EQUILIBRIUM FREE RESPONSE QUESTION #2

Size: px
Start display at page:

Download "EQUILIBRIUM FREE RESPONSE QUESTION #2"

Transcription

1 EQUILBRIUM FREE RESPONSE QUESTION #1 Answer the following questions relating to the solubilities of two silver compounds, Ag 2 CrO 4 and Ag 3 PO 4. Silver chromate dissociates in water according to the equation shown below: Ag 2 CrO 4 (s) -- 2Ag + (aq) + CrO 4 2- (aq) K sp = 2.6 X at 25 o C Write the equilibrium constant expression for the dissolving of Ag 2 CrO 4 (s). Calculate the concentration, in mol L -1, of Ag + (aq) in a saturated solution of Ag 2 CrO 4 at 25 o C. Calculate the maximum mass, in grams of Ag 2 CrO 4 that can dissolve in 100. ml of water at 25 o C. A mol sample of solid AgNO 3 is added to a 1.00 L saturated solution of Ag 2 CrO 4. Assuming no volume change, does [CrO 2-4 ] increase, decrease, or remain the same? Justify your answer. In a saturated solution of Ag 3 PO 4 at 25 o C, the concentration of Ag + (aq) is 5.3 X 10-5 M. The equilibrium constant expression for the dissolving of Ag 3 PO 4 (s) in water is shown below: K sp = [Ag + ] 3 [PO 3-4 ] (e) Write the balanced equation for the dissolving of Ag 3 PO 4 in water. (f) Calculate the value of K sp for Ag 3 PO 4 at 25 o C. (g) A 1.00 L sample of saturated Ag 3 PO 4 solution is allowed to evaporate at 25 o C to a final volume of 500. ml. What is [Ag + ] in the solution? Justify your answer. NO FREE RESPONSE QUESTION #2 The gas-phase conversion reaction between the geometric isomers cis-2-butene and trans-2- butene is represented by the equation above. The value of the equilibrium constant, K eq, for the reaction is 3.2 at 298 K and 1.0 atm. In a mixture of the isomers at equilibrium at 298 K and 1.0 atm, which is present at a high concentration, cis-2-butene or trans-2-butene? Justify your answer.

2 If 1.00 mol of pure cis-2-butene and 1.0 mol of pure trans-2-butene were introduced into an evacuated container at 298 K, in which direction (to the right or to the left) would the reaction proceed to establish equilibrium? Justify your answer. Given that K eq for the reaction at 400 K has the value of 1.3, predict whether the reaction is endothermic or exothermic. Justify your answer. There are other structure isomers of cis-2-butene and trans-2-butene. Draw one of these isomers, including all atoms, and give its IUPAC name. EQUILBRIUM FREE RESPONSE QUESTION #3 N 2 (g) + 3H 2 (g) NH 3 (g) For the reaction represented above, the value of the equilibrium constant, K p, is 3.1 X 10-4 at 700. K. Write the expression for the equilibrium constant, K p, for the reaction. Assume that the initial partial pressures of the gases are as follows: P N2 = atm; P H2 = atm; and P NH3 = atm (i) Calculate the value of the reaction quotient, Q, at these conditions. (ii) Predict the direction in which the reaction will proceed at 700. K if the initial partial pressures are those given above. Justify your answer. Calculate the value of the equilibrium constant, K c, given that the value of K p for the reaction at 700. K is 3.1 X The value of K p for the reaction represented below is 8.3 X 10-3 at 700. K. NH 3 (g) + H 2 S(g) --- NH 4 HS(g) Calculate the value of K p at 700. K for each of the reactions represented below: (i) NH 4 HS(g) --- NH 3 (g) + H 2 S(g) (ii) 2H 2 S(g) + N 2 (g) + 3H 2 (g) -- 2NH 4 HS(g) FREE RESPONSE QUESTION #4 2H 2 S(g) H 2 (g) + S 2 (g) When heated, hydrogen sulfide gas decomposes according to the equation above. A 3.40 gram sample of H 2 S(g) is introduced into an evacuated rigid 1.25 L container. The sealed container is heated to 483 K, and 3.72 X 10-2 mol of S 2 (g) is present at equilibrium. Write the expression for the equilibrium constant, K c, for the decomposition reaction represented above. Calculate the equilibrium concentration, in mol L -1, of the following gases in the container at 483 K. (i) H 2 (g) (ii) H 2 S(g)

3 Calculate the value of the equilibrium constant, K c, for the decomposition reactions at 483 K. Calculate the partial pressure of S 2 (g) in the container at equilibrium at 483 K. (e) For the reaction H 2 (g) + ½ S 2 (g) --- H 2 S(g) at 483 K, calculate the value of the equilibrium constant, K c. FREE RESPONSE QUESTION #5 MgF 2 (s) ---- Mg 2+ (aq) + 2F - (aq) In a saturated solution of MgF 2 is 18 o C, the concentration of Mg 2+ is 1.21 X 10-3 molar. The equilibrium is represented by the equation above. Write the expression for the solubility product constant, K sp, and calculate its value at 18 o C. Calculate the equilibrium concentration of Mg 2+ in liter of saturated MgF 2 solution is 18 o C to which mole of solid KF has been added. The KF dissolves completely. Assume the volume change is negligible. Predict whether a precipitate of MgF 2 will form when milliliters of 3.00 X 10-3 molar Mg(NO 3 ) 2 solution is mixed with milliliters of a 2.00 X 10-3 molar NaF solution at 18 o C. Calculations to support you prediction must be shown. At 27 o C the concentration of Mg 2+ in a saturated solution of MgF 2 is 1.17 X 10-3 molar. Is the dissolving of MgF 2 in water an endothermic or exothermic process? Give an explanation to support your conclusion. FREE RESPONSE QUESTION #6 Answer the following questions relating to the solubility of the chlorides of silver and lead. At 10 o C, 8.9 X 19-5 g of AgCl(s) will dissolve in 100. ml of water. (i) Write the equation for the dissociation of AgCl(s) in water. (ii) Calculate the solubility, in mol L -1, of AgCl(s) in water at 10 o C. (iii) Calculate the value of the solubility product constant, K sp, for AgCl(s) at 10 o C. At 25 o C, the value for K sp for PbCl 2 (s) is 1.6 X 10-5 and the value of K sp for AgCl(s) is 1.8 X (i) If 60.0 ml of M NaCl(aq) is added to 60.0 ml of M Pb(NO 3 ) 2 (aq) at 25 o C, will a precipitate form? Assume that volumes are additive. Show calculations to support your answer. (ii) Calculate the equilibrium value of [Pb 2+ (aq)] in 1.00 L of saturated PbCl 2 solution to which mole of NaCl(s) has been added. Assume that no volume change occurs. (iii) If M NaCl(aq) is added slowly to a beaker containing both M AgNO 3(aq) and M Pb(NO 3 ) 2 (aq) at 25 o C, which will precipitate first, AgCl(s) or PbCl 2 (s)? Show calculations to support your answer.

