A) Fe B) Al C) P D) OH - 5) Which salt would form an acidic solution when it dissolves in water?
|
|
- Philip Stephens
- 5 years ago
- Views:
Transcription
1 AP Chemistry Test (Chapters 14 and 15) 1) Which one would hydrolyze water the most? A) NH 4 + B) Cl C) Na + D) ClO 3 2) Which one is most likely to be a Lewis acid? A) Fe B) Al C) P D) OH 3) What is the conjugate acid of H 7 X 3 Z +4? 4) What is the conjugate base of H 7 X 3 Z +4? 5) Which salt would form an acidic solution when it dissolves in water? A) NaCl B) AlCl 3 C) NaC 2 H 3 O 2 D) CaF 2 6) Which salt would form a basic solution when it dissolves in water? A) Na 2 C 2 O 4 B) Mg(CN) 2 C) NH 4 Cl D) KNO 3 7) Which one could not be neutralized (partial or whole) by a weak base? A) HCl B) H 3 PO 4 C) K 2 O (s) in H 2 O D) Zn(OH) 2 E) Cl 2 O 7 (g) in H 2 O 8) Four of the following pairs of acids list the weaker acid on the left and the stronger acid on the right. Which pair is reversed? Weaker Acid Stronger Acid A) HIO 3 HClO 3 B) HClO HClO 2 C) H 3 PO 4 HNO 3 D) H 2 S H 2 Se E) H 3 PO 4 H 3 AsO 4 9) In a sample of pure water, which statement is always true at all conditions of temperature and pressure? A) [H 3 O + ] = 1.0 X 10 7 M B) [OH ] = 1.0 X 10 7 M C) = 7.0 D) poh = 7.0 E) [H 3 O + ] = [OH ] 10) Which one is matched correctly? A) 14; [H + ]>>>>>[OH ] B) 1; [H + ] <<<<<<<[OH ] C) 7; [H + ]>[OH ] D) 8; [H + ]<[OH ]
2 11) Which of these acids is the strongest? A) K a = 4.25 X 10 9 B) K a = 6.25 X 10 3 C) K a = 2.15 X 10 5 D) K a = 3.00 X ) When solid NaCN is added to water, the?. A) remains at 7. B) becomes greater than 7 because the Na + hydrolyzes water. C) becomes less than 7 because the Na + hydrolyzes water. D) becomes less than 7 because the CN hydrolyzes water. E) becomes greater than 7 because the CN hydrolyzes water. Please consider the following graph to answer questions ) Which one best describes the experimental procedure used to obtain these lab results? A) A strong acid was titrated with a weak base. B) A weak acid was titrated with a strong base. C) A strong base was titrated with a weak acid. D) A strong acid was titrated with a strong base. 14) Which one best describes the contents of the beaker at the equivalence point? A) Excess acid, salt & water B) Excess base, salt & water C) Salt & water D) Water E) Excess acid & base 15) Which one is true about point A? A) The base is the limiting reagent. B) The acid is the limiting reagent. C) The beaker contains only salt & water. D) The beaker contains only excess base. E) The beaker contains only excess acid.
3 16) Which graph illustrates a weak base titrated with a strong acid? A) B) C) D) 17) Which is a primary difference between a weak acid/strong base titration curve & a strong acid/strong base titration curve? A) A weak acid/strong base curve has a greater jump at the equivalence point. B) A weak acid/strong base curve has a small jump at the equivalence point. C) A weak acid/strong base curve has the equivalence point at = 7. D) A strong acid/strong base curve illustrates the hydrolysis of water. 18) Which one is arranged from the strongest to the weakest base? HOCl Ka = 3.5 X 10 8 NH 3 Kb = 1.8 X 10 5 A) H 2 O, NO 3, OCl, NH 3 B) OCl, NH 3, H 2 O, NO 3 C) NO 3, H 2 O, NH 3, OCl D) NH 3, OCl, H 2 O, NO 3 E) OCl, NH 3, NO 3, H 2 O 19) Water has Kw = 1.26 X at 60 o C. What is the of water at 60 o C? A) 7.00 B) 6.45 C) 7.55 D) ) Which one is matched correctly? A) NH 3 = 8 B) H 3 PO 4 = 1 C) HC 2 H 3 O 2 = 10 D) Ca(OH) ) Which one is false about an acid? A) The larger the Ka, the lesser the dissociation in water. B) The larger the Ka, the larger the dissociation in water. C) The larger the Ka, the lower the. D) The larger the Ka, the stronger the acid.
