Chem 1102 Semester 1, 2011 ACIDS AND BASES
|
|
- Amelia Melton
- 6 years ago
- Views:
Transcription
1 Chem 1102 Semester 1, 2011 ACIDS AND BASES
2 Acids and Bases Lecture 23: Weak Acids and Bases Calculations involving pk a and pk b Strong Acids and Bases Lecture 24: Polyprotic Acids Salts of Acids and Bases Buffers Indicators Titrations
3 Polyprotic Acids Monoprotic acids: donate only a single proton to water Diprotic: can donate two protons. Polyprotic: can donate more than two protons. H 3 PO 4(aq) #H + (aq) + H 2 PO 4 (aq) #pk a1 = 2.2 # H 2 PO 4 (aq) #H + (aq) + HPO 4 2 (aq) #pk a2 = 7.2 # HPO 4 2 (aq) #H + (aq) + PO 4 3 (aq) # #pk a3 = 12.4 # removing more protons is harder: increasing pk a = decreasing K a : K a1 > K a2 > K a3 # reason: harder to remove +ve charge against increasing ve charge.# large difference in pk a values: only need to consider one equilibrium at a time (simplifies maths).#
4 pk a1 = 2.2 pk a2 = 7.2 pk a3 = 12.4 pk a1 =3.13, pk a2 = 4.76, pk a3 =6.40.
5
6 Hydrolysis of Ions: Examples Is a solution of NaCN acidic or basic? Does a solution of NH 4 Cl have ph > 7 or < 7?
7 Salt of a Weak Acid & Weak Base What is the ph of ammonium acetate at 25 C? 2 possible reactions are: CH 3 COO (aq) + H 2 O(l) CH 3 COOH(aq) + OH (aq) K b = Anions of weak acids hydrolyse OH Basic effect NH 4+ (aq) + H 2 O(l) NH 3 (aq) + H 3 O + (aq) K a = =5.5 x Cations of weak bases hydrolyse H 3 O + Acid effect In this case K a = K b, so salt is neutral. Also: salts of strong acids & strong bases are always neutral!
8 If K a = K b, then ph = 7 and solu5on is neutral If K a > K b, then ph < 7 and solu5on is acidic (A salt formed between a strong acid and a weak base is an acid salt, e.g. NH 4 Cl) If K a < K b, then ph > 7 and solu5on is basic (A salt formed between a weak acid and a strong base is a basic salt, e.g. NaCH 3 COO) Ions of Neutral Salts Cations Na + K + Rb + Cs + Mg 2+ Ca 2+ Sr 2+ Ba 2+ Anions Cl - Br - I -, ClO 4 - BrO 4 - ClO 3 - NO 3 - Acidic Ions NH 4 + Al 3+ Pb 2+ Sn 2+ Transition metal ions HSO 4 - H 2 PO 4 - Basic Ions F - C 2 H 3 O 2 - NO 2 - HCO 3 - CN - CO 3 2- S 2- SO 4 2- HPO 4 2- PO 4 3-
9 Another Example Rank the following 1.0 M solutions in order of decreasing ph. HNO 3 NaCN KOH HCl CH 3 COOH
10 The Common Ion Effect If you add the salt of a weak acid to a solution of the same acid then the equilibrium will shift towards neutral ph.# CH 3 COOH (aq) + H 2 O (l) CH 3 COO (aq) + H 3 O+ (aq) Addition of CH 3 COO Na + will raise [CH 3 COO ]. From Le Châtelier s principle, the first equilibrium will shift to the left to remove CH 3 COO and therefore decrease [H 3 O + ].!The same holds true for a base: If you add the salt of a weak base to a solution of the same base then the equilibrium will shift towards neutral ph.#
11 Buffers A solution containing both:# a weak acid + its salt# OR# a weak base + its salt# withstands ph changes when (limited) amounts of acid or base are added.# Reason: Le Châtelierʼs principle.#
12 ph Change and Buffers Consider change in ph of pure water (ph = 7) if we add an equal amount of 10 3 M HCl: ##[H 3 O + ] = 5 x 10 4 M (can neglect amount already present in water), so ph drops from 7 to 3.3! ## # # A whopping change! What about buffer solutions?
