Try this one Calculate the ph of a solution containing M nitrous acid (Ka = 4.5 E -4) and 0.10 M potassium nitrite.
|
|
- Piers Blair
- 5 years ago
- Views:
Transcription
1 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 applies to salts with the of a weak base. The calculations are the same as the last two chapters. 4 Logical Steps As we approach these problems: 1. Identify the major species in solution, and consider their acidity or basicity. 2. Identify the important equilibrium that is the source of H+ and therefore determines ph. 3. Tabulate the concentrations at equilibrium (ICE chart) 4. Use the equilibrium-constant expression to calculate [H+] and then ph. Example What is the ph of a solution made by adding 0.30 mole of acetic acid and 0.30 mole of sodium acetate to enough water to make 1.0 Liter of solution? Appendix D gives Ka = 1.8 E -5. Try this one Calculate the ph of a solution containing M nitrous acid (Ka = 4.5 E -4) and 0.10 M potassium nitrite. How about these Calculate the fluoride ion concentration and ph of a solution that is 0.20 M in HF and 0.10 M in HCl. Calculate the formate ion concentration and ph of a solution that is 0.50 M in formic acid (HCOOH, Ka = 1.8 E -4) and 0.10 M nitric acid. 1
2 17.2 Buffered Solutions A solution that Either a and its salt or a and its salt. We can make a buffer of any ph by varying the concentrations of these solutions. Which of the following conjugate acid-base pairs will not function as a buffer? HCOOH and HCOO -1? HCO 3-1 and CO 3-2? HNO 3 and NO 3-1? How buffers work Let s consider a buffer composed of a weak acid (HX) and one of its salts (MX). Write the equation for the dissociation of this weak acid: Write the corresponding acid-dissociation constant expression: Rearrange, solving for [H+]: What do we have? [H+], and thus ph, is determined by two factors: The value of The ratio of the concentrations of the conjugate acid-base pair: As long as [HX]/[X-] in the buffer compared to the amount of H+ or OHadded, the ratio doesn t change much, and thus the change in ph is small. Give it some thought What happens when NaOH is added to a buffer composed of HC 2 H 3 O 2 and C 2 H 3 O 2-1? What happens when HCl is added to this buffer? Calculating the ph of a Buffer Ka = so The [H + ] depends taking the negative log of both sides ph = ph = ph = 2
3 This is called the equation ph = ph = Let s try one What is the ph of a buffer that is 0.12 M in lactic acid (HC3H5O3) and 0.10 M in sodium lactate? For lactic acid, Ka = 1.4 E -4. We can use the ICE CHART or the Henderson-Hasselbalch equation. Preparing a Buffer How many moles of ammonium chloride must be added to 2.0 Liters of a 0.10 M ammonia solution to form a buffer whose ph is 9.00? Assume that the addition of ammonium chloride does not change the volume of the solution. Another one Calculate the concentration of sodium benzoate that must be present in a 0.20 M solution of benzoic acid (HC7H5O2) to produce a ph of Buffer Capacity The ph of a buffered solution is determined by the ratio As long as this doesn t change much the ph won t change much. The more concentrated these two are the more H + and OH - the solution will be able to absorb. Larger concentrations bigger ph Range The ph range over which the buffer acts effectively. Resist a change in ph in either direction when 3
4 Optimal ph of a buffer is when Try to select a buffer whose acid form has a pka close the desired ph. This will give us a usable ph range of + or one ph unit of pka. Give this some thought What is the optimal ph buffered by a solution containing acetic acid and sodium acetate? Ka for acetic acid is 1.8 E -5. Adding a strong acid or base Do the first. A strong base will grab protons from the weak acid reducing [HA] 0 A strong acid will add its proton to the anion of the salt reducing [A - ] 0 Then do the equilibrium problem, most easily done with the Henderson-Hasselbalch equation. Calculating ph Changes in Buffers A buffer is made by adding 0.30 mole acetic acid and 0.30 mole sodium acetate to enough water to make 1.0 L solution. The ph of the buffer is Calculate the ph of this solution after 0.20 mol of NaOH is added For comparison, calculate the ph that would result if 0.20 mole of NaOH was added to 1.0 Liter of pure water. Practice This Determine The ph of the original buffer described in the problem above after the addition of 0.02 mol HCl o To compare, calculate the ph of the solution what would result from the addition of 0.02 mol HCl to 1.0 L pure water. 4