4 Please use the following reaction to answer questions Al(H 2 O) H 2 O H 3 O + + Al(H 2 O) 5 (OH) 2+ 22) Which species is the conjugate base? 23) Which species is the acid? 24) Which statement is correct? A) Strong acids have strong conjugate bases. B) Weak bases have strong conjugate acids. C) Weak bases have strong conjugate bases. D) Strong acids have weak conjugate acids. 25) Please consider the conjugal pair HPO 4 2 /H 2 PO 4 in water. Which statement is true? A) The HPO 2 4 is a base that took an H + from water. B) The H 2 PO 4 is the conjugate base. C) The HPO 2 4 is an acid that took an H + from water. D) The HPO 2 4 is a base that donated an H + to the water. 26) Which one is a polyprotic acid? A) HF B) HNO 3 C) HClO D) H 3 PO 4 27) Which pair could be a buffer? A) HNO 3 /NO 3 B) Ba(OH) 2 /Ba 2+ C) HClO/ClO D) Al(OH) 3 /OH E) NaCl/Cl 28) What is the purpose of a buffer? A) To absorb the conjugate base of an acid B) To absorb H + and OH C) To absorb the conjugate acid of a base D) To absorb salts 29) Please consider the combination of HClO 4 and NaClO 4 in water. Which one is true? A) It is not a buffer because it cannot absorb H +. ` B) It is not a buffer because it absorbs OH. C) It is a buffer because it absorbs H +. D) It is a buffer because it absorbs OH. 30) Which one is false about indicators? A) They are weak organic acids. B) The acid and conjugate base exist as different colors. C) They utilize LeChatelier s principle to shift from one color to another. D) They change when pka of the indicator = of the acid or base used in the titration.
5 31) Which indicator would be most useful in a titration where the equivalence point was approximately 6? A) Bromophenol blue yellow 4 blue B) Bromcresol purpler yellow 6 purple C) Phenolphthalein clear 9 fuschia D) Bromothymol blue yellow 7 blue Please write a net ionic reaction for each of the following. 32) Sodium acetate is added to water. 33) Dichlorine heptoxide gas is bubbled through water. 34) Solid aluminum oxide is added to water. Please consider this buffer: HC 2 O 4 H + + C 2 O 4 2 for ) Please write the reaction that occurs when an acid H + is added to this buffer. 36) Please write the reaction that occurs when a base OH is added to this buffer. Please consider this buffer: CH 3 NH 2 + H 2 O CH 3 NH OH for ) Please write the reaction that occurs when an acid H + is added to this buffer. 38) Please write the reaction that occurs when a base OH is added to this buffer.
C) 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: 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 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 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 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 informationWorksheet 4.1 Conjugate Acid-Base Pairs
Worksheet 4.1 Conjugate AcidBase Pairs 1. List five properties of acids that are in your textbook. Acids conduct electricity, taste sour, neutralize bases, change the color of indicators, and react with
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 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 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 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 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 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 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 informationAcids, Bases, and Salts Review for Sections
1. Consider the following: Review for Sections 4.1 4.9 I H 2 CO 3 + F HCO 3 + HF 2 II HCO 3 + HC 2 O 4 H 2 CO 3 + C 2 O 4 2 III HCO 3 + H 2 C 6 H 6 O 7 H 2 CO 3 + HC 6 H 5 O 7 The HCO 3 is a base in A.
