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

Size: px
Start display at page:

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

Transcription

1 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: ionic compounds dissolved in water only Dissociation Equations Ionic compounds dissolve in water by dissociation (breaking apart) For example: Ba(NO 3 ) 2 (s) Ba 2+ (aq) + 2 NO 3- (aq) 1

2 Example: Dissociation Equations Na 2 SO 4 Ca(C 2 H 3 O 2 ) 2 Describing Solutions The amount of solute in a solvent can be described qualitatively by the terms dilute and concentrated. These are qualitative terms: A concentrated solution has lots of solute per volume of solvent A dilute solution has very little solute per volume of solvent Describing Solutions Every substance has a maximum amount of solute that can dissolve in the solvent. This allows for a quantitative description: Unsaturated solutions have less than the maximum amount of solute Saturated solutions are at the maximum amount Supersaturated solutions have more than the maximum amount of solute, usually achieved by raising the temperature to dissolve the solute and then slowly cooling 2

3 Describing Solutions Dilute Unsaturated Concentrated Saturated Supersaturated Solubility Solubility: how much of something can dissolve in something else When the maximum amount is dissolved, the solution is saturated Very soluble will dissolve a lot, low solubility will dissolve very little Analogy: marbles in a bucket Marbles = ions, bucket size = level of solubility Solubility Chart 3

4 Solubility Solubility is a scale Soluble compounds dissociate 100% in solution Dissociation equation has a one-way arrow NaCl (s) Na + (aq) + Cl - (aq) Low solubility means it dissociates less than 100% (some ions will stay attached) Dissociation equation has an equilibrium arrow PbI 2 (s) Pb 2+ (aq) + 2I - (aq) Determining Solubility Option 1: Solubility Rules Chart Qualitative Sorted by anion Note: soluble = aqueous, low solubility = solid Examples: Solubility Rules Soluble (aq) or low solubility (s)? Ba(OH) 2 Na 3 PO 4 CuI 2 Pb(NO 3 ) 2 AgC 2 H 3 O 2 CaCO 3 4

5 Double Displacement Reactions General form: AB + CD AD + CB If AD and/or CB has low solubility, it will make a solid. Otherwise no reaction occurs everything stays dissolved as ions. Double Displacement Reactions Example: Solubility Rules Na 2 CO 3 (aq) + 2 AgNO 3 (aq) 2 NaNO 3 + Ag 2 CO 3 2 KI (aq) + MgCO 3 (aq) K 2 CO 3 + MgI 2 Al 2 (CrO 4 ) 3 (aq) + H 2 SO 4 (aq) Cu 2 SO 4 (aq) + CaCl 2 (aq) 5

6 Total Ionic Equations In the following reaction, copper(ii) hydroxide has low solubility in water and will form a precipitate: 2 NaOH (aq) + CuCl 2 (aq) 2 NaCl (aq) + Cu(OH) 2 (s) This can be rewritten as a total ionic equation, where all aqueous compounds are more correctly represented as ions: 2 Na + (aq) + 2 OH - (aq) + Cu 2+ (aq) + 2 Cl - (aq) 2 Na + (aq) + 2 Cl - (aq) + Cu(OH) 2 (s) Net Ionic Equations Spectator ions: ions that do not participate in the reaction Net ionic equation: remove spectator ions from total ionic equation (no net ionic if no precipitate) 2 OH - (aq) + Cu 2+ (aq) Cu(OH) 2 (s) Net Ionic Equations Why do double displacement reactions have equilibrium arrows instead of regular arrows? How is a net ionic equation related to a dissociation equation? When should you use a dissociation equation vs a net ionic equation? 6

7 Example: Net Ionic Equations Write the reaction, total ionic and net ionic equations for the reaction between barium nitrate and sodium carbonate that produces a barium carbonate precipitate. (Use the right arrow!) Determining Solubility Option 2: Solubility Product Constant (K sp ) Constant for a compound, in water, at 25 C. Describes how much a compound will dissolve Compounds with no K sp listed are very soluble If listed, compound has low solubility. Large K sp = more soluble, small K sp = less soluble Which is more soluble? PbBr 2 or PbCl 2 Example: K sp BaSO 4 or Ag 2 SO 4 Co(OH) 2 or CuCO 3 7

