BASE WORKSHEET Name: The importance of water - MAKING CONNECTION READING 1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436

More information

Experiment 8 - Double Displacement Reactions

Experiment 8 - Double Displacement Reactions Experiment 8 - Double Displacement Reactions A double displacement reaction involves two ionic compounds that are dissolved in water. In a double displacement reaction, it appears as though the ions are

More information

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. A.P. Chemistry Practice Test: Ch. 11, Solutions Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Formation of solutions where the process is

More information

SCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, "Chemistry 11", McGraw-Hill Ryerson, 2001

SCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, Chemistry 11, McGraw-Hill Ryerson, 2001 SCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, "Chemistry 11", McGraw-Hill Ryerson, 2001 1. A small pin contains 0.0178 mol of iron. How many atoms of iron are in the pin? 2. A sample

More information

2. DECOMPOSITION REACTION ( A couple have a heated argument and break up )

2. DECOMPOSITION REACTION ( A couple have a heated argument and break up ) TYPES OF CHEMICAL REACTIONS Most reactions can be classified into one of five categories by examining the types of reactants and products involved in the reaction. Knowing the types of reactions can help

More information

Ch 8.5 Solution Concentration Units % (m/m or w/w) = mass of solute x 100 total mass of solution mass of solution = mass solute + mass solvent

Ch 8.5 Solution Concentration Units % (m/m or w/w) = mass of solute x 100 total mass of solution mass of solution = mass solute + mass solvent 1 Ch 8.5 Solution Concentration Units % (m/m or w/w) = mass of solute x 100 total mass of solution mass of solution = mass solute + mass solvent % (v/v) = volume of solute x 100 volume of solution filled

More information

Stoichiometry and Aqueous Reactions (Chapter 4)

Stoichiometry and Aqueous Reactions (Chapter 4) Stoichiometry and Aqueous Reactions (Chapter 4) Chemical Equations 1. Balancing Chemical Equations (from Chapter 3) Adjust coefficients to get equal numbers of each kind of element on both sides of arrow.

More information

Solutions. Chapter 13. Properties of Solutions. Lecture Presentation

Solutions. Chapter 13. Properties of Solutions. Lecture Presentation Lecture Presentation Chapter 13 Properties of Yonsei University homogeneous mixtures of two or more pure substances: may be gases, liquids, or solids In a solution, the solute is dispersed uniformly throughout

More information

IB Chemistry. DP Chemistry Review

IB Chemistry. DP Chemistry Review DP Chemistry Review Topic 1: Quantitative chemistry 1.1 The mole concept and Avogadro s constant Assessment statement Apply the mole concept to substances. Determine the number of particles and the amount

More information

Santa Monica College Chemistry 11

Santa Monica College Chemistry 11 Types of Reactions Objectives The objectives of this laboratory are as follows: To perform and observe the results of a variety of chemical reactions. To become familiar with the observable signs of chemical

More information

CHEMICAL REACTIONS. Chemistry 51 Chapter 6

CHEMICAL REACTIONS. Chemistry 51 Chapter 6 CHEMICAL REACTIONS A chemical reaction is a rearrangement of atoms in which some of the original bonds are broken and new bonds are formed to give different chemical structures. In a chemical reaction,

More information

Formulae, stoichiometry and the mole concept

Formulae, stoichiometry and the mole concept 3 Formulae, stoichiometry and the mole concept Content 3.1 Symbols, Formulae and Chemical equations 3.2 Concept of Relative Mass 3.3 Mole Concept and Stoichiometry Learning Outcomes Candidates should be

More information

CHEMISTRY II FINAL EXAM REVIEW

CHEMISTRY II FINAL EXAM REVIEW Name Period CHEMISTRY II FINAL EXAM REVIEW Final Exam: approximately 75 multiple choice questions Ch 12: Stoichiometry Ch 5 & 6: Electron Configurations & Periodic Properties Ch 7 & 8: Bonding Ch 14: Gas

More information

ATOMS. Multiple Choice Questions

ATOMS. Multiple Choice Questions Chapter 3 ATOMS AND MOLECULES Multiple Choice Questions 1. Which of the following correctly represents 360 g of water? (i) 2 moles of H 2 0 (ii) 20 moles of water (iii) 6.022 10 23 molecules of water (iv)

More information

PART I: MULTIPLE CHOICE (30 multiple choice questions. Each multiple choice question is worth 2 points)

