Summer 2003 CHEMISTRY 115 EXAM 3(A)

Save this PDF as:
 WORD  PNG  TXT  JPG

Size: px
Start display at page:

Download "Summer 2003 CHEMISTRY 115 EXAM 3(A)"

Transcription

1 Summer 2003 CHEMISTRY 115 EXAM 3(A) 1. In which of the following solutions would you expect AgCl to have the lowest solubility? A M BaCl 2 B. pure water C M NaCl D M KCl 2. Calculate the ph of a 1L solution containing 0.40 mol HF and 0.1 mol HCl. (K a = 6.8x10 4 for HF) A B. 1.0 C. 2.6 D What is the effect of addition of an acid to a buffered solution of HF and KF? A. [HF] will increase, [F ] will decrease B. [HF] will increase, [F ] will increase C. [HF] will decrease, [F ] will decrease D. [HF] will decrease, [F ] will increase 4. Calculate ph of a buffer composed of M HNO 2 (K a =4.5x10 4 )and 0.1 M KNO 2 A. 8.4 B. 7.0 C. 5.6 D Which of the following substances, when added to a solution of hydrofluoric acid, could be used to prepare a buffer solution? A. NaF B. NaNO 3 C. NaCl D. NaBr 6. Consider the titration diagram shown on the plot below. What type of substance was originally in the flask? A. weak acid B. weak base C. strong acid D. strong base ml of 0.1 M HF (K a =6.8x10 4 ) is titrated with 0.1 M NaOH. What is the ph of the solution when 10 ml of NaOH have been added? A. 7.2 B. 6.3 C. 3.2 D. 2.1

2 8. What is the molar solubility of MgC 2 O 4 (K sp =8.6x10 5 )? [H 2 C 2 O 4 is the oxalic acid.] A. 9.3 x 10 3 B. 6.4 x C. 7.1 x 10 9 D. 2.8 x Which of the following substances will increase in solubility if the ph of the saturated solution of the compound is lowered? A. AgCl B. AgI C. Cr(OH) 3 D. PbCl Which substance is serving as a reducing agent in the following reaction? Fe 2 S HNO 3 2Fe(NO 3 ) 3 + 3S + 6NO 2 + 6H 2 O A. HNO 3 B. S C. NO 2 D. Fe 2 S What is the oxidation number of manganese in KMnO 4? A. 0 B. +1 C. +7 D What is the coefficient of iodine when the following reaction (acidic solution) is correctly balanced? MnO 4 + I Mn 2+ + I 2 A. 5 B. 7 C. 2 D Which of the following transformation could take place at the cathode of an electrochemical cell? A. MnO 2 MnO 4 B. Br 2 BrO 3 C. Mn 2+ MnO 4 D. HSO 4 H 2 SO The standard reduction potentials for Pb 2+ and Ag + are 0.13 V and +0.8 V, respectively. Calculate E 0 for a cell in which the overall reaction is Pb + 2Ag + Pb Ag A B C D Respective standard reduction potentials of Pb 2+ and Ni 2+ are 0.13 V and 0.28 V. An electrochemical cell is built from Pb electrode in Pb 2+ solution and Ni electrode in Ni 2+ solution. The reduction reaction will occur on the electrode which is called: A. Pb, anode

3 B. Pb, cathode C. Ni, anode D. Ni, cathode 16. Calculate G (in J) for the reaction of elemental bromine Br 2 (E 0 red = 1.09 V) with chloride ion (Cl 2, E o red = 1.36) A. 2.1 x 10 4 B x 10 4 C x 10 5 D x The standard emf for Zn/Cu voltaic cell is 1.10 V. Calculate the cell emf when the concentration of Zn 2+ and Cu 2+ in the solution are 0.01 M and 1.0 M, respectively. A V B V C V D V 18. Using the table of standard reduction potentials indicate the metal which could provide cathode protection to zinc: A. Fe B. Ag C. Al D. Cu 19. The electrolysis of NiCl 2 produces Ni and Cl 2. What is the minimum external emf needed to drive electrolysis under standard conditions? A V B V C V D V 20. Identify the products of electrolysis of an aqueous solution of CuI 2 and FeCl 2 (acidic solution). [Hint: Assume that the concentration of OH is equal to zero.] A. Cu and O 2 B. Fe and Cl 2 C. Fe and O 2 D. Cu and I 2 EXAM 3(B) 1. In which of the following solutions would you expect AgCl to have the lowest solubility? A. pure water B M BaCl 2 C M KCl D M NaCl