8 Solubility Product To determine solubility or concentration of one or more ions, given the dissociation equation: A a B b (s) a A + (aq) + b B - (aq) Use an equilibrium constant expression! K sp = A + a B b (Remember solids have a concentration of 1 and are not included in the expression.) Determining Solubility AB (s) A + (aq) + B - (aq) Use K sp to determine how many moles of AB per litre of solution will dissolve. Use x like in the C row on an ICE chart to compare moles for each ion. Example 1: Determining Solubility Determine the solubility of AgBr in mol/l at 25 C. 8

9 Example 2: Determining Solubility Determine the concentration of fluoride ions in a saturated solution of magnesium fluoride. Ion Product Constant Similar to Q c Determines if a precipitate will form Basically: are there enough of each of the ions to saturate the solution? Same calculation as K sp, but use concentrations of ions being mixed together Q sp K sp, precipitate will form Q sp < K sp, no precipitate Example 1: Ion Product You are mixing two solutions of equal volume: M NaCl and M Pb(NO 3 ) 2. Will a precipitate form? 1. Determine solid produced and net ionic equation. 2. Determine new concentrations of ions. 9

10 Example 1: Ion Product (continued) 3. Calculate Q sp. 4. Compare K sp and Q sp. Example 2: Ion Product Will a precipitate form if ml of M Ba(NO 3 ) 2 solution is mixed with ml of M K 2 SO 4 solution? 10

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

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

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

Solubility Equilibria. Dissolving a salt... Chem 30S Review Solubility Rules. Solubility Equilibrium: Dissociation = Crystalization

Solubility Equilibria. Dissolving a salt... Chem 30S Review Solubility Rules. Solubility Equilibrium: Dissociation = Crystalization Chem 30S Review Solubility Rules Solubility Equilibria Salts are generally more soluble in HOT water(gases are more soluble in COLD water) Alkali Metal salts are very soluble in water. NaCl, KOH, Li 3

More information

Practice Worksheet - Answer Key. Solubility #1 (KEY)

Practice Worksheet - Answer Key. Solubility #1 (KEY) Practice Worksheet - Answer Key Solubility #1 (KEY) 1 Indicate whether the following compounds are ionic or covalent a) NaCl ionic f) Sr(OH) 2 ionic b) CaBr 2 ionic g) MgCO 3 ionic c) SO 2 covalent h)

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

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 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

Solubility Multiple Choice. January Which of the following units could be used to describe solubility? A. g/s B. g/l C. M/L D.

Solubility Multiple Choice. January Which of the following units could be used to describe solubility? A. g/s B. g/l C. M/L D. Solubility Multiple Choice January 1999 14. Which of the following units could be used to describe solubility? A. g/s B. g/l C. M/L D. mol/s 15. Consider the following anions: When 10.0mL of 0.20M Pb(NO3)

More information

CHEMISTRY 12 UNIT III Solubility Equilibrium

CHEMISTRY 12 UNIT III Solubility Equilibrium CHEMISTRY 12 UNIT III Solubility Equilibrium G: Solubility Equilibrium (Concept of Solubility) It is expected that students will be able to G1: Classifying solutions as ionic or molecular 1) Write the

More information

Solubility Equilibrium When a substance dissolves an equilibrium results between the precipitate and the dissolved ions. The solution becomes

Solubility Equilibrium When a substance dissolves an equilibrium results between the precipitate and the dissolved ions. The solution becomes Solubility Equilibrium When a substance dissolves an equilibrium results between the precipitate and the dissolved ions. The solution becomes saturated. The particles dissolving equals the particles precipitating.

More information

Advanced Chemistry Practice Problems

Advanced Chemistry Practice Problems Aqueous Equilibria: olar Solubility and the Common Ion Effect 1. Question: Which of the following compounds will decrease the solubility of lead(ii) bromide in water? a. Lead(II) nitrate b. Sodium chloride

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

Chemistry 12 Review Sheet on Unit 3 Solubility of Ionic Substances

Chemistry 12 Review Sheet on Unit 3 Solubility of Ionic Substances Chemistry 12 Review Sheet on Unit 3 Solubility of Ionic Substances 1. Identify each of the following as ionic or molecular substances: a) NaCl (aq)... b) CH 3 COOH (aq)... c) CCl 4(l)... d) HNO 3(aq)...