13 ph Change and Buffers The addition of small amounts of acid or base to a buffer solution will result in a negligible change to the ph. Why? Buffer after addition of H 3 O + # Buffer with equal concentrations of conjugate base and acid # Buffer after addition of OH -# CH 3 COO -# CH 3 COOH # H 3 O +# CH 3 COO -# CH 3 COOH # OH -# CH 3 COO -# CH 3 COOH # H 3 O + + CH 3 COO - H 2 O + CH 3 COOH# CH 3 COOH + OH - H 2 O + CH 3 COO -#
14 Henderson-Hasselbalch Equation For a buffer solution, which contains similar concentrations of a conjugate acid/base pair of a weak acid:# Since the dissociation of HA or protonation of A doesnʼt lead to a significant change in the concentrations of these species:# Rearranging:#
15 Buffer Preparation and Capacity Buffer Preparation If the ph of a required buffer = pk a of available acid then use equimolar amounts of acid and conjugate base. If the required ph differs from the pk a then use the Henderson- Hasselbalch equation to work out ratios of acid and conjugate base.
16 Buffer Preparation and Capacity Buffer capacity is a measure of the ability of a buffer to resist ph change and depends on both the absolute and relative component concentrations. Buffer range is the ph range over which the buffer acts effectively. Buffer capacity is related to the amount of strong acid or base that can be added without causing significant ph change. Depends on amount of acid & conjugate base in solution: - Highest capacity when [HA] and [A ] are large. - Highest capacity when [HA] [A ] (most effective buffers have acid/ base ratio less than 10 and more than 0.1 ph range is ±1).
17 Buffer Example In the H 3 PO 4 / NaH 2 PO 4 / Na 2 HPO 4 / Na 3 PO 4 system, how could you make up a buffer with a ph of 7.40? (K a1 = 7.2 x 10 3, K a2 = 6.3 x 10 8, K a3 = 4.2 x ) To make up a buffer, we need ph ~ pk a pk a1 = 2.14 pk a2 = 7.20 pk a3 = must use mixture of H 2 PO 4 and HPO 2 4 Simply use the Henderson-Hasselbalch equation...
18 Buffer Example cont d ph = pk a2 + log 10 [HPO 4 2 ] [H 2 PO 4 ] original amounts 7.40 = log 10 [HPO 4 2 ] [H 2 PO 4 ] [HPO 4 2 ] [H 2 PO 4 ] = = 1.58 So the required ratio of Na 2 HPO 4 to NaH 2 PO 4 = 1.58:1
19 Buffers in Natural Systems Biological systems, e.g. blood, contain buffers: ph control essential because biochemical reactions are very sensitive to ph.# Human blood is slightly basic, ph # In a healthy person, blood ph is never more than 0.2 ph units from its average value.# ph < 7.2, acidosis ; ph > 7.6, alkalosis.# Death if ph < 6.8 or > 7.8.#
20 Buffer System in Blood Extracellular buffer (outside cell)# H + (aq) + HCO 3 (aq) H 2 CO 3(aq) H 2 CO 3(aq)# H 2 O (l) + CO 2(g)# Removal of CO 2 shifts equilibria to right, reducing [H 3 O + ], i.e. raising the ph.# The ph can be reduced by:# H 2 CO 3(aq) + H 2 O (l) HCO 3 (aq) + H 3 O + (aq)#
21 Acid-Base Titrations Equivalence Point, is the point at which the number of moles of added base = original number of moles of acid.# Strong acid/strong base ph = 7# Weak acid/strong base ph > 7# Strong acid/weak base ph < 7! End Point:#!When a colour change in the indicator is observed.! Always choose an indicator that changes colour close to the equivalence point#
22 Indicators weak acid base# Each form has a different colour # The ph at which acid base depends on the pk a of the indicator.