4 FREE RESPONSE QUESTION #7 NO C(s) + H 2 O(g) -- CO(g) + H 2 (g) H o = +131 kj A rigid container holds a mixture of graphite pellets (C(s)), H 2 O(g), CO(g), and H 2 (g) at equilibrium. State whether the number of moles of CO(g) in the container will increase, decrease, or remain the same after each of the following disturbances is applied to the original mixture. For each case, assume that all other variables remain constant except for the given disturbance. Explain each answer with a short statement. Additional H 2 (g) is added to the equilibrium mixture at constant volume. The temperature of the equilibrium mixture is increased at constant volume The volume of the container is decreased at constant temperature. The graphite pellets are pulverized. FREE RESPONSE QUESTION #8 CO 2 (g) + H 2 (g) --- H 2 O(g) + CO(g) When H 2 (g) is mixed with CO 2 (g) at 2,000 K, equilibrium is achieved according to the equation above. In one experiment, the following equilibrium concentrations were measured. [H 2 ] = 0.20 mol/l [CO 2 ] = 0.30 mol/l [H 2 O] = [CO] = 0.55 mol/l What is the mole fraction of CO(g) in the equilibrium mixture? Using the equilibrium concentrations given above, calculate the value of K c, the equilibrium constant, for the reaction. Determine K p in terms of K c for this system. When the system is cooled from 2,000 K to a lower temperature, 30.0 percent of the CO(g) is converted back to CO 2 (g). Calculate the value of K c at this lower temperature. (e) In a different experiment, 0.50 mole of H 2 (g) is mixed with 0.50 mole of CO 2 (g) in a 3.0 L reaction vessel at 2,000 K. Calculate the equilibrium concentration, in moles per liter, of CO(g) at this temperature.

5 FREE RESPONSE QUESTION #9 NO NH 4 HS(s) ---- NH 3 (g) + H 2 S(g) H o = +93 kj The equilibrium above is established by placing solid NH 4 HS in an evacuated container at 25 o+c. At equilibrium, some solid NH 4 HS remains in the container. Predict and explain each of the following. The effect on the equilibrium partial pressure of NH 3 gas when additional solid NH 4 HS is introduced into the container. The effect on the equilibrium partial pressure of NH 3 gas when additional solid H 2 S is introduced into the container. The effect on the mass of solid NH 4 HS present when the volume of the container is decreased. The effect on the mass of solid NH 4 HS present when the temperature is increased.

Name AP Chemistry / / Chapter 13 Collected AP Exam Free Response Questions 1980 2010 Answers

Name AP Chemistry / / Chapter 13 Collected AP Exam Free Response Questions 1980 2010 Answers Name AP Chemistry / / Chapter 13 Collected AP Exam Free Response Questions 1980 2010 Answers 1980 - #6 NH 4 Cl(s) NH 3 (g) + HCl(g) ΔH = +42.1 kilocalories Suppose the substances in the reaction above

More information

AP Chemistry Unit 7- Homework Problems Equilibrium and K sp

AP Chemistry Unit 7- Homework Problems Equilibrium and K sp AP Chemistry Unit 7- Homework Problems Equilibrium and K sp Nature of the Equilibrium State 1. Draw on this graph where equilibrium has been reached. [X] equilibrium time 2. What are three qualities of

More information

Chapter 14 Review. Student: Br 2 (g) + 5F 2 (g) is

Chapter 14 Review. Student: Br 2 (g) + 5F 2 (g) is Chapter 14 Review Student: 1. Which is the correct equilibrium constant expression for the following reaction? Fe 2 O 3 (s) + 3H 2 (g) 2Fe(s) + 3H 2 O(g) A. K c = [Fe 2 O 3 ] [H 2 ] 3 /[Fe] 2 [H 2 O] 3

More information

2001 AP CHEMISTRY FREE-RESPONSE QUESTIONS

2001 AP CHEMISTRY FREE-RESPONSE QUESTIONS 2001 AP CHEMISTRY FREE-RESPONSE QUESTIONS CHEMISTRY Section II (Total time 90 minutes) Part A Time 40 minutes YOU MAY USE YOUR CALCULATOR FOR PART A. CLEARLY SHOW THE METHOD USED AND THE STEPS INVOLVED

More information

6.1 The Equilibrium Condition. Chapter 6. Equilibrium Systems. Reaching Equilibrium 10/2/2015

6.1 The Equilibrium Condition. Chapter 6. Equilibrium Systems. Reaching Equilibrium 10/2/2015 10//015 6.1 The Equilibrium Condition Chapter 6 Describe equilibrium systems and write the equilibrium constant expression for any chemical reaction. Chemical Equilibrium Chemical Equilibrium Chemical

More information

N 2 + 3H 2 2NH 3 + heat

N 2 + 3H 2 2NH 3 + heat 1. In which reaction will the point of equilibrium shift to the left when the pressure on the system is increased? 1) C(s) + O 2 (g) CO 2 (g) 2) CaCO 3 (s) CaO(s) + CO 2 (g) 3) 2Mg(s) + O 2 (g) 2MgO(s)

More information

(aq) + NO 2 (aq) (B) For equations (i) (iv), write the expressions for the equilibrium constant K p.