More information

SOLUBILITY PRODUCT (K sp ) Slightly Soluble Salts & ph AND BUFFERS (Part Two)

SOLUBILITY PRODUCT (K sp ) Slightly Soluble Salts & ph AND BUFFERS (Part Two) SOLUBILITY PRODUCT (K sp ) Slightly Soluble Salts & ph AND BUFFERS (Part Two) ADEng. PRGORAMME Chemistry for Engineers Prepared by M. J. McNeil, MPhil. Department of Pure and Applied Sciences Portmore

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

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

****************************************************************************

**************************************************************************** **************************************************************************** To quickly summarize: 1. The solubility of a compound is decreased when an ion which is the same as one of the ions in the compound

More information

Net Ionic Reactions. The reaction between strong acids and strong bases is one example:

Net Ionic Reactions. The reaction between strong acids and strong bases is one example: Net Ionic Reactions Model 1 Net Ionic Reactions. Net ionic reactions are frequently used when strong electrolytes react in solution to form nonelectrolytes or weak electrolytes. These equations let you

More information

Part One: Solubility Equilibria. Insoluble and slightly soluble compounds are important in nature and commercially.

Part One: Solubility Equilibria. Insoluble and slightly soluble compounds are important in nature and commercially. CHAPTER 17: SOLUBILITY AND COMPLEX ION EQUILIBRIA Part One: Solubility Equilibria A. Ksp, the Solubility Product Constant. (Section 17.1) 1. Review the solubility rules. (Table 4.1) 2. Insoluble and slightly

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

Solution Stoichiometry

Solution Stoichiometry Chapter 8 Solution Stoichiometry Note to teacher: You will notice that there are two different formats for the Sample Problems in the student textbook. Where appropriate, the Sample Problem contains the

More information

Beaker A Beaker B Beaker C Beaker D NaCl (aq) AgNO 3(aq) NaCl (aq) + AgNO 3(aq) AgCl (s) + Na 1+ 1

Beaker A Beaker B Beaker C Beaker D NaCl (aq) AgNO 3(aq) NaCl (aq) + AgNO 3(aq) AgCl (s) + Na 1+ 1 CH 11 T49 MIXING SOLUTIONS 1 You have mastered this topic when you can: 1) define the terms precipitate, spectator ion, suspension, mechanical mixture, solution. 2) write formula equations, complete/total

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

Unit 3: Solubility Equilibrium Topic B: Precipitation Reactions and Qualitative Analysis

Unit 3: Solubility Equilibrium Topic B: Precipitation Reactions and Qualitative Analysis 1 In this topic we will examine: Unit 3: Solubility Equilibrium Topic B: Precipitation Reactions and Qualitative Analysis how to predict if a precipitate forms when solutions are mixed how to selectively

More information

SOLUTIONS. Solutions - page

SOLUTIONS. Solutions - page SOLUTIONS For gases in a liquid, as the temperature goes up the solubility goes. For gases in a liquid, as the pressure goes up the solubility goes. Example: What is the molarity of a solution with 2.0

More information

Chapter 15 Additional Aspects of

Chapter 15 Additional Aspects of Chemistry, The Central Science Chapter 15 Additional Aspects of Buffers: Solution that resists change in ph when a small amount of acid or base is added or when the solution is diluted. A buffer solution

More information

Chemistry 12 Solubility Equilibrium I. Name: Date: Block: 1. Solutions Vocab & Calculations 2. Predicting Solubility 3.