4 2. Calculate the ph of a 1L solution containing 0.40 mol HF and 0.1 mol HCl. (K a = 6.8x10 4 for HF) A B C. 2.6 D What is the effect of addition of an acid to a buffered solution of HF and KF? A. [HF] will decrease, [F ] will increase B. [HF] will increase, [F ] will increase C. [HF] will decrease, [F ] will decrease D. [HF] will increase, [F ] will decrease 4. Calculate ph of a buffer composed of M HNO 2 (K a =4.5x10 4 )and 0.1 M KNO 2 A. 5.6 B. 7.0 C. 8.4 D Which of the following substances, when added to a solution of hydrofluoric acid, could be used to prepare a buffer solution? A. NaCl B. NaNO 3 C. NaF D. NaBr 6. Consider the titration diagram shown on the plot below. What type of substance was originally in the flask? A. weak acid B. strong acid C. weak base D. strong base ml of 0.1 M HF (K a =6.8x10 4 ) is titrated with 0.1 M NaOH. What is the ph of the solution when 10 ml of NaOH have been added? A. 3.2 B. 6.3 C. 7.2 D What is the molar solubility of MgC 2 O 4 (K sp =8.6x10 5 )? [H 2 C 2 O 4 is the oxalic acid.] A. 6.4 x B. 9.3 x 10 3 C. 2.8 x 10 2 D. 7.1 x Which of the following substances will increase in solubility if the ph of the saturated solution of the compound is lowered? A. PbCl 2 B. AgCl C. Cr(OH) 3 D. AgI

5 10. Which substance is serving as a reducing agent in the following reaction? Fe 2 S HNO 3 2Fe(NO 3 ) 3 + 3S + 6NO 2 + 6H 2 O A. HNO 3 B. Fe 2 S 3 C. NO 2 D. S 11. What is the oxidation number of manganese in KMnO 4? A. +7 B. 0 C. +5 D What is the coefficient of iodine when the following reaction (acidic solution) is correctly balanced? MnO 4 + I Mn 2+ + I 2 A. 7 B. 5 C. 4 D Which of the following transformation could take place at the cathode of an electrochemical cell? A. Mn 2+ MnO 4 B. MnO 2 MnO 4 C. Br 2 BrO 3 D. HSO 4 H 2 SO The standard reduction potentials for Pb 2+ and Ag + are 0.13 V and +0.8 V, respectively. Calculate E 0 for a cell in which the overall reaction is Pb + 2Ag + Pb Ag A B C D Respective standard reduction potentials of Pb 2+ and Ni 2+ are 0.13 V and 0.28 V. An electrochemical cell is built from Pb electrode in Pb 2+ solution and Ni electrode in Ni 2+ solution. The reduction reaction will occur on the electrode which is called: A. Ni, cathode B. Ni, anode C. Pb, cathode D. Pb, anode 16. Calculate G (in J) for the reaction of elemental bromine Br 2 (E 0 red = 1.09 V) with chloride ion (Cl 2, E o red = 1.36) A x 10 5 B x 10 5 C. 2.1 x 10 4 D x The standard emf for Zn/Cu voltaic cell is 1.10 V. Calculate the cell emf when the concentration of Zn 2+ and Cu 2+ in the solution are 0.01 M and 1.0 M, respectively.

6 A V B V C V D V 18. Using the table of standard reduction potentials indicate the metal which could provide cathode protection to zinc: A. Cu B. Fe C. Al D. Ag 19. The electrolysis of NiCl 2 produces Ni and Cl 2. What is the minimum external emf needed to drive electrolysis under standard conditions? A V B V C V D V 20. Identify the products of electrolysis of an aqueous solution of CuI 2 and FeCl 2 (acidic solution). [Hint: Assume that the concentration of OH is equal to zero.] A. Fe and O 2 B. Fe and Cl 2 C. Cu and I 2 D. Cu and O 2

BALANCING REDOX EQUATIONS EXERCISE

BALANCING REDOX EQUATIONS EXERCISE +5 6 1. Ag + NO3 Ag 1+ + NO 0 +5 2 +1 +2 2 4 +4 +2 2 2. N2H4 + H2O2 N2 + H2O 2 +1 +1 1 0 +1 2 +6 6 +4 4 3. CO + Fe2O3 FeO + CO2 +2 2 +3 2 +2 2 +4 2 +5 6 +4 4 +4 4 4. NO3 + CO CO2 + NO2 +5 2 +2 2 +4 2 +4

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. Chemistry 1C-Dr. Larson Chapter 20 Review Questions MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) is reduced in the following reaction: Cr2O7

More information

2. Write the chemical formula(s) of the product(s) and balance the following spontaneous reactions.

2. Write the chemical formula(s) of the product(s) and balance the following spontaneous reactions. 1. Using the Activity Series on the Useful Information pages of the exam write the chemical formula(s) of the product(s) and balance the following reactions. Identify all products phases as either (g)as,

More information

K + Cl - Metal M. Zinc 1.0 M M(NO

K + Cl - Metal M. Zinc 1.0 M M(NO Redox and Electrochemistry This section should be fresh in your minds because we just did this section in the text. Closely related to electrochemistry is redox chemistry. Count on at least one question

