Chemistry 12 Dr. Kline 26 October 2005 Name
|
|
- Robert Oliver
- 5 years ago
- Views:
Transcription
1 Test 1 first letter of last name Chemistry 12 Dr. Kline 26 October 2005 Name This test consists of a combination of multiple choice and other questions. There should be a total of 24 questions on 8 pages; please check to make sure that they are all here. You may use the equation/information sheet and any periodic table provided (on page 9). Do not use your own tables, scratch paper or other information. Do not share your calculator. Please turn off all cell phones, pagers and other communication devices; if they make noise, they will be confiscated. Shared calculators will be confiscated. Multiple Choice Questions Each of the following 19 questions is worth three points, for a total of 57 points. It is not necessary to show work for these questions; however, you may write on the exam. Answer each question by circling the letter(s) corresponding to the correct choice(s). Unless it is stated otherwise in a given problem, there is only one correct answer for each question. In questions where it states that more than one answer is possible, there may be one or more correct answers: please circle all of the correct answers. 1. Which of the following corresponds to the most basic solution? a. [H + ] = 5.0x10-9 M b. [OH - ] = 5.0x10-4 M c. ph = 9.25 d. poh = Which of the following compounds produce a basic solution when dissolved in water (assume water has a ph = 7). More than one answer may be correct. a. Na 2 SO 4 b. Ba(NO 3 ) 2 c. AlBr 3 d. none 3. Is the compound NH 4 CN acidic, basic, or neutral? a. acidic b. basic c. neutral 4. Which of the following net ionic equations accounts for the acid-base behavior of the compound in question #3? a. NH 4 + (aq) NH 3 (aq) + H + (aq) b. NH 3 (aq) + H 2 O(l) NH 4 + (aq) + HO - (aq) c. HCN(aq) CN - (aq) + H + (aq) d. CN - (aq) + H 2 O(l) HCN(aq) + HO - (aq) e. none of them because the compound is neutral 5. Which compound is acting as the Lewis acid in the reaction Ag NH 3 Ag(NH 3 ) 2 +? a. Ag + b. NH 3 c. neither, because it s not a Lewis acid-base reaction Page 1 of 1 Test 2C Intenet Chem 12
2 6. Into which category of acid-base reaction is the reaction F - (aq) + HSO 4 - (aq) HF(aq) + SO 4 2- (aq) classified? More than one answer may be correct. a. Bronsted-Lowry b. Arrhenius c. Lewis d. none, because it s not an acid-base reaction 7. Which of the following solutions has the highest concentration of fluoride ions? a M HF b M HF with 0.10 M HCl c M HF d M HF with 0.10 M HCl e. There is a tie among two or more of the above choices. 8. An aqueous solution is 1.000x10-8 M in HI. Which of the following is true concerning the ph of the solution? a. ph = b. ph = c. ph = d < ph < e < ph < In which of the following are the two species correctly arranged so that the acid predicted to be the stronger acid is listed first? More than one choice may be correct. a. H 2 PO 4 > H 3 PO 4 b. NH 3 > PH 3 c. H 3 PO 4 > H 2 SiO 3 d. none 10. What is true of K for the reaction HIO 2 + BrO - IO HBrO that occurs in aqueous solution? a. K = 1 b. K < 1 c. K > 1 d. it is impossible to tell 11. Suppose that the triprotic acid H 3 Z has K a1 = 4.0x10-3, K a2 = 2.0x10-8, and K a3 = 5.0x What is the value of K for the reaction H 2 Z - (aq) + H 2 O(l) OH - (aq) + H 3 Z? a. 2.5x10 2 b. 5.0x10 7 c. 2.0x10 11 d. 2.5x10-12 e. 5.0x10-7 f. 2.0x10-3 Page 2 of 2 Test 2C Intenet Chem 12
3 12. Which of the following is/are buffer solutions? More than one answer may be correct. a. 50. ml of 0.10 M HClO plus 25 ml of 0.20 M NaOH b. 50. ml of 0.10 M HCl plus 20. ml of 0.10 M NaClO c. 50. ml of 0.10 M HClO plus 20. ml of 0.10 M NaOH d. none of them 13. Which of the following aqueous solutions has the highest ph? a ml of M HBrO plus 100. ml of M KBrO b ml of M HBrO plus 100. ml of M KBrO c ml of M HBrO plus 100. ml of M KBrO d. all of them have the same ph because they contain the same acid-conjugate base pair e. it is impossible to tell without the K a of HBrO or the K b of BrO Suppose that each of the following M aqueous acids is titrated with M NaOH. Which will have the lowest ph at the equivalence point? a. HBrO 2 b. HClO 2 c. HIO d. HBrO e. it is impossible to tell 15. Which of the following statements is true regarding the titration of a weak base (in Erlenmeyer flask) with HCl (in buret)? More than one choice may be correct. a. at the equivalence point, ph > 7 b. the ph of the solution in the flask will decrease as the titration progresses c. the ph at the half-equivalence point can be acid, basic, or neutral, depending on the weak base used d. none of them 16. Which of the following indicators would be the most suitable for the titration of M CH 3 NH 2 (Erlenmeyer flask) with M HCl (buret)? Note: use the diagram below to select the indicator. This diagram is similar to the one in the lab book. a. Picophthalein b. SMC blue c. Corsair red ph Scale Indicator Corsair red red yellow SMC blue blue yellow Picophthalein yellow red Page 3 of 3 Test 2C Intenet Chem 12