5 17.3 Titrations Millimole (mmol) = 1/1000 mol Molarity = mmol/ml = mol/l Makes calculations easier because we will rarely add Liters of solution. Adding a solution of known concentration until the substance being tested is consumed. This is called the Graph of ph vs. ml is a Titration Curves Can be used to determine the equivalence point in the titration Can also be used to determine the Ka of a weak acid or the Kb of the weak base being titrated. 3 Kinds of Titrations: Strong acid with Strong Base Do the There is no. They both dissociate completely. The titration of 50.0 ml of M HNO 3 with M NaOH Analyze the ph Graph of Strong Acid with Strong Base (Draw it in) Equivalence at ph 7 4 Regions of Curve 1. determined by the initial concentration of the strong acid. Example: 0.1 M HCl has ph =1 2. Between the : as NaOH added, ph rises slowly at first, then rapidly when it nears the equivalence point. In this case, the ph is determined by how much HCl has not yet been neutralized. 3. : An equal number of moles of NaOH and HCl have reacted, leaving only a solution of their salt, NaCl. ph = 7 because the cation of a strong base and the anion of a strong acid do not hydrolyze and therefore do not affect ph. 4. : ph of the solution is determined by the concentration of the excess NaOH in the solution. 5
6 Sample Problem Calculate the ph when the following quantities of 0.10 M NaOH solution have been added to 50 ml of 0.10 M HCl solution: 49.0 ml 51.0 ml Weak acid with Strong base Four Areas of the Graph: 1. found by calculations involving Ka (Section Between : 1.Consider the neutralization of the acid by OH- to determine [HX] and [X-]. 2. Calculate the ph of this buffer pair (Section 17.2) 3. : The X- ion is a weak base and therefore affects the ph at the equivalence point. >7 4. : ph is determined by the concentration of the excess NaOH. The X- ion is negligible compared to OH- in this titration. Draw the titration curve here: Summary Strong acid and base just stoichiometry. Determine Ka, use for 0 ml base Weak acid before equivalence point Stoichiometry first Then Henderson-Hasselbach Weak acid at equivalence point Kb Weak base after equivalence - leftover strong base. Summary Determine Ka, use for 0 ml acid. Weak base before equivalence point. Stoichiometry first Then Henderson-Hasselbach Weak base at equivalence point Ka. Weak base after equivalence - leftover strong acid. 6
7 Sample Problems Calculate the ph of the solution formed when 45.0 ml of 0.10 M NaOH is added to 50 ml of 0.10 M HC 2 H 3 O 2. Ka = 1.8 E -5. Calulate the ph in the solution formed by adding 10.0 ml of 0.05 M NaOH to 40 ml of M benzoic acid. Ka = 6.3 E -5. Calculate the ph in the solution formed by adding 10 ml of 0.10 M HCl to 20 ml of 0.1 M NH 3. Try these: Calculate the ph at the equivalence point in the titration of 50 ml of 0.1 M acetic acid with 0.1 M sodium hydroxide. Calculate the ph at the equivalence point when 40 ml of M benzoic acid is titrated with 0.05 M NaOH 40 ml of 0.10 M ammonia is titrated with 0.10 M HCl 7
8 Comparison of Curves The ph titration curves for weak acid-strong base titrations differ from those for strong acid-strong base titrations in 3 ways: 1. The solution of the weak acid has a than a solution of a strong acid of the same concentration. 2. The ph change at the rapid-rise portion of the curve near the equivalence point is for the weak acid than it is for the strong acid. 3. The ph at the equivalence point is for the weak acidstrong base titration. Effect of Ka on Curve Use of Indicators Optimally, an indicator would change color at the equivalence point. Not really necessary in practice. ph changes by several units quickly near the equivalence point by a single drop of titrant the indicator needs to change color where the rise is steep. Called its Indicators Weak acids that change color when they become bases. weak acid written Weak base Equilibrium is controlled - when the indicator changes color. Indicators Since it is equilibrium the color change is gradual. It is noticeable when the ratio of [In - ]/[HI] or [HI]/[In - ] is 1/10 Since the Indicator is a weak acid, it has a Ka. ph the indicator changes at is. ph= ph=pka - 1 on the way up Indicators ph= ph=pka+1 on the way down Choose the indicator with a pka at equivalence point if you are titrating with base. Choose the indicator with a pka at equivalence point if you are titrating with acid. 8
