Problems -- Chapter Write balanced chemical equations for the important equilibrium that is occurring in an aqueous solution of the following.
|
|
- Noreen Jenkins
- 6 years ago
- Views:
Transcription
1 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) NaHCO 3 and H CO 3 (c) HClO and KClO (d) RbF and HF (e) KCl and HCl (f) H 3 PO and KH PO (g) (CH 3 ) NH NO 3 and (CH 3 ) NH. Write the appropriate equilibrium constant expressions (K a, etc.) for each of the the solutions above. 3. Determine the ph of a mixture of M solutions of the two components in part (a) above (Ka =.5 x 10 - ) Answer: ph = Write the appropriate reactions (see end of this document for answers) and calculate the ph of the following: (a) 0.35 M NaIO/0.0M HIO (Ka = 5.x10-9 ) (b) 0.8 M NaIO/0.78 M HIO (Ka =.0x10-11 ) (c) 0.0 M NH3 (Kb = 1.8x10-5 )/0.55 M NHCl. Answers: (a) 8.9 (b) 10.9 (c) HNO is a weak acid whose K a =.5x10 -. How many grams of NaNO would have to be added to 50 ml of a 0.M HNO acid solution to give a buffer of ph =.00. (3. g). A 0.5-gram sample of an unknown weak acid (call it HA for short) is dissolved in enough water to make 5.0 ml of solution. This weak acid solution is then titrated with M NaOH and 5.0 ml of the NaOH solution is required to reach the equivalence point. Using a ph meter, the ph of the solution at the equivalence point is found to be 8.5. Note: writing balanced reactions will solve this problem! (a) Determine the molecular mass of the unknown acid g/mole (b) Determine the pk a value of the unknown acid The pk b value for ammonia (NH 3 ) is.7. Calculate the mass (in grams) of solid ammonium chloride (NH Cl, formula mass = 53.5 g/mole) that must be added to 300 ml of 0.5 M NH 3 solution to make a buffer solution with a ph equal to Like the problems done in class write ALL balanced reactions whether they go essentially to completion or they are at equilibrium. Use the correct arrows g 8. A 50 ml portion of a 0.10 M solution of a weak acid, HA, whose Ka equals 1.0 x 10 -, is diluted to 50 ml and then titrated with 0.10 M NaOH. Calculate ph after the following ml of the NaOH solution have been added. Like the problems done in class write ALL balanced reactions whether they go essentially to completion or they are at equilibrium. Use the correct arrows. (a) 0 (b) 5 (c) 5 (d) 50 (e) 0
2 (a).85 (b) 3.05 (c).00 (d) 8.11 (e) Fifty ml of 0.1 M NH3 is titrated with 0.10 M HCl. The Kb of the weak base NH3 is 1.8 x Calculate the ph after the following ml of the HCl solution have been added. Like the problems done in class write ALL balanced reactions whether they go essentially to completion or they are at equilibrium. Use the correct arrows. (a) 0 (b) 10 (c) 5 (d) 50 (e) 55 (a) ( b) 9.8 (c) 9. (d) 5.8 (e) Shown on the next page is the titration curve for the titration of ml of a solution of the monoprotic acid, HA, with 0.01 M NaOH. What is the molarity of the acid?(show reaction and yoru work) Is the acid a weak acid or a strong one? If it is a weak acid, what is the value of Ka? (0.0 M, weak, Ka=.8 x 10 - ) 1 Titration of ml of HA with 0.01M NaOH 10 8 ph ml NaOH Shown below is the titration curve for the titration of 50.0 ml of a solution of the weak ammoniatype base, methyl amine, CH3NH, with 0.01M HCl. What is the molarity of the base? (show reaction and your work) What is the value of Kb for methyl amine? (0.0 M answer given; K b = 3.x10 - )