(aq) + NO 2 (aq) (B) For equations (i) (iv), write the expressions for the equilibrium constant K p. Chapter 1 Exercises Exercises #1 1. Consider the following reaction: CO(g) + H O(g) CO (g) + H (g) (a) In one experiment 1.0 mole of H O and 1.0 mole of CO are placed in a sealed flask and heated to 50

More information

Solubility. Our start in adventures in Aqueous Equilibria

Solubility. Our start in adventures in Aqueous Equilibria Solubility Our start in adventures in Aqueous Equilibria Sea Shells are essentially Calcium Carbonate crystals held together by proteins Given this information what do you think equilibrium constant will

More information

CHM1 Review for Exam 9

CHM1 Review for Exam 9 Topics 1. Reaction Types a. Combustion b. Synthesis c. Decomposition d. Single replacement i. Metal activity series ii. Nonmetal activity series e. Double replacement i. Precipitates and solubility rules

More information

Equilibrium. 2. Which of the following will change the value of an equilibrium constant?

Equilibrium. 2. Which of the following will change the value of an equilibrium constant? Equilibrium 1. For a chemical reaction at equilibrium, the relationship between the rate constants for the forward and reverse reactions (k f and k r ) and the equilibrium constant for the process (K eq

More information

Review for K sp. 1. What is the K sp of PbCl 2 if, in a **saturated solution of lead (II) chloride, the [Cl - ] is mol/l?

Review for K sp. 1. What is the K sp of PbCl 2 if, in a **saturated solution of lead (II) chloride, the [Cl - ] is mol/l? SCH4U Review for K sp 1. What is the K sp of PbCl 2 if, in a **saturated solution of lead (II) chloride, the [Cl - ] is 0.032 mol/l? PbCl 2(s) Pb 2+ (aq) + 2Cl - (aq) [C] +x +2x [E] 0.016 0.032 **saturated

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. 720) What is the ph of a solution made by adding 0.30 mol of acetic acid (HC 2 H 3 O 2 ) and 0.30 mol of sodium acetate (NaC 2 H 3

More information

AP Chemistry 2004 Scoring Guidelines Form B

AP Chemistry 2004 Scoring Guidelines Form B AP Chemistry 2004 Scoring Guidelines Form B The materials included in these files are intended for noncommercial use by AP teachers for course and exam preparation; permission for any other use must be

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. 15 - Applications of Aqueous Equilibria Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which one of the

More information

Name AP CHEM / / Collected AP Exam Essay Answers for Chapter 16

Name AP CHEM / / Collected AP Exam Essay Answers for Chapter 16 Name AP CHEM / / Collected AP Exam Essay Answers for Chapter 16 1980 - #7 (a) State the physical significance of entropy. Entropy (S) is a measure of randomness or disorder in a system. (b) From each of

More information

A) HCl C) 52 g KCl in 100 g water at 80ºC A) temperature of the solution increases B) supersaturated D) low temperature and high pressure D) KClO3

A) HCl C) 52 g KCl in 100 g water at 80ºC A) temperature of the solution increases B) supersaturated D) low temperature and high pressure D) KClO3 1. Which compound becomes less soluble in water as the temperature of the solution is increased? A) HCl B) 2. The solubility of O3(s) in water increases as the A) temperature of the solution increases

More information

Equilibrium. Definition. Definition. Definition

Equilibrium. Definition. Definition. Definition Definition Class Demo with hall Chemical Equilibrium when the rate of the forward and reverse reactions are equal Dynamic Reactions at eq never stop Equilibrium DOES NOT mean that the amount of reactants

More information

Equilibrium & Solubility: The Solubility Product Constant, K sp

Equilibrium & Solubility: The Solubility Product Constant, K sp Equilibrium & Solubility: The Solubility Product Constant, K sp 1 Prof. Zvi C. Koren 20.07.2010 Precipitation Reactions Gross rxn.: Pb(NO 3 ) 2 (aq) + 2KI(aq) PbI 2 (s) + 2KNO 3 (aq) (recall double-replacement

More information

CHAPTER 16 GENERAL ASPECTS OF EQUILIBRIUM

CHAPTER 16 GENERAL ASPECTS OF EQUILIBRIUM Chapter 16: General Equilibrium Page 1 CHAPTER 16 GENERAL ASPECTS OF EQUILIBRIUM 16-1. Which of the following is true about a chemical system at equilibrium? (a) no reactions take place (b) temperature

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

CHEM 1332 CHAPTER 14

CHEM 1332 CHAPTER 14 CHEM 1332 CHAPTER 14 1. Which is a proper description of chemical equilibrium? The frequencies of reactant and of product collisions are identical. The concentrations of products and reactants are identical.

