Chemistry 116: Exam 3 March 25, 2014
|
|
- Berniece Goodman
- 5 years ago
- Views:
Transcription
1 March 5, Each of the following pairs contains one strong acid and one weak acid except a. HNO3 and HCO3 b. HF and HNO c. HSO4 and HS d. HCH3O and HCl e. HBr and H3PO4. Given that KB of CH3NH is at 5 o C, what is the equilibrium constant for the reaction a b c d e CH3NH3 + + HO(l) CH3NH(aq) + H3O + (aq) 3. Given the net ionic equation HO(l) + CO3 (aq) HCO3 (aq) + OH (aq) a. HO is an acid and OH is its conjugate acid b. HO is an acid and OH is its conjugate base c. CO3 is a Bronsted-Lowry acid because it is a proton acceptor d. HO is a Lewis acid because it is a proton donor e. HO is a Lewis base because it is an electron pair donor 4. The reaction of carbon monoxide and diiodine pentoxide is endothermic. The yield could be increased by 5 CO(g) + IO5(g) I(g) + 5 CO(g) a. Increasing the pressure by decreasing volume b. Decreasing the temperature c. Increasing the temperature d. Both a and b e. Both a and c 5. The ionization constant of water at 60 o C is What is the ph of pure water at this temperature? a b c d e Page 1 of 5
2 March 5, Consider the reaction of the shown below at a given temperature. When the system is at equilibrium, the molar concentrations of Br, Cl, and BrCl are M, M, and M, respectively. What is the value of Kc for this system? a. 0.5 b. 3.9 c. 7 d. 53 e. 60. Br(g) + Cl(g) BrCl(g) 7. The reaction mixture of CO and O at a given temperature is given below. When equilibrium is established, which of the following ratios is constant regardless of the initial concentrations of CO and O? CO(g) + O(g) CO (g) a. [ O b. [ O c. [ O d. [ O e. 1 [ O 8. Consider the reaction shown below. At a certain temperature Kc equals What will happen if mole of HS, 1.0 mole of H, and 1.5 mole of S(g) are added to a.0 L container HS(g) H(g) + S(g) a. Nothing, the system is at equilibrium b. More HS will be formed c. H will be formed 9. At a given temperature, mole NO, mole Cl and 0.50 mole of ClNO were placed in a 10.0 liter container and allowed to come to equilibrium. At equilibrium moles of ClNO are present. What is the value of the equilibrium constant, Kc? a b c d e ClNO(g) NO(g) + Cl(g) Page of 5
3 March 5, The KB of piperidine (an organic base) is What is the ph of a M solution of piperidine? [Be careful a..67 b..80 c d e Calculate the ph of a 0.017M solution of Ba(OH) a b c d e Which of the following mixtures is suitable for making buffers? I. CH3COOH and NaCH3COO II. HF and NaF III. NH4Cl and NH3 d. I and III only e. I, II, and III 13. Carbon disulfide and chlorine react according to the equation given below. When 1.00 mole of CS and 3.00 mole of Cl are placed in a.00 liter container and allowed to come to equilibrium, the mixture is found to contain 0.50 mole of CCl4. What is the amount of Cl at equilibrium? a..5 mole b..75 mole c mole d. 0.5 mole e mole CS(g) + 3 Cl(g) SCl(g) + CCl4(g) Page 3 of 5
4 March 5, A state of dynamic equilibrium exists at constant temperature for I. A stoppered flask half full of water II. An open pan of boiling water III. A stoppered flask of saturated sodium carbonate solution d. I and II only e. I and III only 15. For the reaction NO(g) + ½ O(g) NO(g) at 750 o C, the equilibrium constant Kc equals a. Kp (RT) 3/ b. Kp (RT) 3/ c. Kp (RT) /3 d. Kp (RT) 1/ e. Kp (RT) 1/ 16. What is the ph of a 0.5M solution of hypobromous acid (HOBr, KA= ) a b c. 3.5 d e All of the following are acid-base conjugate pairs except a. CH3NH, CH3NH3 + b. HCO3, HCO3 c. HNO, NO + d. HOCl, OCl e. HSO4, HSO4 18. A 0.10 M aqueous solution of an acid HA has a ph of What is the value of KA for this acid? a b c d e Page 4 of 5