More information

Redox and Electrochemistry

Redox and Electrochemistry Name: Thursday, May 08, 2008 Redox and Electrochemistry 1. A diagram of a chemical cell and an equation are shown below. When the switch is closed, electrons will flow from 1. the Pb(s) to the Cu(s) 2+

More information

Chapter 20. MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

Chapter 20. MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. Chapter 20 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) The gain of electrons by an element is called. A) oxidation B) reduction C) sublimation

More information

38. Consider the following reaction that occurs in a breathalyzer: 2Cr 2 O 7

38. Consider the following reaction that occurs in a breathalyzer: 2Cr 2 O 7 Electrochemistry Multiple Choice January 1999 37. Consider the following redox reaction: 2MnO 4 - + 3ClO 3 - + H 2 O 3ClO 4 - + 2MnO 2 + 2OH - The reducing agent is A. H 2 O B. ClO 3 - C. MnO 2 D. MnO

More information

CHM1 Review Exam 12. Topics REDOX

CHM1 Review Exam 12. Topics REDOX CHM1 Review Exam 12 Topics REDOX REDOX Reactions Oxidation Reduction Oxidizing agent Reducing agent Galvanic (Voltaic) Cells Anode Cathode Salt bridge Electrolyte Half-reactions Voltage o Positive voltages

More information

Oxidation-Reduction Reactions

Oxidation-Reduction Reactions Chapter 18 Oxidation-Reduction Reactions 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

More information

Electrochemistry - ANSWERS

Electrochemistry - ANSWERS Electrochemistry - ANSWERS 1. Using a table of standard electrode potentials, predict if the following reactions will occur spontaneously as written. a) Al 3+ + Ni Ni 2+ + Al Al 3+ + 3e - Al E = -1.68

More information

1332 CHAPTER 18 Sample Questions

1332 CHAPTER 18 Sample Questions 1332 CHAPTER 18 Sample Questions Couple E 0 Couple E 0 Br 2 (l) + 2e 2Br (aq) +1.06 V AuCl 4 + 3e Au + 4Cl +1.00 V Ag + + e Ag +0.80 V Hg 2+ 2 + 2e 2 Hg +0.79 V Fe 3+ (aq) + e Fe 2+ (aq) +0.77 V Cu 2+

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

(All questions may be completed without the use of a calculator. All answers given were generated without the use of a calculator.

(All questions may be completed without the use of a calculator. All answers given were generated without the use of a calculator. ELECTROCHEMISTRY (All questions may be completed without the use of a calculator. All answers given were generated without the use of a calculator.) 1) Balance each skeleton reaction, calculate ε cell,

More information

3. Which of the following describes a conjugate acid-base pair for the following equilibrium? CN - (aq) + CH 3 NH 3 + (aq) H 2 CO 3 (aq) + H 2 O (l)

3. Which of the following describes a conjugate acid-base pair for the following equilibrium? CN - (aq) + CH 3 NH 3 + (aq) H 2 CO 3 (aq) + H 2 O (l) Acids, Bases & Redox 1 Practice Problems for Assignment 8 1. A substance which produces OH ions in solution is a definition for which of the following? (a) an Arrhenius acid (b) an Arrhenius base (c) a

More information

Electrochemistry Worksheet

Electrochemistry Worksheet Electrochemistry Worksheet 1. Assign oxidation numbers to each atom in the following: a. P 4 O 6 b. BiO 3 c. N 2 H 4 d. Mg(BrO 4 ) 2 e. MnSO 4 f. Mn(SO 4 ) 2 2. For each of the reactions below identify

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

Common Ion Effects. CH 3 CO 2 (aq) + Na + (aq)

Common Ion Effects. CH 3 CO 2 (aq) + Na + (aq) Common Ion Effects If two reactions both involve the same ion, then one reaction can effect the equilibrium position of the other reaction. The ion that appears in both reactions is the common ion. Buffers

More information

Balancing Equations Notes

Balancing Equations Notes . Unit 9 Chemical Equations and Reactions What is a Chemical Equation? A Chemical Equation is a written representation of the process that occurs in a chemical reaction. A chemical equation is written

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

Chapter 4: Solution Stoichiometry Cont. Aqueous Solutions

Chapter 4: Solution Stoichiometry Cont. Aqueous Solutions Chapter 4: Solution Stoichiometry Cont. 1 Aqueous Solutions Molarity (dilution calculations, solution stoichiometry); Solubility and Solubility Rules Molecular, Ionic and Net Ionic Equations Precipitation

More information

Solutions CHAPTER Specific answers depend on student choices.

