Chemistry 1A Fall 2010 Exam 2 Key Chapters 4 (part), 5, 6, and 7 (part)

Size: px
Start display at page:

Download "Chemistry 1A Fall 2010 Exam 2 Key Chapters 4 (part), 5, 6, and 7 (part)"

Transcription

1 Chemistry 1A Fall 010 Exam Key Chapters 4 (part), 5, 6, and 7 (part) You might find the following useful kj ΔH = ΔE + (Δn)RT R = K mol kj q = C calδt + m w g C H rxn = Σ H f (products) Σ H f (reactants) Thermodynamic Properties for Some Common Inorganic Substances Substance State H f kj/mol Substance State H f kj/mol Ag s 0 H g 0 AgCl s H O g Al s 0 H O l 85.8 Al O 3 s H O l Br l 0 Hg l 0 HBr g 36.3 I s 0 C(graphite) s 0 HI g 5.94 C(diamond) s 1.90 Mg s 0 CO g MgO s CO g MgCO 3 s Ca s 0 Mg(OH) s CaC s 59.8 N g 0 CaO s NH 3 g 46.5 CaCO 3 s NO g Ca(OH) aq NO g Cl g 0 N O 4 g 9.66 Cu s 0 N O g CuO s O g

2 Substance State H f kj/mol Substance State H f kj/mol F g 0 O g 0 Fe s 0 O 3 g 14. FeO s 7 S 8(rhombic) s 0 Fe O 3 s 84. S 8(monoclinic) s 0.30 Fe 3O 4 s 1118 SO g HCl g 9.31 SO 3 g HF g H S g 0.15 H g 18. ZnO s Thermodynamic Properties for some Common Organic Substances Substance Formula State H f kj/mol Acetic acid HC H 3O l Acetaldehyde CH 3CHO g Acetone CH 3COCH 3 l Acetylene C H g 6.6 Benzene C 6H 6 l Ethanol C H 5OH l Ethane C H 6 g Ethylene C H 4 g 5.3 Formic acid HCO H l Glucose C 6H 1O 6 s Methane CH 4 g Methanol CH 3OH l Sucrose C 1H O 11 s 1.70

3 For each of the following, write the word, words, letter, letters, or number in each blank that best completes each sentence. (1½ points per blank) 1. A chemical change in which atoms of one element displace (or replace) atoms of another element in a compound is called a(n) Single-displacement reaction (displacement) reaction.. Ionize means to form ions (often as a substance dissolves in water). Dissociate means to separate into ions (often as a substance dissolves in water). 3. A(n) weak base is a substance that produces fewer hydroxide ions in water solution than particles of the substance added. 4. A(n) amphoteric substance is a substance that can act as either a Brønsted-Lowry acid and a Brønsted-Lowry base, depending on the circumstances. 5. Any chemical change in which at least one element loses electrons, either completely or partially is called oxidation. 6. Of the three units of energy calorie, dietary Calorie, and joule the joule is the smallest amount of energy. 7. Of the two forms of radiant energy ultraviolet radiation and microwaves microwaves have the longest wavelength. 8. A(n) endergonic (endogonic) change is a change that absorbs energy. A(n) endothermic change is a change that leads the system to absorb heat energy from the surroundings. 9. Thermal energy is the energy associated with the random motion of particles. 10. Heat capacity is the heat necessary to increase the temperature of an object by one kelvin (or one degree Celsius). 11. The formula and state for the standard state of manganese is Mn(s), for carbon is C(graphite), for iodine is I (s), and for sulfur is S 8(s). 1. A(n) principal energy level or shell is a collection of orbitals that have the same potential energy for a hydrogen atom. 3

4 13. Complete the following table. (1½ point per box) Substance Strong acid, weak acid, strong base, weak base, or neutral? Strong electrolyte, weak electrolyte, or nonelectrolyte Sodium nitrate, NaNO 3 Neutral Strong electrolyte Perchloric acid, HClO 4 Strong acid Strong electrolyte Ammonia, NH 3 Weak base Weak electrolyte Benzoic acid, C 6H 5CO H Weak acid Weak electrolyte Potassium hydrogen sulfate, NaHSO 4 Weak acid Strong electrolyte 14. A substance that is often called chromic hydroxide is used as a catalyst and as a tanning agent. It can be formed from the combination of the following two solutions. Write the complete, complete ionic, and net ionic equations for this precipitation reaction. (9 points) 3KOH(aq) + Cr(NO 3) 3(aq) 3KNO 3(aq) + Cr(OH) 3(s) 3K + (aq) + 3OH (aq) + Cr 3+ (aq) + 3NO 3)(aq) 3K + (aq) + 3NO 3 (aq) + Cr(OH) 3(s) 3OH (aq) + Cr 3+ (aq) Cr(OH) 3(s) 15. Write the oxidation number for each atom above its symbol, and identify which substance is oxidized, which substance is reduced, the oxidizing agent, and the reducing agent. (10 points) As4O6(s) + 8KMnO4(aq) + 18HO(l) + 5KCl(aq) Oxidized As in As 4O 6 Reduced Mn in KMnO 4 Oxidizing agent KMnO 4 Reducing agent As 4O K3AsO4(aq) + 8MnCl(aq) + 36HCl(aq) 4

5 For the following numerical problems, be sure to show your work and put a box around your answer. 16. If 6.8 ml of a M HCl solution neutralizes all of the Ca(OH) in 5.00 ml of a Ca(OH) solution, what is the molarity of the calcium hydroxide solution? (6 points) 3? mol Ca(OH) 6.8 ml HCl soln mol HCl 1 mol Ca(OH) 10 ml = 3 L Ca(OH) soln 5.00 ml Ca(OH) soln 10 ml HCl soln mol HCl 1 L 17. Describe how you would make ml of 3.00 M H SO 4 from 18.0 M H SO 4? (6 points) MDVD 3.00 M (500.0 ml) MCV C = M DV D V C= = = 83.3 ml M 18.0 M C = 0.00 M Ca(OH) Carefully add 83.3 ml 18.0 M H SO 4 to about 300 ml water in a 500-mL volumetric flask, swirl, cool, and dilute with water to ml total. 18. How much energy is released when kg calcium carbide, CaC, reacts with excess water in the following reaction: (8 points) CaC (s) + H O(l) C H (g) + Ca(OH) (aq) H rxn = Σ H f (products) Σ H f (reactants) H rxn = [ H f CH(g) + H f Ca(OH)(aq)] [ H f CaC(s) + H f HO(l)] = [(6.6 kj) + ( kj)] [( 59.8 kj + ( 85.8 kj)] = kj 3 10 g 1 mol CaC kj? kj = kg CaC = 378 kj 1 kg g CaC 1 mol CaC 5