PART I: MULTIPLE CHOICE (30 multiple choice questions. Each multiple choice question is worth 2 points) CHEMISTRY 123-07 Midterm #1 Answer key October 14, 2010 Statistics: Average: 74 p (74%); Highest: 97 p (95%); Lowest: 33 p (33%) Number of students performing at or above average: 67 (57%) Number of students

More information

Chemical Reactions 2 The Chemical Equation

Chemical Reactions 2 The Chemical Equation Chemical Reactions 2 The Chemical Equation INFORMATION Chemical equations are symbolic devices used to represent actual chemical reactions. The left side of the equation, called the reactants, is separated

More information

Unit 10A Stoichiometry Notes

Unit 10A Stoichiometry Notes Unit 10A Stoichiometry Notes Stoichiometry is a big word for a process that chemist s use to calculate amounts in reactions. It makes use of the coefficient ratio set up by balanced reaction equations

More information

4.1 Aqueous Solutions. Chapter 4. Reactions in Aqueous Solution. Electrolytes. Strong Electrolytes. Weak Electrolytes

4.1 Aqueous Solutions. Chapter 4. Reactions in Aqueous Solution. Electrolytes. Strong Electrolytes. Weak Electrolytes Chapter 4 Reactions in Aqueous Solution 4.1 Aqueous Solutions Solution homogeneous mixture of 2 or more substances Solute the substance present in a smaller amount (usually solid in Chap. 4) Solvent the

More information

Name period Unit 9: acid/base equilibrium

Name period Unit 9: acid/base equilibrium Name period Unit 9: acid/base equilibrium 1. What is the difference between the Arrhenius and the BronstedLowry definition of an acid? Arrhenious acids give H + in water BronstedLowry acids are proton

More information

ph: Measurement and Uses

ph: Measurement and Uses ph: Measurement and Uses One of the most important properties of aqueous solutions is the concentration of hydrogen ion. The concentration of H + (or H 3 O + ) affects the solubility of inorganic and organic

More information

Chapter 4 Chemical Reactions

Chapter 4 Chemical Reactions Chapter 4 Chemical Reactions I) Ions in Aqueous Solution many reactions take place in water form ions in solution aq solution = solute + solvent solute: substance being dissolved and present in lesser

More information

EXPERIMENT 10 Chemistry 110. Solutions Part 2 ACIDS, BASES, AND ELECTROLYTES

EXPERIMENT 10 Chemistry 110. Solutions Part 2 ACIDS, BASES, AND ELECTROLYTES EXPERIMENT 10 Chemistry 110 Solutions Part 2 ACIDS, BASES, AND ELECTROLYTES PURPOSE: The purpose of this experiment is to determine the properties of solutions of acids, bases and electrolytes. Students

More information

Chemical Reactions in Water Ron Robertson

Chemical Reactions in Water Ron Robertson Chemical Reactions in Water Ron Robertson r2 f:\files\courses\1110-20\2010 possible slides for web\waterchemtrans.doc Properties of Compounds in Water Electrolytes and nonelectrolytes Water soluble compounds

More information

Chemistry B11 Chapter 4 Chemical reactions

Chemistry B11 Chapter 4 Chemical reactions Chemistry B11 Chapter 4 Chemical reactions Chemical reactions are classified into five groups: A + B AB Synthesis reactions (Combination) H + O H O AB A + B Decomposition reactions (Analysis) NaCl Na +Cl

More information

Freezing Point Depression: Why Don t Oceans Freeze? Teacher Advanced Version

Freezing Point Depression: Why Don t Oceans Freeze? Teacher Advanced Version Freezing Point Depression: Why Don t Oceans Freeze? Teacher Advanced Version Freezing point depression describes the process where the temperature at which a liquid freezes is lowered by adding another

More information

Liquid phase. Balance equation Moles A Stoic. coefficient. Aqueous phase

Liquid phase. Balance equation Moles A Stoic. coefficient. Aqueous phase STOICHIOMETRY Objective The purpose of this exercise is to give you some practice on some Stoichiometry calculations. Discussion The molecular mass of a compound is the sum of the atomic masses of all

More information

Solution. Practice Exercise. Concept Exercise

Solution. Practice Exercise. Concept Exercise Example Exercise 8.1 Evidence for a Reaction Which of the following is experimental evidence for a chemical reaction? (a) Pouring vinegar on baking soda gives foamy bubbles. (b) Mixing two solutions produces

More information

48 Practice Problems for Ch. 17 - Chem 1C - Joseph

48 Practice Problems for Ch. 17 - Chem 1C - Joseph 48 Practice Problems for Ch. 17 - Chem 1C - Joseph 1. Which of the following concentration measures will change in value as the temperature of a solution changes? A) mass percent B) mole fraction C) molality

More information

Copyright 2009 by Pearson Education, Inc. Upper Saddle River, New Jersey 07458 All rights reserved.