5 March 5, The equilibrium constant, KC, for the reaction below is 7.4 at 45 o C. The numerical value of value of the equilibrium constant will be changed if ½ H(g) + ½ I(g) HI(g) KC= 7.4 I. The volume of the container is changed II. The temperature is doubled to 500 o C III. The amounts of reactants are doubled d. I and II only e. II and III only 0. For which of the following is the reaction yield the smallest when equilibrium is reached. a. Kc = b. Kc = c. Kc = d. Kc = e. Kc = Bonus: What is the net ionic reaction that occurs when hydrochloric acid is added to the NaHCOO/ HCOOH buffer? a. H + (aq) + HO(l) H3O + (aq) b. H + (aq) + OH (aq) HO(l) c. H + (aq) + HCOO (aq) HCOOH(aq) d. HCl(aq) OH (aq) HO(l) + Cl (aq) e. HCOOH H + (aq) + HCOO (aq) Key 1. B. A 3. B 4. C 5. B 6. B 7. D 8. B 9. D 10. D 11. E 1. E 13. A 14. E 15. D 16. D 17. C 18. B 19. B 0. D 1. C Page 5 of 5
CH3NH2(aq) + H3O + (aq) 3. The reaction of carbon monoxide and diiodine pentoxide is endothermic. The yield could be increased by
1. What is the ph of a 0.020 M HClO4 solution? a. 0.040 b. 1.70 c. 12.30 d. 0.020 Chemistry 116: Exam 2 2. Given that KB of CH3NH2 is 4.2 10 4 at 25 o C, what is the equilibrium constant for the reaction
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 information2. What mass of an aqueous 22.9% sodium chloride solution contains 99.5 g of water?
CHEM 1412 MIDTERM EXAM (100 pts total) ANSWER KEY Student s Name PART A (20 multiple choice questions, 3 pts each): 1. The solubility of a gas in a liquid can always be increased by: a) decreasing the
More informationChem1120pretest2Summeri2015
Name: Class: Date: Chem1120pretest2Summeri2015 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. When the system A + B C + D is at equilibrium, a. the forward
More informationHonors Chemistry Study Guide for Acids and Bases. NH4 + (aq) + H2O(l) H3O + (aq) + NH3(aq) water. a)hno3. b) NH3
Honors Chemistry Study Guide for Acids and Bases 1. Calculate the ph, poh, and [H3O + ] for a solution that has a [OH - ] = 4.5 x 10-5? 2. An aqueous solution has a ph of 8.85. What are the [H + ], [OH
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 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 informationMULTIPLE 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) Which one of the following is the weakest acid? 1) A) HF (Ka = 6.8 10-4) B) HNO2 (Ka
More informationChem1120pretest2Summeri2015
Chem1120pretest2Summeri2015 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. When the system A + B C + D is at equilibrium, a. the forward reaction has
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 informationChemistry 400 Homework #3, Chapter 16: Acid-Base Equilibria
Chemistry 400 Homework #3, Chapter 16: Acid-Base Equilibria I. Multiple Choice (for those with an asterisk, you must show work) These multiple choice (MC) are not "Google-proof", but they were so good
More informationDownloaded from
IMPORTANT POINTS (EQUILLIBRIUM) IMPORTANT QUESTIONS CHAPTER EQUILIBRIUM 1. Equilibrium constant helps in predicting the direction in which a given reaction will proceed at any stage. a) In which one of
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 informationChp 13, 14, 15 SHOW ALL WORK AND CIRCLE FINAL ANSWERS. a) 1 only b) 2 only c) 3 only d) 1 and 2 only e) 1, 2, and H 2
Chp 13, 14, 15 Name: SHOW ALL WORK AND CIRCLE FINAL ANSWERS 1. Which of the following factors affect the initial rate of a reaction? 1) The nature of the reactants. 2) The concentration of the reactants.