6 Answer the following in short answer form. (7 points each) 19. Explain why some chemical reactions absorb heat from their surroundings. Reactants products Stronger bonds weaker bonds More stable less stable Lower PE + energy released higher PE KE converted to PE Decreased KE means decreased temperature Temperature inside container < temperature outside container Heat absorbed 0. Consider the neutralization reaction between the strong acid nitric acid, HNO 3(aq) and the strong base potassium hydroxide, KOH(aq). a. Describe the mixture of the two solutions before the reaction. Your answer should include mention of the particles in solution, the attractions between these particles, and a description of what these particles are doing. At the instant that the solution of nitric acid is added to the aqueous potassium hydroxide, there are four different ions in solution surrounded by water molecules,h 3O +, NO 3, K +, and OH. The oxygen ends of the water molecules surround the hydronium and potassium cations, and the hydrogen ends of water molecules surround the nitrate and hydroxide anions. b. Describe the changes that take place during the reaction. When H 3O + ions and OH ions collide and form water molecules. c. Describe the mixture after the reaction. Your answer should include mention of the particles in solution, the attractions between these particles, and a description of what these particles are doing. The potassium and nitrate ions are unchanged in the reaction. They were separate and surrounded by water molecules at the beginning of the reaction, and they are still separate and surrounded by water molecules at the end of the reaction. 1. 6

7 . Describe how electrons are like vibrating guitar strings. Your answer should include mention of how the information derived from wave mathematics is similar. The wave mathematics of both the guitar string and the electron show that just as the intensity of the movement of a guitar string can vary at different positions along the string, so can the intensity of the negative charge of the electron vary at different positions outside the nucleus. The variation in the intensity of the movement of the guitar string and the electron charge can be described in terms of a standing wave. Although both the electron and the guitar string can have an infinite number of possible waveforms, only certain waveforms are possible. We can focus our attention on the waveform of varying movement for the guitar string or the varying charge intensity of the electron without having to think about the actual physical nature of the electron. 7

Chemistry 1A Spring 2009 Exam 2 Key Chapters 4-6

Chemistry 1A Spring 2009 Exam 2 Key Chapters 4-6 Chemistry 1A Spring 2009 Exam 2 Key Chapters -6 You might find the following useful. 0.00831 kj ΔH = ΔE + ( Δn)RT R = K mol 0.0018 kj q = - C cal + m w Δ T K mol ΔH rxn = Σ ΔH f (products) Σ ΔH f (reactants)

More information

Chapter 4 Reactions in Aqueous Solution

Chapter 4 Reactions in Aqueous Solution Chapter 4 Reactions in Aqueous Solution Homework Chapter 4 11, 15, 21, 23, 27, 29, 35, 41, 45, 47, 51, 55, 57, 61, 63, 73, 75, 81, 85 1 2 Chapter Objectives Solution To understand the nature of ionic substances

More information

SCHOOL YEAR CH- 13 IONS IN AQUEOUS SOLUTIONS AND COLLIGATIVE PROPERTIES SUBJECT: CHEMISTRY GRADE : 11 TEST A

SCHOOL YEAR CH- 13 IONS IN AQUEOUS SOLUTIONS AND COLLIGATIVE PROPERTIES SUBJECT: CHEMISTRY GRADE : 11 TEST A SCHOOL YEAR 2017-18 NAME: CH- 13 IONS IN AQUEOUS SOLUTIONS AND COLLIGATIVE PROPERTIES SUBJECT: CHEMISTRY GRADE : 11 TEST A Choose the best answer from the options that follow each question. 1. A solute

More information

CH 221 Chapter Four Part II Concept Guide

CH 221 Chapter Four Part II Concept Guide CH 221 Chapter Four Part II Concept Guide 1. Solubility Why are some compounds soluble and others insoluble? In solid potassium permanganate, KMnO 4, the potassium ions, which have a charge of +1, are

More information

Chapter 4 Three Major Classes of Chemical Reactions

Chapter 4 Three Major Classes of Chemical Reactions Chapter 4 Three Major Classes of Chemical Reactions Solution Stoichiometry Many reactions (biochemical, marine, etc.) take place in solution. We need to be able to express the number of moles of particles

More information

Chapter 4. Reactions in Aqueous Solution

Chapter 4. Reactions in Aqueous Solution Chapter 4. Reactions in Aqueous Solution 4.1 General Properties of Aqueous Solutions A solution is a homogeneous mixture of two or more substances. A solution is made when one substance (the solute) is

More information

CHEMpossible. Final Exam Review

CHEMpossible. Final Exam Review CHEMpossible Final Exam Review 1. Given the following pair of reactions and their equilibrium constants: 2NO 2 (g) 2NO (g) + O 2 (g) K c = 15.5 2NO (g) + Cl 2 (g) 2 NOCl (g) K c = 3.20 10-3 Calculate a

More information

Chapter 4: Types of Chemical Reactions and Solution Stoichiometry

Chapter 4: Types of Chemical Reactions and Solution Stoichiometry Chapter 4: Types of Chemical Reactions and Solution Stoichiometry 4.1 Water, the Common Solvent 4.2 The Nature of Aqueous Solutions: Strong and Weak Electrolytes 4.3 The Composition of Solutions (MOLARITY!)