3 ph ml 0.01M HCl 1. Consider reactions involving the following acids and bases. State in each case whether the ph at the equivalence point would be below 7, at 7, or above 7. (a) acid = HClO base = KOH (b) acid = HNO3 base = NH3 (c) acid = HF base = LiOH (a) 7 (b) <7 (c) >7 13. A 3.0 ml sample of a 0.0 M HNO 3 solution was titrated with 0.8 M KOH. Calculate the ph after the following volumes of KOH have been added: Like the problems done in class write ALL reactions whether they go essentially to completion or they are at equilibrium. Use the correct arrows. (a) 0 ml (b) 10.0 ml (c) 0.0 ml (30.0 ml (e) 0.0 ml ( f) 50.0 ml. (a) 0.0 (b) 0.8 (c) 1.07 d) 7.00 (e) 1.80 (f) Calculate the ph s of the following: Like the problems done in class write ALL reactions whether they go essentially to completion or they are at equilibrium. Use the correct arrows. Note, that you will need TWO reactions in some cases! THINK! (a) the solution formed by mixing 0.0 ml of a 0.30M HCl solution with 1 ml of a 0.5 M NaOH. (b) the solution formed by mixing 18.0 ml of a 0.M HC H 7 O solution with 10.0 ml of a 0.35M NaOH (K a for HC H 7 O = 8.0x10 5 ) (c) the solution formed by mixing 15.0 ml of a 0.7M HF with 0.0 ml of a 0.0M KOH solution (K a for HF = 7.1x10 ) (d) the solution formed by mixing 30.0 ml of a 0.0 M HCHO solution with.0 ml of a 0.0 M KOH solution (K a for HCHO = 1.7x10 ) (e) the solution formed by dissolving.85 g of KF in 10 ml of a 0.30 M HF solution (K a for HF = 7.1x10 ) (f) the end point of the titration of 58.0 ml of a 0.8 M HCHO with 0.0 M KOH. (a) 1.03 (b) 3.9 (c) 3.7 (d) 1.73 (e) 3.8 (f) 8.55
4 15. A 0.0 ml sample of a 0.0 M HNO solution was titrated with 0.80 M KOH. Given that HNO is a weak acid whose K a =.5x10 -, calculate the ph after the following volumes of KOH have been added: Like the problems done in class write ALL reactions whether they go essentially to completion or they are at equilibrium. Use the correct arrows. (a) 0 ml; (b) 5.0 ml; (c) 10.0 ml; (d) 0.0 ml; (e) 30.0 ml; (f) 0.0 ml (a) 1.87 (b).87 (c) 3.35 (d) 8.39 (e) 13.0 (f) Drawn below is a plot of ph vs ml of 0.0 M NaOH for the titration of 50.0 ml of a weak diprotic acid. What is the concentration of the acid? What are the values of Ka1 and Ka for the acid? Write the reaction that is occurring for each equivalence point. (Answer: 0.80M, Ka1 = 5.0x10-3, Ka =.3x10-8 ) ph ml 0.M NaOH 17. The Ksp of Pb(IO3) at 5 C = 3. x What is the solubility of Pb(IO3) in moles per liter and in grams per liter? Write the reaction. (.3 x 10-5 mol/l ; g/l = 0.0) 18. Calculate the Ksp of the following compounds. The solubilities are given in moles per liter. Write the reaction. (a) Mg(OH) = 1.3 x 10 - M (8.8 x 10-1 ) (b) AgCO = 1. x 10 - M (1.1 x ) 19. Calculate the Ksp of the following salts. Solubilities are given in grams/liter. Write the reaction. (a) BaCrO =.3 x g/l (8.3 x ) (b) CaF =.7 x 10 - g/l (1.7 x ) 0. What [SO - ] must be exceeded to produce a RaSO precipitate in 500 ml of a solution containing moles of Ra +? (Ksp = x ). Write the reaction. ( x 10-7 M) 1. A solution contains an Mg + concentration of mole/liter. Will Mg(OH) (Ksp = 8.9 x 10-1 ) precipitate if the OH - concentration of the solution is Write the reaction. (a) 10-5 mole/liter? (b) 10 - mole/liter? (a) Q = 1x10-13, no (b) Q = 1x10-11, yes]. How many grams of NaOH are required to start the precipitation of Mg(OH) in 100 ml of a solution which contains 0.1 g of MgCl? Write the reaction. (1.1 x 10 - g)