More informationDynamic equilibrium: rate of evaporation = rate of condensation II. In a closed system a solid obtains a dynamic equilibrium with its dissolved state
CHEMISTRY 111 LECTURE EXAM III Material PART 1 CHEMICAL EQUILIBRIUM Chapter 14 I Dynamic Equilibrium I. In a closed system a liquid obtains a dynamic equilibrium with its vapor state Dynamic equilibrium:
More informationUnit 9: Acid and Base Multiple Choice Practice
Unit 9: Acid and Base Multiple Choice Practice Name June 14, 2017 1. Consider the following acidbase equilibrium: HCO3 H2O H2CO3 OH In the reaction above, the BrönstedLowry acids are: A. H2O and OH B.
More information*In every acid-base reaction, equilibrium favors transfer of a proton from the stronger acid to the stronger base.
16.2 Bronsted-Lowry Acids and Bases An acid is a substance that can transfer a proton to another substance. A base is a substance that can accept a proton. A proton is a hydrogen ion, H +. Proton transfer
More informationWhat does the magnitude of the equilibrium constant tell us? N2(g) + O2(g) N2 O2(g) N2(g) + 3H2(g) 2NH3(g) In Short
What does the magnitude of the equilibrium constant tell us? N2(g) + O2(g) N2 O2(g) N2(g) + 3H2(g) 2NH3(g) In Short 1 D. Altering Chemical Equations and the Effect on the Equilibrium Constant What is the
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 informationChemical Equilibrium
Chemical Equilibrium Ch 17 Apr 28 7:40 AM A Reversible reaction is a chemical reaction that can occur in both the forward and the reverse directions N 2 (g) + 3 H 2 (g) 2NH3(g) Apr 16 1:21 PM 1 Equilibrium
More information1002_1st Exam_
1002_1st Exam_1010321 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Consider the following reaction: POCl3(g) POCl(g) + Cl2(g) Kc = 0.450 A sample
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 informationChemistry 40S Acid-Base Equilibrium (This unit has been adapted from
Chemistry 40S Acid-Base Equilibrium (This unit has been adapted from https://bblearn.merlin.mb.ca) Name: 1 Lesson 1: Defining Acids and Bases Goals: Outline the historical development of acid base theories.
More informationMERIDIAN Academy OF SCIENCE REVISION SHEET Sub : CHEMISTRY CHEMICAL & IONIC EQUILIBRIUM Batch : 11 TH GSEB
Chemical Equilibrium - LEVEL I- Part - I 1. Concentration of reactant & product does not become equal but constant at constant temperature is equilibrium state. Justify the statement. 2. Define reversible
More informationChem1120pretest2Summeri2016
Chem1120pretest2Summeri2016 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. When the system A + B C + D is at equilibrium, a. the forward reaction has
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 informationSUPeR Chemistry CH 223 Practice Exam
SUPeR Chemistry CH 223 Practice Exam This exam has been designed to help you practice working multiple choice problems over the topics presented in CH 223. The actual exams for each section of CH 223 will
More informationCHM 112 Chapter 13 Extra Credit : Chemical Equilibrium Name:
CHM 112 Chapter 13 Extra Credit : Chemical Equilibrium Name: 1. Write the equilibrium expression for following reactions. In each case indicate whether the equilibrium is Homogeneous or Heterogeneous 2
More informationGeneral Chemistry II CHM 1046 E Exam 2
General Chemistry II CHM 1046 E Exam 2 Dr. Shanbhag Name: 1. The formation of ammonia from elemental nitrogen and hydrogen is an exothermic process. N 2 (g) + 3 H 2 (g) 2 NH 3 (g) H= -92.2 kj Which of
More information6. Which expression correctly describes the equilibrium constant for the following reaction? 4NH 3 (g) + 5O 2 (g) 4NO(g) + 6H 2 O(g)
1. Which of the following can we predict from an equilibrium constant for a reaction? 1. The extent of a reaction 2. Whether the reaction is fast or slow 3. Whether a reaction is exothermic or endothermic
More informationK P VERSUS K C PROPERTIES OF THE EQUILIBRIUM CONSTANT
K P VERSUS K C 1. What are the units of K p and K c for each of the following? a) 2H 2 S(g) 2H 2 (g) + S 2 (g) b) 4NH 3 (g) + 3O 2 (g) 2N 2 (g) + 6H 2 O(g) 2. What are the units of K p and K c for each
More information3. The osmotic pressure of a ml solution of an unknown nonelectrolyte is 122 torr at 25 C. Determine the molarity of the solution.