9 Titrations of Polyprotic Acids (Draw the general curve here) Solubility Equilibria Will it all dissolve, and if so, how much? All dissolving is an. If there is not much solid it will all dissolve. As more solid is added the solution will become. The solid will precipitate as fast as it dissolves. Equilibrium General equation M + stands for the cation (usually metal). Nm - stands for the anion (a nonmetal). K = But the concentration of a solid doesn t change. K sp = Called the for each compound. Watch out Solubility is not the same as solubility product. Solubility product is an. it doesn t change except with temperature. Solubility is an equilibrium position for how. A common ion can change this. Calculating K sp from Solubility Solid silver chromate is added to pure water at 25 C. Some of the solid remains undissolved at the bottom of the flask. The mixture is stirred for several days to ensure that equilibrium is achieved between the undissolved silver chromate and the solution. Analysis of the equilibrated solution shows that its silver ion concentration is 1.3 E -4M. Assuming that silver chromate completely dissociates in water and that there are no other important equilibria involving the two ions in the solution, calculate the Ksp for the compound. 9
10 Another Practice A saturated solution of magnesium hydroxide in contact with undissolved solid is prepared at 25 C. The ph of the solution is found to be Assuming that magnesium hydroxide dissociates completely in water and that there are no other simultaneous equilibria involving the two ions in the solution, calculate the Ksp for this compound. Calculating Solubility from Ksp The Ksp for calcium fluoride is 3.9 E -11 at 25 C. Assuming that calcium fluoride dissociates completely upon dissolving and that there are no other important equilibria affecting its solubility, calculate the solubility of calcium fluoride in grams per liter. Another Try The Ksp for LaF3 is 2 E -19. What is the solubility of LaF3 in water in moles per liter? 17.5 Factors that Affect Solubility Solubility is not only affected by temperature, but also by the presence of other solutes. There are 3 factors that affect the solubility of ionic compounds: affects both ph and complexing agents. 10
11 Common Ion Effect If we try to dissolve the solid in a solution with either the cation or anion already present less will dissolve. Sample Exercise: Calculate the molar solubility of calcium fluoride at 25 C in a solution that is: (Appendix D shows a Ksp for CaF2 = 3.9 E -11) M in calcium nitrate M in sodium fluoride Practice Some More The value for Ksp for manganese II hydroxide is 1.6 E -13. Calculate the molar solubility of manganese II hydroxide in a solution that contains M NaOH. ph and solubility OH - can be a common ion. More soluble in acid. For other anions if they come from a weak acid they are more soluble in an acidic solution than in water. CaC 2 O 4 H + + C 2 O 4-2 Reduces C 2 O 4-2 in acidic solution. General Rule The solubility of slightly soluble salts containing basic anions increases Carbonates, phosphates, cyanides, sulfides, etc. 11
12 The, the more the solubility is influenced by ph. Salts with anions of negligible basicity (the anions of strong acids) are by ph changes. Predicting the Effect of Acid on Solubility Which of the following substances will be more soluble in acidic solution than in basic solution? Nickel II hydroxide Calcium carbonate Barium fluoride Silver chloride Practice this Write the net ionic equation for the reaction of the following copper (II) compounds with acid: CuS Cu(N3)2 Formation of Complex Ions Metal ions have the ability to act as, (electron pair acceptors), towards water molecules, which act as, (electron pair donors). ions can interact with other molecules, such as NH3. An assembly of a metal ion and the Lewis bases bonded to it, such as Ag(NH3)2 +, is called a. Complex ion Equilibria A charged ion surrounded by. Ligands are Lewis bases using their lone pair to stabilize the. Common ligands are Coordination number is the number of attached ligands. Cu(NH 3 ) 4 +2 has a coordination # of 12
13 Kf the equilibrium constant for the formation of a complex ion. The magnitude of this number indicates the ion s stability. Larger the number, The addition of each ligand has its own equilibrium Usually the ligand is in large excess. And the individual K s will be large so we can treat them as if they go to equilibrium. The complex ion will be the biggest ion in solution. Practice Exercise Calculate the concentration of Ag+ present in solution at equilibrium when concentrated ammonia is added to a M solution of silver nitrate to give an equilibrium concentration of [NH3] = 0.20 M. Neglect the small volume change that occurs when ammonia is added. Try this one Calculate the [Cr +3 ] in equilibrium with Cr(OH)4-1 when mol of chromium III nitrate is dissolved in a liter of solution buffered at ph General Rule: The solubility of metal salts increases in the presence of suitable Lewis bases, such as 13