23 Titrations: Strong Acid / Strong Base Equivalence point at ph 7#
24 Titrations: Weak Acid / Strong Base Equivalence point ph > 7# (ph value depends on starting# concentrations)# ph change is more gradual#
25 Titrations: Weak Base / Strong Acid Equivalence point ph < 7# ph value depends on starting # concentrations#
26 What is the ph of a 0.10 M solu5on of NH 4 Br, if the pk b of NH 3 is 4.74?
Unless otherwise stated, all images in this file have been reproduced from:
Unless otherwise stated, all images in this file have been reproduced from: Blackman, Bottle, Schmid, Mocerino and Wille, Chemistry, 3 rd Edition 2016 (John Wiley & Sons) The University of Sydney Page
More informationLecture 12. Acid/base reactions. Equilibria in aqueous solutions.
Lecture 12 Acid/base reactions. Equilibria in aqueous solutions. Titrations Kotz 7 th ed. Section 18.3, pp.821-832. In a titration a solution of accurately known concentration is added gradually added
More informationBuffer Solutions. Buffer Solutions
Buffer Solutions A buffer solution is comprised of a mixture of an acid (base) with its conjugate base (acid) that resists changes in ph when additional acid or base is added The Henderson-Hasselbalch
More informationAcid Base Equilibria
Acid Base Equilibria Acid Ionization, also known as acid dissociation, is the process in where an acid reacts with water to produce a hydrogen ion and the conjugate base ion. HC 2 H 3 O 2(aq) H + (aq)
More informationKotz 7 th ed. Section 18.3, pp
Lecture 15 Acid/base reactions. Equilibria in aqueous solutions. Titrations Kotz 7 th ed. Section 18.3, pp.821-832. In a titration a solution of accurately known concentration is added gradually added
More informationAcids and bases, ph and buffers. Dr. Mamoun Ahram Lecture 2
Acids and bases, ph and buffers Dr. Mamoun Ahram Lecture 2 ACIDS AND BASES Acids versus bases Acid: a substance that produces H+ when dissolved in water (e.g., HCl, H2SO4) Base: a substance that produces
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 informationCHAPTER 8: ACID/BASE EQUILIBRIUM
CHAPTER 8: ACID/BASE EQUILIBRIUM Already mentioned acid-base reactions in Chapter 6 when discussing reaction types. One way to define acids and bases is using the Brønsted-Lowry definitions. A Brønsted-Lowry
More informationIB Chemistry ABS Introduction An acid was initially considered a substance that would produce H + ions in water.
IB Chemistry ABS Introduction An acid was initially considered a substance that would produce H + ions in water. The Brønsted-Lowry definition of an acid is a species that can donate an H + ion to any
More 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 information5.111 Lecture Summary #22 Wednesday, October 31, 2014
5.111 Lecture Summary #22 Wednesday, October 31, 2014 Reading for Today: Sections 11.13, 11.18-11.19, 12.1-12.3 in 5 th ed. (10.13, 10.18-10.19, 11.1-11.3 in 4 th ed.) Reading for Lecture #23: Sections
More informationAcid-Base Character of Salt Solutions. Cations. Cations are potentially acidic, but some have no effect on ph.
Acid-Base Character of Salt Solutions The ph of a salt solution will depend on the acidbase nature of both the cation and anion. Cations Cations are potentially acidic, but some have no effect on ph. M(H
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 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 informationPreparation of different buffer solutions
Preparation of different buffer solutions 1 - Buffers: - All biochemical reactions occur under strict conditions of the concentration of hydrogen ion. - Biological life cannot withstand large changes in
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 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 informationLast week, we discussed the Brønsted Lowry concept of acids and bases. According to this model:
Last week, we discussed the Brønsted Lowry concept of acids and bases This model is not limited to aqueous solutions; it can be extended to reactions in the gas phase! According to this model: Acids are
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 informationK w. Acids and bases 8/24/2009. Acids and Bases 9 / 03 / Ionization of water. Proton Jumping Large proton and hydroxide mobility
Chapter 2 Water Acids and Bases 9 / 03 / 2009 1. How is the molecular structure of water related to physical and chemical behavior? 2. What is a Hydrogen Bond? 3Wh 3. What are Acids Aid and db Bases? 4.