1. Which of the following has a correct van t Hoff factor indicated? A. Al 2 (SO 4 ) 3, i = 5 C. CaBr 2, i = 2 B. Na 2 CO 3, i = 6 D. C 6 H 12 O 6, i = 3 2. Calculate the vapor pressure of a solution containing
More informationAll answers are to be done on test paper. If more room is needed use the back side of the paper and indicate.
1 Chem 1105-Final Exam Date: August 10, 2016 Instructor: Calvin Howley Time Period: 3 hour Student: Student #: Instructions: Please turn off all cell phones. Only scientific calculators are allowed in
More informationFormation of a salt (ionic compound): Neutralization reaction. molecular. Full ionic. Eliminate spect ions to yield net ionic
Formation of a salt (ionic compound): Neutralization reaction molecular Full ionic Eliminate spect ions to yield net ionic Hydrolysis/ reaction with water Anions of Weak Acids Consider the weak acid HF
More informationCHM 1046 FINAL REVIEW
CHM 1046 FINAL REVIEW Prepared & Presented By: Marian Ayoub PART II Chapter Description 14 Chemical Equilibrium 15 Acids and Bases 16 Acid-Base Equilibrium 17 Solubility and Complex-Ion Equilibrium 19
More informationConjugate Pairs Practice #1
Name: Key Skill: Learning to Draw Tie Lines Conjugate Pairs Practice #1 Look at each example drawn below. Sets of partners (called s) are matched with tie lines. HNO3 + OH - NO3 - + H2O CH3NH2 + H2O CH3NH3
More informationUnit Nine Notes N C U9
Unit Nine Notes N C U9 I. AcidBase Theories A. Arrhenius Acids and Bases 1. Acids contain hydronium ions (H O ) commonly referred to as hydrogen ions (H ) that dissociate in water a. Different acids release
More information5 Acid Base Reactions
Aubrey High School AP Chemistry 5 Acid Base Reactions 1. Consider the formic acid, HCOOH. K a of formic acid = 1.8 10 4 a. Calculate the ph of a 0.20 M solution of formic acid. Name Period Date / / 5.2
More informationWrite equilibrium law expressions from balanced chemical equations for heterogeneous and homogeneous systems. Include: mass action expression.
Equilibrium 1 UNIT 3: EQUILIBRIUM OUTCOMES All important vocabulary is in Italics and bold. Relate the concept of equilibrium to physical and chemical systems. Include: conditions necessary to achieve
More informationAcid-Base Equilibria (Chapter 10.) Problems: 2,3,6,13,16,18,21,30,31,33
Acid-Base Equilibria (Chapter 10.) Problems: 2,3,6,13,16,18,21,30,31,33 Review acid-base theory and titrations. For all titrations, at the equivalence point, the two reactants have completely reacted with
More informationANALYTICAL CHEMISTRY - CLUTCH 1E CH.8 - MONOPROTIC ACID-BASE EQUILIBRIA.