14 Amphoteric Oxides and Bases Some metal oxides and hydroxides that are relatively insoluble in neutral water dissolve in strongly acidic and strongly basic solutions. Because they themselves act as either an. Include those of 17.6 Precipitation and Separation of Ions Use the, Q, to determine the direction in which a reaction must proceed to reach equilibrium. Precipitation Ion Product, Q = If Q>Ksp a If Q<Ksp. If Q =. Predicting Whether a Precipitate forms Will a precipitate form when 0.10 L of 8 E -3 M lead II nitrate is added to 0.40 L 5 E -3 M sodium sulfate? Will a precipitate form when L of 2.0 E -2 M NaF is mixed with L of 1.0 E -2 M calcium nitrate? Selective Precipitation of Ions Used to separate of metal ions in solutions. Add anions that will only precipitate certain metals at a time. Used to purify mixtures. Sample Problem A solution contains 1.0 E -2 M Ag+ ion and 2.0 E -2 Pb +2 ion. When Cl -1 is added to the solution, both AgCl (Ksp = 1.8 E -10) and PbCl 2 (Ksp = 1.7 E -5) precipitate from the solution. What concentration of Cl -1 is necessary to begin the precipitation of each salt? Which salt precipitates first? 14
15 Try This One A solution consists of M Mg +2 and M Cu +2. Which ion will precipitate first as OH - is added to the solution? What concentration of OH - is necessary to begin the precipitation of each cation? [Ksp = 1.8 E -11 for magnesium hydroxide, and Ksp = 2.2 E -20 for copper II hydroxide] Selective Precipitation Often use because in acidic solution Hg +2, Cd +2, Bi +3, Cu +2, Sn +4 will precipitate. In Basic adding OH - solution S -2 will increase so more soluble sulfides will precipitate. Co+2, Zn +2, Mn +2, Ni +2, Fe +2, Cr(OH) 3, Al(OH) 3 Selective precipitation Alkali metals and NH 4 + remain in solution. Putting it all together A sample of 1.25 L of HCl gas at 21 C and atm is bubbled through L of 0.15 M ammonia solution. Assuming that all the HCl dissolves and that the volume of the solution remains L, calculate the ph of the resulting solution. 15
Chapter 17. Additional Aspects of Equilibrium
Chapter 17. Additional Aspects of Equilibrium Sample Exercise 17.1 (p. 726) What is the ph of a 0.30 M solution of acetic acid? Be sure to use a RICE table, even though you may not need it. (2.63) What
More 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 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 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 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 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 informationChapter 17: Additional Aspects of Aqueous equilibria. Common-ion effect
Chapter 17: Additional Aspects of Aqueous equilibria Learning goals and key skills: Describe the common ion effect. Explain how a buffer functions. Calculate the ph of a buffer solution. Calculate the
More informationName AP CHEM / / Chapter 15 Outline Applications of Aqueous Equilibria
Name AP CHEM / / Chapter 15 Outline Applications of Aqueous Equilibria Solutions of Acids or Bases Containing a Common Ion A common ion often refers to an ion that is added by two or more species. For
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 informationChapter 17. Additional Aspects of Aqueous Equilibria 蘇正寬 Pearson Education, Inc.
Chapter 17 Additional Aspects of Aqueous Equilibria 蘇正寬 chengkuan@mail.ntou.edu.tw Additional Aspects of Aqueous Equilibria 17.1 The Common-Ion Effect 17.2 Buffers 17.3 Acid Base Titrations 17.4 Solubility
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 informationChapter 17 Additional Aspects of
Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 17 Additional Aspects of John D. Bookstaver St. Charles Community College Cottleville,
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 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 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 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 informationSolubility Equilibria
Solubility Equilibria Heretofore, we have investigated gas pressure, solution, acidbase equilibriums. Another important equilibrium that is used in the chemistry lab is that of solubility equilibrium.