More information

Reactions in Aqueous Solutions

Reactions in Aqueous Solutions Reactions in Aqueous Solutions 1 Chapter 4 General Properties of Aqueous Solutions (4.1) Precipitation Reactions (4.2) Acid-Base Reactions (4.3) Oxidation-Reduction Reactions (4.4) Concentration of Solutions

More information

CHE 105 FA17 Exam 2. How many moles of beryllium are in 15.0 grams of Be?

CHE 105 FA17 Exam 2. How many moles of beryllium are in 15.0 grams of Be? CHE 105 FA17 Exam 2 Your Name: Your ID: Question #: 1 How many moles of beryllium are in 150 grams of Be? A 66 B 13515 C 901 D 0601 Question #: 2 Vanillin, C8H8O3, is the molecule responsible for the vanilla

More information

Chapter 4 Electrolytes and Aqueous Reactions. Dr. Sapna Gupta

Chapter 4 Electrolytes and Aqueous Reactions. Dr. Sapna Gupta Chapter 4 Electrolytes and Aqueous Reactions Dr. Sapna Gupta Aqueous Solutions Solution - a homogeneous mixture of solute + solvent Solute: the component that is dissolved Solvent: the component that does

More information

Chapter 4: Types of Chemical reactions and Solution Stoichiometry

Chapter 4: Types of Chemical reactions and Solution Stoichiometry Chapter 4: Types of Chemical reactions and Solution Stoichiometry 4.1 Water, The Common Solvent State why water acts as a common solvent. Draw the structure of water, including partial charge. Write equations

More information

Reactions in Aqueous Solutions

Reactions in Aqueous Solutions Reactions in Aqueous Solutions Chapter 4 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. A solution is a homogenous mixture of 2 or more substances. The solute

More information

Chapter 6. Types of Chemical Reactions and Solution Stoichiometry

Chapter 6. Types of Chemical Reactions and Solution Stoichiometry Chapter 6 Types of Chemical Reactions and Solution Stoichiometry Chapter 6 Table of Contents (6.1) (6.2) (6.3) (6.4) (6.5) (6.6) (6.7) (6.8) Water, the common solvent The nature of aqueous solutions: Strong

More information

Chapter 8 Chemical Reactions

Chapter 8 Chemical Reactions Chemistry/ PEP Name: Date: Chapter 8 Chemical Reactions Chapter 8: 1 7, 9 18, 20, 21, 24 26, 29 31, 46, 55, 69 Practice Problems 1. Write a skeleton equation for each chemical reaction. Include the appropriate

More information

Chemistry 101 Chapter 4 STOICHIOMETRY

Chemistry 101 Chapter 4 STOICHIOMETRY STOICHIOMETRY Stoichiometry is the quantitative relationship between the reactants and products in a balanced chemical equation. Stoichiometry allows chemists to predict how much of a reactant is necessary

More information

Aqueous Reactions. The products are just the cation-anion pairs reversed, or the outies (A and Y joined) and the innies (B and X joined).

Aqueous Reactions. The products are just the cation-anion pairs reversed, or the outies (A and Y joined) and the innies (B and X joined). Aqueous Reactions Defining Aqueous Reactions Aqueous reactions are reactions that take place in water. To understand them, it is important to understand how compounds behave in water. Some compounds are

More information

Which of the following answers is correct and has the correct number of significant figures?

Which of the following answers is correct and has the correct number of significant figures? Avogadro s Number, N A = 6.022 10 23 1. [7 points] Carry out the following mathematical operation: 6.06 10 3 + 1.1 10 2 Which of the following answers is correct and has the correct number of significant

More information

7/16/2012. Chapter Four: Like Dissolve Like. The Water Molecule. Ionic Compounds in Water. General Properties of Aqueous Solutions

7/16/2012. Chapter Four: Like Dissolve Like. The Water Molecule. Ionic Compounds in Water. General Properties of Aqueous Solutions General Properties of Aqueous Solutions Chapter Four: TYPES OF CHEMICAL REACTIONS AND SOLUTION STOICHIOMETRY A solution is a homogeneous mixture of two or more substances. A solution is made when one substance

More information

Chapter 4. The Major Classes of Chemical Reactions 4-1

Chapter 4. The Major Classes of Chemical Reactions 4-1 Chapter 4 The Major Classes of Chemical Reactions 4-1 The Major Classes of Chemical Reactions 4.1 The Role of Water as a Solvent 4.2 Writing Equations for Aqueous Ionic Reactions 4.3 Precipitation Reactions

More information

Chapter 4 Electrolytes Acid-Base (Neutralization) Oxidation-Reduction (Redox) Reactions. Dr. Sapna Gupta

Chapter 4 Electrolytes Acid-Base (Neutralization) Oxidation-Reduction (Redox) Reactions. Dr. Sapna Gupta Chapter 4 Electrolytes Acid-Base (Neutralization) Oxidation-Reduction (Redox) Reactions Dr. Sapna Gupta Types of Reactions Two classifications: one how atoms are rearrangement and the other is chemical

More information

Chapter 4. Reactions in Aqueous Solution. Solutions. 4.1 General Properties of Aqueous Solutions

Chapter 4. Reactions in Aqueous Solution. Solutions. 4.1 General Properties of Aqueous Solutions Chapter 4 in Solution 4.1 General Properties of Solutions Solutions Solutions are defined as homogeneous mixtures of two or more pure substances. The solvent is present in greatest abundance. All other

More information

IB Chemistry Solutions Gasses and Energy

IB Chemistry Solutions Gasses and Energy Solutions A solution is a homogeneous mixture it looks like one substance. An aqueous solution will be a clear mixture with only one visible phase. Be careful with the definitions of clear and colourless.