Chemistry 12 Solubility Equilibrium I. Name: Date: Block: 1. Solutions Vocab & Calculations 2. Predicting Solubility 3. Chemistry 12 Solubility Equilibrium I Name: Date: Block: 1. Solutions Vocab & Calculations 2. Predicting Solubility 3. Writing Equations Solutions Vocab & Calculations What is a solution? A homogenous

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

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

Chapter 19. Solubility and Simultaneous Equilibria p

Chapter 19. Solubility and Simultaneous Equilibria p Chapter 19 Solubility and Simultaneous Equilibria p. 832 857 Solubility Product ) The product of molar concentrations of the constituent ions, each raised ot the power of its stoichiometric coefficients

More information

Solutions CHAPTER OUTLINE

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

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

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

Modified Dr. Cheng-Yu Lai

Modified Dr. Cheng-Yu Lai Ch16 Aqueous Ionic Equilibrium Solubility and Complex Ion Equilibria Lead (II) iodide precipitates when potassium iodide is mixed with lead (II) nitrate Modified Dr. Cheng-Yu Lai Solubility-product constant

More information

Double Displacement (Exchange or Metathesis) Reactions Practicum

Double Displacement (Exchange or Metathesis) Reactions Practicum Double Displacement (Exchange or Metathesis) Reactions Practicum Part I: Instructions: Write the molecular, complete ionic and net ionic equations for every one of the following reactions. If a reaction

More information

Calculating equilibrium constants

Calculating equilibrium constants Equilibrium Work Book Writing Equilibrium Constants Expressions 1. Write the equilibrium law (mass action expression) for each of the following reactions: a. SO 2 (g) + NO 2 (g) SO 3 (g) + NO(g) b. 2 C(s)

More information

AP Chemistry Table of Contents: Ksp & Solubility Products Click on the topic to go to that section

AP Chemistry Table of Contents: Ksp & Solubility Products Click on the topic to go to that section Slide 1 / 91 Slide 2 / 91 AP Chemistry Aqueous Equilibria II: Ksp & Solubility Products Table of Contents: K sp & Solubility Products Slide 3 / 91 Click on the topic to go to that section Introduction

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

Intro to Reactions/ Balancing Equations

Intro to Reactions/ Balancing Equations Intro to Reactions/ Balancing Equations Chemical Reactions Chemical reactions involve change. Evidence of a chemical reaction could include the following Evolution of heat, light, and/or sound Production

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

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

SOLUBILITY CURVES WORKSHEET

SOLUBILITY CURVES WORKSHEET SOLUBILITY CURVES WORKSHEET 1.) Which compound is least soluble at: (A) 20 o C? (B) 80 o C? 2.) Which substance is the most soluble at: (A) 10 o C? (B) 50 o C? (C) 90 o C? 3.) The solubility of which substance

More information

Solubility & Equilibrium Unit Review

Solubility & Equilibrium Unit Review Solubility & Equilibrium Unit Review This review is worth 3 marks of your total test marks. It must be completed on test day. 3 marks will be given to students who have fully completed this review with

More information

(A) Composition (B) Decomposition (C) Single replacement (D) Double replacement: Acid-base (E) Combustion

(A) Composition (B) Decomposition (C) Single replacement (D) Double replacement: Acid-base (E) Combustion AP Chemistry - Problem Drill 08: Chemical Reactions No. 1 of 10 1. What type is the following reaction: H 2 CO 3 (aq) + Ca(OH) 2 (aq) CaCO 3 (aq) + 2 H 2 O (l)? (A) Composition (B) Decomposition (C) Single

More 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 17. Additional Aspects of Equilibrium

Chapter 17. Additional Aspects of Equilibrium Chapter 17. Additional Aspects of Equilibrium Sample Exercise 17.1 (p. 726) What is the ph of a 0.30 M solution of acetic acid? Be sure to use a RICE table, even though you may not need it. (2.63) What

More information

Unit 3 ~ Learning Guide Name:

Unit 3 ~ Learning Guide Name: Unit 3 ~ Learning Guide Name: Instructions: Using a pencil, complete the following notes as you work through the related lessons. Show ALL work as is explained in the lessons. You are required to have

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

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

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

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

NET IONIC EQUATIONS. Electrolyte Behavior

NET IONIC EQUATIONS. Electrolyte Behavior NET IONIC EQUATIONS Net ionic equations are useful in that they show only those chemical species directly participating in a chemical reaction. They are thus simpler than the overall equation, and help

More information

ANITA S WORK H I4 6 I6 5

ANITA S WORK H I4 6 I6 5 ANITA S WORK Multiple Choice Section: Please DO NOT WRITE or MAKE ANY MARKS on this test paper. Put all answers on your SCANTRON CARD. Please make sure that you fill in your Scantron Card correctly: use

More information

Unit 3: Solubility. Chem 12 Solubility Notes. I) Ionic & Covalent Solutions What is a solution?