Solutions CHAPTER Specific answers depend on student choices. CHAPTER 15 1. Specific answers depend on student choices.. A heterogeneous mixture does not have a uniform composition: the composition varies in different places within the mixture. Examples of non homogeneous

More information

CHAPTER 21 ELECTROCHEMISTRY

CHAPTER 21 ELECTROCHEMISTRY Chapter 21: Electrochemistry Page 1 CHAPTER 21 ELECTROCHEMISTRY 21-1. Consider an electrochemical cell formed from a Cu(s) electrode submerged in an aqueous Cu(NO 3 ) 2 solution and a Cd(s) electrode submerged

More information

2. In a double displacement reaction, 3. In the chemical equation, H 2 O 2 H 2 + O 2, the H 2 O 2 is a

2. In a double displacement reaction, 3. In the chemical equation, H 2 O 2 H 2 + O 2, the H 2 O 2 is a What are the missing coefficients for the skeleton equation below? Al 2 (SO 4 ) 3 + KOH Al(OH) 3 + K 2 SO 4 2. In a double displacement reaction, A. 1,6,2,3 B. 2,12,4,6 C. 1,3,2,3 D. 4,6,2,3 E. 2,3,1,1

More information

Two Types of Chemical Rxns. Oxidation/Reduction. Two Types of Chemical Rxns. Two Types of Chemical Rxns. Review of Oxidation Numbers

Two Types of Chemical Rxns. Oxidation/Reduction. Two Types of Chemical Rxns. Two Types of Chemical Rxns. Review of Oxidation Numbers Two Types of Chemical Rxns Oxidation/Reduction Chapter 20 1. Exchange of Ions no change in charge/oxidation numbers Acid/Base Rxns NaOH + HCl Two Types of Chemical Rxns Precipitation Rxns Pb(NO 3 ) 2 (aq)

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

AP Chemistry CHAPTER 20- Electrochemistry 20.1 Oxidation States

AP Chemistry CHAPTER 20- Electrochemistry 20.1 Oxidation States AP Chemistry CHAPTER 20- Electrochemistry 20.1 Oxidation States Chemical reactions in which the oxidation state of a substance changes are called oxidation-reduction reactions (redox reactions). Oxidation

More information

Name AP CHEM / / Collected Essays Chapter 17 Answers

Name AP CHEM / / Collected Essays Chapter 17 Answers Name AP CHEM / / Collected Essays Chapter 17 Answers 1980 - #2 M(s) + Cu 2+ (aq) M 2+ (aq) + Cu(s) For the reaction above, E = 0.740 volt at 25 C. (a) Determine the standard electrode potential for the

More information

OXIDATION REDUCTION. Section I. Cl 2 + 2e. 2. The oxidation number of group II A is always (+) 2.

OXIDATION REDUCTION. Section I. Cl 2 + 2e. 2. The oxidation number of group II A is always (+) 2. OXIDATION REDUCTION Section I Example 1: Na Example 2: 2C1 Example 3: K + + e Na + + e Cl 2 + 2e K Example 4: C1 2 + 2e 2Cl 1. The oxidation number of group I A is always (+) 1. 2. The oxidation number

More information

Unit 9.2 Stoichiometry - Balancing Reactions-2. Types of Chemical Reactions. Single Replacement Reactions

Unit 9.2 Stoichiometry - Balancing Reactions-2. Types of Chemical Reactions. Single Replacement Reactions Unit 9.2 Stoichiometry - Reactions-2 State College Area School District Teacher: Van Der Sluys Types of Chemical Reactions Combustion C n H m + O 2 > CO 2 + H 2 O Synthesis (Combination) Decomposition

More information

ELECTROCHEMISTRY. these are systems involving oxidation or reduction there are several types METALS IN CONTACT WITH SOLUTIONS OF THEIR IONS

ELECTROCHEMISTRY. these are systems involving oxidation or reduction there are several types METALS IN CONTACT WITH SOLUTIONS OF THEIR IONS 1 ELECTROCHEMISTRY REDOX Reduction gain of electrons Cu + 2e > Cu(s) Oxidation removal of electrons Zn(s) > Zn + 2e HALF CELLS these are systems involving oxidation or reduction there are several types

More information

4 theoretical problems 2 practical problems

4 theoretical problems 2 practical problems 1 st 4 theoretical problems 2 practical problems FIRST INTERNATIONAL CHEMISTRY OLYMPIAD PRAGUE 1968 CZECHOSLOVAKIA THEORETICAL PROBLEMS PROBLEM 1 A mixture of hydrogen and chlorine kept in a closed flask

More information

Chemistry Continuing Practice Packet

Chemistry Continuing Practice Packet Chemistry Continuing Practice Packet Mrs. Andrechek Webberville High School The best way to learn and remember chemistry is to practice. Check out the following websites: http://www.chemistrylecturenotes.com

More information

CHEM 103 Spring 2006 Final Exam 5 June 2006

CHEM 103 Spring 2006 Final Exam 5 June 2006 Name CHEM 103 Spring 2006 Final Exam 5 June 2006 Multiple Choice (5 points each) Write the letter of the choice that best completes the statement or answers the question in the blank provided 1. An aqueous

More information

Balancing Equations Notes

Balancing Equations Notes Unit 7 Chemical Equations and Reactions What is a Chemical Equation? A Chemical Equation is a written representation of the process that occurs in a chemical reaction. A chemical equation is written with

More information

Chapter 6 Oxidation-Reduction Reactions. Section 6.1 2. Which one of the statements below is true concerning an oxidation-reduction reaction?