More informationUnit 7, Lesson 08: The ph of Salt Solutions, Answers
1. Complete the following chart: Unit 7, Lesson 08: The ph of Salt Solutions, Answers on NH 4 PO 3 3- Parent Acid or Base s the parent strong or weak? Will this ion hydrolyze? f the ion will hydrolyze
More informationADVANCED PLACEMENT CHEMISTRY ACIDS, BASES, AND AQUEOUS EQUILIBRIA
ADVANCED PLACEMENT CHEMISTRY ACIDS, BASES, AND AQUEOUS EQUILIBRIA Acids- taste sour Bases(alkali)- taste bitter and feel slippery Arrhenius concept- acids produce hydrogen ions in aqueous solution while
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 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 informationmol of added base 36. Equal moles of which of the following chemicals could be used to make a basic (1 mark)
59. 34. Consider the following titration curve: 14 13 Consider the following titration curve: 14 1 13 11 14 1 1 13 119 1 18 ph 119 7 18 6 ph 97 5 86 4 ph 75 3 64 53 1 4 31 mol of added base Select a suitable
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 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 informationChapter 14 Acid- Base Equilibria Study Guide
Chapter 14 Acid- Base Equilibria Study Guide This chapter will illustrate the chemistry of acid- base reactions and equilibria, and provide you with tools for quantifying the concentrations of acids and
More informationAcids And Bases. H + (aq) + Cl (aq) ARRHENIUS THEORY
Acids And Bases A. Characteristics of Acids and Bases 1. Acids and bases are both ionic compounds that are dissolved in water. Since acids and bases both form ionic solutions, their solutions conduct electricity
More informationAdvanced Chemistry. Approximate Timeline. Students are expected to keep up with class work when absent. CHAPTER 14 ACIDS & BASES
Advanced Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 14 ACIDS & BASES Day Plans for the day Assignment(s) for the day 14.1 The Nature of Acids &
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 informationChapter 17 Additional Aspects of Aqueous Equilibria (Part A)
Chapter 17 Additional Aspects of Aqueous Equilibria (Part A) What is a dominant equilibrium? How do we define major species? Reactions between acids and bases 1. Strong Acids + Strong Base The reaction
More informationTopic 9: Acids & Bases
Topic 9: Acids & Bases Regents Chemistry Mr. Mancuso Electrolytes Substances that conduct electricity when Include Ability to conduct electricity is due to the presence of Dissociation: ~ 1 ~ Acids and
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 informationReally useful information = H + = K w. K b. 1. Calculate the ph of a solution made by pouring 5.0 ml of 0.20 M HCl into 100. ml of water.
Acid Base Equilibrium Putting it all together HA H + + A H + A incomingsa HA +incomingsa Strong Acids HCl HNO3 HBr H2SO4 HI HClO4 HClO3 Really useful information K w H + OH K w M V M V B + H2O OH + HB
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 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 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 informationConsider a 1.0 L solution of 0.10 M acetic acid. Acetic acid is a weak acid only a small percent of the weak acid is ionized
Chemistry 12 Acid- Base Equilibrium V Name: Date: Block: 1. Buffers 2. Hydrolysis Buffers An acid- base buffer is a solution that resists changes in ph following the addition of relatively small amounts
More informationUnit 4: ACIDS, BASES AND SALTS
ABS - 1 Unit 4: ACIDS, BASES AND SALTS 4.1 Arrhenius Acids and Bases Acids release H + in water Bases release OH - in water Salts are products of an acid-base neutralization reaction. The salt is an ionic
More informationReview: Acid-Base Chemistry. Title
Review: Acid-Base Chemistry Title Basics General properties of acids & bases Balance neutralization equations SA + SB water + salt Arrhenius vs. Bronsted-Lowry BL plays doubles tennis match with H+) Identify
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 informationEquations. M = n/v. M 1 V 1 = M 2 V 2 if the moles are the same n 1 n 2 you can cancel out the n s. ph = -log [H + ] poh = -log [OH - ] ph + poh = 14
Equations M = n/v M 1 V 1 = M 2 V 2 if the moles are the same n 1 n 2 you can cancel out the n s. ph = -log [H + ] poh = -log [OH - ] ph + poh = 14 [H 3 O + ] = 10^-pH [OH - ] = 10^-pOH [H 3 O + ] [OH
More informationAcids, Bases and Salts
(Hebden Unit 4 page 109 182) 182) We will cover the following topics: 1. Definition of Acids and Bases 2. Bronsted-Lowry Acids and Bases 2 1 Arrhenius Definition of Acids and Bases An acid is a substance
More information1. What do a chemical indicator and a buffer solution typically both contain?