4 17. Which of the following has the greatest molar solubility? a. Mn(OH) 2 b. Ag 2 CrO 4 c. BaSO 4 d. Ag 3 PO 4 e. Cu(OH) In which of the following aqueous solutions is BaCrO 4 the least soluble? a. plain deionized water b M HCl c M H 2 CrO 4 d M H 2 CrO 4 e M BaCl 2 f. it is impossible to tell 19. Suppose that three drops of 0.20 M KI are added to ml of M Pb(NO 3 ) 2. Will a precipitate of PbI 2 form? Assume that one drop is 0.05 ml a. yes b. no Problems and Questions Each of the following is worth the indicated number of points, for a total of 43 points. Please show work with units to receive credit. Also, be sure to provide all of the information requested for each question points Rank the following 0.10 M aqueous solutions in order of increasing ph using the blank lines near the bottom of this page. Please do not use arrows to adjust your answer. It is not necessary to show work for this question. NaOH HBrO LiI HClO 4 KBrO 2 KIO 2 HBrO 2 < < < < < < low ph high ph Page 4 of 4 Test 2C Intenet Chem 12
5 points Consider the diprotic acid telluric acid, H 2 Te, that has K a1 = 2.3x10-3 and K a2 = 1.6x a. Write the reaction equations that correspond to K a1 and K a2. b. Calculate the total concentration of each aqueous species in your reaction equations that is present in a solution of M telluric acid. c. Calculate the ph of M aqueous telluric acid points What volume of M HCl is needed to combine with 125 ml of M KNO 2 in order to produce a buffer with a ph of 3.25? points Consider the titration of ml of M HCHO 2 with M NaOH. What is the ph at the equivalence point of this titration? points Suppose that 45.0 ml of M HgNO 3 is combined with 25.0 ml of M K 2 CO 3, resulting in a precipitate of Hg 2 CO 3. Calculate the concentrations of all non-spectator ions present in the reaction mixture at the end of the reaction. <note since mercury (I) is diatomic, the formula of the first reactant should have been Hg 2 (NO 3 ) 2, but I didn t catch this until I was grading them; we ll just pretend that this problem concerned a rare form of mercury (I) that s not diatomic and that happens to have the same Ksp as the normal one when combined with carbonate> 2 HgNO 3 (aq) + K 2 CO 3 (aq) Hg 2 CO 3 (s) + 2 KNO 3 (aq) Page 5 of 5 Test 2C Intenet Chem 12
6 TEST #2 Information Fall 2005 You may (carefully) remove this sheet from the test. Quadratic Equation For an equation of the type ax 2 + bx + c = 0 x = "b ± b2 " 4ac 2a Acids, Bases and Buffers ph = -log(h + ) poh = -log(oh - ) K w = (H + )(OH - ) pk w = ph + poh K w = 1.0 x at 25 C pk w = at 25 C For a weak acid and its conjugate base, K a xk b =K w pk a = -logk a # & ph = pka + log na " # & % ( poh = pkb + log nha % ( $ nha ' $ na "' Dissociation Constants for Some Acids at 25 C (listed numerically by Ka) Name Formula K a Chromic acid H 2 CrO 4 K a1 = 0.18 K a2 = 3.2 x 10-7 Hydrogen sulfate ion HSO x 10 2 Nitrous acid HNO x 10-4 Formic acid HCHO x 10-4 Acetic acid HC 2 H 3 O x 10-5 Hydrocyanic acid HCN 6.2 x Ammonium ion + NH x Hydrolysis Constants for Two Bases at 25 C (alphabetical order by name) Name Formula K b Ammonia NH x 10-5 Methylamine CH 3 NH x 10-4 Page 6 of 6 Test 2C Intenet Chem 12
7 Selected Solubility Product Constants at 25 C (listed alphabetically by formula) Name Formula K sp Silver chromate Ag 2 CrO x Silver phosphate Ag 3 PO x Barium chromate BaCrO x Barium sulfate BaSO x Copper (II) hydroxide Cu(OH) x Iron (III) hydroxide Fe(OH) x Lead (II) iodide PbI x 10-9 Lead (II) iodate Pb(IO 3 ) x Manganese (II) hydroxide Mn(OH) x Mercury (I) carbonate Hg 2 CO x Page 7 of 7 Test 2C Intenet Chem 12
Test 2 first letter of last name --> Chemistry 12 Dr. Kline October 25, 2007
Test 2 first letter of last name --> Chemistry 12 Dr. Kline October 25, 2007 Name This test consists of a combination of multiple choice and other questions. There should be a total of 21 questions on
More informationChem 112, Fall 05 Exam 3A
Before you begin, make sure that your exam has all 10 pages. There are 32 required problems (3 points each, unless noted otherwise) and two extra credit problems (3 points each). Stay focused on your exam.