Chapter 6 Oxidation-Reduction Reactions. Section 6.1 2. Which one of the statements below is true concerning an oxidation-reduction reaction? Chapter 6 Oxidation-Reduction Reactions 1. Oxidation is defined as a. gain of a proton b. loss of a proton c. gain of an electron! d. loss of an electron e. capture of an electron by a neutron 2. Which

More information

Exam 3 Review Problems: Useful Equations: G o = RTlnK G o = H o T S o G o = nfe o ln K = ne o /0.0257 E cell = E o cell RT/nF lnq

Exam 3 Review Problems: Useful Equations: G o = RTlnK G o = H o T S o G o = nfe o ln K = ne o /0.0257 E cell = E o cell RT/nF lnq Exam 3 Review Problems: Useful Equations: G o = RTlnK G o = H o T S o G o = nfe o ln K = ne o /0.0257 E cell = E o cell RT/nF lnq 1. Assuming the following reaction proceeds in the forward direction, 2

More information

Chapter 16 Acid-Base Equilibria and Solubility Equilibria

Chapter 16 Acid-Base Equilibria and Solubility Equilibria Chapter 16 Acid-Base Equilibria and Solubility Equilibria Student: NOTE: A table of ionization constants and K a 's is required to work some of the problems in this chapter. 1. In which one of the following

More information

Galvanic Cells. SCH4U7 Ms. Lorenowicz. Tuesday, December 6, 2011

Galvanic Cells. SCH4U7 Ms. Lorenowicz. Tuesday, December 6, 2011 Galvanic Cells SCH4U7 Ms. Lorenowicz 1 Electrochemistry Concepts 1.Redox reactions involve the transfer of electrons from one reactant to another 2.Electric current is a flow of electrons in a circuit

More information

CH302 Exam 4 Practice Problems (buffers, titrations, Ksp)

CH302 Exam 4 Practice Problems (buffers, titrations, Ksp) CH302 Exam 4 Practice Problems (buffers, titrations, Ksp) 1 Equilibrium Constants The following equilibrium constants will be useful for some of the problems. Substance Constant Substance Constant HCO

More information

ELECTROCHEMISTRY. these are systems involving oxidation or reduction there are several types METALS IN CONTACT WITH SOLUTIONS OF THEIR IONS

ELECTROCHEMISTRY. these are systems involving oxidation or reduction there are several types METALS IN CONTACT WITH SOLUTIONS OF THEIR IONS 1 ELECTROCHEMISTRY REDOX Reduction gain of electrons Cu 2+ + 2e > Cu (s) Oxidation removal of electrons Zn (s) > Zn 2+ + 2e HALF CELLS these are systems involving oxidation or reduction there are several

More information

Chemistry Continuing Practice Packet

Chemistry Continuing Practice Packet Chemistry Continuing Practice Packet Mrs. Andrechek Webberville High School The best way to learn and remember chemistry is to practice. Check out the following apps: - Mahjong Chem - Formulas Lite - Atoms

More information

Single Replacement Reactions

Single Replacement Reactions Single Replacement Reactions http://group.chem.iastate.edu/greenbowe/sections/projectfolder/flashfiles/redox/home.html Activity 1 Mg(NO 3 ) 2 Zn(NO 3 ) 2 Cu(NO 3 ) 2 AgNO 3 Mg (s) (Reaction 1) (Reaction

More information

Lecture 6. Classes of Chemical Reactions

Lecture 6. Classes of Chemical Reactions Lecture 6 Classes of Chemical Reactions Lecture 6 Outline 6.1 The Role of Water as a Solvent 6.2 Precipitation Reactions 6.3 Acid-Base Reactions 1 Electron distribution in molecules of H 2 and H 2 O The

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

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

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

D. Combustion Reaction CxHy + O 2 CO 2 + H 2 O Example: i) C 4 H 10 + O 2 CO 2 + H 2 O. ii) C 6 H 12 O 6 + O 2 CO 2 + H 2 O

D. Combustion Reaction CxHy + O 2 CO 2 + H 2 O Example: i) C 4 H 10 + O 2 CO 2 + H 2 O. ii) C 6 H 12 O 6 + O 2 CO 2 + H 2 O 1 A. Combination Reaction A + B AB i) SO 3 + H 2 O H 2 SO 4 ii) P + S P 2 S 5 iii) N 2 + H 2 NH 3 B. Decomposition Reaction AB A + B i) H 2 CO 3 H 2 O + CO 2 ii) KClO 3 KCl + O 2 C. Single Displacement

