# Chemistry 106 Fall 2006 Exam 3 Form A

Save this PDF as:

Size: px
Start display at page:

## Transcription

1 1. In some towns where steel mills and paper pulp mills are close together a brown deposit of FeS(s) forms from the reaction of H 2 S and particulate iron from the steel mill. The overall reaction is shown below. K total = What is the value of the equilibrium constant for the reverse reaction? 4Fe(s) + 3O 2 (g) + 4H 2 S(g) + 4H + (aq) 6H 2 O(l) + 4FeS(s) K total A B x C D E Write the equilibrium expression for the reaction Zn 2+ (aq) + 2 NH 3 [Zn(NH 3 ) ] 2+ 2 A. K = [Zn 2+ (aq)] + 2 [NH 3 ] + [[Zn(NH 3 ) 2 ] 2+ ] B. K = [[Zn(NH 3 ) 2 ] 2+ ] / {[Zn 2+ (aq)] [NH 3 ] 2 } C. K = { [Zn 2+ (aq)] + 2 [NH 3 ] } / [[Zn(NH 3 ) 2 ] 2+ ] D. K = [[Zn(NH 3 ) 2 ] 2+ ]/{ [Zn 2+ (aq)] + 2 [NH 3 ] } E. K = [Zn 2+ (aq)] [NH 3 ] 2 / [[Zn(NH 3 ) 2 ] 2+ ] 3. If the reaction quotient Q has a larger value than the related equilibrium constant K A. the reaction will release heat to achieve equilibrium. B. the reaction will absorb heat to achieve equilibrium. C. the reaction will continue to make more products. D. the reaction is at equilibrium. E. the reaction will consume products and make reactants. 4. Given the following reactions and their equilibrium constants calculate the equilibrium constant for the overall reaction. H 3PO 4(aq) H 2 PO 4- (aq) + H + (aq) K 1 = 7.52 # 10-3 H 2PO 4- (aq) HPO 4 2- (aq) + H + (aq) K 2 = 6.2 # 10-8 HPO (aq) PO (aq) + H + (aq) K 3 = 2.2 # Ca 3 (PO 4 ) 2 (s) 3Ca 2 + (aq) + 2PO (aq) K 4 = 2.1 # Overall reaction: 2H 3 PO 4 (aq) + 3Ca 2 + (aq) Ca 3(PO 4) 2(s) + 6H + (aq) A. 7.2 x B. 4.6 x C. 2.2 x D. 2.0 x E. 5.0 x Page 1

2 5. What is equal in an equilibrium? A. the rate constants for the forward and reverse reactions B. the time that a particular atom or molecule spends as a reactant and product C. the concentrations of reactant and products D. the rate of the forward and reverse reaction 6. If K for a reaction is very small A. ΔHº is definitely positive. B. ΔGº is definitely positive. C. ΔGº is definitely negative. D. ΔHº is definitely negative. 7. Consider the equilibrium: 2SO 2(g) + O 2(g) 2SO 3(g) K C = 2.62 # 10 3 What is K p for pressure units of atm at a temperature of 298 K? A. 107 B x 104 C D x 106 E For a particular hypothetical reaction A + 2B > C G o = kj/mol. What is the equilibrium constant for this reaction at 298 K? A x B x 1021 C D E x Under what conditions are the values of K c and K p for a given gas phase equilibrium the same? A. same temperature B. no change in moles of gas in the reaction C. if the stoichiometric coefficients are the same on the reactant and product sides D. all the above 10. Given the two measurements below, calculate ΔHº. T, ºC K A. 170 kj/mol B. 452 J/mol C kj/mol D kj/mol E. 161 kj/mol Page 2