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 informationK A K B = K W pk A + pk B = 14
Relationship between the ionization constants of an acid and its conjugate base HCN (aq) H 2 O(l) CN (aq) H O (aq) Conjugate couple The product between of an acid and of its conjugate base is : p p 14
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 informationCHAPTER 7 Acid Base Equilibria
1 CHAPTER 7 Acid Base Equilibria Learning Objectives Acid base theories Acid base equilibria in water Weak acids and bases Salts of weak acids and bases Buffers Logarithmic concentration diagrams 2 ACID
More informationDr. Diala Abu-Hassan, DDS, PhD Lecture 3 MD summer 2014
ph, DDS, PhD Dr.abuhassand@gmail.com Lecture 3 MD summer 2014 www.chem4kids.com 1 Outline ph Henderson-Hasselbalch Equation Monoprotic and polyprotic acids Titration 2 Measuring the acidity of solutions,
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 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 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 informationAcid-Base Equilibria. And the beat goes on Buffer solutions Titrations
Acid-Base Equilibria And the beat goes on Buffer solutions Titrations 1 Common Ion Effect The shift in equilibrium due to addition of a compound having an ion in common with the dissolved substance. 2
More informationAcid-Base Solutions - Applications
Acid-Base Solutions - Applications 1 The Common Ion Effect Consider the equilibrium established when acetic acid, HC 2 H 3 O 2, is added to water. CH 3 COOH(aq) + H 2 O(l) CH 3 COO - (aq) + H 3 O + (aq)
More informationAcid-Base Equilibria. 1.NH 4 Cl 2.NaCl 3.KC 2 H 3 O 2 4.NaNO 2. Solutions of a Weak Acid or Base
Acid-Base Equilibria 1 Will the following salts be acidic, basic or neutral in aqueous solution? 1.NH 4 Cl.NaCl.KC H O 4.NaNO A = acidic B = basic C = neutral Solutions of a Weak Acid or Base The simplest
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 informationLECTURE #25 Wed. April 9, 2008
CHEM 206 section 01 LECTURE #25 Wed. April 9, 2008 LECTURE TOPICS: TODAY S CLASS: 18.1-18.2 NEXT CLASS: finish Ch.18 (up to 18.5) (1) 18.1 The Common Ion Effect basis of all Ch.18 = shift in eqm position
More informationAcid-Base Equilibria. Contents and Concepts. Learning Objectives
Acid-Base Equilibria Contents and Concepts Solutions of a Weak Acid or Base 1. Acid-Ionization Equilibria. Polyprotic Acids 3. Base-Ionization Equilibria 4. Acid Base Properties of Salt Solutions Solutions
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 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 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 2 Acids and Bases
Unit 2 Acids and Bases 1 Topics Properties / Operational Definitions Acid-Base Theories ph & poh calculations Equilibria (Kw, K a, K b ) Indicators Titrations STSE: Acids Around Us 2 Operational Definitions
More informationChapter 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 informationCh 15, Applications of Aq Equilibria
Ch 15, Applications of Aq Equilibria We will focus on 3 areas: 1) buffers (incl. Henderson-Hasselbalch Transformation) 2) titrations 3) solubility equilibria 1 I. Neutralization Reactions A. Strong acid-strong
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 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 informationProblem 1 C 6 H 5 [ COOH C 6 H[H 5 COO + ] - + H [ I C - x + x + x E x x x
Problem 1 What is the ph of a 291mL sample of 2.993M benzoic acid (C 6 H 5 COOH) (K a =6.4x10 5 )? Write out acid dissociation reaction: C 6 H 5 COOH C 6 H 5 COO H Make an ICE chart since this is a weak
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 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 informationx x10. Hydromiun ion already in solution before acid added. NH 3 /NH4+ buffer solution
10/15/01 Commonion effect In the last chapter, we calculated the [H 3 O ] of a M O as 6.010 5 M. The percent dissociation for this solution would be: More Acid and Base Chemistry 6.010 5 100 0.089% [H
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 informationCHEMISTRY Matter and Change
CHEMISTRY Matter and Change UNIT 18 Table Of Contents Section 18.1 Introduction to Acids and Bases Unit 18: Acids and Bases Section 18.2 Section 18.3 Section 18.4 Strengths of Acids and Bases Hydrogen