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 Aqueous Equilibria. Lecture Presentation. James F. Kirby Quinnipiac University Hamden, CT
Lecture Presentation Chapter 17 Additional Aspects of James F. Kirby Quinnipiac University Hamden, CT Effect of Acetate on the Acetic Acid Equilibrium Acetic acid is a weak acid: CH 3 COOH(aq) H + (aq)
More informationSolubility and Complex-ion Equilibria
Solubility and Complex-ion Equilibria Contents and Concepts Solubility Equilibria 1. The Solubility Product Constant 2. Solubility and the Common-Ion Effect 3. Precipitation Calculations 4. Effect of ph
More informationLecture Presentation. Chapter 16. Aqueous Ionic Equilibrium. Sherril Soman Grand Valley State University Pearson Education, Inc.
Lecture Presentation Chapter 16 Aqueous Ionic Equilibrium Sherril Soman Grand Valley State University The Danger of Antifreeze Each year, thousands of pets and wildlife species die from consuming antifreeze.
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 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 informationWhat is the ph of a 0.25 M solution of acetic acid (K a = 1.8 x 10-5 )?
1 of 17 After completing this chapter, you should, at a minimum, be able to do the following. This information can be found in my lecture notes for this and other chapters and also in your text. Correctly
More informationChemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; Bruce E. Bursten; Catherine J. Murphy.
Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; Bruce E. Bursten; Catherine J. Murphy Chapter 17 Additional Aspects of Aqueous Equilibria Ahmad Aqel Ifseisi Assistant
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 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 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 informationAcid-Base Equilibria and Solubility Equilibria
Acid-Base Equilibria and Solubility Equilibria Acid-Base Equilibria and Solubility Equilibria Homogeneous versus Heterogeneous Solution Equilibria (17.1) Buffer Solutions (17.2) A Closer Look at Acid-Base
More informationMore About Chemical Equilibria
1 More About Chemical Equilibria Acid-Base & Precipitation Reactions Chapter 15 & 16 1 Objectives Chapter 15 Define the Common Ion Effect (15.1) Define buffer and show how a buffer controls ph of a solution
More informationChapter 16 Aqueous Ionic Equilibrium
Chemistry: A Molecular Approach, 1 st Ed. Nivaldo Tro Chapter 16 Aqueous Ionic Equilibrium Roy Kennedy Massachusetts Bay Community College Wellesley Hills, MA 2008, Prentice Hall The Danger of Antifreeze
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 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 informationAdditional Aspects of Aqueous Equilibria David A. Katz Department of Chemistry Pima Community College
Additional Aspects of Aqueous Equilibria David A. Katz Department of Chemistry Pima Community College 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)
More information2/4/2016. Chapter 15. Chemistry: Atoms First Julia Burdge & Jason Overby. Acid-Base Equilibria and Solubility Equilibria The Common Ion Effect
Chemistry: Atoms First Julia Burdge & Jason Overby 17 Acid-Base Equilibria and Solubility Equilibria Chapter 15 Acid-Base Equilibria and Solubility Equilibria Kent L. McCorkle Cosumnes River College Sacramento,
More informationAPPLICATIONS OF AQUEOUS EQUILIBRIA REACTIONS AND EQUILIBRIA INVOLVING ACIDS, BASES, AND SALTS
APPLICATIONS OF AQUEOUS EQUILIBRIA REACTIONS AND EQUILIBRIA INVOLVING ACIDS, BASES, AND SALTS COMMON IONS Common ion effect- The addition of an ion already present(common) in a system causes equilibrium
More informationSOLUBILITY EQUILIBRIA (THE SOLUBILITY PRODUCT)
SOLUBILITY EQUILIBRIA (THE SOLUBILITY PRODUCT) Saturated solutions of salts are another type of chemical equilibria. Slightly soluble salts establish a dynamic equilibrium with the hydrated cations and
More informationChapter 17. Additional Aspects of Aqueous Equilibria. Lecture Presentation. John D. Bookstaver St. Charles Community College Cottleville, MO
Lecture Presentation Chapter 17 Additional Aspects of John D. Bookstaver St. Charles Community College Cottleville, MO The Common-Ion Effect Consider a solution of acetic acid: CH 3 COOH(aq) + H 2 O(l)