3 11. The equilibrium constant for an endothermic reaction A. is temperature independent. B. increases with increasing temperature. C. decreases with increasing temperature. D. cannot be predicted. E. cannot be predicted without knowing S too. 12. Mercury ions exist as the mercurous dimer Hg 2 2+ and Hg +. If Hg 2 2+ is in contact with liquid mercury, Hg(l), the equilibrium below is established: Hg + (aq)+ Hg(l) Hg 2 2+ (aq) + Hg(l) K = If a M solution of Hg + is put in contact with liquid mercury, what will be the resulting equilibrium concentration of Hg 2 2+? A M B M C M D M E M 13. When can an "x" be ignored in solving an algebraic form of an equilibrium expression? A. whenever it simplifies the algebraic expression enough to allow calculation B. whenever it is added to or subtracted from a concentration value C. whenever it is in the denominator D. whenever it is added to or subtracted from a concentration value that is large in comparison to it E. whenever it is squared or raised to any power higher than A catalyst A. lowers activation energies in both the forward and reverse reactions in a chemical equilibrium. B. is necessary for any reaction to go to completion. C. changes the value of an equilibrium constant by changing the forward and reverse activation energies. D. stresses an equilibrium by consuming reactants. 15. For a particular hypothetical reaction A + 2B > C in the gas phase how does decreasing the pressure affect the equilibrium? A. It shifts the equilibrium towards more reactants. B. It does not change the equilibrium concentrations. C. The relative concentrations of B and C do not change. D. It only changes the concentration of B. E. It shifts the equilibrium towards more products. Page 3

4 16. In equilibrium expressions, solids and sovents are ignored because they A. have the assigned value of zero. B. are not necessary for the rection C. are treated with different rate constants. D. do not change concentration. E. have constant values, K s and K l. 17. The SO 2 in the exhaust gas from coal burning power plants may be removed by the reaction: CaO(s) + SO 2 (g) CaSO 3 (s) The equilibrium expression for this scrubbing reaction of calcium oxide and sulfur dioxide to make calcium sulfite is A. K c = [CaO] + [SO 2 ]. B. K c = [CaSO 3 ]/[SO 2 ][CaO]. C. K c = 1/[SO 2 ]. D. K c = [CO 2 ]. E. K c = [CaSO 3 ]/{[SO 2 ]+[CaO]}. 18. The expression for K a where HA represents a weak acid is: A. [HA]/{[H + ]+[A - ]} B. {[H + ]+[A - ]}/[HA] C. [H 2 A + ][OH - ]/[HA] D. [HA]/{[H + ][A - ]} E. {[H + ][A - ]}/[HA] 19. The degree of ionization of a weak acid is A. between 10 and 100%. B. 100%. C. between 1 and 10%. D. dependent on the total concentration of the acid. 20. The equilibrium constant K b describes the following reaction for a weak base, B, in aqueous solution: A. B + 2OH - BH + + H 2 O B. C. D. B + OH - BH - + O 2- B + H + BH + B + H 3 O + BH + + H 2 O E. B + H2 O BH + + OH - Page 4

5 21. What is the ph of a M solution of acetic acid, given that the weak acids K a is ? A B C D What is the concentration of the molecular form of HF in a 1.00 M solution of HF given that the K a of the weak acid is ? A M B M C M D M E M 23. Which of these is a strong acid that ionizes to make a weak acid? A. H 2 SO 3 B. HCl C. HNO 3 D. H 2 SO 4 E. H 3 PO The weaker the acid, A. the weaker its conjugate base. B. the less concentrated the acid. C. the more concentrated the conjugate base. D. the stronger its conjugate base. 25. A solution with ph of 9.50 has a poh of A B C D E A Lewis base is A. an electron pair acceptor B. a proton donor C. an electron pair donor D. a proton acceptor 27. An acidic solution has A. a poh more than 7. B. a ph less than 7. C. more H + than OH -. D. all the above. 28. Lead(II) chloride salt is not very soluble in water. How does the solubility of lead chloride change as sodium chloride is added to the water in contact with solid lead(ii) chloride? A. Sodium chloride increases the solubility of lead(ii) chloride. B. Sodium chloride has no effect it is an inert electrolyte. C. It depends on how vigorously you stir the solution. D. Sodium chloride has no effect lead(ii) chloride is insoluble in water and also insoluble in salt water. E. Sodium chloride decreases the solubility of lead(ii) chloride. Page 5

6 29. Which of the following is NOT a buffer system? A solution containing roughly equal concentrations of A. fluoride ion and hydrofluoric acid. B. phosphate ion and monophosphate ion. C. chloride ion and hydrochloric acid. D. carbonate ion and bicarbonate ion. E. they are all buffers 30. Compounds that are reactive as both an acid and base are called: A. amphibious B. amphoteric C. bacidic D. androgynous 31. A solution of sulfuric acid (25.00 ml) was titrated to completion (all protons reacted) with ml of M sodium hydroxide. What was the concentration of the sulfuric acid? A M B M C M D M E M 32. A buffer system is set up with [HA] = 2[A ]. If pk a = 5.5, what is the ph of the buffer? A. 5.8 B. 7.0 C. 5.2 D. 3.5 E What is the ph of a 0.15 M solution of ammonium bromide? The K b value of ammonia is A B C D E Which is NOT related to K w A. 2 H2 O H 3 O + + OH -. B at 25º C. C. [H 3 O + ] [OH - ]. D. [H + ] [A - ]/[HA] E. [H + ] [OH - ] Page 6