!! www.clutchprep.com CONCEPT: ARRHENIUS ACIDS AND BASES The most general definition for acids and bases was developed by Svante Arrhenius near the end of the 19 th century. According to him, the cation
More informationIndicator Color in acid (ph < 7) Color at ph = 7 Color in base (ph > 7) Phenolphthalein Bromothymol Blue Red Litmus Blue Litmus
Unit 9: Acids and Bases Notes Introduction and Review 1. Define Acid: 2. Name the following acids: HCl H2SO4 H2SO3 H2S 3. Bases usually contain 4. Name the following bases: NaOH Ca(OH)2 Cu(OH)2 NH4OH Properties
More informationAP Chemistry 1st Semester Final Review Name:
AP Chemistry 1st Semester Final Review Name: 2015-2016 1. Which of the following contains only sigma (s) bonds? 5. H2O(g) + CO(g) H2(g) + CO2(g) A) CO2 B) C3H6 C) CH3Cl D) N2O3 E) SiO2 2. What is the equilibrium
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 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 information2017:2 (a) Ammonia, NH3, is a weak base. pka (NH4 + ) = 9.24 Ka (NH4 + ) = (i) Calculate the ph of a mol L 1 NH3 solution.
AS 91392 Demonstrate understanding of equilibrium principles in aqueous systems Collated Buffer Questions 2017:2 (a) Ammonia, NH3, is a weak base. pka (NH4 + ) = 9.24 Ka (NH4 + ) = 5.75 10 10 (i) Calculate
More informationf) Perchloric acid g) Dihydrogen sulfide i) Barium phosphate j) Copper(II) sulfate pentahydrate
1 2 1. For the following provide the correct name or formula. [8] a) Hg2(NO3)2 b) Mg(C2H3O2)2 c) (NH4)2CO3 d) Ca(OH)2 f) Perchloric acid g) Dihydrogen sulfide i) Barium phosphate j) Copper(II) sulfate
More informationQuestions 1 15 cover Exam 1 material
Questions 1 15 cover Exam 1 material 1. Which molecule cannot hydrogen bond to another molecule of itself? A. CH3OH C. CH3CH3 B. CH3NH2 D. HF 2. Concerning surface tension, which of the following is incorrect?
More information1. Consider the following Lewis structure: Which statement about the molecule is false?
CHY 116 Final Exam, Spring 2017 Multiple Choice (68 points): Each question is intended to have one correct answer. Please write this answer on the answer sheet. Each question is worth 1.25 points. 1. Consider
More informationChem 1046 Lecture Notes Chapter 17
Chem 1046 Lecture Notes Chapter 17 Updated 01-Oct-2012 The Chemistry of Acids and Bases These Notes are to SUPPLIMENT the Text, They do NOT Replace reading the Text Book Material. Additional material that
More information2011 AP CHEMISTRY FREE-RESPONSE QUESTIONS (Form B)
2011 AP CHEMISTRY FREE-RESPONSE QUESTIONS (Form B) 5. A student is instructed to prepare 100.0 ml of 1.250 M NaOH from a stock solution of 5.000 M NaOH. The student follows the proper safety guidelines.