More information

Chapter 4: Reaction in Aqueous Solution

Chapter 4: Reaction in Aqueous Solution Chapter 4: Reaction in Aqueous Solution What is a Solution? Solute + substance dissolved typically smaller quantity Solvent! dissolving medium typically larger quantity Solution homogeneous mixture variable

More information

Answers and Solutions to Text Problems

Answers and Solutions to Text Problems Chapter 6 Answers and Solutions 6 Answers and Solutions to Text Problems 6.1 A chemical change occurs when the atoms of the initial substances rearrange to form new substances. Chemical change is indicated

More information

Chapter 11. Electrochemistry Oxidation and Reduction Reactions. Oxidation-Reduction Reactions. Oxidation-Reduction Reactions

Chapter 11. Electrochemistry Oxidation and Reduction Reactions. Oxidation-Reduction Reactions. Oxidation-Reduction Reactions Oxidation-Reduction Reactions Chapter 11 Electrochemistry Oxidation and Reduction Reactions An oxidation and reduction reaction occurs in both aqueous solutions and in reactions where substances are burned

More information

5.111 Principles of Chemical Science

5.111 Principles of Chemical Science MIT OpenCourseWare http://ocw.mit.edu 5.111 Principles of Chemical Science Fall 2008 For information about citing these materials or our Terms of Use, visit: http://ocw.mit.edu/terms. Page 1 of 10 pages

More information

CHEM 36 General Chemistry EXAM #3 April 17, 2002

CHEM 36 General Chemistry EXAM #3 April 17, 2002 CHEM 36 General Chemistry EXAM #3 April 17, 2002 Name: Anne Sir Kei INSTRUCTIONS: Read through the entire exam before you begin. Answer all of the questions. For questions involving calculations, show

More information

Do Now CHEMICAL REACTIONS. Chemical Reaction. chemical reaction. Chemical Equations. Evidence

Do Now CHEMICAL REACTIONS. Chemical Reaction. chemical reaction. Chemical Equations. Evidence Do Now CHEMICAL REACTIONS What are some signs that a chemical change may have taken place? Where are the reactants and products in a reaction? What do they represent? Describe the law of conservation of

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

Iodometry Titration. Redox titration of iodine and sodium thiosulphate ( Iodometry)

Iodometry Titration. Redox titration of iodine and sodium thiosulphate ( Iodometry) Iodometry Titration Redox titration of iodine and sodium thiosulphate ( Iodometry) Page: 1 Iodometry: When an oxidizing agent (e.g. KMnO 4, H 2 O 2 etc.) is added to excess iodide (I ) to produce iodine

More information

ionic substances (separate) based on! Liquid Mixtures miscible two liquids that and form a immiscible two liquids that form a e.g.

ionic substances (separate) based on! Liquid Mixtures miscible two liquids that and form a immiscible two liquids that form a e.g. Unit 7 Solutions, Acids & Bases Solution mixture + solvent - substance present in the amount solute - in the solvent solvent molecules solute particles ionic substances (separate) based on! Liquid Mixtures

More information

Decomposition. Composition

Decomposition. Composition Decomposition 1. Solid ammonium carbonate is heated. 2. Solid calcium carbonate is heated. 3. Solid calcium sulfite is heated in a vacuum. Composition 1. Barium oxide is added to distilled water. 2. Phosphorus

More information

Chemistry Sample Questions

Chemistry Sample Questions Chemistry Sample Questions Name: 1) Which phase change represents deposition? A) liquid gas B) gas solid C) solid liquid D) gas liquid 2) Which pair has identical electron configurations? A) K 0 and Na

More information

Name Electrochemical Cells Practice Exam Date:

Name Electrochemical Cells Practice Exam Date: Name Electrochemical Cells Practice Exam Date: 1. Which energy change occurs in an operating voltaic cell? 1) chemical to electrical 2) electrical to chemical 3) chemical to nuclear 4) nuclear to chemical

More information

Reaction Type & Balancing Review Questions

Reaction Type & Balancing Review Questions Reaction Type & Balancing Review Questions There are 20 questions sets in this review. The corresponding answers can be found in the second half of this document. 1. Match the term with its proper description.

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

16. What is the H 3 O + concentration of a solution that has an OH concentration of 1 10 3 M? 1) 1 10 4 M 3) 1 10 11 M

16. What is the H 3 O + concentration of a solution that has an OH concentration of 1 10 3 M? 1) 1 10 4 M 3) 1 10 11 M 1. If the [OH ] = 1 10 4 at 298 K for a given solution, the [H + ] of the solution is equal to 1) 1 10 14 3) 1 10 6 2) 1 10 10 4) 1 10 4 2. Based on Reference Table V, which is the strongest base? 1) NO

More information

Ch 20 Electrochemistry: the study of the relationships between electricity and chemical reactions.