7 No. in Q-Bank No. on Test D B E E D B A A D A B B D A A D C E D E B A D D B C D E C B C C C D Answer Key for Test Exam 3 F06 Form A.mte, 11/4/07 Correct Answer Page 1

### 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

### Chapter 17. How are acids different from bases? Acid Physical properties. Base. Explaining the difference in properties of acids and bases

Chapter 17 Acids and Bases How are acids different from bases? Acid Physical properties Base Physical properties Tastes sour Tastes bitter Feels slippery or slimy Chemical properties Chemical properties

### Write the acid-base equilibria connecting all components in the aqueous solution. Now list all of the species present.

Chapter 16 Acids and Bases Concept Check 16.1 Chemists in the seventeenth century discovered that the substance that gives red ants their irritating bite is an acid with the formula HCHO 2. They called

### 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

### CHAPTER 9. ANS: a. ANS: d. ANS: c. ANS: a. ANS: c

CHAPTER 9 1. Which one of the following is the acid in vinegar? a. acetic acid b. citric acid c. muriatic acid d. ascorbic acid 2. Which is a basic or alkaline substance? a. gastric fluid b. black coffee

### CHEM 10123/10125, Exam 2

CHEM 10123/10125, Exam 2 March 7, 2012 (50 minutes) Name (please print) Please box your answers, and remember that significant figures, phases (for chemical equations), and units do count! 1. (13 points)

### Chapter 4 Notes - Types of Chemical Reactions and Solution Chemistry

AP Chemistry A. Allan Chapter 4 Notes - Types of Chemical Reactions and Solution Chemistry 4.1 Water, the Common Solvent A. Structure of water 1. Oxygen's electronegativity is high (3.5) and hydrogen's

### 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

### SECTION 14 CHEMICAL EQUILIBRIUM

1-1 SECTION 1 CHEMICAL EQUILIBRIUM Many chemical reactions do not go to completion. That is to say when the reactants are mixed and the chemical reaction proceeds it only goes to a certain extent, and

### BRØNSTED ACIDS & BASES

ACIDS & BASES BRØNSTED ACIDS & BASES BRØNSTED ACIDS & BASES Brønsted acids are proton donors. Brønsted bases are proton acceptors. Amphoteric species can act as either an acid or a base, depending on the

### An acid is a substance that produces H + (H 3 O + ) Ions in aqueous solution. A base is a substance that produces OH - ions in aqueous solution.

Chapter 8 Acids and Bases Definitions Arrhenius definitions: An acid is a substance that produces H + (H 3 O + ) Ions in aqueous solution. A base is a substance that produces OH - ions in aqueous solution.

### 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

### 1. For the equilibrium that exists in an aqueous solution of nitrous acid (HNO 2, a weak acid), the equilibrium constant expression is:

1. For the equilibrium that exists in an aqueous solution of nitrous acid (HNO 2, a weak acid), the equilibrium constant expression is: a) K = [H+ ][NO 2 ] [HNO 2 ] b) K = [H+ ][N][O] 2 [HNO 2 ] c) K =

### Chemistry: Chemical Equations

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

### Chem101: General Chemistry Lecture 9 Acids and Bases

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

### 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

### Chemistry 212 EXAM 2 February 17, 2004 KEY

1 Chemistry 212 EXAM 2 February 17, 2004 100_ (of 100) KEY Name Part 1: Multiple Choice. (1 point 4. The equilibrium constant for the each, circle only one answer, reaction 1. For the equilibrium that

### Potassium + Chlorine. K(s) + Cl 2 (g) 2 KCl(s)

Types of Reactions Consider for a moment the number of possible chemical reactions. Because there are millions of chemical compounds, it is logical to expect that there are millions of possible chemical

### Chapter 19: Acids and Bases Homework Packet (50 pts) Name: Score: / 50

Chapter 19: Acids and Bases Homework Packet (50 pts) Topic pg Section 19.1 1-3 Section 19.2 3-6 Section 19.3 6-7 Section 19.4 8 Naming Acids 9 Properties of Acids/Bases 10-11 Conjugate Acid/Base Pairs