More informationChapter 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 informationPlease print: + log [A- ] [HA]
Please print: Last name: First name: Chem 1062 Exam 3 Spring 2005 Andy Aspaas, Instructor Thursday, April 7, 2005 Equations: K c = [C]c [D] d [A] a [B] b ph =! log[h 3 O + ] poh =! log[oh! ] ph + poh =
More informationCHEMISTRY 102 Fall 2010 Hour Exam III. 1. My answers for this Chemistry 102 exam should be graded with the answer sheet associated with:
1. My answers for this Chemistry 10 exam should be graded with the answer sheet associated with: a) Form A b) Form B c) Form C d) Form D e) Form E Consider the titration of 30.0 ml of 0.30 M HCN by 0.10
More informationC) SO 4 H H. C) The N-atom is the Lewis base because it accepted a pair of electrons to form the
AP Chemistry Test (Chapters 14 and 15) 1) Which one would hydrolyze water the most? A) Ca 2+ B) NO 3 - C) SO 4 2- H H D) CN - 2) Which one is true about the compound? H B-N H A) The N-atom is the Lewis
More informationAP CHEMISTRY NOTES 10-1 AQUEOUS EQUILIBRIA: BUFFER SYSTEMS
AP CHEMISTRY NOTES 10-1 AQUEOUS EQUILIBRIA: BUFFER SYSTEMS THE COMMON ION EFFECT The common ion effect occurs when the addition of an ion already present in the system causes the equilibrium to shift away
More informationWksht 3.3 Acid-Base Equilibria II Supplemental Instruction Iowa State University
Wksht 3.3 Acid-Base Equilibria II Supplemental Instruction Iowa State University Leader: Deborah Course: CHEM 178 Instructor: Bonaccorsi/Vela Date: 2/13/18 1. What are the conjugate bases of a. HCO3 -?
More informationAP Chapter 15 & 16: Acid-Base Equilibria Name
AP Chapter 15 & 16: Acid-Base Equilibria Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. AP Chapter 15 & 16: Acid-Base Equilibria 2 Warm-Ups (Show
More informationReview 7: Solubility Equilibria
Review 7: Solubility Equilibria Objectives: 1. Be able to write dissociation equations for ionic compounds dissolving in water. 2. Given Ksp, be able to determine the solubility of a substance in both
More informationCHEM 1412 Zumdahl & Zumdahl Practice Exam II (Ch. 14, 15 & 16) Multiple Choices: Please select one best answer. Answer shown in bold.
CHEM 1412 Zumdahl & Zumdahl Practice Exam II (Ch. 14, 15 & 16) Multiple Choices: Please select one best answer. Answer shown in bold. 1. Consider the equilibrium: PO -3 4 (aq) + H 2 O (l) HPO 2-4 (aq)
More informationExam 2 Sections Covered: 14.6, 14.8, 14.9, 14.10, 14.11, Useful Info to be provided on exam: K K [A ] [HA] [A ] [B] [BH ] [H ]=
Chem 101B Study Questions Name: Chapters 14,15,16 Review Tuesday 3/21/2017 Due on Exam Thursday 3/23/2017 (Exam 3 Date) This is a homework assignment. Please show your work for full credit. If you do work
More informationExam 2 Practice (Chapter 15-17)
Exam 2 Practice (Chapter 15-17) 28. The equilibrium constant Kp for reaction (1) has a value of 0.112. What is the value of the equilibrium constant for reaction (2)? (1) SO2 (g) + 1/2 O2(g) SO3 (g) Kp
More informationChapter 17. Additional Aspects of Equilibrium
Chapter 17. Additional Aspects of Equilibrium 17.1 The Common Ion Effect The dissociation of a weak electrolyte is decreased by the addition of a strong electrolyte that has an ion in common with the weak
More informationREVIEW QUESTIONS Chapter 17
Chemistry 102 REVIEW QUESTIONS Chapter 17 1. A buffer is prepared by adding 20.0 g of acetic acid (HC 2 H 3 O 2 ) and 20.0 g of sodium acetate (NaC 2 H 3 O 2 ) in enough water to prepare 2.00 L of solution.