Copyright 2009 by Pearson Education, Inc. Upper Saddle River, New Jersey 07458 All rights reserved. Sample Exercise 17.1 Calculating the ph When a Common Ion is Involved What is the ph of a solution made by adding 0.30 mol of acetic acid and 0.30 mol of sodium acetate to enough water to make 1.0 L of

More information

Chem101: General Chemistry Lecture 9 Acids and Bases

Chem101: General Chemistry Lecture 9 Acids and Bases : General Chemistry Lecture 9 Acids and Bases I. Introduction A. In chemistry, and particularly biochemistry, water is the most common solvent 1. In studying acids and bases we are going to see that water

More information

Chapter 11 Properties of Solutions

Chapter 11 Properties of Solutions Chapter 11 Properties of Solutions 11.1 Solution Composition A. Molarity moles solute 1. Molarity ( M ) = liters of solution B. Mass Percent mass of solute 1. Mass percent = 1 mass of solution C. Mole

More information

CHEM 36 General Chemistry EXAM #1 February 13, 2002

CHEM 36 General Chemistry EXAM #1 February 13, 2002 CHEM 36 General Chemistry EXAM #1 February 13, 2002 Name: Serkey, Anne INSTRUCTIONS: Read through the entire exam before you begin. Answer all of the questions. For questions involving calculations, show

More information

Other Stoich Calculations A. mole mass (mass mole) calculations. GIVEN mol A x CE mol B. PT g A CE mol A MOLE MASS :

Other Stoich Calculations A. mole mass (mass mole) calculations. GIVEN mol A x CE mol B. PT g A CE mol A MOLE MASS : Chem. I Notes Ch. 12, part 2 Using Moles NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. 1 MOLE = 6.02 x 10 23 representative particles (representative particles

More information

Chapter 17. The best buffer choice for ph 7 is NaH 2 PO 4 /Na 2 HPO 4. 19)

Chapter 17. The best buffer choice for ph 7 is NaH 2 PO 4 /Na 2 HPO 4. 19) Chapter 17 2) a) HCl and CH 3 COOH are both acids. A buffer must have an acid/base conjugate pair. b) NaH 2 PO 4 and Na 2 HPO 4 are an acid/base conjugate pair. They will make an excellent buffer. c) H

More information

Chapter 5. Chemical Reactions and Equations. Introduction. Chapter 5 Topics. 5.1 What is a Chemical Reaction

Chapter 5. Chemical Reactions and Equations. Introduction. Chapter 5 Topics. 5.1 What is a Chemical Reaction Introduction Chapter 5 Chemical Reactions and Equations Chemical reactions occur all around us. How do we make sense of these changes? What patterns can we find? 1 2 Copyright The McGraw-Hill Companies,

More information

CHAPTER 5: MOLECULES AND COMPOUNDS

CHAPTER 5: MOLECULES AND COMPOUNDS CHAPTER 5: MOLECULES AND COMPOUNDS Problems: 1-6, 9-13, 16, 20, 31-40, 43-64, 65 (a,b,c,e), 66(a-d,f), 69(a-d,f), 70(a-e), 71-78, 81-82, 87-96 A compound will display the same properties (e.g. melting

More information

Chapter 13. Properties of Solutions

Chapter 13. Properties of Solutions Sample Exercise 13.1 (p. 534) By the process illustrated below, water vapor reacts with excess solid sodium sulfate to form the hydrated form of the salt. The chemical reaction is Na 2 SO 4(s) + 10 H 2

More information

Chemical Equations and Chemical Reactions. Chapter 8.1

Chemical Equations and Chemical Reactions. Chapter 8.1 Chemical Equations and Chemical Reactions Chapter 8.1 Objectives List observations that suggest that a chemical reaction has taken place List the requirements for a correctly written chemical equation.