5 3. The value of Ksp for PbCl is 1. x Will a precipitate of PbCl form when the following solutions are mixed? Write the reaction. 5 (a) 100 ml of 0.01 M Pb(NO3) and 100 ml of 0.00 M NaCl. (b) 10 ml of 0.01 M Pb(NO3) and 30 ml of 0. M NaCl. (c) 10 ml of 0.01 M Pb(NO3) and 0 ml of 0.0 M NaCl. (d) 10 ml of 0.01 M Pb(NO3) and 0 ml of 0.0 M CaCl. (a) no, Q = 5x10 9 (b) yes, Q= 5.x10 5 (c) no, Q= 5.3x10 (d) yes, Q=.1x10 5. Silver chromate, Ag CrO, is an "insoluble" substance with a K sp value of 1. x Silver ion forms a stable complex ion with cyanide ion that has the formula Ag(CN) - and a formation constant (K f ) of 5.3 x Calculate the molar solubility of Ag CrO in each of the following solutions. Write balanced chemical equations for any important equilibrium reactions that are occurring. (a) in water.9 x 10-5 M (b) in.00 M Na CrO 3.87 x 10-7 M (c).00 M NaCN 0.50 M 5. A saturated solution of Mg 3 (PO ) has a concentration of mg per liter. Calculate the solubility product constant for Mg 3 (PO )..7 x Cadmium carbonate, CdCO3, is a sparingly soluble salt whose Ksp=.5x10-1. It is also known that Cd + forms the [Cd(NH3)] + complex ion that has a formation constant, Kf = 1.0x10 7. (a) Calculate the molar solubility of CdCO3 in.0m NH3. (0.018 mol/l) (b) What NH3 concentration would be required to dissolve.00 mmol of CdCO3 in one liter of the solution? (.83 M)
6 Answers to #1 (a) HNO H + + NO - (b) H CO 3 HCO H + (c) HClO H + + ClO - (d) HF F - + H + (e) not a buffer: the only equilibrium in this neutral solutions is dissociation of water, i.e., H O H + + OH - (f) H 3 PO H + + H PO - (g) (CH 3 ) NH + H + + (CH 3 ) NH. NOTE: ION CHARGES ARE CRITICALLY IMPORTANT! a. Buffer: HIO H + + IO - K a applies or IO - + H O OH - + HIO K b applies b. Buffer: HIO H + + IO - K a applies or IO - + H O OH - + HIO K b applies c. Buffer: NH + H + + NH 3 K a applies or NH 3 + H O NH + + OH - K b applies 5. HNO H + + NO - use K a. a. reaction is critically important: HA + NaOH NaA + NaCl (note the direction of the arrow: REXN is COMPLETE, not an equilibrium b. What is in the beaker at the equivalence point? By now you should be able to write this reaction! THINK befor you look at the answer! A - + H O HA + OH -
Ch 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 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 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 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 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 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 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 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 informationEquilibri acido-base ed equilibri di solubilità. Capitolo 16
Equilibri acido-base ed equilibri di solubilità Capitolo 16 The common ion effect is the shift in equilibrium caused by the addition of a compound having an ion in common with the dissolved substance.
More informationChemistry 1A Fall 2013 MWF 9:30 Final Test Form A
Chemistry 1A Fall 2013 MWF 9:30 Final Test Form A 1. How many moles of P 4 molecules are in 141.4 g of phosphorus? A) 4.566 mol B) 1.752 x10 4 mol C) 1.141 mol D) 2.348 x 10 1 mol E) 1.414 x 10 1 mol 2.