More informationNorthern Arizona University Exam #3. Section 2, Spring 2006 April 21, 2006
Northern Arizona University Exam #3 CHM 152, General Chemistry II Dr. Brandon Cruickshank Section 2, Spring 2006 April 21, 2006 Name ID # INSTRUCTIONS: Code the answers to the True-False and Multiple-Choice
More informationCHM 152/154 HOUR EXAM II Diebolt Summer multiple choice 52 Parts II and III 73 Total Pts 125
CHM 152/154 HOUR EXAM II Diebolt Summer 2010 pts earned name pts possible multiple choice 52 Parts II and III 73 Total Pts 125 Part One: Multiple choice. Mark the correct answers on the provided scantron
More informationNorthern Arizona University Exam #3. Section 2, Spring 2006 April 21, 2006
Northern Arizona University Exam #3 CHM 152, General Chemistry II Dr. Brandon Cruickshank Section 2, Spring 2006 April 21, 2006 Name ID # INSTRUCTIONS: Code the answers to the True-False and Multiple-Choice
More informationChem 103 Exam #1. Identify the letter of the choice that best completes the statement or answers the question. Multiple Choice
Chem 103 Exam #1 Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. Which of the following can act as a Bronsted-Lowry base, but not as a Bronsted-Lowry
More informationFORMULA SHEET (tear off)
FORMULA SHEET (tear off) N A = 6.022 x 10 23 C = ( 5 / 9) ( F - 32) F = ( 9 / 5)( C) + 32 1 amu = 1.661 x 10-27 kg C = K - 273.15 K = C + 273.15 1 atm = 760 torr = 760 mm Hg 1 atm = 1.013 bar pv = nrt
More informationCh 16 and 17 Practice Problems
Ch 16 and 17 Practice Problems 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 informationPERIODIC TABLE OF THE ELEMENTS
Chem 114 Exam 3 April 4, 2016 Name: PLEASE print your name on the exam and sign the academic integrity pledge. Print your name and fill in the circles with your I.D. # on side 1 (blue) of the scantron.
More informationCHEM 121b Exam 4 Spring 1999
Name SSN CHEM 121b Exam 4 Spring 1999 This exam consists of 10 multiple choice questions (each worth 2 points), and 6 written problems (points noted below). There are a total of 100 possible points. Carefully
More informationCHEM Dr. Babb s Sections Exam #3 Review Sheet
CHEM 116 Dr. Babb s Sections Exam #3 Review Sheet Acid/Base Theories and Conjugate AcidBase Pairs 111. Define the following terms: Arrhenius acid, Arrhenius base, Lewis acid, Lewis base, BronstedLowry
More informationHonors Unit 4 Homework Packet
1 Honors Homework Packet Reactions in Aqueous Solutions Part I: Aqueous Solns. Part II: Acid/Base Chemistry Part III: Redox Reactions Name: 2 Molarity of Solutions (pg. 2 & 3) Directions: Solve each of
More informationCHE 107 Spring 2017 Exam 3
CHE 107 Spring 2017 Exam 3 Your Name: Your ID: Question #: 1 What is the ph of a 0.20 M solution of hydrocyanic acid at 25ºC? The Ka of HCN at 25ºC is 4.9 10 10. A. 2.08 B. 5.00 C. 3.89 D. 8.76 Question
More informationCHAPTER 7.0: IONIC EQUILIBRIA
Acids and Bases 1 CHAPTER 7.0: IONIC EQUILIBRIA 7.1: Acids and bases Learning outcomes: At the end of this lesson, students should be able to: Define acid and base according to Arrhenius, Bronsted- Lowry
More informationPractice test Chapters 15 and 16: Acids and Bases
Name: Class: Date: Practice test Chapters 15 and 16: Acids and Bases 1. Which of the following pairs of species is not a conjugate acid base pair? A) HOCl, OCl B) HNO 2, NO + 2 C) O 2, OH D) HSO 4, SO
More informationChapter 17. Additional Aspects of Equilibrium
Chapter 17. Additional Aspects of Equilibrium 17.1 The Common Ion Effect The dissociation of a weak electrolyte is decreased by the addition of a strong electrolyte that has an ion in common with the weak
More informationACID BASE TEST (2 nd half of class) Acid-base titration lab 2 nd half. Chapter 18 Acids and Bases Campbell Chemistry Name
Date In Class 3/31 Thurs. Equilibrium Test Homework (to be done that night, or before coming to the next class) Watch Acid Base Video 1. What are Acids and Bases? 4/1 Fri Video 1 discussion: Identifying
More informationChem. 1A Final. Name. Student Number
Chem. 1A Final Name Student Number All work must be shown on the exam for partial credit. Points will be taken off for incorrect or no units. Calculators are allowed. Cell phones may not be used for calculators.