Unit 3: Solubility. Chem 12 Solubility Notes. I) Ionic & Covalent Solutions What is a solution? Unit 3: Solubility I) Ionic & Covalent Solutions What is a solution? What are some examples of different types of solutions? solid solid: liquid solid: liquid liquid: liquid gas: gas gas: Jul 23 2:07 PM

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

Unit 3: Solubility. solubilitynotesbqv3.notebook. October 11, I) Ionic & Covalent Solutions What is a solution?

Unit 3: Solubility. solubilitynotesbqv3.notebook. October 11, I) Ionic & Covalent Solutions What is a solution? Unit 3: Solubility I) Ionic & Covalent Solutions What is a solution? What are some examples of different types of solutions? solid solid: liquid solid: liquid liquid: liquid gas: gas gas: Jul 23 2:07 PM

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

III.1 SOLUBILITY CONCEPT REVIEW

III.1 SOLUBILITY CONCEPT REVIEW III.1 SOLUBILITY CONCEPT REVIEW Read Hebden p. 73 76 and review basic solubility definitions. Soluble means Insoluble means The Dissolving Process IONIC Solutions MOLECULAR Solutions (Covalent compounds)

More information

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

Chapter 7 Chemical Reactions

Chapter 7 Chemical Reactions Chapter 7 Chemical Reactions Evidence of Chemical Change Release or Absorption of Heat Color Change Emission of Light Formation of a Gas Formation of Solid Precipitate Tro's "Introductory 2 How Do We Represent

More information

Chemistry 12 Provincial Exam Workbook Unit 03: Solubility Equilibrium. Multiple Choice Questions

Chemistry 12 Provincial Exam Workbook Unit 03: Solubility Equilibrium. Multiple Choice Questions R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P 1 / 7 Chemistry 1 Provincial Exam Workbook Unit 0: Solubility Equilibrium Multiple Choice Questions 1. Which of the following would be true

More information

Solubility Equilibrium

Solubility Equilibrium 2016 Ksp note.notebook Solubility Equilibrium Learning Goals: to understand what happens when a compound dissolves in water to calculate the extent of dissolution...the molar solubility to calculate the

More information

CHEMICAL REACTIONS. Introduction. Chemical Equations

CHEMICAL REACTIONS. Introduction. Chemical Equations CHEMICAL REACTIONS Chemistry I Chapter 7 1 Chemical Equations Their Job: Depict the kind of reactants and products and their relative amounts in a reaction. 4 Al (s) + 3 O 2 (g) ---> 2 Al 2 O 3 (s) The

More information

NET IONIC REACTIONS in AQUEOUS SOLUTIONS AB + CD AD + CB

NET IONIC REACTIONS in AQUEOUS SOLUTIONS AB + CD AD + CB NET IONIC REACTIONS in AQUEOUS SOLUTIONS Double replacements are among the most common of the simple chemical reactions. Consider the hypothetical reaction: AB + CD AD + CB where AB exists as A + and B

More information

Chapter 4: Phenomena. Electrolytes. Electrolytes. Electrolytes. Chapter 4 Types of Chemical Reactions and Solution Stoichiometry.