More information

Chap. 4 AQUEOUS RXNS. O H δ+ 4.1 WATER AS A SOLVENT 4.2 AQUEOUS IONIC REACTIONS. Page 4-1. NaOH(aq) + HCl(g) NaCl(aq) +H 2 O

Chap. 4 AQUEOUS RXNS. O H δ+ 4.1 WATER AS A SOLVENT 4.2 AQUEOUS IONIC REACTIONS. Page 4-1. NaOH(aq) + HCl(g) NaCl(aq) +H 2 O Chap. AQUEOUS RXNS.1 WATER AS A SOLVENT Describe solution composition in terms of molarity Describe strong and weak electrolyte solutions, including acids and bases Use ionic equations to describe neutralization

More information

1. Hydrochloric acid is mixed with aqueous sodium bicarbonate Molecular Equation

1. Hydrochloric acid is mixed with aqueous sodium bicarbonate Molecular Equation NAME Hr Chapter 4 Aqueous Reactions and Solution Chemistry Practice A (Part 1 = Obj. 1-3) (Part 2 = Obj. 4-6) Objective 1: Electrolytes, Acids, and Bases a. Indicate whether each of the following is strong,

More information

Chapter 4. Reactions In Aqueous Solution

Chapter 4. Reactions In Aqueous Solution Chapter 4 Reactions In Aqueous Solution I) General Properties of Aqueous Solutions Homogeneous mixture on a molecular level - prop. same throughout - separable by physical means - variable composition

More information

Types of Reactions: Reactions

Types of Reactions: Reactions 1 Reactions On the A.P. Test there will be one question (question #4) that will say: Give the formulas to show the reactants and the products for the following chemical reactions. Each occurs in aqueous

More information

Electrolytes do conduct electricity, in proportion to the concentrations of their ions in solution.

Electrolytes do conduct electricity, in proportion to the concentrations of their ions in solution. Chapter 4 (Hill/Petrucci/McCreary/Perry Chemical Reactions in Aqueous Solutions This chapter deals with reactions that occur in aqueous solution these solutions all use water as the solvent. We will look

More information

Types of Reactions: Reactions

Types of Reactions: Reactions 1 Reactions On the A.P. Test there will be one question (question #4) that will say: Give the formulas to show the reactants and the products for the following chemical reactions. Each occurs in aqueous

More information

CHEMISTRY Midterm #2 October 26, Pb(NO 3 ) 2 + Na 2 SO 4 PbSO 4 + 2NaNO 3

CHEMISTRY Midterm #2 October 26, Pb(NO 3 ) 2 + Na 2 SO 4 PbSO 4 + 2NaNO 3 CHEMISTRY 123-02 Midterm #2 October 26, 2004 The total number of points in this exam is 100. The total exam time is 50 min. Good luck! PART I: MULTIPLE CHOICE (Each multiple choice question has a 2-point

More information

Page 1. Exam 2 Review Summer A 2002 MULTIPLE CHOICE. 1. Consider the following reaction: CaCO (s) + HCl(aq) CaCl (aq) + CO (g) + H O(l)

Page 1. Exam 2 Review Summer A 2002 MULTIPLE CHOICE. 1. Consider the following reaction: CaCO (s) + HCl(aq) CaCl (aq) + CO (g) + H O(l) Page 1 MULTIPLE CHOICE 1. Consider the following reaction: CaCO (s) + HCl(aq) CaCl (aq) + CO (g) + H O(l) The coefficient of HCl(aq) in the balanced reaction is. a) 1 b) 2 c) 3 d) 4 e) 0 2. Given the information

More information

(g) Fe(OH) 3 : ; (h) Cr(NO 3 ) 3 : ; (c) Chromium(III) sulfate: ; (h) Dinitrogen tetroxide:

(g) Fe(OH) 3 : ; (h) Cr(NO 3 ) 3 : ; (c) Chromium(III) sulfate: ; (h) Dinitrogen tetroxide: 1. Name each of the following compounds: (a) Ca(OCl) 2 : ; (b) (NH 4 ) 3 PO 4 : ; (c) K 2 Cr 2 O 7 : ; (d) HBrO 2 : ; (e) PF 5 : ; (f) B 2 O 3 : ; (g) Fe(OH) 3 : ; (h) Cr(NO 3 ) 3 : ; (i) Na 2 C 2 O 4

More information

ed. Brad Collins Aqueous Chemistry Chapter 5 Some images copyright The McGraw-Hill Companies, Inc. Sunday, August 18, 13

ed. Brad Collins Aqueous Chemistry Chapter 5 Some images copyright The McGraw-Hill Companies, Inc. Sunday, August 18, 13 ed. Brad Collins Aqueous Chemistry Chapter 5 Some images copyright The McGraw-Hill Companies, Inc. A solution is a homogenous mixture of 2 or more substances at the molecular level The solute(s) is(are)

More information

Chapter 5 Classification and Balancing of Chemical Reactions

Chapter 5 Classification and Balancing of Chemical Reactions Chapter 5 Classification and Balancing of Chemical Reactions 5.1 Chemical Equations Chemical equations describe chemical reactions. - As words: hydrogen plus oxygen combine to form water - As a chemical

More information

Quick Review. - Chemical equations - Types of chemical reactions - Balancing chemical equations - Stoichiometry - Limiting reactant/reagent

Quick Review. - Chemical equations - Types of chemical reactions - Balancing chemical equations - Stoichiometry - Limiting reactant/reagent Quick Review - Chemical equations - Types of chemical reactions - Balancing chemical equations - Stoichiometry - Limiting reactant/reagent Water H 2 O Is water an ionic or a covalent compound? Covalent,

More information

Chapter 3. Molecules, Moles, and Chemical Equations

Chapter 3. Molecules, Moles, and Chemical Equations Chapter 3 Molecules, Moles, and Chemical Equations Law of Conservation of Matter Matter is neither created nor destroyed. In chemistry the number of atoms going into a chemical reaction must be the same

More information

H H H H H O H O. Role of Water. Role of Water. Chapter 4. Chemical Reactions in Aqueous Solution H 2 H H H 2 O. Role of H 2 O(l) as solvent.