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 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 informationAcid-Base Equilibria and Solubility Equilibria Chapter 17
PowerPoint Lecture Presentation by J. David Robertson University of Missouri Acid-Base Equilibria and Solubility Equilibria Chapter 17 The common ion effect is the shift in equilibrium caused by the addition
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 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 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 informationCHEMISTRY - BURDGE-ATOMS FIRST 3E CH.17 - ACID-BASE EQUILIBRIA AND SOLUBILITY EQUILIBRIA
!! www.clutchprep.com CONCEPT: CLASSIFICATION AND IDENTIFICATION OF BUFFERS Solutions which contain a acid and its base are called buffer solutions because they resist drastic changes in ph. They resist
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 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 15 Additional Aspects of
Chemistry, The Central Science Chapter 15 Additional Aspects of Buffers: Solution that resists change in ph when a small amount of acid or base is added or when the solution is diluted. A buffer solution
More informationSolubility and Complex Ion Equilibria
Solubility and Complex Ion Equilibria a mineral formed by marine organisms through biological precipitation CALCITE CaCO 3(s) Ca + (aq)+ CO 3 - (aq) K K sp [Ca + ][CO 3 - ].8 x 10-9 K sp solubility product
More informationCHAPTER 15 APPLICATIONS OF AQUEOUS EQUILIBRIA
Advanced Chemistry Name Hour Advanced Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 15 APPLICATIONS OF AQUEOUS EQUILIBRIA Day Plans for the day Assignment(s)
More informationSolubility and Complex Ion Equilibria
CALCITE Solubility and Complex Ion Equilibria a mineral formed by marine organisms through biological precipitation CaCO (s) Ca + (aq)+ CO (aq) K K sp [Ca + ][CO ].8 x 10-9 K sp solubility product constant
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 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 informationChap 17 Additional Aspects of Aqueous Equilibria. Hsu Fu Yin
Chap 17 Additional Aspects of Aqueous Equilibria Hsu Fu Yin 1 17.1 The Common-Ion Effect Acetic acid is a weak acid: CH 3 COOH(aq) H + (aq) + CH 3 COO (aq) Sodium acetate is a strong electrolyte: NaCH
More informationTry this one Calculate the ph of a solution containing M nitrous acid (Ka = 4.5 E -4) and 0.10 M potassium nitrite.
Chapter 17 Applying equilibrium 17.1 The Common Ion Effect When the salt with the anion of a is added to that acid, it reverses the dissociation of the acid. Lowers the of the acid. The same principle
More informationOperational Skills. Operational Skills. The Common Ion Effect. A Problem To Consider. A Problem To Consider APPLICATIONS OF AQUEOUS EQUILIBRIA
APPLICATIONS OF AQUEOUS EQUILIBRIA Operational Skills Calculating the common-ion effect on acid ionization Calculating the ph of a buffer from given volumes of solution Calculating the ph of a solution
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 informationChapter 19. Solubility and Simultaneous Equilibria p
Chapter 19 Solubility and Simultaneous Equilibria p. 832 857 Solubility Product ) The product of molar concentrations of the constituent ions, each raised ot the power of its stoichiometric coefficients
More informationk 1 I 2 2 I k -1 k 2 2 HI H I
Example: Write the overall reaction and the rate law for the reaction that occurs in the following two steps. The second step is the rate determining step. I 2 k 1 k -1 2 I H 2 + 2 I k 2 2 HI Example.