More information

Chapter 3 - Solubility Practice Test #1

Chapter 3 - Solubility Practice Test #1 Chapter 3 - Solubility Practice Test #1 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

More information

Chemical Equilibrium Pearson Education, Inc. Mr. Matthew Totaro Legacy High School AP Chemistry

Chemical Equilibrium Pearson Education, Inc. Mr. Matthew Totaro Legacy High School AP Chemistry Chemical 2012 Pearson Education, Inc. Mr. Matthew Totaro Legacy High School AP Chemistry The Concept of Chemical equilibrium occurs when a reaction and its reverse reaction proceed at the same rate. 2012

More information

1332 -CHAPTER 17 Sample Problems

1332 -CHAPTER 17 Sample Problems 1332 -CHAPTER 17 Sample Problems Important Data Compound ΔH f S ΔG f kj/mol J/mol K kj/mol SO 2 (g) -301 SO 3 (g) -372 NO(g) 211 86.7 NO 2 (g) 240 51.8 NOCl(g) 264 66.3 N 2 O(g) 220 103.6 Cr (s) 23.77

More information

Solubility and Complex Ion Equilibria

Solubility and Complex Ion Equilibria Solubility and Complex Ion Equilibria The Solubility Product Constant (K sp ) is the equilibrium constant for the solubility equilibrium of a slightly soluble (or nearly insoluble) ionic compound. CaC

More information

3.Determine the empirical formula and name of the compound made when 8.65 g of iron combines with 3.72 g of oxygen.

3.Determine the empirical formula and name of the compound made when 8.65 g of iron combines with 3.72 g of oxygen. Final Review Academic Chemistry Second Semester 2016 Chapter 7- Chemical Reactions Chapter 9- Chemical Quantities Chapter 10 Heat Energy Chapter 13- Gas Laws Chapter 15 solutions Chapter 17-Kinetics You

More information

(3) AgCl(s) Ag + (aq) + Cl (aq) (4) 2 HgO(s) 2 Hg( ) + O 2. A(g) + B(g) AB(g) 2 SO 2 (g) + O 2 (g) 2 SO 3 (g)

(3) AgCl(s) Ag + (aq) + Cl (aq) (4) 2 HgO(s) 2 Hg( ) + O 2. A(g) + B(g) AB(g) 2 SO 2 (g) + O 2 (g) 2 SO 3 (g) 1. Given the reaction at equilibrium: H 2 + Cl 2 2 HCl As the pressure s at constant temperature, the number of moles of HCl (1) s (3) remains the same (2) s 2. The Haber process is represented by the

More information

AP* Chemistry Solubility Equilibrium

AP* Chemistry Solubility Equilibrium AP* Chemistry Solubility Equilibrium SOLUBILITY EQUILIBRIA (The Solubility-Product Constant, K sp ) We ve got good news and we ve got bad news Which do you want first? The good news: Solubility equilibrium

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

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

SOLUBILITY AND PRECIPITATION EQUILIBRIA

SOLUBILITY AND PRECIPITATION EQUILIBRIA 16 CHAPTER SOLUBILITY AND PRECIPITATION EQUILIBRIA 16.1 The Nature of Solubility Equilibria 16.2 Ionic Equilibria between Solids and Solutions 16.3 Precipitation and the Solubility Product 16.4 The Effects

More information

Solution Review 1) C 6 H 12 2) CH 3 3) C 12 H 22. 4) NaOH. 1) 43 g. 2) 86 g. 3) 134 g. 4) 268 g 1) KI 2) KNO 3. 3) NaNO 3. 4) NaCl. 1) 0.

Solution Review 1) C 6 H 12 2) CH 3 3) C 12 H 22. 4) NaOH. 1) 43 g. 2) 86 g. 3) 134 g. 4) 268 g 1) KI 2) KNO 3. 3) NaNO 3. 4) NaCl. 1) 0. 1. How many moles of KNO 3 are required to make 0.50 liter of a 2.0 M solution of KNO 3? 6. A 0.100-molal aqueous solution of which compound has the lowest freezing point? 1) 1.0 2) 2.0 3) 0.50 4) 4.0

More information

Kinetics and Equilibrium Review

Kinetics and Equilibrium Review 1. A 5.0-gram sample of zinc and a 50.-milliliter sample of hydrochloric acid are used in a chemical reaction. Which combination of these samples has the fastest reaction rate? 1) a zinc strip and 1.0

More information

Dr. Fus CHEM 1220 CHAPTER 17 PRACTICE EXAM

Dr. Fus CHEM 1220 CHAPTER 17 PRACTICE EXAM CHEMISTRY 1220 CHAPTER 17 PRACTICE EXAM All questions listed below are problems taken from old Chemistry 123 exams given here at The Ohio State University. Read Chapter 17.4 17.7 and complete the following

More information

stronger than the attraction of the water to either the Pb 2+ or SO 4

stronger than the attraction of the water to either the Pb 2+ or SO 4 Reactions in solution Precipitation reactions not all ionic compounds are soluble in water. If PbSO 4 is added to water none of the lead(ii)sulfate will dissolve (the interaction between Pb 2+ and SO 4

More information

CHEMISTRY 100 CHRISTMAS EXAM

CHEMISTRY 100 CHRISTMAS EXAM CHEMISTRY 100 CHRISTMAS EXAM - 2006 Name: ID#: Prof.: PLEASE READ THIS BEFORE YOU BEGIN: This exam comprises 13 pages (including this page) plus a periodic table. Please make sure you have a complete exam

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

V. POLYPROTIC ACID IONIZATION. NOTICE: K a1 > K a2 > K a3 EQUILIBRIUM PART 2. A. Polyprotic acids are acids with two or more acidic hydrogens.