More informationAcid - Base Equilibria 3
Acid - Base Equilibria 3 Reading: Ch 15 sections 8 9 Ch 16 sections 1 7 * = important homework question Homework: Chapter 15: 97, 103, 107, Chapter 16: 29*, 33*, 35, 37*, 39*, 41, 43*, 49, 55, 57, 61,
More informationSaturated vs. Unsaturated
Solubility Equilibria in Aqueous Systems K sp (Equilibria of Slightly Soluble Salts, Ionic Compounds) Factors that Affect Solubility (Common Ion Effect, AcidBase Chemistry) Applications of Ionic Equilibria
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 informationCh. 17 Applications of Aqueous Equilibria: Buffers and Titrations
Ch. 17 Applications of Aqueous Equilibria: Buffers and Titrations Sec 1 The Common-Ion Effect: The dissociation of a weak electrolyte decreases when a strong electrolyte that has an ion in common with
More informationSolubility and Complex-ion Equilibria
Solubility and Complex-ion Equilibria Solubility Equilibria Many natural processes depend on the precipitation or dissolving of a slightly soluble salt. In the next section, we look at the equilibria of
More informationLearning Objectives. Solubility and Complex-ion Equilibria. Contents and Concepts. 3. Precipitation Calculations. 4. Effect of ph on Solubility
Solubility and Comple-ion Equilibria. Solubility and the Common-Ion Effect a. Eplain how the solubility of a salt is affected by another salt that has the same cation or anion. (common ion) b. Calculate
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 informationChapter 17 Additional Aspects of
Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 17 Additional Aspects of AP Chemistry 2014-15 North Nova Education Centre Mr. Gauthier
More informationChapter 17 Additional Aspects of
Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 17 Additional Aspects of John D. Bookstaver St. Charles Community College Cottleville,
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 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 informationCHEMISTRY 1102 NOTES ZUMDAHL CHAPTER 15 - APPLICATIONS OF AQUEOUS EQUILIBRIA
CHEMISTRY 1102 NOTES ZUMDAHL CHAPTER 15 - APPLICATIONS OF AQUEOUS EQUILIBRIA The introduction refers to the formation of stalactites and stalagmites as an example of the material in this chapter: CO 2
More informationConsider a normal weak acid equilibrium: Which direction will the reaction shift if more A is added? What happens to the % ionization of HA?
ch16blank Page 1 Chapter 16: Aqueous ionic equilibrium Topics in this chapter: 1. Buffers 2. Titrations and ph curves 3. Solubility equilibria Buffersresist changes to the ph of a solution. Consider a
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 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 information(Label the Conjugate Pairs) Water in the last example acted as a Bronsted-Lowry base, and here it is acting as an acid. or
Chapter 16 - Acid-Base Equilibria Arrhenius Definition produce hydrogen ions in aqueous solution. produce hydroxide ions when dissolved in water. Limits to aqueous solutions. Only one kind of base. NH
More informationChapter 4; Reactions in Aqueous Solutions. Chapter 4; Reactions in Aqueous Solutions. V. Molarity VI. Acid-Base Titrations VII. Dilution of Solutions
Chapter 4; Reactions in Aqueous Solutions I. Electrolytes vs. NonElectrolytes II. Precipitation Reaction a) Solubility Rules III. Reactions of Acids a) Neutralization b) Acid and Carbonate c) Acid and
More informationChapter 16. Solubility and Complex Ion Equilibria
Chapter 16 Solubility and Complex Ion Equilibria Section 16.1 Solubility Equilibria and the Solubility Product Solubility Equilibria Solubility product (K sp ) equilibrium constant; has only one value
More informationChem 103 Exam #1. Identify the letter of the choice that best completes the statement or answers the question. Multiple Choice
Chem 103 Exam #1 Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. Which of the following can act as a Bronsted-Lowry base, but not as a Bronsted-Lowry
More 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 informationUnit 4a: Solution Stoichiometry Last revised: October 19, 2011 If you are not part of the solution you are the precipitate.