Chapter 4: Phenomena. Electrolytes. Electrolytes. Electrolytes. Chapter 4 Types of Chemical Reactions and Solution Stoichiometry. Chapter 4: Phenomena Phenomena: Many different reactions are known to occur. Scientists wondered if these reactions could be separated into groups based on their properties. Look at the reactions below

More information

Chapter 4: Phenomena. Electrolytes. Electrolytes. Electrolytes. Chapter 4 Types of Chemical Reactions and Solution Stoichiometry

Chapter 4: Phenomena. Electrolytes. Electrolytes. Electrolytes. Chapter 4 Types of Chemical Reactions and Solution Stoichiometry Chapter 4: Phenomena Phenomena: Many different reactions are known to occur. Scientists wondered if these reactions could be separated into groups based on their properties. Look at the reactions below

More information

Chapter 4: Phenomena. (aq)+ 4H + (aq)+ 2e - Chapter 4: Types of Chemical Reactions and Solution Stoichiometry

Chapter 4: Phenomena. (aq)+ 4H + (aq)+ 2e - Chapter 4: Types of Chemical Reactions and Solution Stoichiometry Chapter 4: Phenomena Phenomena: Many different reactions are known to occur. Scientists wondered if these reactions could be separated into groups based on their properties. Look at the reactions below

More information

Chapter 16. Solubility Equilibria 10/14/2010. Solubility Equilibria. Solubility Product (Constant), K sp. Solubility and the Solubility Product

Chapter 16. Solubility Equilibria 10/14/2010. Solubility Equilibria. Solubility Product (Constant), K sp. Solubility and the Solubility Product Solubility Equilibria These are associated with ionic solids dissolving in water to form aqueous solutions Chapter 16 Solubility Equilibria It is assumed that when an ionic compound dissolves in water,

More information

AP Chemistry. Slide 1 / 39. Slide 2 / 39. Slide 3 / 39. Equilibrium Part C : Solubility Equilibrium. Table of Contents

AP Chemistry. Slide 1 / 39. Slide 2 / 39. Slide 3 / 39. Equilibrium Part C : Solubility Equilibrium. Table of Contents Slide 1 / 39 AP Chemistry Slide 2 / 39 Equilibrium Part C : Solubility Equilibrium 2014-10-29 www.njctl.org Table of Contents click on the topic to go to that section Slide 3 / 39 Molar Solubility Calculating

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

] after equilibrium has been established?

] after equilibrium has been established? Chemistry 1 Solubility Equilibrium onster Review 1. A saturated solution forms when a 0. 10 mol of salt is added to 10. L of water. The salt is A. Li S B. CuBr C. Zn( OH) ( ) D. NH CO 4. Consider the following

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

Chapter 4 Types of Chemical Reaction and Solution Stoichiometry

Chapter 4 Types of Chemical Reaction and Solution Stoichiometry Chapter 4 Types of Chemical Reaction and Solution Stoichiometry Water, the Common Solvent One of the most important substances on Earth. Can dissolve many different substances. A polar molecule because

More information

Chapter 4. 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

Saturated vs. Unsaturated

Saturated vs. Unsaturated Solubility Equilibria in Aqueous Systems K sp (Equilibria of Slightly Soluble Salts, Ionic Compounds) Factors that Affect Solubility (Common Ion Effect, AcidBase Chemistry) Applications of Ionic Equilibria

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

Chemical Equations and Chemical Reactions

Chemical Equations and Chemical Reactions Chemical Equations Chemical Equations and Chemical Reactions Chemical equations are concise representations of chemical reactions. Chemical Equations Symbols Used in Chemical Equations The formulas of

More information

4.4: Solubility and Ionic Equations

4.4: Solubility and Ionic Equations 4.4: Solubility and Ionic Equations Solubility Curves Graphs of solubility (maximum concentration) against temperature allow quick and easy reference, and are very useful for a wide variety of questions

More information

Solubility & Net Ionic review

Solubility & Net Ionic review Solubility & Net Ionic review Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Which of the following statements is/are correct? 1. All ionic compounds

More 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

SOLUBILITY EQUILIBRIUM

SOLUBILITY EQUILIBRIUM Introduction SOLUBILITY EQUILIBRIUM A. Ionic vs Molecular Solutions 1. Ionic Compounds form Ionic Solutions a) Ionic compounds ( + ) dissolved in water to form Ionic Solutions eg1: equation AlCl3(s) Al3+

More information

D O UBLE DISPL Ac EMENT REACTIONS

D O UBLE DISPL Ac EMENT REACTIONS Experiment 8 Name: D O UBLE DISPL Ac EMENT REACTIONS In this experiment, you will observe double displacement reactions and write the corresponding balanced chemical equation and ionic equations. Double