More information(B) K2O potassium dioxide
PRACTICE CHEMISTRY EOC TEST 1. Which substance is a conductor of electricity? (A) NaCl(s) (B) NaCl(l) (C) C6H12O6(s) (D) C6H12O6(l) 2. Which formula is correctly paired with its name? (A) MgCl2 magnesium
More informationAdvanced Chemistry Practice Problems
Finding ph 1. Question: Determine the ph for each of the given solutions. a. 0.150 M HNO3 b. 0.150 M CH3COOH, a = 1.8 10-5 c. 0.150 M CHOOH, a = 3.5 10-4 Answer: The method to determine the ph of a solution
More informationI II III IV. Volume HCl added. 1. An equation representing the reaction of a weak acid with water is
1. An equation representing the reaction of a weak acid with water is A. HCl + H 2 O H 3 O + + Cl B. NH 3 + H 2 O NH 4 + + OH C. HCO 3 H 2 O H 2 CO 3 + OH D. HCOOH + H 2 O H 3 O + + HCOO 2. The equilibrium
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 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 informationChem12 Acids : Exam Questions M.C.-100
Chem12 Acids : Exam Questions M.C.-100 1) Given : HPO 4 2- (aq) + NH 4 + (aq) H 2 PO 4 - (aq) + NH 3 (aq), the strongest acid in the above equation is : a) NH 4 + b) HPO 4 2- c) NH 3 d) H 2 PO 4-2)
More informationChapter 15 Chemical Equilibrium
Equilibrium To be in equilibrium is to be in a state of balance: Chapter 15 Chemical Equilibrium - Static Equilibrium (nothing happens; e.g. a tug of war). - Dynamic Equilibrium (lots of things happen,
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 informationX Unit 15 HW Solutions Acids & Bases. Name:
X Unit 15 HW Solutions Acids & Bases Name: Homework #1: Solubility Curve Worksheet Use the solubility chart below to answer the following questions: Graph from U. Va Department of Physics. 1) What is the
More informationAcid-Base Titration Solution Key
Key CH3NH2(aq) H2O(l) CH3NH3 (aq) OH - (aq) Kb = 4.38 x 10-4 In aqueous solution of methylamine at 25 C, the hydroxide ion concentration is 1.50 x 10-3 M. In answering the following, assume that temperature
More informationChapter 16 Acids and Bases. Chapter 16 Acids and Bases
. Chapter 16 Acids and Bases 1 Some Definitions Arrhenius Acid: Substance that, when dissolved in water, increases the concentration of hydrogen ions. Base: Substance that, when dissolved in water, increases
More informationAcids and Bases. A strong base is a substance that completely ionizes in aqueous solutions to give a cation and a hydroxide ion.
Acid-Base Theories Arrhenius Acids and Bases (1884) Acids and Bases An acid is a substance that, when dissolved in water, increases the concentration of hydrogen ions. A base is a substance that, when
More informationExam 2 Sections Covered: (the remaining Ch14 sections will be on Exam 3) Useful Information Provided on Exam 2:
Chem 101B Study Questions Name: Chapters 12,13,14 Review Tuesday 2/28/2017 Due on Exam Thursday 3/2/2017 (Exam 2 Date) This is a homework assignment. Please show your work for full credit. If you do work
More informationUnit 2 Pre-Test Reaction Equilibrium
Unit 2 Pre-Test Reaction Equilibrium Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Consider the following equilibrium system: 2HF(g) F 2(g) + H 2 (g)
More informationCH Practice Exam #2
CH1810 - Practice Exam #2 Part I - Multiple Choice - Choose the best answer and place the letter corresponding to the answer in the space provided. 1. Consider the following reaction and its equilibrium
More informationAS Demonstrate understanding of equilibrium principles in aqueous systems. Collated Buffer Questions
2016: AS 91392 Demonstrate understanding of equilibrium principles in aqueous systems No separate buffer question asked. 2015: 3 Collated Buffer Questions 20.0 ml of 0.258 mol L 1 hydrofluoric acid, HF,
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 information1. Strengths of Acids and Bases 2. K a, K b 3. Ionization of Water 4. Relative Strengths of Brønsted-Lowry Acids and Bases
Chemistry 12 Acid-Base Equilibrium II Name: Date: Block: 1. Strengths of Acids and Bases 2. K a, K b 3. Ionization of Water 4. Relative Strengths of Brønsted-Lowry Acids and Bases Strengths of Acids and
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 information1) What is the Arrhenius definition of an acid? Of a base? 2) What is the Bronsted-Lowry definition of an acid? Of a base?