More informationTest 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 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 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 informationLe Chatlier's principle can be used to decide whether the above equilibrium will be shifted left or right
Problems, Chapter 17 (with solutions) NOTE: Unless otherwise stated, assume T = 25. C in all problems) 1) In which of these solutions will HNO2 ionize less than it does in pure water? a) 0.10 M NaCl b)
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 informationAcid-Base Equilibria and Solubility Equilibria
ACIDS-BASES COMMON ION EFFECT SOLUBILITY OF SALTS Acid-Base Equilibria and Solubility Equilibria Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 2 The common
More informationAqueous Equilibria: Part II- Solubility Product
Aqueous Equilibria: Part II- Solubility Product PSI AP Chemistry Name-------------------------- I Solubility Product, K sp MC #63-103 a) Writing K sp expression b) Solving for K sp c) Solving for (molar)
More informationChemistry 12 Review Sheet on Unit 3 Solubility of Ionic Substances
Chemistry 12 Review Sheet on Unit 3 Solubility of Ionic Substances 1. Identify each of the following as ionic or molecular substances: a) NaCl (aq)... b) CH 3 COOH (aq)... c) CCl 4(l)... d) HNO 3(aq)...
More informationCHM 2046 Test #3 Review: Chapters , 15, & 16
Chapter 14 1. For the following reaction Kc = 0.513 at 500 K. N 2 O 4 (g) 2 NO 2 (g) If a reaction vessel initially contains an N 2 O 4 concentration of 0.0500 M at 500 K, what are the equilibrium concentrations
More informationCHAPTER 16 ACID-BASE EQUILIBRIA AND SOLUBILITY EQUILIBRIA
CHAPTER 16 ACID-BASE EQUILIBRIA AND SOLUBILITY EQUILIBRIA 16.3 (a) This is a weak acid problem. Setting up the standard equilibrium table: CH 3 COOH(aq) H + (aq) + CH 3 COO (aq) Initial (M): 0.40 0.00
More informationAqueous Equilibria Pearson Education, Inc. Mr. Matthew Totaro Legacy High School AP Chemistry
2012 Pearson Education, Inc. Mr. Matthew Totaro Legacy High School AP Chemistry The Common-Ion Effect Consider a solution of acetic acid: HC 2 H 3 O 2 (aq) + H 2 O(l) H 3 O + (aq) + C 2 H 3 O 2 (aq) If
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 informationDuring photosynthesis, plants convert carbon dioxide and water into glucose (C 6 H 12 O 6 ) according to the reaction:
Example 4.1 Stoichiometry During photosynthesis, plants convert carbon dioxide and water into glucose (C 6 H 12 O 6 ) according to the reaction: Suppose that a particular plant consumes 37.8 g of CO 2
More informationUnit 3: Solubility Equilibrium
Unit 3: Chem 11 Review Preparation for Chem 11 Review Preparation for It is expected that the student understands the concept of: 1. Strong electrolytes, 2. Weak electrolytes and 3. Nonelectrolytes. CHEM
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 informationCh. 14/15: Acid-Base Equilibria Sections 14.6, 14.7, 15.1, 15.2
Ch. 14/15: Acid-Base Equilibria Sections 14.6, 14.7, 15.1, 15.2 Creative Commons License Images and tables in this file have been used from the following sources: OpenStax: Creative Commons Attribution
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 informationTYPES OF CHEMICAL REACTIONS
TYPES OF CHEMICAL REACTIONS Precipitation Reactions Compounds Soluble Ionic Compounds 1. Group 1A cations and NH 4 + 2. Nitrates (NO 3 ) Acetates (CH 3 COO ) Chlorates (ClO 3 ) Perchlorates (ClO 4 ) Solubility
More 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 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 informationQuick Review. - Chemical equations - Types of chemical reactions - Balancing chemical equations - Stoichiometry - Limiting reactant/reagent
Quick Review - Chemical equations - Types of chemical reactions - Balancing chemical equations - Stoichiometry - Limiting reactant/reagent Water H 2 O Is water an ionic or a covalent compound? Covalent,
More informationChemistry 51 Chapter 8 TYPES OF SOLUTIONS. Some Examples of Solutions. Type Example Solute Solvent Gas in gas Air Oxygen (gas) Nitrogen (gas)
TYPES OF SOLUTIONS A solution is a homogeneous mixture of two substances: a solute and a solvent. Solute: substance being dissolved; present in lesser amount. Solvent: substance doing the dissolving; present
More informationUnit 3: Solubility Equilibrium
Unit 3: Chem 11 Review Preparation for Chem 11 Review Preparation for It is expected that the student understands the concept of: 1. Strong electrolytes, 2. Weak electrolytes and 3. Nonelectrolytes. CHEM
More informationSolubility Multiple Choice. January Which of the following units could be used to describe solubility? A. g/s B. g/l C. M/L D.