Acids, Bases & Redox 2 - Practice Problems for Assignment 9 1. What do a chemical indicator and a buffer solution typically both contain? (a) A strong acid and its conjugate acid (b) A strong acid and
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 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 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 informationHomework #6 Chapter 7 Homework Acids and Bases
Homework #6 Chapter 7 Homework Acids and Bases 20. a) 2H 2O(l) H 3O (aq) OH (aq) K [H 3 O ][OH ] Or H 2O(l) H (aq) OH (aq) K [H ][OH ] b) HCN(aq) H 2O(l) H 3O (aq) CN (aq) K [H 3O ][CN ] [HCN] Or HCN(aq)
More informationMr. Storie 40S Chemistry Student Acid and bases Unit. Acids and Bases
Acids and Bases 1 UNIT 4: ACIDS & BASES OUTCOMES All important vocabulary is in Italics and bold. Outline the historical development of acid base theories. Include: Arrhenius, BronstedLowry, Lewis. Write
More informationAssignment 16 A incorrect
Assignment 16 A 1- What is the concentration of hydronium ions in a solution with a hydroxide-ion concentration of 2.31 10 4 M at 25 C? a) 4.33 10 11 M b) 2.31 10 4 M c) 2.31 10 18 M d) 2.31 10 10 M (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 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 informationMASTERING IONIC EQUILLIBRIA. By : S.K.Sinha A CENTRE FOR CONCEPTUAL & SYSTEMATIC STUDY
MASTERING IONIC EQUILLIBRIA By : S.K.Sinha A CENTRE FOR CONCEPTUAL & SYSTEMATIC STUDY MASTERING PHYSICAL CHEMISTRY ACIDS AND BASES The Nature of Acids and Bases Arrhenius concept: Acid a substance that
More informationAcids and Bases Review Worksheet II Date / / Period. Molarity. moles L. Normality [H 3 O +1 ] [OH -1 ] ph poh
Honors Chemistry Name Acids and Bases Review Worksheet II Date / / Period Solute Name of Solute Molar Mass grams mole Molarity moles L Normality [H 3 O +1 ] [OH ] ph poh Acidic or Basic 1. HCl Hydrochloric
More informationChemistry 102 Chapter 15 ACID-BASE CONCEPTS
General Properties: ACID-BASE CONCEPTS ACIDS BASES Taste sour Bitter Change color of indicators Blue Litmus turns red no change Red Litmus no change turns blue Phenolphtalein Colorless turns pink Neutralization
More informationAcids and Bases. Feb 28 4:40 PM
Acids and Bases H O s O Cl H O O H H N H Na O H H Feb 28 4:40 PM Properties of Acids 1. Taste sour 2. Conduct electrical current 3. Liberate H 2 gas when reacted with a metal. 4. Cause certain dyes to
More information16.3 Weak Acids Weak Bases Titration
16.3 Weak Acids Weak Bases Titration Titration of Weak Acid with Strong Base Titration of Base Acid with Strong Acid Dr. Fred Omega Garces Chemistry 201 Miramar College 1 Weak Acids Weak Bases Titration
More informationCHEM 142 Exam 3 Study Guide Chapter 15: Acid-Base Equilibria
CHEM 142 Exam 3 Study Guide Chapter 15: AcidBase Equilibria A. Terminologies and Concepts 1. BronstedLowry definitions acids vs. bases; give examples 2. Amphoteric substances define and give examples 3.