More information

Chapter 13 Properties of Solutions

Chapter 13 Properties of Solutions Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 13 Properties of are homogeneous mixtures of two or more pure substances. In a solution,

More information

David A. Katz Department of Chemistry Pima Community College

David A. Katz Department of Chemistry Pima Community College Solutions David A. Katz Department of Chemistry Pima Community College A solution is a HOMOGENEOUS mixture of 2 or more substances in a single phase. One constituent t is usually regarded as the SOLVENT

More information

Moles. Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Equations

Moles. Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Equations Moles Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Equations Micro World atoms & molecules Macro World grams Atomic mass is the mass of an

More information

Chemical Equations & Stoichiometry

Chemical Equations & Stoichiometry Chemical Equations & Stoichiometry Chapter Goals Balance equations for simple chemical reactions. Perform stoichiometry calculations using balanced chemical equations. Understand the meaning of the term

More information

CST Practice Test. Multiple Choice Questions

CST Practice Test. Multiple Choice Questions CST Practice Test Young NAME CST Practice Test Multiple Choice Questions 1) At 1 atm and 298 K, which of the K a values listed below represents the strongest acid? 5) Which electron-dot symbol represents

More information

CP Chemistry Review for Stoichiometry Test

CP Chemistry Review for Stoichiometry Test CP Chemistry Review for Stoichiometry Test Stoichiometry Problems (one given reactant): 1. Make sure you have a balanced chemical equation 2. Convert to moles of the known substance. (Use the periodic

More information

Writing and Balancing Chemical Equations

Writing and Balancing Chemical Equations Name Writing and Balancing Chemical Equations Period When a substance undergoes a chemical reaction, chemical bonds are broken and new bonds are formed. This results in one or more new substances, often

More information

CHEMICAL DETERMINATION OF EVERYDAY HOUSEHOLD CHEMICALS

CHEMICAL DETERMINATION OF EVERYDAY HOUSEHOLD CHEMICALS CHEMICAL DETERMINATION OF EVERYDAY HOUSEHOLD CHEMICALS Purpose: It is important for chemists to be able to determine the composition of unknown chemicals. This can often be done by way of chemical tests.

More information

Number of moles of solute = Concentration (mol. L ) x Volume of solution (litres) or n = C x V

Number of moles of solute = Concentration (mol. L ) x Volume of solution (litres) or n = C x V 44 CALCULATIONS INVOLVING SOLUTIONS INTRODUCTION AND DEFINITIONS Many chemical reactions take place in aqueous (water) solution. Quantities of such solutions are measured as volumes, while the amounts

More information

- electrolytes: substances that dissolve in water to form charge-carrying solutions

- electrolytes: substances that dissolve in water to form charge-carrying solutions 111 Electrolytes and Ionic Theory - electrolytes: substances that dissolve in water to form charge-carrying solutions * Electrolytes form ions in solution - (ions that are mobile are able to carry charge!).

More information

Moles. Moles. Moles. Moles. Balancing Eqns. Balancing. Balancing Eqns. Symbols Yields or Produces. Like a recipe:

Moles. Moles. Moles. Moles. Balancing Eqns. Balancing. Balancing Eqns. Symbols Yields or Produces. Like a recipe: Like a recipe: Balancing Eqns Reactants Products 2H 2 (g) + O 2 (g) 2H 2 O(l) coefficients subscripts Balancing Eqns Balancing Symbols (s) (l) (aq) (g) or Yields or Produces solid liquid (pure liquid)

More information

Writing Chemical Equations

Writing Chemical Equations Writing Chemical Equations Chemical equations for solution reactions can be written in three different forms; molecular l equations, complete ionic i equations, and net ionic equations. In class, so far,

More information

WRITING CHEMICAL FORMULA

WRITING CHEMICAL FORMULA WRITING CHEMICAL FORMULA For ionic compounds, the chemical formula must be worked out. You will no longer have the list of ions in the exam (like at GCSE). Instead you must learn some and work out others.