Solubility Multiple Choice January 1999 14. Which of the following units could be used to describe solubility? A. g/s B. g/l C. M/L D. mol/s 15. Consider the following anions: When 10.0mL of 0.20M Pb(NO3)
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 informationPart One: Solubility Equilibria. Insoluble and slightly soluble compounds are important in nature and commercially.
CHAPTER 17: SOLUBILITY AND COMPLEX ION EQUILIBRIA Part One: Solubility Equilibria A. Ksp, the Solubility Product Constant. (Section 17.1) 1. Review the solubility rules. (Table 4.1) 2. Insoluble and slightly
More information] after equilibrium has been established?
Chemistry 1 Solubility Equilibrium onster Review 1. A saturated solution forms when a 0. 10 mol of salt is added to 10. L of water. The salt is A. Li S B. CuBr C. Zn( OH) ( ) D. NH CO 4. Consider the following
More informationTopic 1 (Review) What does (aq) mean? -- dissolved in water. Solution: a homogeneous mixture; solutes dissolved in solvents
Solutions Unit 6 Topic 1 (Review) What does (aq) mean? -- dissolved in water. Solution: a homogeneous mixture; solutes dissolved in solvents Solute: dissolved particles in a solution (i.e. NaCl) Solvent:
More informationph + poh = 14 G = G (products) G (reactants) G = H T S (T in Kelvin) 1. Which of the following combinations would provide buffer solutions?
JASPERSE CHEM 210 PRACTICE TEST 3 VERSION 3 Ch. 17: Additional Aqueous Equilibria Ch. 18: Thermodynamics: Directionality of Chemical Reactions Key Equations: For weak acids alone in water: [H + ] = K a
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 informationCHAPTER 16 ACID-BASE EQUILIBRIA AND SOLUBILITY EQUILIBRIA
CHAPTER 16 ACID-BASE EQUILIBRIA AND SOLUBILITY EQUILIBRIA 16.5 (a) This is a weak acid problem. Setting up the standard equilibrium table: CH 3 COOH(aq) H (aq) CH 3 COO (aq) Initial (): 0.40 0.00 0.00
More informationChemistry 102 Discussion #8, Chapter 14_key Student name TA name Section
Chemistry 102 Discussion #8, Chapter 14_key Student name TA name Section 1. If 1.0 liter solution has 5.6mol HCl, 5.mol NaOH and 0.0mol NaA is added together what is the ph when the resulting solution
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 informationph + poh = 14 G = G (products) G (reactants) G = H T S (T in Kelvin)
JASPERSE CHEM 210 PRACTICE TEST 3 VERSION 2 Ch. 17: Additional Aqueous Equilibria Ch. 18: Thermodynamics: Directionality of Chemical Reactions Key Equations: For weak acids alone in water: [H + ] = K a
More informationX212F Which of the following is a weak base in aqueous solution? A) H 2 CO 3 B) B(OH) 3 C) N 2 H 4 D) LiOH E) Ba(OH) 2