1 Unit 4a: Solution Stoichiometry Last revised: October 19, 2011 If you are not part of the solution you are the precipitate. You should be able to: Vocabulary of water solubility Differentiate between
More informationCHAPTER FIFTEEN APPLICATIONS OF AQUEOUS EQUILIBRIA. For Review
CHAPTER FIFTEEN APPLICATIONS OF AQUEOUS EQUILIBRIA For Review 1. A common ion is an ion that appears in an equilibrium reaction but came from a source other than that reaction. Addition of a common ion
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 informationChem 1A Dr. White Fall Handout 4
Chem 1A Dr. White Fall 2014 1 Handout 4 4.4 Types of Chemical Reactions (Overview) A. Non-Redox Rxns B. Oxidation-Reduction (Redox) reactions 4.6. Describing Chemical Reactions in Solution A. Molecular
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 informationChapter 15. Acid-Base Equilibria
Chapter 15 Acid-Base Equilibria The Common Ion Effect The common-ion effect is the shift in an ionic equilibrium caused by the addition of a solute that provides an ion already involved in the equilibrium
More informationIonic Equilibria in Aqueous Systems
Ionic Equilibria in Aqueous Systems Chapter Nineteen AP Chemistry There are buffers in our blood that keep the ph of our blood at a constant level. The foods that we eat are often acidic or basic. This
More informationThe ph of aqueous salt solutions
The ph of aqueous salt solutions Sometimes (most times), the salt of an acid-base neutralization reaction can influence the acid/base properties of water. NaCl dissolved in water: ph = 7 NaC 2 H 3 O 2
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 informationApplications of Aqueous Equilibrium Chapter 15. Common Ion Effect & Buffers Sections 1-3
Applications of Aqueous Equilibrium Chapter 15 Common Ion Effect & Buffers Sections 1-3 Solutions of Acids or Bases Containing a Common Ion NaF Na + + F - HF H + + F - What effect does the NaF have on
More informationChapter 16. Equilibria in Aqueous Systems
Chapter 16 Equilibria in Aqueous Systems Buffers! buffers are solutions that resist changes in ph when an acid or base is added! they act by neutralizing the added acid or base! but just like everything
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 informationCHAPTER 4 TYPES OF CHEMICAL REACTIONS & SOLUTION STOICHIOMETRY
Advanced Chemistry Name Hour Advanced Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 4 TYPES OF CHEMICAL REACTIONS & SOLUTION STOICHIOMETRY Day Plans
More 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 informationAP Chemistry Note Outline Chapter 4: Reactions and Reaction Stoichiometry:
AP Chemistry Note Outline Chapter 4: Reactions and Reaction Stoichiometry: Water as a solvent Strong and Weak Electrolytes Solution Concentrations How to Make up a solution Types of Reactions Introduction
More information1. Hydrochloric acid is mixed with aqueous sodium bicarbonate Molecular Equation
NAME Hr Chapter 4 Aqueous Reactions and Solution Chemistry Practice A (Part 1 = Obj. 1-3) (Part 2 = Obj. 4-6) Objective 1: Electrolytes, Acids, and Bases a. Indicate whether each of the following is strong,
More 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 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 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 informationChapter 4. The Major Classes of Chemical Reactions 4-1
Chapter 4 The Major Classes of Chemical Reactions 4-1 The Major Classes of Chemical Reactions 4.1 The Role of Water as a Solvent 4.2 Writing Equations for Aqueous Ionic Reactions 4.3 Precipitation Reactions
More 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 informationSolubility Equilibria. Dissolving a salt... Chem 30S Review Solubility Rules. Solubility Equilibrium: Dissociation = Crystalization
Chem 30S Review Solubility Rules Solubility Equilibria Salts are generally more soluble in HOT water(gases are more soluble in COLD water) Alkali Metal salts are very soluble in water. NaCl, KOH, Li 3
More information1002_2nd Exam_
1002_2nd Exam_1010418 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) How will addition of sodium acetate to an acetic acid solution affect the
More informationAP Chemistry Unit #4. Types of Chemical Reactions & Solution Stoichiometry
AP Chemistry Unit #4 Chapter 4 Zumdahl & Zumdahl Types of Chemical Reactions & Solution Stoichiometry Students should be able to: Predict to some extent whether a substance will be a strong electrolyte,
More informationName Date Class ACID-BASE THEORIES
19.1 ACID-BASE THEORIES Section Review Objectives Define the properties of acids and bases Compare and contrast acids and bases as defined by the theories of Arrhenius, Brønsted-Lowry, and Lewis Vocabulary
More informationChemical Equilibrium
Chemical Equilibrium THE NATURE OF CHEMICAL EQUILIBRIUM Reversible Reactions In theory, every reaction can continue in two directions, forward and reverse Reversible reaction! chemical reaction in which
More informationStoichiometry: Chemical Calculations. Chemistry is concerned with the properties and the interchange of matter by reaction i.e. structure and change.