Ch 20 Electrochemistry: the study of the relationships between electricity and chemical reactions. Ch 20 Electrochemistry: the study of the relationships between electricity and chemical reactions. In electrochemical reactions, electrons are transferred from one species to another. Learning goals and

More information

2. Write a balanced chemical equation which corresponds to the following equilibrium constant expression. 1/2 3/ 2

2. Write a balanced chemical equation which corresponds to the following equilibrium constant expression. 1/2 3/ 2 Practice Problems for Chem. 1B Exam 1 F2011 These represent the concepts covered for exam 1. There may be some additional net ionic equations from chem. 1A. This is not the exact exam! Sections 16.1-16.3

More information

Oxidation-Reduction Reactions

Oxidation-Reduction Reactions CHAPTER 19 REVIEW Oxidation-Reduction Reactions SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. All the following equations involve redox reactions except (a) CaO H 2 O

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

Chemistry 1000 A Fall 2004 Answers to Problem Set #3

Chemistry 1000 A Fall 2004 Answers to Problem Set #3 Chemistry 1000 A Fall 2004 Answers to Problem Set #3 1. Balance the following equations, and name the reaction products: (a) UO 2 (s) + 4 HF(l) UF 4 (s) + 2 H 2 O(l): Uranium tetrafluoride and water (dihydrogen

More information

Similarities and Differences Galvanic and Electrolytic Cell:

Similarities and Differences Galvanic and Electrolytic Cell: Electrolytic Cells Voltaic cells are driven by a spontaneous chemical reaction that produces an electric current through an outside circuit. These cells are important because they are the basis for the

More information

How Many Cookies Can I Make? You can make cookies until you run out of one of the ingredients Once you run out of sugar, you will stop making cookies

How Many Cookies Can I Make? You can make cookies until you run out of one of the ingredients Once you run out of sugar, you will stop making cookies Limi$ng reactants How Many Cookies Can I Make? You can make cookies until you run out of one of the ingredients Once you run out of sugar, you will stop making cookies How Many Cookies Can I Make? In this

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

Spring 2009 CH302 Practice Exam 2 Answer Key

Spring 2009 CH302 Practice Exam 2 Answer Key Spring 2009 CH302 Practice Exam 2 Answer Key 1. What would be the ph of a solution prepared by dissolving 120.1 g of CH 3 COOH and 82 g of NaCH 3 COO in 1 L of water? Acetic acid has a K a of 1.8 x 10

More information

What physical evidence do we have that sodium hydroxide dissociates into ions when it dissolves in water? NaOH(s) Na + + OH -

What physical evidence do we have that sodium hydroxide dissociates into ions when it dissolves in water? NaOH(s) Na + + OH - Chemistry Date Period Name CW double replacement reactions 030812.doc Double Replacement Reactions Double replacement reactions are some of the most common reactions that are performed in the laboratory.

More information

Chapter 20 Electrochemistry

Chapter 20 Electrochemistry Chapter 20 Electrochemistry Electrochemistry deals with the relationships between electricity and chemical reactions. Oxidation-reduction (redox) reactions were introduced in Chapter 4 Can be simple displacement

More information

AP Chem Unit 1 Assignment 3 Chemical Equations

AP Chem Unit 1 Assignment 3 Chemical Equations Symbols used in chemical equations: Symbol Meaning + used to separate one reactant or product from another used to separate the reactants from the products - it is pronounced "yields" or "produces" when

More information

Chemistry 106 Fall 2007 Exam 3 1. Which one of the following salts will form a neutral solution on dissolving in water?

Chemistry 106 Fall 2007 Exam 3 1. Which one of the following salts will form a neutral solution on dissolving in water? 1. Which one of the following salts will form a neutral solution on dissolving in water? A. NaCN B. NH 4 NO 3 C. NaCl D. KNO 2 E. FeCl 3 2. Which one of the following is a buffer solution? A. 0.10 M KCN

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

Equilibrium Constants The following equilibrium constants will be useful for some of the problems.

Equilibrium Constants The following equilibrium constants will be useful for some of the problems. 1 CH302 Exam 4 Practice Problems (buffers, titrations, Ksp) Equilibrium Constants The following equilibrium constants will be useful for some of the problems. Substance Constant Substance Constant HCO

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

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

Combination Reactions 2H 2 + O 2 2H 2 O. 2Na + I 2 2NaI. Ca + Cl 2 CaCl 2. C + O 2 CO 2 or 2C + O 2 2CO 3H 2 + N 2 2NH 3

Combination Reactions 2H 2 + O 2 2H 2 O. 2Na + I 2 2NaI. Ca + Cl 2 CaCl 2. C + O 2 CO 2 or 2C + O 2 2CO 3H 2 + N 2 2NH 3 Combination Reactions Predict the product and write balanced reactions for each of the following. 1. Hydrogen burned in oxygen. 2H 2 + O 2 2H 2 O 2. Sodium plus iodine. 2Na + I 2 2NaI 3. Calcium burned

More information

STOICHOMETRY UNIT Determine the mass of carbon present in a sample of glucose weighing 5.4 g.