PX212SP14 Practice Exam II / Spring 2014 1. Which of the following statements are characteristic of acids? 1. They are proton donors. 2. They react with bases to produce a salt and water. 3. They taste
More informationLecture #12 Complex Ions and Solubility
Lecture #12 Complex Ions and Solubility Stepwise exchange of NH 3 for H 2 O in M(H 2 O) 4 2+ M(H 2 O) 2 (NH 3 ) 2 2+ M(H 2 O) 4 2+ M(NH 3 ) 4 2+ M(H 2 O) 3 (NH 3 ) 2+ M(H 2 O)(NH 3 ) 3 2+ Formation Constants
More informationChapter 8: Applications of Aqueous Equilibria
Chapter 8: Applications of Aqueous Equilibria 8.1 Solutions of Acids or Bases Containing a Common Ion 8.2 Buffered Solutions 8.3 Exact Treatment of Buffered Solutions 8.4 Buffer Capacity 8.5 Titrations
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 informationChapter 4. Aqueous Reactions and Solution Stoichiometry
Sample Exercise 4.1 (p. 127) The diagram below represents an aqueous solution of one of the following compounds: MgCl 2, KCl, or K 2 SO 4. Which solution does it best represent? Practice Exercise 1 (4.1)
More informationLe Chatlier's principle can be used to decide whether the above equilibrium will be shifted left or right
Problems, Chapter 17 (with solutions) NOTE: Unless otherwise stated, assume T = 25. C in all problems) 1) In which of these solutions will HNO2 ionize less than it does in pure water? a) 0.10 M NaCl b)
More informationChapter 4. Reactions in Aqueous Solution
Chapter 4. Reactions in Aqueous Solution 4.1 General Properties of Aqueous Solutions A solution is a homogeneous mixture of two or more substances. A solution is made when one substance (the solute) is
More informationToday. Solubility The easiest of all the equilibria. Polyprotic Acids determining something about an unknown by reacting it with a known solution
Today Solubility The easiest of all the equilibria Polyprotic Acids determining something about an unknown by reacting it with a known solution Solubility Equilibria Mg(OH)2 (s) Mg 2+ (aq) + 2OH - (aq)
More informationUNIT III: SOLUBILITY EQUILIBRIUM YEAR END REVIEW (Chemistry 12)
I. Multiple Choice UNIT III: SOLUBILITY EQUILIBRIUM YEAR END REVIEW (Chemistry 12) 1) Which one of the following would form an ionic solution when dissolved in water? A. I 2 C. Ca(NO 3 ) 2 B. CH 3 OH D.
More informationHomework: 14, 16, 21, 23, 27, 29, 39, 43, 48, 49, 51, 53, 55, 57, 59, 67, 69, 71, 77, 81, 85, 91, 93, 97, 99, 104b, 105, 107
Homework: 14, 16, 21, 23, 27, 29, 39, 43, 48, 49, 51, 53, 55, 57, 59, 67, 69, 71, 77, 81, 85, 91, 93, 97, 99, 104b, 105, 107 Chapter 15 Applications of Aqueous Equilibria (mainly acid/base & solubility)
More informationChemistry. Approximate Timeline. Students are expected to keep up with class work when absent.