V. POLYPROTIC ACID IONIZATION. NOTICE: K a1 > K a2 > K a3 EQUILIBRIUM PART 2. A. Polyprotic acids are acids with two or more acidic hydrogens. EQUILIBRIUM PART 2 V. POLYPROTIC ACID IONIZATION A. Polyprotic acids are acids with two or more acidic hydrogens. monoprotic: HC 2 H 3 O 2, HCN, HNO 2, HNO 3 diprotic: H 2 SO 4, H 2 SO 3, H 2 S triprotic:

More information

Name Exam No. C. CHEM 60 Fall 2015 Exam 2 Ch 5-8, 100 points total, however, there are a maximum of 110 points. sodium bicarbonate

Name Exam No. C. CHEM 60 Fall 2015 Exam 2 Ch 5-8, 100 points total, however, there are a maximum of 110 points. sodium bicarbonate Name Exam No. C CHEM 60 Fall 2015 Exam 2 Ch 5-8, 100 points total, however, there are a maximum of 110 points. In the space provided below each problem, show a neat, complete, and logical method for solving

More information

Stoichiometry. Stoichiometry Which of the following forms a compound having the formula KXO 4? (A) F (B) S (C) Mg (D) Ar (E) Mn

Stoichiometry. Stoichiometry Which of the following forms a compound having the formula KXO 4? (A) F (B) S (C) Mg (D) Ar (E) Mn The Advanced Placement Examination in Chemistry Part I Multiple Choice Questions Part II - Free Response Questions Selected Questions from 1970 to 2010 Stoichiometry Part I 1984 2. Which of the following

More information

Standard Free Energies of Formation at 298 K. Average Bond Dissociation Energies at 298 K

Standard Free Energies of Formation at 298 K. Average Bond Dissociation Energies at 298 K 1 Thermodynamics There always seems to be at least one free response question that involves thermodynamics. These types of question also show up in the multiple choice questions. G, S, and H. Know what

More information

AP CHEMISTRY 2013 SCORING GUIDELINES

AP CHEMISTRY 2013 SCORING GUIDELINES 2013 SCORING GUIDELINES Question 1 (10 points) Answer the following questions about the solubility of some fluoride salts of alkaline earth metals. (a) A student prepares 100. ml of a saturated solution

More information

Equilibrium Worksheet Answers are at the back. Do these on your own and correct yourself.

Equilibrium Worksheet Answers are at the back. Do these on your own and correct yourself. Equilibrium Worksheet Answers are at the back. Do these on your own and correct yourself. 1. Write equilibrium constant expressions, K c, for the following reactions: a. 2 NO (g) + O 2 (g) 2 NO 2 (g) b.

More information

AP CHEMISTRY 2010 SCORING GUIDELINES

AP CHEMISTRY 2010 SCORING GUIDELINES AP CHEMISTRY 2010 SCORING GUIDELINES Question 1 (10 points) Several reactions are carried out using AgBr, a cream-colored silver salt for which the value of the solubilityproduct-constant, K sp, is 5.0

More information

2. A pure sample of acetylacetone (C5H8O2) has a mass of 8.0 g. What is the mass of oxygen in the sample? A g C. 2.6 g B. 16 g D. 0.

2. A pure sample of acetylacetone (C5H8O2) has a mass of 8.0 g. What is the mass of oxygen in the sample? A g C. 2.6 g B. 16 g D. 0. 1. A glucose molecule contains six carbons, twelve hydrogens and six oxygens. The empirical formula is CH2O. How would you calculate the molecular mass of glucose? A. 1 12.01 amu + 2 1.01 amu + 1 16.00

More information

Classes at: - Topic: Chemical Equilibrium

Classes at: - Topic: Chemical Equilibrium PHYSICAL CHEMISTRY by: SHAILENDRA KR. Classes at: - SCIENCE TUTORIALS; Opp. Khuda Baksh Library, Ashok Rajpath, Patna PIN POINT STUDY CIRCLE; House No. 5A/65, Opp. Mahual Kothi, Alpana Market, Patna Topic:

More information

I. Equilibrium a dynamic condition in which a forward reaction proceeds at the same rate as the reverse reaction; no changes will be observed

I. Equilibrium a dynamic condition in which a forward reaction proceeds at the same rate as the reverse reaction; no changes will be observed UNIT IX EQUILIBRIUM 1 I. Equilibrium a dynamic condition in which a forward reaction proceeds at the same rate as the reverse reaction; no changes will be observed II. Chemical Equilibrium * physical equilibrium

More information

Solubility Multiple Choice

Solubility Multiple Choice Solubility Multiple Choice August 1998 13) In 0.20M Na 2 CrO 4, the ion concentrations are [Na + ] [CrO 2-4 ] A 0.40M 0.20M B 0.20M 0.20M C 0.20M 0.40M D 0.40M 0.80M 14) Which of the following compounds

More information

Honors Chemistry. Chapter 18: Equilibrium Worksheet Date / / Period

Honors Chemistry. Chapter 18: Equilibrium Worksheet Date / / Period Honors Chemistry Name Chapter 18: Equilibrium Worksheet Date / / Period 1. Write the expressions for the equilibrium constant K c and indicate if the reactions are homogeneous equilibriums or s for the

More information

Chapter 17: Solubility & Complex Ion Equilibria

Chapter 17: Solubility & Complex Ion Equilibria Chapter 17: Solubility & Complex Ion Equilibria Solubility Equilibria equilibrium between a solid and its ions in solution ex. for calcium phosphate Ca3(PO4)2 (s) 3 Ca2+ (aq) + 2 PO43 (aq) this is a heterogeneous

More information

SOLUBILITY REVIEW Page 1 of 18

SOLUBILITY REVIEW Page 1 of 18 SOLUBILITY REVIEW Page 1 of 18 1. Two solutions are mixed and a precipitate forms, then the trial ion product is A. equal to Ksp. B. greater than Ksp. C. less than Ksp. D. less than OR equal to Ksp. 2.