H H H H H O H O. Role of Water. Role of Water. Chapter 4. Chemical Reactions in Aqueous Solution H 2 H H H 2 O. Role of H 2 O(l) as solvent. Role of Water Role of Water Chemical Reactions in Aqueous Solution Role of H 2 O(l) as solvent The polar nature of water molecule Two key features: 1. The distribution of bonding electrons O H covalent

More information

Reactions in Aqueous Solutions

Reactions in Aqueous Solutions Copyright 2004 by houghton Mifflin Company. Reactions in Aqueous Solutions Chapter 7 All rights reserved. 1 7.1 Predicting if a Rxn Will Occur When chemicals are mixed and one of these driving forces can

More information

2. If a gas is released in a reaction (ex: Hydrogen gas bubbles off), is it written as a reactant or a product?

2. If a gas is released in a reaction (ex: Hydrogen gas bubbles off), is it written as a reactant or a product? PRE-AP CHEMISTRY SPRING FINAL EXAM REVIEW Name _ Period Exam Date 100% COMPLETION OF THIS REVIEW BY THE DAY OF YOUR FINAL EXAM WILL COUNT AS A 5 POINT BONUS ADDED TO YOUR FINAL EXAM SCORE. THERE WILL BE

More information

Chem 110 General Principles of Chemistry

Chem 110 General Principles of Chemistry Chem 110 General Principles of Chemistry Chapter 3 (Page 88) Aqueous Reactions and Solution Stoichiometry In this chapter you will study chemical reactions that take place between substances that are dissolved

More information

Name:. Correct Questions = Wrong Questions =.. Unattempt Questions = Marks =

Name:. Correct Questions = Wrong Questions =.. Unattempt Questions = Marks = Name:. Correct Questions = Wrong Questions =.. Unattempt Questions = Marks = 1. (12%) Compound X contains 2.239% hydrogen, 26.681% carbon and 71.080 % oxygen by mass. The titration of 0.154 g of this compound

More information

Ions in Aqueous Solutions and Colligative Properties

Ions in Aqueous Solutions and Colligative Properties CHAPTER 13 REVIEW Ions in Aqueous Solutions and Colligative Properties SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. Use the guidelines in Table 1 on page 437 of the text

More information

Chapter Four: Reactions in Aqueous Solution

Chapter Four: Reactions in Aqueous Solution Chapter Four: Reactions in Aqueous Solution Learning Outcomes: Identify compounds as acids or bases, and as strong, weak, or nonelectrolytes Recognize reactions by type and be able to predict the products

More information

Chapter 4 Suggested end-of-chapter problems with solutions

Chapter 4 Suggested end-of-chapter problems with solutions Chapter 4 Suggested end-of-chapter problems with solutions a. 5.6 g NaHCO 1 mol NaHCO 84.01 g NaHCO = 6.69 10 mol NaHCO M = 6.69 10 mol 50.0 m 1000 m = 0.677 M NaHCO b. 0.1846 g K Cr O 7 1 mol K 94.0 g

More information

Chemistry 12. Resource Exam B. Exam Booklet

Chemistry 12. Resource Exam B. Exam Booklet Chemistry 12 Resource Exam B Exam Booklet Contents: 21 pages Examination: 2 hours 50 multiple-choice questions in the Exam Booklet Additional Time Permitted: 60 minutes Province of British Columbia PART

More information

Chapter 4. Aqueous Reactions and Solution Stoichiometry

Chapter 4. Aqueous Reactions and Solution Stoichiometry Sample Exercise 4.1 (p. 127) The diagram below represents an aqueous solution of one of the following compounds: MgCl 2, KCl, or K 2 SO 4. Which solution does it best represent? Practice Exercise 1 (4.1)

More information

Solubility Rules See also Table 4.1 in text and Appendix G in Lab Manual

Solubility Rules See also Table 4.1 in text and Appendix G in Lab Manual Ch 4 Chemical Reactions Ionic Theory of Solutions - Ionic substances produce freely moving ions when dissolved in water, and the ions carry electric current. (S. Arrhenius, 1884) - An electrolyte is a

More information

Name. Practice Test 2 Chemistry 111

Name. Practice Test 2 Chemistry 111 Name Practice Test 2 Chemistry 111 1) In the aqueous reaction of K 2 SO 4 (aq) + Ba(NO 3 ) 2 (aq) BaSO 4 (s) + 2KNO 3 (aq), which ions are the spectator ions? A) Ba 2+ 2- and SO 4 B) Ba 2+ and K + C) Ba

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. Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) When the following equation is balanced, the coefficients are. 1) NH3 (g) + O2 (g) NO2

More information

During photosynthesis, plants convert carbon dioxide and water into glucose (C 6 H 12 O 6 ) according to the reaction:

During photosynthesis, plants convert carbon dioxide and water into glucose (C 6 H 12 O 6 ) according to the reaction: Example 4.1 Stoichiometry During photosynthesis, plants convert carbon dioxide and water into glucose (C 6 H 12 O 6 ) according to the reaction: Suppose that a particular plant consumes 37.8 g of CO 2

More information

Funsheet 9.1 [VSEPR] Gu 2015

Funsheet 9.1 [VSEPR] Gu 2015 Funsheet 9.1 [VSEPR] Gu 2015 Molecule Lewis Structure # Atoms Bonded to Central Atom # Lone Pairs on Central Atom Name of Shape 3D Lewis Structure NI 3 CF 4 OCl 2 C 2 F 2 HOF Funsheet 9.1 [VSEPR] Gu 2015

More information

Unit 4a: Solution Stoichiometry Last revised: October 19, 2011 If you are not part of the solution you are the precipitate.