Chemistry is concerned with the properties and the interchange of matter by reaction i.e. structure and change. In order to do this, we need to be able to talk about numbers of atoms. The key concept is
More informationSOLUBILITY PRODUCT (K sp ) Slightly Soluble Salts & ph AND BUFFERS (Part Two)
SOLUBILITY PRODUCT (K sp ) Slightly Soluble Salts & ph AND BUFFERS (Part Two) ADEng. PRGORAMME Chemistry for Engineers Prepared by M. J. McNeil, MPhil. Department of Pure and Applied Sciences Portmore
More informationChapter 6. Types of Chemical Reactions and Solution Stoichiometry
Chapter 6 Types of Chemical Reactions and Solution Stoichiometry Chapter 6 Table of Contents (6.1) (6.2) (6.3) (6.4) (6.5) (6.6) (6.7) (6.8) Water, the common solvent The nature of aqueous solutions: Strong
More informationChemical Equilibrium
Chemical Equilibrium Many reactions are reversible, i.e. they can occur in either direction. A + B AB or AB A + B The point reached in a reversible reaction where the rate of the forward reaction (product
More informationChapter 4 Reactions in Aqueous Solution
Chapter 4 Reactions in Aqueous Solution Homework Chapter 4 11, 15, 21, 23, 27, 29, 35, 41, 45, 47, 51, 55, 57, 61, 63, 73, 75, 81, 85 1 2 Chapter Objectives Solution To understand the nature of ionic substances
More 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 informationSolubility Equilibria
Chapter 17 SOLUBILITY EQUILIBRIA (Part II) Dr. Al Saadi 1 Solubility Equilibria The concept of chemical equilibrium helps to predict how much of a specific ionic compound (salt) will dissolve in water.
More informationChapter 16. Acid-Base Equilibria
Chapter 16 Acid-Base Equilibria Arrhenius Definition Acids produce hydrogen ions in aqueous solution. Bases produce hydroxide ions when dissolved in water. Limits to aqueous solutions. Only one kind of
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 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 informationEquilibrium principles in aqueous systems are limited to qualitative descriptions and/or calculations involving:
NCEA Chemistry 3.6 Aqueous Systems AS 91392 Demonstrate understanding of equilibrium principles in aqueous systems Aqueous systems are limited to those involving sparingly soluble ionic solids Equilibrium
More informationModified Dr. Cheng-Yu Lai
Ch16 Aqueous Ionic Equilibrium Solubility and Complex Ion Equilibria Lead (II) iodide precipitates when potassium iodide is mixed with lead (II) nitrate Modified Dr. Cheng-Yu Lai Solubility-product constant
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 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 informationMake a mixture of a weak acid and its conjugate base (as the SALT) Make a mixture of a weak base and its conjugate acid (as the SALT)
175 BUFFERS - resist ph change caused by either the addition of strong acid/base OR by dilution Made in one of two ways: Make a mixture of a weak acid and its conjugate base (as the SALT) Make a mixture
More informationAcid-Base Equilibria. 1.NH 4 Cl 2.NaCl 3.KC 2 H 3 O 2 4.NaNO 2. Acid-Ionization Equilibria. Acid-Ionization Equilibria
Acid-Ionization Equilibria Acid-Base Equilibria Acid ionization (or acid dissociation) is the reaction of an acid with water to produce hydronium ion (hydrogen ion) and the conjugate base anion. (See Animation:
More information