### Chapter 14 - Acids and Bases

Chapter 14 - Acids and Bases 14.1 The Nature of Acids and Bases A. Arrhenius Model 1. Acids produce hydrogen ions in aqueous solutions 2. Bases produce hydroxide ions in aqueous solutions B. Bronsted-Lowry

### Experiment 9 - Double Displacement Reactions

Experiment 9 - Double Displacement Reactions A double displacement reaction involves two ionic compounds that are dissolved in water. In a double displacement reaction, it appears as though the ions are

### 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

### CHEM 102: Sample Test 5

CHEM 102: Sample Test 5 CHAPTER 17 1. When H 2 SO 4 is dissolved in water, which species would be found in the water at equilibrium in measurable amounts? a. H 2 SO 4 b. H 3 SO + 4 c. HSO 4 d. SO 2 4 e.

### Buffer Solutions. Buffer Solutions

Chapter 18 Common Ion Effect Buffers and Titration Curves A/B Titrations Salts and Solubility Product The Common Ion Effect and If a solution is made in which the same ion is produced by two different

### Acid-Base (Proton-Transfer) Reactions

Acid-Base (Proton-Transfer) Reactions Chapter 17 An example of equilibrium: Acid base chemistry What are acids and bases? Every day descriptions Chemical description of acidic and basic solutions by Arrhenius

### p3 Recognizing Acid/Base Properties when p11 Recognizing Basic versus Nonbasic

General Chemistry II Jasperse Acid-Base Chemistry. Extra Practice Problems 1 General Types/Groups of problems: Conceptual Questions. Acids, Bases, and p1 K b and pk b, Base Strength, and using K b or p7-10

### Suggested Problems: p. 625-627 #58, 59, 65, 69, 74, 80, 85, 86, 90, 92, 93, 98, 99

Chemistry I Accelerated Study Guideline - Chapter 19 Acids, Bases and Salts ------------------------------------------------------------------------------ By the end of this unit, the skills you should

### Problems you need to KNOW to be successful in the upcoming AP Chemistry exam.

Problems you need to KNOW to be successful in the upcoming AP Chemistry exam. Problem 1 The formula and the molecular weight of an unknown hydrocarbon compound are to be determined by elemental analysis

### UNIT (6) ACIDS AND BASES

UNIT (6) ACIDS AND BASES 6.1 Arrhenius Definition of Acids and Bases Definitions for acids and bases were proposed by the Swedish chemist Savante Arrhenius in 1884. Acids were defined as compounds that

### AP Review: Predicting Reactions (Question 4) Answers

AP Review: Predicting Reactions (Question 4) Answers For each of the following three reactions, in part (i) write a balanced equation for the reaction and in part (ii) answer the question about the reaction.

### 12.1 How do sub-atomic particles help us to understand the structure of substances?

12.1 How do sub-atomic particles help us to understand the structure of substances? Simple particle theory is developed in this unit to include atomic structure and bonding. The arrangement of electrons

### Equilibrium, Acids and Bases Unit Summary:

Equilibrium, Acids and Bases Unit Summary: Prerequisite Skills and Knowledge Understand concepts of concentration, solubility, saturation point, pressure, density, viscosity, flow rate, and temperature

### C u ( O H ) 2. N i ( N O 3 ) 2. N a m e C a t i o n Cation A n i o n A n i o n

Name Exam 3 Page 1 AQUEUS SLUTINS 1. (8 points) Names, formulas, and water-solubility of compounds. N a m e F o r m u l a Soluble in Water? Ammonium chloride N H 4 C l y e s C u ( H N i ( N 3 Iron(III)

### 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

### AP Chemistry- Acids and Bases General Properties of Acids and Bases. Bases- originally defined as any substance that neutralized an acid

AP Chemistry Acids and Bases General Properties of Acids and Bases Acids Electrolyte Taste Litmus Phenolphthalein React with metals to give off H 2 gas H 2 SO 4 (aq) + Mg (s) MgSO 4 (aq) + H 2 (g) Ionize

### Chemical Reactions Chapter 8 Assignment & Problem Set

Chemical Reactions Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Chemical Reactions 2 Study Guide: Things You Must Know Vocabulary (know the

### WEAK ACIDS AND BASES

WEAK ACIDS AND BASES [MH5; Chapter 13] Recall that a strong acid or base is one which completely ionizes in water... In contrast a weak acid or base is only partially ionized in aqueous solution... The

### Chapter 16 Acid-Base Equilibria

Chapter 16 Acid-Base Equilibria Learning goals and key skills: Understand the nature of the hydrated proton, represented as either H + (aq) or H 3 O + (aq) Define and identify Arrhenuis acids and bases.