More information

Chapter 16 Cartoon from: Strong Acid/Base Neutralization

Chapter 16 Cartoon from:  Strong Acid/Base Neutralization Chapter 16 Applications of Aqueous Equilibria Chapter 16 Cartoon from: http://www.nearingzero.net/sci_chemistry.html 1 Strong Acid/Base Neutralization When a strong acid and a strong base react, the products

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

= 5.16 x 10 3 = 5.2 x 10 3 M. -7 = 1.19 x 10 2 = 1.2 x 10 2 M

= 5.16 x 10 3 = 5.2 x 10 3 M. -7 = 1.19 x 10 2 = 1.2 x 10 2 M Chemistry B1B Chapter 17 Homework Answers 17.16. a. The chemical equations are AX A + + X AX 2 A 2+ + 2X AX 3 A 3+ + 3X b. The concentration of each solution in the compound is 0.25 M. This is because

More information

ALE 17. Equilibria of Slightly Soluble Compounds. How is the solubility of a salt related to its solubility product constant?

ALE 17. Equilibria of Slightly Soluble Compounds. How is the solubility of a salt related to its solubility product constant? Name Chem 163 Section: Team Number: ALE 17. Equilibria of Slightly Soluble Compounds (Reference: 19.3 Silberberg 5 th edition) How is the solubility of a salt related to its solubility product constant?

More information

9.3. Predicting the Formation of a Precipitate. Comparing the Ion Product With the Solubility Product

9.3. Predicting the Formation of a Precipitate. Comparing the Ion Product With the Solubility Product Predicting the Formation of a Precipitate In section 9.2, you worked with concentrations of ions in solutions at equilibrium. You used K sp to determine the solubility of ionic substances in pure water

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

Acid-Base Equilibria and Solubility Equilibria. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.

Acid-Base Equilibria and Solubility Equilibria. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Acid-Base Equilibria and Solubility Equilibria 1 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. A buffer solution is a solution of: 1. A weak acid or a weak

More information

Learning Objectives. Solubility and Complex-ion Equilibria. Contents and Concepts

Learning Objectives. Solubility and Complex-ion Equilibria. Contents and Concepts Solubility and Complex-ion Equilibria 1 Contents and Concepts Solubility Equilibria 1. The Solubility Product Constant. Solubility and the Common-Ion Effect 3. Precipitation Calculations. Effect of ph

More information

Test 11: Equilibrium

Test 11: Equilibrium Name: Sunday, April 05, 2009 Test 11: Equilibrium 1. Given the reaction at equilibrium: Which change will shift the equilibrium to the right? A. increasing the temperature C. decreasing the amount of SO

More information

AP*Chemistry Solubility Equilibria

AP*Chemistry Solubility Equilibria AP*Chemistry Solubility Equilibria SOLUBILITY EQUILIBRIA (K sp, THE SOLUBILITY PRODUCT) Saturated solutions of salts are another type of chemical equilibria. Remember those solubility rules? The fine print

More information

Composition of Solutions

Composition of Solutions 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

More information

. Which one of the following mixtures is suitable for making buffers? 1. H3PO4 and NaH2PO4 2. Na2CO3 and NaHCO3 3. NH4Cl and NH3

. Which one of the following mixtures is suitable for making buffers? 1. H3PO4 and NaH2PO4 2. Na2CO3 and NaHCO3 3. NH4Cl and NH3 . Which one of the following mixtures is suitable for making buffers? 1. H3PO4 and NaH2PO4 2. Na2CO3 and NaHCO3 3. NH4Cl and NH3 [A] 3 only [B] 2 only [C] 1 only [D] 1, 2, and 3 [E] 1 and 2 only 2. For

More information

Ch. 15 Solutions Problem Set 15.1 Problem Set 15.2 Problem Set 15.3 Ch. 19 Acids and Bases

Ch. 15 Solutions Problem Set 15.1 Problem Set 15.2 Problem Set 15.3 Ch. 19 Acids and Bases Ch. 15 Solutions Problem Set 15.1 Solution terminology Why/how dissolving occurs Factors affecting rate of solvation vs. solubility Heats of solution Problem Set 15.2 Concentration (Molarity) problems

More information

Assignment 17 A 1- (i) (ii)

Assignment 17 A 1- (i) (ii) Assignment 17 A 1- Does the ph increase, decrease, or remain the same on addition of each of the following? (i) NaNO 2 to a solution of HNO 2, (ii) HCl to a solution of NaC 2 H 3 O 2 a) (i) increase, (ii)

More information

Chapter 17: Equilibrium: The Extent of Chemical Reactions

Chapter 17: Equilibrium: The Extent of Chemical Reactions CHEM 1B: GENERAL CHEMISTRY Chapter 17: Equilibrium: The Extent of Chemical Reactions Instructor: Dr. Orlando E. Raola Santa Rosa Junior College 17-1 Chapter 17 Equilibrium: The Extent of Chemical Reactions

More information

COMMON ION & BUFFER PROBLEMS KEY

COMMON ION & BUFFER PROBLEMS KEY COMMON ION & BUFFER PROBLEMS KEY 1) What is the ph of a solution containing 0.0 M NH and 0.15 M NH 4 NO? K b for NH = 1.810-5 NH is a weak base: NH H O NH 4 OH - NH 4 NO is a salt: NH 4 NO NH 4 NO ; thus

More information

Equilibrium Process. Practice Exam Equilibrium. Quadratic Equation: ax 2 + bx + c = 0. Equilibrium constant K p and K c : K p = K c (RT) Δn.