More informationAcid/Base Definitions
Acids and Bases Acid/Base Definitions Arrhenius Model Acids produce hydrogen ions in aqueous solutions Bases produce hydroxide ions in aqueous solutions Bronsted-Lowry Model Acids are proton donors Bases
More informationPlease take a seat in Row Seat according to the following map
ABCDEG Name Practice Chem 105X Fall 2009 Keller Hour Exam 2 Chap 3 &4 Kotz Please take a seat in Row_ Seat_ according to the following map Please: Keep this booklet closed until instructed to open it.
More informationWeak acids are only partially ionized in aqueous solution: mixture of ions and un-ionized acid in solution.
16.6 Weak Acids Weak acids are only partially ionized in aqueous solution: mixture of ions and un-ionized acid in solution. Therefore, weak acids are in equilibrium: HA(aq) + H 2 O(l) H 3 O + (aq) + A
More informationCHEMISTRY 102 Fall 2010 Hour Exam III Page My answers for this Chemistry 102 exam should be graded with the answer sheet associated with:
Hour Exam III Page 1 1. My answers for this Chemistry 102 exam should be graded with the answer sheet associated with: a) Form A b) Form B c) Form C d) Form D e) Form E Consider the titration of 30.0 ml
More informationis considered acid 1, identify the other three terms as acid 2, base 1, and base 2 to indicate the conjugate acid-base pairs.
18.1 Introduction to Acids and Bases 1. Name the following compounds as acids: a. H2SO4 d. HClO4 b. H2SO3 e. HCN c. H2S 2. Which (if any) of the acids mentioned in item 1 are binary acids? 3. Write formulas
More informationCalorimetry, Heat and ΔH Problems
Calorimetry, Heat and ΔH Problems 1. Calculate the quantity of heat involved when a 70.0g sample of calcium is heated from 22.98 C to 86.72 C. c Ca= 0.653 J/g C q = 2.91 kj 2. Determine the temperature
More informationIonic Equilibria. weak acids and bases. salts of weak acids and bases. buffer solutions. solubility of slightly soluble salts
Ionic Equilibria weak acids and bases salts of weak acids and bases buffer solutions solubility of slightly soluble salts Arrhenius Definitions produce H + ions in the solution strong acids ionize completely
More informationCHEMISTRY - BROWN 13E CH.16 - ACID-BASE EQUILIBRIA - PART 2.
!! www.clutchprep.com CONCEPT: ph and poh To deal with incredibly small concentration values of [H + ] and [OH - ] we can use the ph scale. Under normal conditions, the ph scale operates within the range
More informationDougherty Valley High School AP Chemistry Chapters 14 and 15 Test - Acid-Base Equilibria
Dougherty Valley High School AP Chemistry Chapters 14 and 15 Test - Acid-Base Equilibria This is a PRACTICE TEST. Complete ALL questions. Answers will be provided so that you may check your work. I strongly
More informationChem Chapter 18: Sect 1-3 Common Ion Effect; Buffers ; Acid-Base Titrations Sect 4-5 Ionic solubility Sect 6-7 Complex Formation
Chem 106 3--011 Chapter 18: Sect 1-3 Common Ion Effect; Buffers ; Acid-Base Titrations Sect 4-5 Ionic solubility Sect 6-7 Complex Formation 3//011 1 The net ionic equation for the reaction of KOH(aq) and
More informationAP Chemistry: Acid-Base Chemistry Practice Problems
Name AP Chemistry: Acid-Base Chemistry Practice Problems Date Due Directions: Write your answers to the following questions in the space provided. For problem solving, show all of your work. Make sure
More informationCHEMISTRY - CLUTCH CH.15 - ACID AND BASE EQUILIBRIUM.
!! www.clutchprep.com CONCEPT: ACID IDENTIFICATION The most common feature of an acid is that many possess an H + ion called the. When it comes to acids there are 2 MAJOR TYPES that exist: are acids where
More informationAcids and Bases Written Response
Acids and Bases Written Response January 1999 4. Consider the salt sodium oxalate, Na2C2O4. a) Write the dissociation equation for sodium oxalate. (1 mark) b) A 1.0M solution of sodium oxalate turns pink
More informationSolutions are aqueous and the temperature is 25 C unless stated otherwise.
Solutions are aqueous and the temperature is 25 C unless stated otherwise. 1. According to the Arrhenius definition, an acid is a substance that produces ions in aqueous solution. A. H C. OH B. H + D.