### CHEM 101/105 Aqueous Solutions (continued) Lect-07

CHEM 101/105 Aqueous Solutions (continued) Lect-07 aqueous acid/base reactions a. a little bit more about water Water is a polar substance. This means water is able to "solvate" ions rather well. Another

### 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

### Chemical reactions. Classifications Reactions in solution Ionic equations

Chemical reactions Classifications Reactions in solution Ionic equations Learning objectives Distinguish between chemical and physical change Write and balance chemical equations Describe concepts of oxidation

### HOMEWORK 4A. Definitions. Oxidation-Reduction Reactions. Questions

HOMEWORK 4A Oxidation-Reduction Reactions 1. Indicate whether a reaction will occur or not in each of following. Wtiring a balcnced equation is not necessary. (a) Magnesium metal is added to hydrochloric

### Summer Holidays Questions

Summer Holidays Questions Chapter 1 1) Barium hydroxide reacts with hydrochloric acid. The initial concentration of the 1 st solution its 0.1M and the volume is 100ml. The initial concentration of the

### 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

### What is a chemical reaction?

Chapter 5 Chemical Reactions and Equations What is a chemical reaction? How do we know a chemical reaction occurs? Writing chemical equations Predicting chemical reactions Representing reactions in aqueous

### 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,

### Acids and Bases: Definitions. Brønsted-Lowry Acids and Bases. Brønsted-Lowry Acids and Bases CHEMISTRY THE CENTRAL SCIENCE

CHEMISTRY THE CENTRAL SCIENCE Professor Angelo R. Rossi Department of Chemistry Spring Semester Acids and Bases: Definitions Arrhenius Definition of Acids and Bases Acids are substances which increase

### Laboratory 6: Double Displacement Reactions

Introduction Double displacement reactions are among the most common of the simple chemical reactions to study and understand. We will explore the driving forces behind the chemical reactions, and use

### Acids and Bases: A Brief Review

Acids and : A Brief Review Acids: taste sour and cause dyes to change color. : taste bitter and feel soapy. Arrhenius: acids increase [H ] bases increase [OH ] in solution. Arrhenius: acid base salt water.

### CHEMISTRY 101 EXAM 3 (FORM A) DR. SIMON NORTH

CHEMISTRY 101 EXAM 3 (FORM A) DR. SIMON NORTH 1. When considering conjugate acids and bases, (2 points) a) Strong acids have strong conjugate bases. b) Strong bases have strong conjugate acids. c) Weak

### CHEMISTRY 101 EXAM 3 (FORM B) DR. SIMON NORTH

1. Is H 3 O + polar or non-polar? (1 point) a) Polar b) Non-polar CHEMISTRY 101 EXAM 3 (FORM B) DR. SIMON NORTH 2. The bond strength is considerably greater in HF than in the other three hydrogen halides

### CHM1 Review for Exam 12

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

### Lecture Summary #21

21.1 5.111 Lecture Summary #21 AcidBase Equilibrium Read Chapter 10 Topics: Classification of AcidBases, Autoionization of Water, p unction, Strength of Acids and Bases, Equilibrium Involving Weak Acids.

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

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

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

CHE 1400 - Spring 2015 - Chapter 7 Homework 7 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1)According to Arrhenius, an acid and a base will react

### Single and Double Displacement Reactions

Single and Double Displacement Reactions Objectives To perform and observe a variety of single and double displacement reactions To record observations in detail To identify the products formed in each

### Experiment 8 - Double Displacement Reactions

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

### 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

### Molarity of Ions in Solution

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

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

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

### Chapter 9 Lecture Notes: Acids, Bases and Equilibrium

Chapter 9 Lecture Notes: Acids, Bases and Equilibrium Educational Goals 1. Given a chemical equation, write the law of mass action. 2. Given the equilibrium constant (K eq ) for a reaction, predict whether

### Chapter 4: Reactions in Aqueous Solution (Sections )

Chapter 4: Reactions in Aqueous Solution (Sections 4.1-4.12) Chapter Goals Be able to: Classify substances as electrolytes or nonelectrolytes. Write molecular, ionic, and net ionic equations for precipitation,

### Stoichiometry Chapter 9 Assignment & Problem Set

Stoichiometry Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Stoichiometry 2 Study Guide: Things You Must Know Vocabulary (know the definition

### Enthalpy, Entropy, and Free Energy Calculations

Adapted from PLTL The energies of our system will decay, the glory of the sun will be dimmed, and the earth, tideless and inert, will no longer tolerate the race which has for a moment disturbed its solitude.