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 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 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 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 informationApplications of Aqueous Equilibria. Chapter 18
Applications of Aqueous Equilibria Chapter 18 What we learn from Chap 18 This chapter is the third in the three-chapter sequence about equilibrium, this one building upon the core principles raised in
More informationph and buffers Dr. Mamoun Ahram Summer, 2018
ph and buffers Dr. Mamoun Ahram Summer, 2018 Kw Kw is called the ion product for water What is ph? Example: Find the K a of a 0.04 M weak acid HA whose [H + ] is 1 x 10-4? HA H + + A - K a = [A - ] [H
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 informationLecture #11-Buffers and Titrations The Common Ion Effect
Lecture #11-Buffers and Titrations The Common Ion Effect The Common Ion Effect Shift in position of an equilibrium caused by the addition of an ion taking part in the reaction HA(aq) + H2O(l) A - (aq)
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 informationcapable of neutralizing both acids and bases
Buffers Buffer n any substance or mixture of compounds that, added to a solution, is capable of neutralizing both acids and bases without appreciably changing the original acidity or alkalinity of the
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 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 information[H ] [OH ] 5.6 " 10
Howemork set solutions 10: 11.1 Table 11.5 of the tet contains a list of important Brønsted acids and bases. (a) both, base, (c) acid, (d) base, (e) acid, (f) base, (g) base, (h) base, (i) acid, (j) acid.
More informationChapter 17 Answers. Practice Examples [H3O ] 0.018M, 1a. HF = M. 1b. 30 drops. 2a.
Chapter 17 Answers Practice Examples 1a. + [HO ] 0.018M, 1b. 0 drops [HF] = 0.8 M. [H O + ] = 0.10 M, HF = 0.97 M. a. + HO 1.10 M, CHO = 0.150 M. b. 15g NaCHO a. The hydronium ion and the acetate ion react
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 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 informationWhat we learn from Chap 18
Applications of Aqueous Equilibria Chapter 18 What we learn from Chap 18 18.2 This chapter is the third in the three-chapter sequence about equilibrium, this one building upon the core principles raised
More informationBuffer Calculations. The Standard Equilibrium Approach to Calculating a Buffer s ph
Buffer Calculations A buffer is a solution that has the ability to resist a change in ph upon the addition of a strong acid or a strong base. For a buffer to exist it must satisfy two conditions: (1) the
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 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 informationLecture 10. Professor Hicks Inorganic Chemistry II (CHE152) Scale of [H 3 O + ] (or you could say [H + ]) concentration
Lecture 10 Professor Hicks Inorganic Chemistry II (CHE152) ph Scale of [H 3 O + ] (or you could say [H + ]) concentration More convenient than scientific notation ph = log [H 3 O + ] still not sure? take
More 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 information+(aq) + Cl - (aq) HA(aq) A - (aq) + H + (aq) CH 3COO - (aq) + H + (aq)
1 A2 Chemistry: F325 Equilibria, Energetics and Elements 5.1.3 Acids, Bases and Buffers. Lesson 6 Buffer Solutions. Learning Outcomes: All Describe what is meant by the term buffer solution (5.1.3 k) Explain
More informationChapter 15. Titration Curves for Complex Acid/Base Systems
Chapter 15 Titration Curves for Complex Acid/Base Systems Polyfunctional acids and bases Carbonic acid/bicarbonate buffer system Buffers for human blood ph = 7.35-7.45 CO 2(g) + H 2 O H 2 CO 3(aq) H 2
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 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 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 informationAcids, Bases and the Common Ion Effect. More quantitative. Continued [F - ] = M. Consider the following acid equilibrium of a weak acid:
Acids, Bases and the Common Ion Effect Consider the following acid equilibrium of a weak acid: HF + H O H 3 O + + F - K a = [H 3 O + ][F - ] [HF] By LeChatelier s principle, we predict the HF dissociation
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 information*In every acid-base reaction, equilibrium favors transfer of a proton from the stronger acid to the stronger base.