Unit 4a: Solution Stoichiometry Last revised: October 19, 2011 If you are not part of the solution you are the precipitate. 1 Unit 4a: Solution Stoichiometry Last revised: October 19, 2011 If you are not part of the solution you are the precipitate. You should be able to: Vocabulary of water solubility Differentiate between

More information

CH 4 AP. Reactions in Aqueous Solutions

CH 4 AP. Reactions in Aqueous Solutions CH 4 AP Reactions in Aqueous Solutions Water Aqueous means dissolved in H 2 O Moderates the Earth s temperature because of high specific heat H-bonds cause strong cohesive and adhesive properties Polar,

More information

TYPES OF CHEMICAL REACTIONS

TYPES OF CHEMICAL REACTIONS TYPES OF CHEMICAL REACTIONS Precipitation Reactions Compounds Soluble Ionic Compounds 1. Group 1A cations and NH 4 + 2. Nitrates (NO 3 ) Acetates (CH 3 COO ) Chlorates (ClO 3 ) Perchlorates (ClO 4 ) Solubility

More information

Chapter 4. Reactions in Aqueous Solution

Chapter 4. Reactions in Aqueous Solution Chapter 4 Reactions in Aqueous Solution Topics General properties of aqueous solutions Precipitation reactions Acid base reactions Oxidation reduction reactions Concentration of solutions Aqueous reactions

More information

Chemical Reactions: An Introduction

Chemical Reactions: An Introduction Chemical Reactions: An Introduction Ions in Aqueous Solution Ionic Theory of Solutions Many ionic compounds dissociate into independent ions when dissolved in water H 2O NaCl(s) Na Cl These compounds that

More information

Chapter 6. Chemical Reactions. Sodium reacts violently with bromine to form sodium bromide.

Chapter 6. Chemical Reactions. Sodium reacts violently with bromine to form sodium bromide. Chapter 6 Chemical Reactions Sodium reacts violently with bromine to form sodium bromide. Evidence of Chemical Reactions Chemical Equations Reactants Products Reactant(s): Substance(s) present before the

More information

Chapter 17. Additional Aspects of Equilibrium

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

More information

Reaction Classes. Precipitation Reactions

Reaction Classes. Precipitation Reactions Reaction Classes Precipitation: synthesis of an ionic solid a solid precipitate forms when aqueous solutions of certain ions are mixed AcidBase: proton transfer reactions acid donates a proton to a base,

More information

Aqueous Reactions and Solution Stoichiometry (continuation)

Aqueous Reactions and Solution Stoichiometry (continuation) Aqueous Reactions and Solution Stoichiometry (continuation) 1. Electrolytes and non-electrolytes 2. Determining Moles of Ions in Aqueous Solutions of Ionic Compounds 3. Acids and Bases 4. Acid Strength

More information

Chemistry 1A. Chapter 5

Chemistry 1A. Chapter 5 Chemistry 1A Chapter 5 Water, H 2 O Water Attractions Liquid Water Solutions A solution, also called a homogeneous mixture, is a mixture whose particles are so evenly distributed that the relative concentrations

More information

Basic SL Concepts. D. 2.0 (Total 1 mark) When the equation above is balanced, what is the coefficient for oxygen? D.

Basic SL Concepts. D. 2.0 (Total 1 mark) When the equation above is balanced, what is the coefficient for oxygen? D. Basic SL Concepts 1. 3.0 dm 3 of sulfur dioxide is reacted with.0 dm 3 of oxygen according to the equation below. SO(g) + O(g) SO3(g) What volume of sulfur trioxide (in dm 3 ) is formed? (Assume the reaction

More information

CH 101 Fall 2018 Discussion #8 Chapter 6 Your name: TF s name: Discussion Day/Time: Things you should know when you leave Discussion today:

CH 101 Fall 2018 Discussion #8 Chapter 6 Your name: TF s name: Discussion Day/Time: Things you should know when you leave Discussion today: CH 101 Fall 2018 Discussion #8 Chapter 6 Your name: TF s name: Discussion Day/Time: Things you should know when you leave Discussion today: Precipitation Reaction & Solubility Solubility of Ionic compounds

More information

Section 4: Aqueous Reactions

Section 4: Aqueous Reactions Section 4: Aqueous Reactions 1. Solution composition 2. Electrolytes and nonelectrolytes 3. Acids, bases, and salts 4. Neutralization ti reactions 5. Precipitation reactions 6. Oxidation/reduction reactions

More information

AP Chemistry. 4. Which atom in its ground state has the most unpaired electrons? a. Ge b. As c. Se d. Br e. Ga

AP Chemistry. 4. Which atom in its ground state has the most unpaired electrons? a. Ge b. As c. Se d. Br e. Ga Name AP Chemistry Take Home Quiz Due Thursday, 1/9/2014 Bubble the correct answer on your scantron for each of the following. 1. Barium sulfate is LEAST soluble in a 0.01-molar solution of which of the

More information

AP Chemistry Note Outline Chapter 4: Reactions and Reaction Stoichiometry:

AP Chemistry Note Outline Chapter 4: Reactions and Reaction Stoichiometry: AP Chemistry Note Outline Chapter 4: Reactions and Reaction Stoichiometry: Water as a solvent Strong and Weak Electrolytes Solution Concentrations How to Make up a solution Types of Reactions Introduction

More information

Chemistry 150/151 Review Worksheet

Chemistry 150/151 Review Worksheet Chemistry 150/151 Review Worksheet This worksheet serves to review concepts and calculations from first semester General Chemistry (CHM 150/151). Brief descriptions of concepts are included here. If you

More information

Chapter 4; Reactions in Aqueous Solutions. Chapter 4; Reactions in Aqueous Solutions. V. Molarity VI. Acid-Base Titrations VII. Dilution of Solutions

Chapter 4; Reactions in Aqueous Solutions. Chapter 4; Reactions in Aqueous Solutions. V. Molarity VI. Acid-Base Titrations VII. Dilution of Solutions Chapter 4; Reactions in Aqueous Solutions I. Electrolytes vs. NonElectrolytes II. Precipitation Reaction a) Solubility Rules III. Reactions of Acids a) Neutralization b) Acid and Carbonate c) Acid and

More information

Review Material for Exam #2

Review Material for Exam #2 Review Material for Exam #2 1. a. Calculate the molarity of a solution made with 184.6 mg sample of potassium dichromate dissolved in enough water to give 500.0 ml of solution. b. What is the molarity

More information

I. Properties of Aqueous Solutions A) Electrolytes and Non-Electrolytes B) Predicting Solubility* II. Reactions of Ionic Compounds in Solution*