Problems, Chapter 16 (with solutions) NOTE: Unless otherwise stated, assume T = 25. C in all problems) 1) What is the Arrhenius definition of an acid? Of a base? An Arrhenius acid is a substance that produces
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 informationph = pk a + log 10 {[base]/[acid]}
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 informationFormulas and Possibly Necessary Data
Chemistry Quarter IV Review - Answers Formulas and Possibly Necessary Data Δtf = Kf m Δtb = Kb m m = mol solute / mass solvent(kg) C = n V m = nm - log[h3o + ] = ph - log[oh - ] = poh [H3O + ] = 10 =ph
More informationQuiz name: Equilibria + Acids/Bases
Name: Quiz name: Equilibria + Acids/Bases Date: 1. 2. At 450 C, 2.0 moles each of H 2(g), I 2(g), and HI are combined in a 1.0 L rigid container. The value of K c at 450 C is 50. Which of the following
More information8.1 Explaining the Properties of Acids & Bases. SCH4U - Chemistry, Gr. 12, University Prep
8.1 Explaining the Properties of Acids & Bases SCH4U - Chemistry, Gr. 12, University Prep Equilibrium & Acids & Bases 2 So far, we have looked at equilibrium of general chemical systems: We learned about
More informationAcid Base Review. 2. Identify the acid base conjugate pairs in each of the following reactions according with the Bronsted Lowry framework:
Acid Base Review 1. Identify Lewis Acid, in the following reactions: a. Zn 2 4 H 2 O qwwwwe Zn (H 2 O) 4 2 b. BF 3 F 1 qwwwwe BF 4 1 c. Ag 1 2NH 3 qwwwwe Ag(NH 3 ) 2 1 2. Identify the acid base conjugate
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 informationStation 1 ACIDS, BASES, AND NEUTRALS Classify each statement as talking about an [A]cid, [B]ase, or [N]eutral. feels slippery.
Name Period Date / / Station 1 ACIDS, BASES, AND NEUTRALS Classify each statement as talking about an [A]cid, [B]ase, or [N]eutral. feels slippery CH3OH tastes sour H + donor KOH increases [OH - ] turns
More informationWhat is the correct name and bonding of BF 3? What is the correct name and bonding of BF 3?
What is the correct name and bonding of BF 3? 1. boron trifluoride, covalent compound 2. boron trifluoride, ionic compound 3. boron fluoride, covalent compound 4. boron fluoride, ionic compound What is
More informationCHAPTER-7 EQUILIBRIUM ONE MARK QUESTIONS WITH ANSWERS. CHAPTER WEIGHTAGE: 13
CHAPTER-7 EQUILIBRIUM ONE MARK QUESTIONS WITH ANSWERS. CHAPTER WEIGHTAGE: 13 1.What is a reversible reaction? Ans. The reaction in which both forward and backward reaction takes place simultaneously is
More informationChapter How many grams of a 23.4% by mass NaF solution is needed if you want to have 1.33 moles of NaF?
Chapter 13 1. Which of the following compounds is a strong electrolyte? a. NH 4Cl b. NaCl c. NaC 2H 3O 2 d. HCl e. All of the above 2. A solution that is 13.58% by mass of sugar contains 13.75 grams of
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 informationCHAPTER 11 ACIDS AND BASES
CHAPTER 11 ACIDS AND BASES 11.1 Table 11.5 of the text contains a list of important Brønsted acids and bases. (a) both (why?), (b) base, (c) acid, (d) base, (e) acid, (f) base, (g) base, (h) base, (i)
More informationIB Chemistry ABS Introduction An acid was initially considered a substance that would produce H + ions in water.
IB Chemistry ABS Introduction An acid was initially considered a substance that would produce H + ions in water. The Brønsted-Lowry definition of an acid is a species that can donate an H + ion to any
More informationUnit 4-1 Provincial Practice Questions Page 1
Page 1 Page 2 Page 3 Page 4 Page 5 1.00 Page 6 Page 7 Page 8 55. The conjugate base of HAsO 4 2 is A. H 3 O + B. 3 AsO 4 C. H 3 AsO 4 D. H 2 AsO 4 56. Consider the following acidbase equilibrium: HC 6
More informationChapter #021. What is the poh of a M KOH solution? Student Response a. 2.1 b. 4.8 c. 9.2 d e. None of these choices is correct.