More informationChapter 16: Acids and Bases
1. Which is not a characteristic property of acids? A) neutralizes bases B) turns litmus from blue to red C) reacts with active metals to produce H 2 (g) D) reacts with CO 2 (g) to form carbonates E) All
More informationPart One: Pure Solutions of Weak Acids, Bases (water plus a single electrolyte solute)
CHAPTER 16: ACID-BASE EQUILIBRIA Part One: Pure Solutions of Weak Acids, Bases (water plus a single electrolyte solute) A. Weak Monoprotic Acids. (Section 16.1) 1. Solution of Acetic Acid: 2. See Table
More informationProblem 5: Problem 6 Sig. Fig.: Units:
DEPARTMENT OF CHEMISTRY AND CHEMICAL TECHNOLOGY CHEMISTRY OF SOLUTIONS 202-NYB-05 05 TEST 2 7 NOVEMBER 2011 INSTRUCTOR: I. DIONNE Print your name: Answers INSTRUCTIONS: Answer all questions in the space
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 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 informationAcid / Base Properties of Salts
Acid / Base Properties of Salts n Soluble ionic salts produce may produce neutral, acidic, or basic solutions depending on the acidbase properties of the individual ions. n Consider the salt sodium nitrate,
More informationChem 106 Thursday, March 10, Chapter 17 Acids and Bases
Chem 106 Thursday, March 10, 2011 Chapter 17 Acids and Bases K a and acid strength Acid + base reactions: Four types (s +s, s + w, w + s, and w + w) Determining K from concentrations and ph ph of aqueous
More informationChapter 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 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 informationChapter 17 Additional Aspects of Aqueous Equilibria (Part A)
Chapter 17 Additional Aspects of Aqueous Equilibria (Part A) Often, there are many equilibria going on in an aqueous solution. So, we must determine the dominant equilibrium (i.e. the equilibrium reaction
More informationAcid Base Review Package
Acid Base Review Package 1. In which of the following eqb systems is HCO 3 acting as a BronstedLowry base? 2 a. HCO 3 H+ + CO 3 b. HCO 3 + HS 2 H 2 S + CO 3 c. HCO 3 + H 2 S H 2 CO 3 + HS d. HCO 3 + H
More informationUnderstanding the shapes of acid-base titration curves AP Chemistry
Understanding the shapes of acidbase titration curves AP Chemistry Neutralization Reactions go to Completion Every acidbase reaction produces another acid and another base. A neutralization reaction is
More informationph calculations MUDr. Jan Pláteník, PhD Brønsted-Lowry concept of acids and bases Acid is a proton donor Base is a proton acceptor
ph calculations MUDr. Jan Pláteník, PhD Brønsted-Lowry concept of acids and bases Acid is a proton donor Base is a proton acceptor HCl(aq) + H 2 O(l) H 3 O + (aq) + Cl - (aq) Acid Base Conjugate acid Conjugate
More informationUNIT IV PPT #3 Ka and Kb KEY.notebook. November 23, WHAT IS Ka? UNIT IV. CALCULATIONS USING Ka. WHAT IS Ka? Nov 10 9:42 PM.