More 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

Concentration of Solutions

Concentration of Solutions Solutions We carry out many reactions in solutions Remember that in the liquid state molecules move much easier than in the solid, hence the mixing of reactants occurs faster Solute is the substance which

More information

1. Which one of the following would form an ionic solution when dissolved in water? A. I2 C. Ca(NO3)2 B. CH3OH D. C12H22O11

1. Which one of the following would form an ionic solution when dissolved in water? A. I2 C. Ca(NO3)2 B. CH3OH D. C12H22O11 Chemistry 12 Solubility Equilibrium Review Package Name: Date: Block: I. Multiple Choice 1. Which one of the following would form an ionic solution when dissolved in water? A. I2 C. Ca(NO3)2 B. CH3OH D.

More information

Definition: the process by which one or more substances are rearranged to form different substances. Another name for a chemical change.

Definition: the process by which one or more substances are rearranged to form different substances. Another name for a chemical change. Chemical Reactions I. What is a chemical reaction? Definition: the process by which one or more substances are rearranged to form different substances. Another name for a chemical change. A. How can you

More information

Reference: Chapter 4 in textbook. PART 6B Precipitate. textbook

Reference: Chapter 4 in textbook. PART 6B Precipitate. textbook PART 6A Solution Reference: Chapter 4 in textbook PART 6B Precipitate Reference: Chapter 16.5 16.8 in the textbook 1 Solution Solute, Solvent, and Solution Saturated solution and Solubility Saturated solution:

More information

Name Date Class PROPERTIES OF SOLUTIONS

Name Date Class PROPERTIES OF SOLUTIONS 16.1 PROPERTIES OF SOLUTIONS Section Review Objectives Identify the factors that determine the rate at which a solute dissolves Identify the units usually used to express the solubility of a solute Calculate

More information

D O UBLE DISPL Ac EMENT REACTIONS

D O UBLE DISPL Ac EMENT REACTIONS Experiment 8 Name: D O UBLE DISPL Ac EMENT REACTIONS In this experiment, you will observe double displacement reactions and write the corresponding balanced chemical equation and ionic equations. Double

More 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

Flashback - Aqueous Salts! PRECIPITATION REACTIONS Chapter 15. Analysis of Silver Group. Solubility of a Salt. Analysis of Silver Group

Flashback - Aqueous Salts! PRECIPITATION REACTIONS Chapter 15. Analysis of Silver Group. Solubility of a Salt. Analysis of Silver Group Page III-15-1 / Chapter Fifteen Lecture Notes Flashback - Aqueous Salts! If one ion from the Soluble Compd. list is present in a compound, the compound is water soluble. PRECIPITATION REACTIONS Chapter

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

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

Chemistry 12 Unit III Solubility Notes

Chemistry 12 Unit III Solubility Notes Chemistry 12 Unit III Solubility Notes III.1 A Review Of Solubility There are only three classes of compounds that form ionic solutions: ACIDS, BASES and SALTS. This unit will deal only with SALTS. Acids

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

Check Your Solution The net ionic equation is balanced, including the charges on the ions.

Check Your Solution The net ionic equation is balanced, including the charges on the ions. Ba 2+ (aq) + 2PO (aq) Ba (PO ) 2 (s) 2. Practice Problem (page 10) Write the net ionic equation for this reaction: Na 2 SO (aq) + Sr(OH) 2 (aq) SrSO (s) + NaOH(aq) You need to write the net ionic equation

More information

CHEM J-6 June 2014

CHEM J-6 June 2014 CHEM1102 2014-J-6 June 2014 A solution is prepared that contains sodium chloride and sodium chromate (both 0.10 M). When a concentrated solution of silver nitrate is added slowly, white AgCl(s) begins

More information

Chem 12 Practice Solubility Test

Chem 12 Practice Solubility Test Chem 12 Practice Solubility Test 1. Which combination of factors will affect the rate of the following reaction? Zn (s) + 2HCl ZnCl 2 + H 2(g) A. Temperature and surface area only B. Temperature and concentration

More information