I. Properties of Aqueous Solutions A) Electrolytes and Non-Electrolytes B) Predicting Solubility* II. Reactions of Ionic Compounds in Solution* Chapter 5 Reactions in Aqueous Solutions Titrations Kick Acid!!! 1 I. Properties of Aqueous Solutions A) Electrolytes and Non-Electrolytes B) Predicting Solubility* II. Reactions of Ionic Compounds in

More information

Name Period CH 180 Practice Test: Chapters 3 and 4

Name Period CH 180 Practice Test: Chapters 3 and 4 Name Period CH 180 Practice Test: Chapters 3 and 4 Multiple Choice: 1. 11. 2. 12. 3. 13. 4. 14. 5. 15. 6. 16. 7. 17. 8. 18. 9. 19. 10. 20. 21. 22. 23. 24. 25. 26. 27. 1 Directions: Answer all questions.

More information

Ch 4-5 Practice Problems - KEY

Ch 4-5 Practice Problems - KEY Ch 4-5 Practice Problems - KEY The following problems are intended to provide you with additional practice in preparing for the exam. Questions come from the textbook, previous quizzes, previous exams,

More information

October 19, 1999 Page 1. Chapter 4 Practice Worksheet Dr. Palmer Graves, Instructor MULTIPLE CHOICE

October 19, 1999 Page 1. Chapter 4 Practice Worksheet Dr. Palmer Graves, Instructor MULTIPLE CHOICE October 19, 1999 Page 1 MULTIPLE CHOICE Section 4.1 Some Ways that Chemical Reactions Occur 1. The reaction of HNO (aq) + KOH(aq) KNO (aq) + H O(l) is best classified as a(n) a) acid-base neutralization

More information

CHEM 200/202. Professor Jing Gu Office: EIS-210. All s are to be sent to:

CHEM 200/202. Professor Jing Gu Office: EIS-210. All  s are to be sent to: CHEM 200/202 Professor Jing Gu Office: EIS-210 All emails are to be sent to: chem200@mail.sdsu.edu My office hours will be held in GMCS-212 on Monday from 9 am to 11 am or by appointment. ANNOUNCEMENTS

More information

Chapter 3 Chemical Reactions

Chapter 3 Chemical Reactions Chapter 3 Chemical Reactions Jeffrey Mack California State University, Sacramento Chemical Reactions Reactants: Zn + I 2 Product: ZnI 2 Chemical Reactions Evidence of a chemical reaction: Gas Evolution

More information

Slide 1 / Objects can possess energy as: (a) endothermic energy (b) potential energy (c) kinetic energy. a only b only c only a and c b and c

Slide 1 / Objects can possess energy as: (a) endothermic energy (b) potential energy (c) kinetic energy. a only b only c only a and c b and c Slide 1 / 84 1 Objects can possess energy as: (a) endothermic energy (b) potential energy (c) kinetic energy A B C D E a only b only c only a and c b and c Slide 2 / 84 2 The internal energy of a system

More information

11/3/09. Aqueous Solubility of Compounds. Aqueous Solubility of Ionic Compounds. Aqueous Solubility of Ionic Compounds

11/3/09. Aqueous Solubility of Compounds. Aqueous Solubility of Ionic Compounds. Aqueous Solubility of Ionic Compounds Aqueous Solubility of Compounds Not all compounds dissolve in water. Solubility varies from compound to compound. Chapter 5: Chemical Reactions Soluble ionic compounds dissociate. Ions are solvated Most

More information

Chapter 4 Reactions in Aqueous Solutions. Copyright McGraw-Hill

Chapter 4 Reactions in Aqueous Solutions. Copyright McGraw-Hill Chapter 4 Reactions in Aqueous Solutions Copyright McGraw-Hill 2009 1 4.1 General Properties of Aqueous Solutions Solution - a homogeneous mixture Solute: the component that is dissolved Solvent: the component

More information

Chapter 4 Notes Types of Chemical Reactions and Solutions Stoichiometry A Summary

Chapter 4 Notes Types of Chemical Reactions and Solutions Stoichiometry A Summary Chapter 4 Notes Types of Chemical Reactions and Solutions Stoichiometry A Summary 4.1 Water, the Common Solvent A. Structure of water 1. Oxygen s electronegativity is high (3.5) and hydrogen s is low (2.1)

More information

Arrhenius Acid-Base Concept Svante Arrhenius, 1884

Arrhenius Acid-Base Concept Svante Arrhenius, 1884 Arrhenius Acid-Base Concept Svante Arrhenius, 1884 O Acids and bases are electrolytes. O Acids are substances that produce hydrogen ion, H + (aq), in solution. O Bases are substances that produce hydroxide

More information

Lesson (1) Mole and chemical equation

Lesson (1) Mole and chemical equation Lesson (1) Mole and chemical equation 1 When oxygen gas reacts with magnesium, magnesium oxide is formed. Such Reactions are described by balanced equations known as "chemical equations" Δ 2Mg(s) + O2(g)

More information

Chapter 4. Reactions in Aqueous Solution. Lecture Presentation. John D. Bookstaver St. Charles Community College Cottleville, MO

Chapter 4. Reactions in Aqueous Solution. Lecture Presentation. John D. Bookstaver St. Charles Community College Cottleville, MO Lecture Presentation Chapter 4 in Solution 2012 Pearson Education, Inc. John D. Bookstaver St. Charles Community College Cottleville, MO Properties of Solutions Solute: substance in lesser quantity in

More information

Chemistry 2 Summer 2008 Exam 2 Chapters 6(part), 7-10

Chemistry 2 Summer 2008 Exam 2 Chapters 6(part), 7-10 Name Chemistry 2 Summer 2008 Exam 2 Chapters 6(part), 7-10 Answer the following by writing the word, words, letter, letters or number in each blank that best completes each sentence. (1 point each) 1.