STOICHOMETRY UNIT Determine the mass of carbon present in a sample of glucose weighing 5.4 g. PERCENTAGE COMPOSITION STOICHOMETRY UNIT 3 1. A sample of magnesium weighing 2.246 g burns in oxygen to form 3.724 g of magnesium oxide. What are the percentages of magnesium and oxygen in magnesium oxide?

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. 14, Acids and Bases Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) The conjugate base of HSO4 - is A) H2SO4

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

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

21-1. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.

21-1. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 21-1 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Chapter 21 Electrochemistry: Chemical Change and Electrical Work 21-2 Electrochemistry: Chemical Change and

More information

EXPERIMENT #12 DOUBLE-REPLACEMENT REACTIONS

EXPERIMENT #12 DOUBLE-REPLACEMENT REACTIONS EXPERIMENT #12 DOUBLE-REPLACEMENT REACTIONS Purpose: 1. To study the most common type of double-replacement reactions. Principles: In double-replacement reactions, two compounds are involved in a reaction,

More information

Oxidation-Reduction Summary and Study Assignment

Oxidation-Reduction Summary and Study Assignment Oxidation-Reduction Summary and Study Assignment The atoms in elements, ions or molecules involved in electrochemical reactions are characterized by the number of protons the atom has compared to the number

More information

EXPERIMENT 9: Double Replacement Reactions

EXPERIMENT 9: Double Replacement Reactions EXPERIMENT 9: Double Replacement Reactions PURPOSE a) To identify the ions present in various aqueous solutions. b) To systematically combine solutions and identify the reactions that form precipitates

More information

Chapter 12: Oxidation and Reduction.

Chapter 12: Oxidation and Reduction. 207 Oxidation- reduction (redox) reactions Chapter 12: Oxidation and Reduction. At different times, oxidation and reduction (redox) have had different, but complimentary, definitions. Compare the following

More information

Net Ionic Equations Making Sense of Chemical Reactions

Net Ionic Equations Making Sense of Chemical Reactions 14 Making Sense of Chemical Reactions OBJECTIVE Students will be able to write net ionic equations from balanced molecular equations. LEVEL Chemistry NATIONAL STANDARDS UCP.1, UCP.2, B.3 T E A C H E R

More information

Multiple Choice Questions NCERT

Multiple Choice Questions NCERT CHAPTER 3 Metals and Non-metals Multiple Choice Questions 1. Which of the following property is generally not shown by metals? (a) Electrical conduction (b) Sonorous in nature (c) Dullness (d) Ductility

More information

Types of Chemical Reactions

Types of Chemical Reactions Why? Types of Chemical Reactions Do atoms rearrange in predictable patterns during chemical reactions? Recognizing patterns allows us to predict future behavior. Weather experts use patterns to predict

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

1. According to Reference Table J, which metal will react spontaneously with Ag + ions, but not with Zn 2+ ions? 1) Cu 3) Al 2) Au 4) Mg 2. Which will oxidize Zn(s) to Zn 2+, but will not oxidize Pb(s)

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

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

Chapter 13: Electrochemistry. Electrochemistry. The study of the interchange of chemical and electrical energy.

Chapter 13: Electrochemistry. Electrochemistry. The study of the interchange of chemical and electrical energy. Chapter 13: Electrochemistry Redox Reactions Galvanic Cells Cell Potentials Cell Potentials and Equilbrium Batteries Electrolysis Electrolysis and Stoichiometry Corrosion Prevention Electrochemistry The

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

CHAPTERS 15 FAKE TEST QUESTIONS. 1. According to the Brønsted Lowry definition, which species can function both as an acid and as a base?

CHAPTERS 15 FAKE TEST QUESTIONS. 1. According to the Brønsted Lowry definition, which species can function both as an acid and as a base? You might need to know the following K values: CHAPTERS 15 FAKE TEST QUESTIONS CH 3 COOH K a = 1.8 x 10 5 Benzoic Acid K a = 6.5 x 10 5 HNO 2 K a = 4.5 x 10 4 NH 3 K b = 1.8 x 10 5 HF K a = 7.2 x 10 4

More information

Experiment 5: Studying Chemical Reactions

Experiment 5: Studying Chemical Reactions 1 Experiment 5: Studying Chemical Reactions When a chemical reaction occurs, substances called reactants are transformed into different substances called products that may have different appearances and

More information