For answers, send email to: admin@tutor-homework.com. Include file name: Chemistry_Worksheet_0052 Price: $3 (c) 2012 www.tutor-homework.com: Tutoring, homework help, help with online classes. 1. 016 Chapter
More informationGENERAL CHEMISTRY II CHEM SYSTEM FINAL EXAM VERSION A Summer 2107
GENERAL CHEMISTRY II CHEM 1412 SYSTEM FINAL EXAM VERSION A Summer 2107 Page1 1 Part I: Multiple Choice (2 points each) 1. The density of 96.0 % H2SO4(aq) is 1.87 g/ml. Calculate the molarity of the solution.
More informationChemistry I Notes Unit 10: Acids and Bases
Chemistry I Notes Unit 10: Acids and Bases Acids 1. Sour taste. 2. Acids change the color of acid- base indicators (turn blue litmus red). 3. Some acids react with active metals and release hydrogen gas,
More informationCH 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 informationChemical Equilibrium
Chemical Equilibrium Concept of Equilibrium Equilibrium Constant Equilibrium expressions Applications of equilibrium constants Le Chatelier s Principle The Concept of Equilibrium The decomposition of N
More informationCHEMISTRY 1220 CHAPTER 16 PRACTICE EXAM
CHEMISTRY 1220 CHAPTER 16 PRACTICE EXAM 1. The ph of a 0.10 M solution of NH3 containing 0.10 M NH 4 Cl is 9.20. What is the [H3O + ]? a) 1.6 x 10-5 b) 1.0 x 10-1 c) 6.3 x 10-10 d) 1.7 x 10-10 e) 2.0 x
More informationMultiple Choice Neatly write your choice in the blank provided. (3 pts each)
Name CH302H EXAM 2 Spring 2013 Multiple Choice Neatly write your choice in the blank provided. (3 pts each) 1. What is the effect of a volume decrease on the reaction: C(s) H2O(g) CO(g) H2(g)? (a) K increases
More informationAnswers to Unit 4 Review Questions
0. NH + 4 (aq) + H O(l) H 3 O + (aq) + NH 3 (aq) unbuffered 0.35 x 0.35 [H K a 3 O + ][NH 3 ] [NH + x(0.35) 5.6 10 10 4 ] 0.35 x 5.6 10 10 ph log 5.6 10 10 9.5 NH + 4 (aq) + H O(l) H 3 O + (aq) + NH 3
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 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 informationDuncan. UNIT 14 - Acids & Bases. COMMON ACIDS NOTES lactic acetic phosphoric NAMING ACIDS NOTES
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) 1. hydro- - HF 2. root of
More informationCHEMICAL EQUILIBRIUM. Chapter 15
Chapter 15 P a g e 1 CHEMICAL EQUILIBRIUM Examples of Dynamic Equilibrium Vapor above a liquid is in equilibrium with the liquid phase. rate of evaporation = rate of condensation Saturated solutions rate
More informationa. rate = k[no] 2 b. rate = k([no][o 2 ] c. rate = k[no 2 ] 2 [NO] -2 [O 2 ] -1/2 d. rate = k[no] 2 [O 2 ] 2 e. rate = k([no][o 2 ]) 2
General Chemistry III 1046 E Exam 1 1. Cyclobutane, C 4 H 8, decomposes as shown: C 4 H 8 (g)! 2 C 2 H 4 (g). In the course of a study of this reaction, the rate of consumption of C 4 H 8 at a certain
More informationChemistry 12 Provincial Exam Workbook Unit 04: Acid Base Equilibria. Multiple Choice Questions
R. Janssen, MSEC Chemistry 1 Provincial Workbook (Unit 0), P. 1 / 69 Chemistry 1 Provincial Exam Workbook Unit 0: Acid Base Equilibria Multiple Choice Questions 1. Calculate the volume of 0.00 M HNO needed
More information