Equilibrium Process. Practice Exam Equilibrium. Quadratic Equation: ax 2 + bx + c = 0. Equilibrium constant K p and K c : K p = K c (RT) Δn. Equilibrium Process Practice Exam Equilibrium Name (last) (First) Read all questions before you start. Show all work and explain your answers to receive full credit. Report all numerical answers to the

More information

SOLUBILITY EQUILIBRIUM

SOLUBILITY EQUILIBRIUM Introduction SOLUBILITY EQUILIBRIUM A. Ionic vs Molecular Solutions 1. Ionic Compounds form Ionic Solutions a) Ionic compounds ( metal + non-metal ) dissolved in water to form Ionic Solutions eg1: dissociation

More information

Chapter 16 Additional Aspects of Aqueous Equilibria. The Common Ion Effect and Buffers A buffer is a combination of a weak acid or base with its salt.

Chapter 16 Additional Aspects of Aqueous Equilibria. The Common Ion Effect and Buffers A buffer is a combination of a weak acid or base with its salt. Chapter 16 Additional Aspects of Aqueous Equilibria The Common Ion Effect and Buffers A buffer is a combination of a weak acid or base with its salt. 0.1 M HOAc and 0.1 M NaOAc HOAc H + + OAc Addition

More information

CHEMICAL REACTIONS. When sodium bicarbonate, e.g. baking soda, is combined with an acid, a gas is produced

CHEMICAL REACTIONS. When sodium bicarbonate, e.g. baking soda, is combined with an acid, a gas is produced CHEMICAL REACTIONS OBJECTIVES 1. To study reactions between ions in aqueous solutions 2. To observe exothermic and endothermic reactions 3. To study oxidation-reduction reactions 4. To practice balancing

More information

are the common ions from Ag 2 CrO 4. Also [Ag + ] must be twice [Ag 2 CrO 4 ] from the balanced dissolution equation:

are the common ions from Ag 2 CrO 4. Also [Ag + ] must be twice [Ag 2 CrO 4 ] from the balanced dissolution equation: Problem 16.9 A saturated solution of Ag 2 CrO 4 prepared by dissolving Ag 2 CrO 4 solid (whereby there is excess solid remaining) has [CrO 4 ] = 6.5 x 10-5 M. Calculate K sp for Ag 2 CrO 4. Ag + and CrO

More information

Since this is an equilibrium reaction, we can write the equilibrium constant expression as

Since this is an equilibrium reaction, we can write the equilibrium constant expression as Solubility Equilibrium Solubility is the ability of a substance to dissolve in water. The solubility is measured in terms of concentration of an ion that is present in a smaller ratio in solution. On the

More information

Solubility. Solubility. 13-Jun-11. Chem 1011 Intersession 2011 Class #32. Solubility Equilibria / Solubility Product Constant (K sp ) 1

Solubility. Solubility. 13-Jun-11. Chem 1011 Intersession 2011 Class #32. Solubility Equilibria / Solubility Product Constant (K sp ) 1 1 2 Class 32: Solubility Equilibria / Solubility Product (K sp ) Sec 16.5 Solubility Equilibria and Solubility Product Constant K sp and Molar Solubility K sp and Relative Solubility The Effect of a Common

More information

Chemical Reactions. Chapter 4

Chemical Reactions. Chapter 4 Chemical Reactions Chapter 4 Chemical Equations A balanced chemical equation gives us a variety of information about the relative amounts of substances reacting and forming. Law of Conservation of Mass

More information

Kinetics and Equilibrium

Kinetics and Equilibrium Kinetics and Equilibrium 1. In a chemical reaction the use of a catalyst results in a decrease in the (1) activation energy; (2) potential energy of the reactants; (3) heat of reaction; (4) amount of products.

More information

Lab 2: Properties of Systems in Chemical Equilibrium

Lab 2: Properties of Systems in Chemical Equilibrium Lab 2: Properties of Systems in Chemical Equilibrium The two key purposes of this lab are: 1) To observe how systems in equilibrium respond to stress by: increasing or decreasing the concentration of one

More information

Solubility and Complex-ion Equilibria

Solubility and Complex-ion Equilibria Solubility and Complex-ion Equilibria 1 1 Contents and Concepts Solubility Equilibria 1. The Solubility Product Constant 2. Solubility and the Common-Ion Effect 3. Precipitation Calculations 4. Effect

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

Solubility Equilibria

Solubility Equilibria Chapter 17: Acid-Base Equilibria and Solubility Equilibria Key topics: Common ion effect Buffers Acid-base equilibria Solubility equilibria; complex ion formation The Common Ion Effect If we have two solutes

More information

Reading: Moore chapter 17, sections Questions for Review and Thought: 54, 56, 58, 60, 62, 66, 72, 74, 86.

Reading: Moore chapter 17, sections Questions for Review and Thought: 54, 56, 58, 60, 62, 66, 72, 74, 86. Applications of Aqueous Equilibria II: Solubility and Ksp Reading: Moore chapter 17, sections 17.4-17.6 Questions for Review and Thought: 54, 56, 58, 60, 62, 66, 72, 74, 86. Key Concepts and Skills: definition

More information

Equlibrium Practice Exam Key

Equlibrium Practice Exam Key Equlibrium Practice Exam Key Note: All problems included in this practice exam are drawn from problems used in previous semesters. Exams typically include 7 or 8 problems that are a mixture of qualitative

More information

Equilibrium A State of Balance. Chapter 15

Equilibrium A State of Balance. Chapter 15 Equilibrium A State of Balance Chapter 15 Reactions are reversible A + B C + D ( forward) C + D A + B (reverse) Initially there is only A and B so only the forward reaction is possible As C and D build

More information

Salt Solubility. Chapter 18

Salt Solubility. Chapter 18 Salt Solubility Chapter 18 1 1 Solubility product constant K sp Unitless CaF 2(s) Ca 2+ (aq) + 2F - (aq) K sp = [Ca 2+ ][F - ] 2 [Ca 2+ ] = molar solubility (in M) Get K sp values from Appendix J, pages