More information

Acids and Bases. Properties of Acids. Properties of Bases

Acids and Bases. Properties of Acids. Properties of Bases Chemistry 2A/2B Term 3 Notes B 1 Coghlan Chemistry 2A/2B Term 3 Notes B Properties of Acids Acids and Bases 1. Neutralise. 2. Turns litmus red. 3. Conducts when in with water form an (acids ). 4. React

More information

Reactions in Aqueous Solution

Reactions in Aqueous Solution 1 Reactions in Aqueous Solution Chapter 4 For test 3: Sections 3.7 and 4.1 to 4.5 Copyright The McGrawHill Companies, Inc. Permission required for reproduction or display. 2 A solution is a homogenous

More information

2. What is the charge of the nucleus in an atom of oxygen-17? (1) 0 (2) 2 (3) +8 (4) +17

2. What is the charge of the nucleus in an atom of oxygen-17? (1) 0 (2) 2 (3) +8 (4) +17 60 Most Missed Chemistry Regents Exams Questions 1. In the wave-mechanical model, an orbital is a region of space in an atom where there is (1) a high probability of finding an electron (2) a high probability

More information

CHAPTER 4 TYPES OF CHEMICAL EQUATIONS AND SOLUTION STOICHIOMETRY

CHAPTER 4 TYPES OF CHEMICAL EQUATIONS AND SOLUTION STOICHIOMETRY CHAPTER 4 TYPES OF CHEMICAL EQUATIONS AND SOLUTION STOICHIOMETRY Water, the common solvent Solution is a homogeneous mixture Solvent is the substance that does the dissolving Solute is the substance that

More information

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

2. Write a balanced chemical equation which corresponds to the following equilibrium constant expression. Practice Problems for Chem 1B Exam 1 Chapter 14: Chemical Equilibrium 1. Which of the following statements is/are CORRECT? 1. For a chemical system, if the reaction quotient (Q) is greater than K, products

More information

Acids and Bases. Unit 10

Acids and Bases. Unit 10 Acids and Bases Unit 10 1 Properties of Acids and Bases Acids Bases Taste Sour Turns Litmus Dye Red Reacts with Metals to give H 2 (g) Taste Bitter Turns Litmus Dye Blue Do Not React with Metals Reacts

More information

6. Place the following elements in order of increasing atomic radii: Mg, Na, Rb, Cl.

6. Place the following elements in order of increasing atomic radii: Mg, Na, Rb, Cl. CH141 Practice Problems/Practice Final Exam Page 1 of 12 Name: 1. What is the SO 4 2- concentration of a solution prepared by dissolving 3.00 g of Na 2 SO 4 in 1.00 L of water? 2. What is the hybridization

More information

9/24/12. Chemistry Second Edition Julia Burdge. Reactions in Aqueous Solutions

9/24/12. Chemistry Second Edition Julia Burdge. Reactions in Aqueous Solutions Chemistry Second Edition Julia Burdge 4 Reactions in Aqueous Solutions Copyright (c) The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 4 Reactions in Aqueous Solutions

More information

CH 221 Sample Exam Exam II Name: Lab Section:

CH 221 Sample Exam Exam II Name: Lab Section: Exam II Name: Lab Section: Part I: Multiple Choice Questions (100 Points) Use a scantron sheet for Part I. There is only one best answer for each question. 1. When methanol undergoes complete combustion,

More information

15 Acids, Bases, and Salts. Lemons and limes are examples of foods that contain acidic solutions.

15 Acids, Bases, and Salts. Lemons and limes are examples of foods that contain acidic solutions. 15 Acids, Bases, and Salts Lemons and limes are examples of foods that contain acidic solutions. Chapter Outline 15.1 Acids and Bases 15.2 Reactions of Acids and Bases 15.3 Salts 15.4 Electrolytes and

More information

Chem II - Wed, 9/14/16

Chem II - Wed, 9/14/16 Chem II - Wed, 9/14/16 Do Now Drop off any study guides you want color coded Pull out stoich HW Homework See board Agenda Stoich Ch 4 Labish thing Chapter 4 Chemical Reactions & Solution Stoich Water Possesses

More information

A reaction in which a solid forms is called a precipitation reaction. Solid = precipitate

A reaction in which a solid forms is called a precipitation reaction. Solid = precipitate Chapter 7 Reactions in Aqueous Solutions 1 Section 7.1 Predicting Whether a Reaction Will Occur Four Driving Forces Favor Chemical Change 1. Formation of a solid 2. Formation of water 3. Transfer of electrons

More information

Chapter 10. Acids and Bases

Chapter 10. Acids and Bases Chapter 10 Acids and Bases 1 Properties of Aqueous Solutions of Acids and Bases Aqueous acidic solutions have the following properties: 1. They have a sour taste.. They change the colors of many indicators.

More information

Chem 101 Review. Fall 2012

Chem 101 Review. Fall 2012 Chem 101 Review Fall 2012 Elements, Atoms, Ions Elements in nature symbols Constant composition chemical formula Dalton s atomic theory Atomic structure what makes up the atom ions isotopes Periodic table

More information

CHM152LL Solution Chemistry Worksheet

CHM152LL Solution Chemistry Worksheet Name: Section: CHM152LL Solution Chemistry Worksheet Many chemical reactions occur in solution. Solids are often dissolved in a solvent and mixed to produce a chemical reaction that would not occur if

More information

2. Relative molecular mass, M r - The relative molecular mass of a molecule is the average mass of the one molecule when compared with

2. Relative molecular mass, M r - The relative molecular mass of a molecule is the average mass of the one molecule when compared with Chapter 3: Chemical Formulae and Equations 1. Relative atomic mass, A r - The relative atomic mass of an element is the average mass of one atom of an element when compared with mass of an atom of carbon-12

More information

CHE 105 Spring 2018 Exam 2

CHE 105 Spring 2018 Exam 2 CHE 105 Spring 2018 Exam 2 Your Name: Your ID: Question #: 1 A penny contains 373 x 10 2 moles of zinc How many atoms of zinc are in a penny? A 225 x 10 22 atoms B 221 x 10 23 atoms C 375 x 10 22 atoms

More information