More informationChemistry Lab Equilibrium Practice Test
Chemistry Lab Equilibrium Practice Test Basic Concepts of Equilibrium and Le Chatelier s Principle 1. Which statement is correct about a system at equilibrium? (A) The forward and reverse reactions occur
More information= ) = )
Basics of calculating ph 1. Find the ph of 0.07 M HCl. 2. Find the ph of 0.2 M propanoic acid (K a = 10-4.87 ) 3. Find the ph of 0.4 M (CH 3 ) 3 N (K b = 10-4.20 ) 4. Find the ph of 0.3 M CH 3 COO - Na
More information2. 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 informationFORMULA SHEET (tear off)
FORMULA SHEET (tear off) N A = 6.022 x 10 23 C = ( 5 / 9) ( F - 32) F = ( 9 / 5)( C) + 32 1 amu = 1.661 x 10-27 kg C = K - 273.15 K = C + 273.15 1 atm = 760 torr = 760 mm Hg 1 atm = 1.013 bar pv = nrt
More informationJudith Herzfeld 1996,1998. These exercises are provided here for classroom and study use only. All other uses are copyright protected.
Judith Herzfeld 1996,1998 These exercises are provided here for classroom and study use only. All other uses are copyright protected. 3.3-010 According to Bronsted-Lowry Theory, which of the following
More informationSolubility & Net Ionic review
Solubility & Net Ionic review Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Which of the following statements is/are correct? 1. All ionic compounds
More informationCH 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 informationPart 01 - Assignment: Introduction to Acids &Bases
Part 01 - Assignment: Introduction to Acids &Bases Classify the following acids are monoprotic, diprotic, or triprotic by writing M, D, or T, respectively. 1. HCl 2. HClO4 3. H3As 4. H2SO4 5. H2S 6. H3PO4
More informationProblems -- Chapter Write balanced chemical equations for the important equilibrium that is occurring in an aqueous solution of the following.
Problems -- Chapter 1 1. Write balanced chemical equations for the important equilibrium that is occurring in an aqueous solution of the following. (a) NaNO and HNO answers: see end of problem set (b)
More informationFind this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site.
Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site. Still having trouble understanding the material? Check
More informationFORMULA SHEET (tear off)
FORMULA SHEET (tear off) N A = 6.022 x 10 23 C = ( 5 / 9) ( F - 32) F = ( 9 / 5)( C) + 32 1 amu = 1.661 x 10-27 kg C = K - 273.15 K = C + 273.15 1 atm = 760 torr = 760 mm Hg 1 atm = 1.013 bar pv = nrt
More information5. What is the percent ionization of a 1.4 M HC 2 H 3 O 2 solution (K a = ) at 25 C? A) 0.50% B) 0.36% C) 0.30% D) 0.18% E) 2.
Name: Date: 1. For which of the following equilibria does K c correspond to an acid-ionization constant, K a? A) NH 3 (aq) + H 3 O + (aq) NH 4 + (aq) + H 2 O(l) B) NH 4 + (aq) + H 2 O(l) NH 3 (aq) + H
More informationCHEMICAL EQUILIBRIUM. Cato Maximilian Guldberg and his brother-in-law Peter Waage developed the Law of Mass Action
CHEMICAL EQUILIBRIUM Cato Maximilian Guldberg and his brother-in-law Peter Waage developed the Law of Mass Action Chemical Equilibrium Reversible Reactions: A chemical reaction in which the products can
More informationMore About Chemical Equilibria
1 More About Chemical Equilibria Acid-Base & Precipitation Reactions Chapter 15 & 16 1 Objectives Chapter 15 Define the Common Ion Effect (15.1) Define buffer and show how a buffer controls ph of a solution
More informationCreate assignment, 48975, Exam 2, Apr 05 at 9:07 am 1
Create assignment, 48975, Exam 2, Apr 05 at 9:07 am 1 This print-out should have 30 questions. Multiple-choice questions may continue on the next column or page find all choices before making your selection.
More informationFind this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site.
Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site. Still having trouble understanding the material? Check
More informationBCIT Winter Chem Exam #2
BCIT Winter 2017 Chem 0012 Exam #2 Name: Attempt all questions in this exam. Read each question carefully and give a complete answer in the space provided. Part marks given for wrong answers with partially
More informationDouble Displacement (Exchange or Metathesis) Reactions Practicum
Double Displacement (Exchange or Metathesis) Reactions Practicum Part I: Instructions: Write the molecular, complete ionic and net ionic equations for every one of the following reactions. If a reaction
More informationName Date Class ACID-BASE THEORIES
19.1 ACID-BASE THEORIES Section Review Objectives Define the properties of acids and bases Compare and contrast acids and bases as defined by the theories of Arrhenius, Brønsted-Lowry, and Lewis Vocabulary
More informationHA(aq) H + (aq) + A (aq) We can write an equilibrium constant expression for this dissociation: [ ][ ]
16.6 Weak Acids Weak acids are only partially ionized in aqueous solution. There is a mixture of ions and un-ionized acid in solution. Therefore, weak acids are in equilibrium: Or: HA(aq) + H 2 O(l) H
More informationCh 8 Practice Problems
Ch 8 Practice Problems 1. What combination of substances will give a buffered solution that has a ph of 5.05? Assume each pair of substances is dissolved in 5.0 L of water. (K a for NH 4 = 5.6 10 10 ;
More informationAP Study Questions
ID: A AP 16.4-16.7 Study Questions Multiple Choice Identify the choice that best completes the statement or answers the question. 1 What is the ph of an aqueous solution at 25.0 C in which [H + ] is 0.0025
More informationAP Chemistry. CHAPTER 17- Buffers and Ksp 17.1 The Common Ion Effect Buffered Solutions. Composition and Action of Buffered Solutions
AP Chemistry CHAPTER 17- Buffers and Ksp 17.1 The Common Ion Effect The dissociation of a weak electrolyte is decreased by the addition of a strong electrolyte that has an ion in common with the weak electrolyte.
More informationEXAM 2 PRACTICE KEY. Leaders: Deborah Course: CHEM 178
Leaders: Deborah Course: CHEM 178 EXAM 2 PRACTICE KEY Instructor: Bonaccorsi/Vela Date: 3/6/18 Make sure you (also) know: Acid-base definitions Arrhenius Bronsted-Lowry Lewis Autoionization process of
More informationChapter 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 information7/16/2012. 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 informationCHEM 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 informationA) Arrhenius Acids produce H+ and bases produce OH not always used because it only IDs X OH as basic species
3 ACID AND BASE THEORIES: A) Arrhenius Acids produce H+ and bases produce OH not always used because it only IDs X OH as basic species B) Bronsted and Lowry Acid = H + donor > CB = formed after H + dissociates
More informationCHEMISTRY - BROWN 14E CH.16 - ACID-BASE EQUILIBRIA.
!! www.clutchprep.com CONCEPT: ACID IDENTIFICATION The most common feature of an acid is that many possess an H + ion called the. When it comes to acids there are 2 MAJOR TYPES that exist: are acids where
More informationCHE 107 Fall 2016 Exam 3
CHE 107 Fall 2016 Exam 3 Your Name: Your ID: Question #: 1 [H3O + ] in a typical solution of hand soap is 3.2 10 10 M. The ph of this solution is 1. Report your answer with two decimal places. Do NOT include
More informationChemistry 102 Chapter 17 COMMON ION EFFECT
COMMON ION EFFECT Common ion effect is the shift in equilibrium caused by the addition of an ion that takes part in the equilibrium. For example, consider the effect of adding HCl to a solution of acetic
More informationACIDS, BASES, AND SALTS
ACIDS, BASES, AND SALTS Chapter Quiz Choose the best answer and write its letter on the line. 1. A solution in which the hydroxide-ion concentration is 1 10 2 is a. acidic. c. neutral. b. basic. d. none
More informationHonors General Chemistry Test 3 Prof. Shattuck, practice
Honors General Chemistry Test 3 Prof. Shattuck, practice Name R = 8.314 J mol -1 K -1 1 L atm = 101.3 J T(0 C) = 273.2 K Answer 8 of the following 10 questions. If you answer more than 8 cross out the
More informationChapter 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.
More informationGuide to Chapter 15. Aqueous Equilibria: Acids and Bases. Review Chapter 4, Section 2 on how ionic substances dissociate in water.