### Answer the following questions on notebook paper, to be collected and graded for correctness.

nswer the following questions on notebook paper, to be collected and graded for correctness. 1. Name the following binary acids: a. HCl hydrochloric acid b. HF hydrofluoric acid c. H 2 S hydrosulfuric

### Acids and Bases: A Brief Review, see also pp and pp Brønsted-Lowry Acids and Bases 143. The H + Ion in Water

Quiz number 5 will be given in recitation next week, Feb 26Mar 2 on the first part of Chapter 16, to be covered in lectures this week. 16.1 Acids and Bases: A Brief Review 16.2 BronstedLowry Acids and

### QUESTION (2012:3) (a) (i) Complete the table below showing the conjugate acids and bases. CO 3 H 2 O OH HCN CN -

QUESTION (2012:3) (i) Complete the table below showing the conjugate acids and bases. Conjugate acid Conjugate base - HCO 3 2 CO 3 H 2 O OH HCN CN - (ii) HPO 4 2 (aq) Write equations for the reactions

### Worksheet # 11. 4. When heated, nickel (II) carbonate undergoes a decomposition reaction. Write a balanced equation to describe this reaction

Worksheet # 11 1. A solution of sodium chloride is mixed with a solution of lead (II) nitrate. A precipitate of lead (II) chloride results, leaving a solution of sodium nitrated. Determine the class of

### Chapter 16: Acid-Base and Solubility Equilibria: Reactions in Soil and Water

Chapter 16: Acid-Base and Solubility Equilibria: Reactions in Soil and Water Problems: 16.2-16.86 16.1 ACIDS AND BASES: THE BRØNSTED-LOWRY MODEL PROPERTIES OF ACIDS & BASES Acids produce hydrogen ions,

### Western Carolina University. Prelaboratory Exercise Write out the answers on a separate sheet of paper and turn in the paper at the start of lab.

Name Chemistry 132 Lab 09 Lab Section Chemical Reactions Part II Prelaboratory Exercise Write out the answers on a separate sheet of paper and turn in the paper at the start of lab. 1. Define the terms

### Identify the letter of the choice that best completes the statement or answers the question.

Chemistry Test - Chapter 10 Chemical Equations Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. When balancing a chemical equation, insert

### EXPERIMENT 5: CHEMICAL REACTIONS AND EQUATIONS

PURPOSE EXPERIMENT 5: CHEMICAL REACTIONS AND EQUATIONS To perform and observe simple chemical reactions. To identify the products of chemical reactions and write balanced equations for those reactions.

### UNIT 14 - Acids & Bases

COMMON ACIDS NOTES lactic acetic phosphoric citric malic PROPERTIES OF ACIDS 1. 1. PROPERTIES OF BASES 2. 2. 3. 3. 4. 4. 5. 5. NAMING ACIDS NOTES Binary acids (H + one element) Practice: 1. hydro- - HF

### Chapter 8: Chemical Equations and Reactions

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

### 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

### Balancing Chemical Equations Worksheet

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

### 4. Aluminum chloride is 20.2% aluminum by mass. Calculate the mass of aluminum in a 35.0 gram sample of aluminum chloride.

1. Calculate the molecular mass of table sugar sucrose (C 12 H 22 O 11 ). A. 342.30 amu C. 320.05 amu B. 160.03 amu D. 171.15 amu 2. How many oxygen atoms are in 34.5 g of NaNO 3? A. 2.34 10 23 atoms C.