Chemistry Name Hour Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 15 SOLUTIONS Day Plans for the day Assignment(s) for the day 1 Begin Chapter 15
More informationCHEM134- Fall 2018 Dr. Al-Qaisi Chapter 4b: Chemical Quantities and Aqueous Rxns So far we ve used grams (mass), In lab: What about using volume in lab? Solution Concentration and Solution Stoichiometry
More informationChapter 4 Reactions in Aqueous Solutions. Copyright McGraw-Hill
Chapter 4 Reactions in Aqueous Solutions Copyright McGraw-Hill 2009 1 4.1 General Properties of Aqueous Solutions Solution - a homogeneous mixture Solute: the component that is dissolved Solvent: the component
More informationChapter 15 - Applications of Aqueous Equilibria
Neutralization: Strong Acid-Strong Base Chapter 15 - Applications of Aqueous Equilibria Molecular: HCl(aq) + NaOH(aq) NaCl(aq) + H 2 O(l) SA-SB rxn goes to completion (one-way ) Write ionic and net ionic
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 informationAP Chemistry Table of Contents: Ksp & Solubility Products Click on the topic to go to that section
Slide 1 / 91 Slide 2 / 91 AP Chemistry Aqueous Equilibria II: Ksp & Solubility Products Table of Contents: K sp & Solubility Products Slide 3 / 91 Click on the topic to go to that section Introduction
More informationChapter 16 exercise. For the following reactions, use figure 16.4 to predict whether the equilibrium lies predominantly. - (aq) + OH - (aq)
1 Chapter 16 exercise Q1. Practice exercise page 671 Write the formula for the conjugate acid of the following, HSO 3, F, PO 4 3 and CO. HSO 3 H H 2 SO 4 F H HF PO 4 3 H HPO 4 2 CO H HCO Q2. Practice exercise
More informationChapter 4. Reactions in Aqueous Solution
Chapter 4 Reactions in Aqueous Solution Topics General properties of aqueous solutions Precipitation reactions Acid base reactions Oxidation reduction reactions Concentration of solutions Aqueous reactions
More 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 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 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 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 informationSolubility Equilibrium
2016 Ksp note.notebook Solubility Equilibrium Learning Goals: to understand what happens when a compound dissolves in water to calculate the extent of dissolution...the molar solubility to calculate the
More informationChapter 10. Acids, Bases, and Salts
Chapter 10 Acids, Bases, and Salts Topics we ll be looking at in this chapter Arrhenius theory of acids and bases Bronsted-Lowry acid-base theory Mono-, di- and tri-protic acids Strengths of acids and
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 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 informationANSWER KEY CHEMISTRY F14O4 FIRST EXAM 2/16/00 PROFESSOR J. MORROW EACH QUESTION IS WORTH 1O POINTS O. 16.
discard 1 2 ANSWER KEY CHEMISTRY F14O4 FIRST EXAM 2/16/00 PROFESSOR J. MORROW PRINT NAME, LAST: FIRST: I.D.# : EACH QUESTION IS WORTH 1O POINTS 1. 7. 13. 2. 8. 14. 3. 9. 15. 4. 1O. 16. 5. 11. 17. 6. 12.
More informationName Date. 9. Which substance shows the least change in solubility (grams of solute) from 0 C to 100 C?
Solubility Curve Practice Problems Directions: Use the graph to answer the questions below. Assume you will be using 100g of water unless otherwise stated. 1. How many grams of potassium chloride (KCl)
More informationClasses at: - Topic: Ionic Equilibrium
PHYSICAL CHEMISTRY by: SHAILENDRA KR Classes at: - SCIENCE TUTORIALS; Opp Khuda Baksh Library, Ashok Rajpath, Patna PIN POINT STUDY CIRCLE; House No 5A/65, Opp Mahual Kothi, Alpana Market, Patna Topic:
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 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 informationToday. Complex Equilibria. Approximations when do your previous formulas fail?
Today Complex Equilibria Approximations when do your previous formulas fail? In short hand notation what is dimethylamine? A. HA B. A - C. B D. BH + Amines are like ammonia with other substituents instead
More informationpotassium formate? In short hand notation what is dimethylamine? Today Complex Equilibria Approximations when do your previous formulas fail?
In short hand notation what is dimethylamine? Today Complex Equilibria A. HA Approximations when do your previous formulas fail? B. A - C. B D. BH + Amines are like ammonia with other substituents instead
More informationReview of Chemistry 11
Review of Chemistry 11 HCl C 3 H 8 SO 2 NH 4 Cl KOH H 2 SO 4 H 2 O AgNO 3 PbSO 4 H 3 PO 4 Ca(OH) 2 Al(OH) 3 P 2 O 5 Ba(OH) 2 CH 3 COOH 1. Classify the above as ionic or covalent by making two lists. Describe
More informationSecondary Topics in Equilibrium
Secondary Topics in Equilibrium Outline 1. Common Ions 2. Buffers 3. Titrations Review 1. Common Ions Include the common ion into the equilibrium expression Calculate the molar solubility in mol L -1 when
More information