More information

Appendix D. Reaction Stoichiometry D.1 INTRODUCTION

Appendix D. Reaction Stoichiometry D.1 INTRODUCTION Appendix D Reaction Stoichiometry D.1 INTRODUCTION In Appendix A, the stoichiometry of elements and compounds was presented. There, the relationships among grams, moles and number of atoms and molecules

More information

Chapter 5 Chemical Quantities and Reactions

Chapter 5 Chemical Quantities and Reactions Chapter 5 Chemical Quantities and Reactions 1 Avogadro's Number Small particles such as atoms, molecules, and ions are counted using the mole. 1 mole = 6.02 x 10 23 items Avogadro s number 602 000 000

More information

17.1 The Common-Ion Effect

17.1 The Common-Ion Effect Lecture Presentation Chapter 17 Additional Aspects of Yonsei University 17.1 The Common-Ion Effect Consider a solution of acetic acid: CH 3 COOH(aq) + H 2 O(l) H 3 O + (aq) + CH 3 COO (aq) If acetate ion

More information

Chapter 14. CHEMICAL EQUILIBRIUM

Chapter 14. CHEMICAL EQUILIBRIUM Chapter 14. CHEMICAL EQUILIBRIUM 14.1 THE CONCEPT OF EQUILIBRIUM AND THE EQUILIBRIUM CONSTANT Many chemical reactions do not go to completion but instead attain a state of chemical equilibrium. Chemical

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

AgCl(s) º Ag + (aq) + Cl (aq) Ag 3 PO 4 (s) º 3 Ag + (aq) + PO 4 3 (aq) Introduction to Sparingly Soluble Salts. Ag + (aq) Cl (aq) AgCl(s)

AgCl(s) º Ag + (aq) + Cl (aq) Ag 3 PO 4 (s) º 3 Ag + (aq) + PO 4 3 (aq) Introduction to Sparingly Soluble Salts. Ag + (aq) Cl (aq) AgCl(s) Introduction to Sparingly Soluble Salts All ionic compounds dissolve to some extent in water, but the range of solubilities is quite remarkable. (See the table on the right.) Sparingly soluble salts are

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

3- (aq) K sp = [Ba 2+ ] 3 [PO 4 3- ] 2

3- (aq) K sp = [Ba 2+ ] 3 [PO 4 3- ] 2 Name: 1 Solubility Problems SOLUTIONS 1. Write balanced chemical equations and the K sp expressions for the dissolving of the following compounds in water. a) sodium sulfide Na 2 S (s) 2 Na + + S K sp

More information

- soluble none Cl - soluble except Ag +, Hg 2 2+, *Pb 2+ I soluble except Ag +, Hg 2 2+, Pb 2+ SO 4. PO 3-4 insoluble except Group IA and NH + 4

- soluble none Cl - soluble except Ag +, Hg 2 2+, *Pb 2+ I soluble except Ag +, Hg 2 2+, Pb 2+ SO 4. PO 3-4 insoluble except Group IA and NH + 4 1a. Define the terms precipitation and solubility. Precipitation is the act of precipitating or forming a precipitate. A precipitate is an insoluble solid formed by the reaction of two or more solutions

More information

Learning Objectives. Solubility and Complex-ion Equilibria. Contents and Concepts. 3. Precipitation Calculations. 4. Effect of ph on Solubility

Learning Objectives. Solubility and Complex-ion Equilibria. Contents and Concepts. 3. Precipitation Calculations. 4. Effect of ph on Solubility Solubility and Complex-ion Equilibria. Solubility and the Common-Ion Effect a. Explain how the solubility of a salt is affected by another salt that has the same cation or anion. (common ion) b. Calculate

More information

Thermodynamics. S (reactants) S S (products) AP Chemistry. Period Date / / R e v i e w. 1. Consider the first ionization of sulfurous acid:

Thermodynamics. S (reactants) S S (products) AP Chemistry. Period Date / / R e v i e w. 1. Consider the first ionization of sulfurous acid: AP Chemistry Thermodynamics 1. Consider the first ionization of sulfurous acid: H 2SO 3(aq) H + (aq) + HSO 3 - (aq) Certain related thermodynamic data are provided below: H 2SO 3(aq) H + (aq) HSO 3 - (aq)

More information

Stoichiometry Homework Packet

Stoichiometry Homework Packet Name: Period: Stoichiometry Homework Packet Chapter 16: 16.1 and 16.2 Chapter 11: 11.1 and 11.2 Chapter 12: All sections Upon completion of the Stoichiometry Unit, you should be able to: Explain how a

More information

7. Consider the reaction coordinate diagram shown. Which statement is true? C D

7. Consider the reaction coordinate diagram shown. Which statement is true? C D SPRING 2001 FINAL 1. A solution prepared by dissolving 6.54 g of a non-volatile solute in 60.0 g of water boils at 100.37 C. What is the approximate molar mass of the solute? K b of H 2 O = 0.512 C/m.

More information

Chemistry 132 NT. Solubility Equilibria. The most difficult thing to understand is the income tax. Solubility and Complex-ion Equilibria

Chemistry 132 NT. Solubility Equilibria. The most difficult thing to understand is the income tax. Solubility and Complex-ion Equilibria Chemistry 13 NT The most difficult thing to understand is the income tax. Albert Einstein 1 Chem 13 NT Solubility and Complex-ion Equilibria Module 1 Solubility Equilibria The Solubility Product Constant

More information

Problems -- Chapter Write balanced chemical equations for the important equilibrium that is occurring in an aqueous solution of the following.

Problems -- Chapter Write balanced chemical equations for the important equilibrium that is occurring in an aqueous solution of the following. Problems -- Chapter 1 1. Write balanced chemical equations for the important equilibrium that is occurring in an aqueous solution of the following. (a) NaNO and HNO answers: see end of problem set (b)

More information