Guide to Chapter 15. Aqueous Equilibria: Acids and Bases We will spend five lecture days on this chapter. During the first two class meetings we will introduce acids and bases and some of the theories
More informationCHEMICAL REACTIONS. There are three ways we write chemical equations. 1. Molecular Equations 2. Full Ionic Equations 3. Net Ionic Equations
CHEMICAL REACTIONS Reactants: Zn + I 2 Product: Zn I 2 Unit 2 Chemical Reactions The unit 2 exam will cover material from multiple chapters. You are responsible for the following from your text on exam
More informationAcid-Base Equilibria and Solubility Equilibria
Acid-Base Equilibria and Solubility Equilibria Acid-Base Equilibria and Solubility Equilibria Homogeneous versus Heterogeneous Solution Equilibria (17.1) Buffer Solutions (17.2) A Closer Look at Acid-Base
More informationHomework #7 Chapter 8 Applications of Aqueous Equilibrium
Homework #7 Chapter 8 Applications of Aqueous Equilibrium 15. solution: A solution that resists change in ph when a small amount of acid or base is added. solutions contain a weak acid and its conjugate
More informationLecture 10. Professor Hicks Inorganic Chemistry II (CHE152) Scale of [H 3 O + ] (or you could say [H + ]) concentration
Lecture 10 Professor Hicks Inorganic Chemistry II (CHE152) ph Scale of [H 3 O + ] (or you could say [H + ]) concentration More convenient than scientific notation ph = log [H 3 O + ] still not sure? take
More informationCH 15 Summary. Equilibrium is a balance between products and reactants
CH 15 Summary Equilibrium is a balance between products and reactants Use stoichiometry to determine reactant or product ratios, but NOT reactant to product ratios. Capital K is used to represent the equilibrium
More informationExample 15.1 Identifying Brønsted Lowry Acids and Bases and Their Conjugates
Example 15.1 Identifying Brønsted Lowry Acids and Bases and Their Conjugates For Practice 15.1 In each reaction, identify the Brønsted Lowry acid, the Brønsted Lowry base, the conjugate acid, and the conjugate
More informationChapter 14. Acids and Bases
Chapter 14 Acids and Bases Section 14.1 The Nature of Acids and Bases Models of Acids and Bases Arrhenius: Acids produce H + ions in solution, bases produce OH - ions. Brønsted Lowry: Acids are proton
More informationCHE 107 Summer 2017 Exam 3
CHE 107 Summer 2017 Exam 3 Question #: 1 What is the ph of a 0.10 M hydrocyanic acid (HCN) solution. Ka = 4.9 10-10. A. 2.56 C. 4.04 B. 3.17 D. 5.15 Question #: 2 Original Windex has a ph = 11.60 and [H
More information1032_2nd Exam_ (A)
1032_2nd Exam_1040422 (A) MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Give the equation for a saturated solution in comparing Q with Ksp. A)
More informationAcids, Bases and Buffers
1 Acids, Bases and Buffers Strong vs weak acids and bases Equilibrium as it relates to acids and bases ph scale: [H+(aq)] to ph, poh, etc ph of weak acids ph of strong acids Conceptual about oxides (for
More informationAqueous Equilibria: Acids and Bases
Slide 1 Chapter 14 Aqueous Equilibria: Acids and Bases Slide 2 Acid Base Concepts 01 Arrhenius Acid: A substance which dissociates to form hydrogen ions (H + ) in solution. HA(aq) H + (aq) + A (aq) Arrhenius
More informationFind this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site.
Find this material useful? You can help our team to keep this site up and bring you even more content consider donating via the link on our site. Still having trouble understanding the material? Check
More information(Label the Conjugate Pairs) Water in the last example acted as a Bronsted-Lowry base, and here it is acting as an acid. or
Chapter 16 - Acid-Base Equilibria Arrhenius Definition produce hydrogen ions in aqueous solution. produce hydroxide ions when dissolved in water. Limits to aqueous solutions. Only one kind of base. NH
More informationSCHOOL 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 informationUnit 2 Acids and Bases
Unit 2 Acids and Bases 1 Topics Properties / Operational Definitions Acid-Base Theories ph & poh calculations Equilibria (Kw, K a, K b ) Indicators Titrations STSE: Acids Around Us 2 Operational Definitions
More informationChapter 16. Acid-Base Equilibria
Chapter 16. Acid-Base Equilibria 16.1 Acids and Bases: A Brief Review Acids taste sour and cause certain dyes to change color. Bases taste bitter and feel soapy. Arrhenius concept of acids and bases: An
More information7. A solution has the following concentrations: [Cl - ] = 1.5 x 10-1 M [Br - ] = 5.0 x 10-4 M
Solubility, Ksp Worksheet 1 1. How many milliliters of 0.20 M AlCl 3 solution would be necessary to precipitate all of the Ag + from 45ml of a 0.20 M AgNO 3 solution? AlCl 3(aq) + 3AgNO 3(aq) Al(NO 3)
More informationCHM 112 Dr. Kevin Moore
CHM 112 Dr. Kevin Moore Reaction of an acid with a known concentration of base to determine the exact amount of the acid Requires that the equilibrium of the reaction be significantly to the right Determination
More informationCHAPTER 4 TYPES OF CHEMICAL REACTIONS & SOLUTION STOICHIOMETRY
Advanced Chemistry Name Hour Advanced Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 4 TYPES OF CHEMICAL REACTIONS & SOLUTION STOICHIOMETRY Day Plans
More informationChem 1412 Exam The substance HOBr is considered
Chem 1412 Exam 3 Student: 1. The substance HOBr is considered A.a weak Arrhenius acid. B.a weak Arrhenius base. C.a strong Arrhenius acid. D.a strong Arrhenius base. E.a neutral compound. 2. Which one
More information