More information

MOLES AND MOLE CALCULATIONS

MOLES AND MOLE CALCULATIONS 35 MOLES ND MOLE CLCULTIONS INTRODUCTION The purpose of this section is to present some methods for calculating both how much of each reactant is used in a chemical reaction, and how much of each product

More information

Formulas, Equations and Moles

Formulas, Equations and Moles Chapter 3 Formulas, Equations and Moles Interpreting Chemical Equations You can interpret a balanced chemical equation in many ways. On a microscopic level, two molecules of H 2 react with one molecule

More information

NET IONIC EQUATIONS. A balanced chemical equation can describe all chemical reactions, an example of such an equation is:

NET IONIC EQUATIONS. A balanced chemical equation can describe all chemical reactions, an example of such an equation is: NET IONIC EQUATIONS A balanced chemical equation can describe all chemical reactions, an example of such an equation is: NaCl + AgNO 3 AgCl + NaNO 3 In this case, the simple formulas of the various reactants

More information

CHM1 Review for Exam 12

CHM1 Review for Exam 12 Topics Solutions 1. Arrhenius Acids and bases a. An acid increases the H + concentration in b. A base increases the OH - concentration in 2. Strong acids and bases completely dissociate 3. Weak acids and

More information

Chemistry Themed. Types of Reactions

Chemistry Themed. Types of Reactions Chemistry Themed Types of Reactions 1 2 Chemistry in the Community-2015-2016 Types of Reactions Date In-Class Assignment Homework T 10/20 TEST on Reactivity of Metals and Redox None W 10/21 Late Start

More information

Question Bank Electrolysis

Question Bank Electrolysis Question Bank Electrolysis 1. (a) What do you understand by the terms (i) electrolytes (ii) non-electrolytes? (b) Arrange electrolytes and non-electrolytes from the following substances (i) sugar solution

More information

Chapter 4. Chemical Composition. Chapter 4 Topics H 2 S. 4.1 Mole Quantities. The Mole Scale. Molar Mass The Mass of 1 Mole

Chapter 4. Chemical Composition. Chapter 4 Topics H 2 S. 4.1 Mole Quantities. The Mole Scale. Molar Mass The Mass of 1 Mole Chapter 4 Chemical Composition Chapter 4 Topics 1. Mole Quantities 2. Moles, Masses, and Particles 3. Determining Empirical Formulas 4. Chemical Composition of Solutions Copyright The McGraw-Hill Companies,

More information

A. Types of Mixtures:

A. Types of Mixtures: I. MIXTURES: SOLUTIONS 1) mixture = a blend of two or more kinds of matter, each of which retains its own identity and properties a) homogeneous mixture = a mixture that is uniform in composition throughout

More information

In the box below, draw the Lewis electron-dot structure for the compound formed from magnesium and oxygen. [Include any charges or partial charges.

In the box below, draw the Lewis electron-dot structure for the compound formed from magnesium and oxygen. [Include any charges or partial charges. Name: 1) Which molecule is nonpolar and has a symmetrical shape? A) NH3 B) H2O C) HCl D) CH4 7222-1 - Page 1 2) When ammonium chloride crystals are dissolved in water, the temperature of the water decreases.

More information

Name Class Date. In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question.

Name Class Date. In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. Assessment Chapter Test A Chapter: States of Matter In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. 1. The kinetic-molecular

More information

10. Calculate the mass percent nitrogen in (NH 4 ) 2 CO 3 (molar mass = 96.09 g/mol). a. 29.1 % c. 17.9 % e. 14.6 % b. 35.9 % d. 0.292 % f. 96.

10. Calculate the mass percent nitrogen in (NH 4 ) 2 CO 3 (molar mass = 96.09 g/mol). a. 29.1 % c. 17.9 % e. 14.6 % b. 35.9 % d. 0.292 % f. 96. Chem 171-2-3: Final Exam Review Multiple Choice Problems 1. What is the molar mass of barium perchlorate, Ba(ClO 4 ) 2? a. 189.90 g/mol c. 272.24 g/mol e. 336.20 g/mol b. 240.24 g/mol d. 304.24 g/mol f.

More information

H 2 + O 2 H 2 O. - Note there is not enough hydrogen to react with oxygen - It is necessary to balance equation.

H 2 + O 2 H 2 O. - Note there is not enough hydrogen to react with oxygen - It is necessary to balance equation. CEMICAL REACTIONS 1 ydrogen + Oxygen Water 2 + O 2 2 O reactants product(s) reactant substance before chemical change product substance after chemical change Conservation of Mass During a chemical reaction,

More information

Aqueous Chemical Reactions

Aqueous Chemical Reactions Name: Date: Lab Partners: Lab section: Aqueous Chemical Reactions The purpose of this lab is to introduce you to three major categories of reactions that occur in aqueous solutions: precipitation reactions,

More information