### Acids, Bases and Concentrations

61 Chapter 7 Acids, Bases and Concentrations Thoughts or pictures of a shark usually evoke fear. But most sharks are not harmful to humans and shark attacks while dangerous and sometimes fatal are extremely

### Chemical Equations and Chemical Reactions. Chapter 8.1

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

### 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

### How many ml of 0.250M potassium permangenate are needed to react with 3.36 g of iron(ii) sulfate?

How many ml of 0.250M potassium permangenate are needed to react with 3.36 g of iron(ii) sulfate? 1 - Change the mass of iron(ii) sulfate to moles using the formula weight.of iron(ii) sulfate 2 - Change

### CHEM 1212 Test II. MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

CHEM 1212 Test II MULTIPLE CHOICE. Choose the one alternative that est completes the statement or answers the question. 1) At 1000 K, the equilirium constant for the reaction is K p = 0.013. 2NO (g) +

### 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

### Titrations. Acid-Base Indicators and Titration Curves. Shapes of Titration Curves. A titration curve is a graphical history of a titration

Acid-Base Indicators and Titration Curves Titrations In a titration a solution of accurately known concentration is added gradually added to another solution of unknown concentration until the chemical

### 4. Using the data from Handout 5, what is the standard enthalpy of formation of BaO (s)? What does this mean?

HOMEWORK 3A 1. In each of the following pairs, tell which has the higher entropy. (a) One mole of liquid water or one mole of water vapor (b) One mole of dry ice or one mole of carbon dioxide at 1 atm

### b. Calculate these values based on the given information and your calculations in (a). ph poh [H3O +1 ] [OH 1 ] [H3O +1 ] [OH 1 ]

Name Period Date Pre-AP Chemistry Review: Acids & Bases 1. 0.18 M phenol acid forms this equilibrium: C6H5OH (aq) + H2O(l) C6H5O -1 (aq) + H3O +1 (aq) + Energy ; (K=1.60 10-10 ) a. Complete the ICE chart

### 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

### Chapter 9 Acids, Bases and Buffers in the Body Outline 9.1 Acids and Bases Definitions Acids

Lecture Presentation Chapter 9 Acids, Bases and Buffers in the Body Julie Klare Fortis College Smyrna, GA Outline 9.1 Acids and Bases Definitions 9.2 Strong Acids and Bases 9.3 Chemical Equilibrium 9.4

### Types of Reactions. What are Acids &Bases? Chapter 15. Acids & Bases. Definition? a) Arrhenius. b) Bronsted-Lowry. c) Lewis

Chapter 15. Acids & Bases Acid/Base Definitions Types of Acids/bases Polyprotic Acids The Ion Product for Water The ph and Other p Scales Aqueous Solutions of Acids and Bases Hydrolysis The Common Ion

### Acids and Bases. Ch a pt e r Aqueous Equilibria: Chemistry 4th Edition McMurry/Fay. MOH(aq) M + (aq) + OH (aq)

15 Ch a pt e r Aqueous Equilibria: Acids and Bases Chemistry th Edition McMurry/Fay Dr. Paul Charlesworth Michigan Technological University AcidBase Concepts 01 Arrhenius Acid: A substance which dissociates

### 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

### 1. Identify the Bronsted-Lowry acids and bases and the conjugate acid base pairs in the following reactions.

Exercise #1 Brønsted-Lowry s and Bases 1. Identify the Bronsted-Lowry acids and bases and the conjugate acid base pairs in the following reactions. (a) HCl(aq) + H 2 O(l) H 3 O + (aq) + Cl (aq) (b) H 2

### Topic 8 Acids and bases 6 hours

Topic 8 Acids and bases 6 hours Hydronium ion (H3O + ) = more stable form of hydrogen ion (H + ) H + + H2O H3O + 8.1 Theories of acids and bases 2 hours 1. Arrhenius H-X / M-OH ACID a substance that dissociates

### Chapter 7: Chemical Reactions: An Introduction. Chemical Reactions, Equations and Balancing

Chapter 7: Chemical Reactions: An Introduction Chemical Reactions, Equations and Balancing Learning Target Chapter 7 Vocabulary 4 words 1. Chemical reaction 2. Reactant 3. Product 4. Coefficients balanced

### Q1. The chart shows the processes involved in the manufacture of nitric acid from ammonia.

Chemistry C2 Foundation and Higher Questions Q1. The chart shows the processes involved in the manufacture of nitric acid from ammonia. (a) Complete the word equation for the reaction that takes place

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

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

### 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:

### Chapter 14: Acids and Bases

Ch 14 Page 1 Chapter 14: Acids and Bases Properties of Acids Sour taste React with some metals Turns blue litmus paper red React with bases Some Common Acids HCl, hydrochloric acid H 2 SO 4, sulfuric acid