WHAT IS Ka? Recall: Find ph of 0.100 M HCl. But What is ph of 0.10 M HF? UNIT IV Ka and Kb CALCULATIONS USING Ka I. [H 3O + ] (or ph) from Ka Ex. Find the [H 3O + ] in 0.10 M HF. WHAT IS Ka? Look at equilibrium
More informationCompletion of acid/base/buffer chemistry. Hanson Activity Clicker quiz 3/11/2013. Chs 7 8 of Zumdahl
Completion of acid/base/buffer chemistry Chs 7 8 of Zumdahl Hanson Activity 16 3 Discuss Key Questions 1 of Activity 16 3, page 301, with your partner for three minutes. The clicker quiz will commence
More informationChapter 17 Homework Problem Solutions
Chapter 17 Homework Problem Solutions 17.40 D 2 O D + + OD, K w = [D + ] [OD ] = 8.9 10 16 Since [D + ] = [OD ], we can rewrite the above expression to give: 8.9 10 16 = ([D + ]) 2, [D + ] = 3.0 10 8 M
More informationChapter 8 Acid-Base Equilibria
Chapter 8 Acid-Base Equilibria 8-1 Brønsted-Lowry Acids and Bases 8-2 Water and the ph Scale 8-3 The Strengths of Acids and Bases 8-4 Equilibria Involving Weak Acids and Bases 8-5 Buffer Solutions 8-6
More informationAqueous Equilibria, Part 2 AP Chemistry Lecture Outline
Aqueous Equilibria, Part 2 AP Chemistry Lecture Outline Name: The Common-Ion Effect Suppose we have a weak acid and a soluble salt of that acid. CH 3 COOH NaCH 3 COO CH 3 COOH CH 3 COO + H + Since NaCH
More informationPart One: Acid-Base Concepts. 1. Sour taste. (Examples: vinegar = acetic acid; lemons - citric acid) yellow
CHAPTER 15: ACIDS AND BASES Part One: Acid-Base Concepts A. Properties of Aqueous Solutions of Acids. 1. Sour taste. (Examples: vinegar = acetic acid; lemons - citric acid) 2. Change the colors of many
More informationLewis Acid/Base. Lewis acid is a different way to look at some type of acids. Lewis Acid/base reactions track the electrons rather then the protons.
Acid Base Wrap up topics Lewis acid Bases Structural indicators of the strength of acids Non-metal oxides/ metal oxides Amphoteric substances Acidic properties of swimming pools Schweitzer 1-29-05 Lewis
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 14: Acids and Bases
Chapter 14: Acids and Bases 14.1 The Nature of Acids and Bases Bronsted-Lowry Acid-Base Systems Bronsted acid: proton donor Bronsted base: proton acceptor Bronsted acid base reaction: proton transfer from
More informationProton Transfer Acids - Base. Dr. Fred Omega Garces Chemistry 201. Miramar College
16.2 Acids Base Proton Transfer Dr. Fred Omega Garces Chemistry 201 Miramar College Important Notes: K a when H 3 O + is produced, K b when OH is produced 1 Acids Bases; Proton Transfer BrønstedLowry AcidsBases
More information-a base contains an OH group and ionizes in solutions to produce OH - ions: Neutralization: Hydrogen ions (H + ) in solution form
NOTES Acids, Bases & Salts Arrhenius Theory of Acids & Bases: an acid contains hydrogen and ionizes in solutions to produce H+ ions: a base contains an OH group and ionizes in solutions to produce OH ions:
More information[base] [acid] ph = pka + log
Fall 2013 CCBC-Catonsville (Wed 10/30/13) Use your time wisely. Do not get stuck on one question. NO CREDIT WILL BE GIVEN UNLESS WORK IS SHOWN CLEARLY. UNITS MUST BE INCLUDED IN YOUR SETUPS. Answers must
More information2. Calculate the ph of a buffer solution composed of 0.12 M benzoic acid and 0.20 M sodium benzoate.!
AP Chem worksheet:buffers, The common ion effect Page 1 1. Calculate the ph of a buffer solution that is 0.060 M formic acid and 0.030 M potassium formate. (3.44) 2. Calculate the ph of a buffer solution
More informationAdvanced Placement Chemistry Chapters Syllabus
As you work through the chapter, you should be able to: Advanced Placement Chemistry Chapters 14 16 Syllabus Chapter 14 Acids and Bases 1. Describe acid and bases using the Bronsted-Lowry, Arrhenius, and
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 information1. (3) The pressure on an equilibrium mixture of the three gases N 2, H 2 and NH 3
1. (3) The pressure on an equilibrium mixture of the three gases N 2, H 2 and NH 3 N 2 (g) + 3 H 2 (g) 2 NH 3 (g) is suddenly decreased by doubling the volume of the container at constant temperature.
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 informationU N I T T E S T P R A C T I C E
South Pasadena Honors Chemistry Name 4 Salts and Solutions Period Date U N I T T E S T P R A C T I C E You may use a pencil, eraser, and scientific calculator to complete the test. You will be given a
More informationCh 7 Practice Problems
Ch 7 Practice Problems 1. For the equilibrium that exists in an aqueous solution of nitrous acid (HNO 2, a eak acid), the equilibrium constant expression is [H ] [NO 2 ] = [HNO ] 2 [H ][N][O] [HNO 2] =
More informationUnit 6: ACIDS AND BASES
Unit 6: Acids and Bases Honour Chemistry Unit 6: ACIDS AND BASES Chapter 16: Acids and Bases 16.1: Brønsted Acids and Bases Physical and Chemical Properties of Acid and Base Acids Bases Taste Sour (Citric
More informationCHAPTER 14 ACIDS AND BASES
CHAPTER 14 ACIDS AND BASES Topics Definition of acids and bases Bronsted-Lowry Concept Dissociation constant of weak acids Acid strength Calculating ph for strong and weak acids and bases Polyprotic acids
More informationReactions with water do NOT go to completion, so to find ion concentrations, need to know K eq and solve an equilibrium problem!
Strong Acid and Base Solutions Easy to find ion concentrations! 0.1 M HCl = [H 3 O + ] = 0.1 M [OH ] = 1 x 10 13 M 0.1 M NaOH = [OH ] = 0.1 M [H 3 O + ] = 1 x 10 13 M Weak Acid and Base Solutions Reactions
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 informationAcids and Bases. Chapter 15. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Acids and Bases Chapter 15 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Acids Have a sour taste. Vinegar owes its taste to acetic acid. Citrus fruits contain
More informationACIDS AND BASES. HCl(g) = hydrogen chloride HCl(aq) = hydrochloric acid HCl(g) H + (aq) + Cl (aq) ARRHENIUS THEORY
ACIDS AND BASES A. CHARACTERISTICS OF ACIDS AND BASES 1. Acids and bases are both ionic compounds that are dissolved in water. Since acids and bases both form ionic solutions, their solutions conduct electricity
More informationChapter 10 - Acids & Bases
Chapter 10 - Acids & Bases 10.1-Acids & Bases: Definitions Arrhenius Definitions Acids: substances that produce hydrogen ions when dissolved in H 2 O Common Strong Acids: Common Weak acids: Organic carboxylic
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 informationAcids, Bases, and ph. ACIDS, BASES, & ph
I. Arrhenius Acids and Bases ACIDS, BASES, & ph Acid any substance which delivers hydrogen ion (H + ) _ to the solution. Base any substance which delivers hydroxide ion (OH ) to the solution. II ph ph
More informationUnit 9. Acids, Bases, & Salts Acid/Base Equilibrium
Unit 9 Acids, Bases, & Salts Acid/Base Equilibrium Properties of Acids sour or tart taste strong acids burn; weak acids feel similar to H 2 O acid solutions are electrolytes acids react with most metals
More informationHALFWAY to EQUIVALENCE POINT: ph = pk a of the acid being titrated.
CHEMISTRY 109 Help Sheet #33 Titrations Chapter 15 (Part II); Section 15.2 ** Cover topics appropriate for your lecture** Prepared by Dr. Tony Jacob http://www.chem.wisc.edu/areas/clc (Resource page) Nuggets:
More informationCHAPTER 13: ACIDS & BASES. Section Arrhenius Acid & Bases Svante Arrhenius, Swedish chemist ( ).
CHAPTER 13: ACIDS & BASES Section 13.1 Arrhenius Acid & Bases Svante Arrhenius, Swedish chemist (1839-1927). He understood that aqueous solutions of acids and bases conduct electricity (they are electrolytes).
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 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 information