16.2 Bronsted-Lowry Acids and Bases An acid is a substance that can transfer a proton to another substance. A base is a substance that can accept a proton. A proton is a hydrogen ion, H +. Proton transfer
More informationChapter 13 Acids and Bases
William L Masterton Cecile N. Hurley http://academic.cengage.com/chemistry/masterton Chapter 13 Acids and Bases Edward J. Neth University of Connecticut Outline 1. Brønsted-Lowry acid-base model 2. The
More information1) Write the Brønsted-Lowry reaction for weak acid HCN reacting with H 2 O.
1) Write the Brønsted-Lowry reaction for weak acid HCN reacting with H O. HCN + H O º H O + + CN ) Write the Brønsted-Lowry reaction for weak base NH reacting with H O NH + H O º OH + NH + ) Using the
More informationacid : a substance which base : a substance which H +
4.4. BronstedLowry Theory of A&B acid : a substance which base : a substance which H Typical BronstedLowry AB rxn eqn: eg1) NH 3 H 2 O NH 4 base acid OH eg2) CH 3 COOH H 2 O CH 3 COO H 3 O H 2 O an acid
More informationStrong acids and bases
h.8 & 9 Systematic Treatment of Equilibrium & Monoprotic Acid-base Equilibrium Strong acids and bases.0 onc. (M) ph 0..0 -.0.0-5 5.0.0-8 8.0? We have to consider autoprotolysis of water: H O Kw OH - H
More informationChapter 15, Applications of Aqueous Equilibria
Chapter 15, Applications of Aqueous Equilibria We will focus on 3 areas: 1) titrations 2) buffers (incl. the Henderson- Hasselbalch Transformation), 3) solubility equilibria. 1 I. Neutralization Reactions
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 information10/16/17 ACIDS AND BASES, DEFINED WATER IS AMPHOTERIC OUTLINE. 9.1 Properties of Acids and Bases. 9.2 ph. 9.3 Buffers
ACIDS AND BASES, DEFINED A hydrogen atom contains a proton and an electron, thus a hydrogen ion (H + ) is a proton: Acids: Proton (H + ) transfer between molecules is the basis of acid/base chemistry Ø
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 informationChem 112, Fall 05 Exam 3A
Before you begin, make sure that your exam has all 10 pages. There are 32 required problems (3 points each, unless noted otherwise) and two extra credit problems (3 points each). Stay focused on your exam.
More informationChapter 16: Applications of Aqueous Equilibrium Part 2. Acid-Base Titrations
Chapter 16: Applications of Aqueous Equilibrium Part 2 Acid-Base Titrations When you add an acid and a base together, a neutralization rxn occurs. In the lab, we do neutralization rxns all the time as
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 informationPart 01 - Assignment: Introduction to Acids &Bases
Part 01 - Assignment: Introduction to Acids &Bases Classify the following acids are monoprotic, diprotic, or triprotic by writing M, D, or T, respectively. 1. HCl 2. HClO4 3. H3As 4. H2SO4 5. H2S 6. H3PO4
More 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 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 informationChem Chapter 18: Sect 1-3 Common Ion Effect; Buffers ; Acid-Base Titrations Sect 4-5 Ionic solubility Sect 6-7 Complex Formation
Chem 106 3--011 Chapter 18: Sect 1-3 Common Ion Effect; Buffers ; Acid-Base Titrations Sect 4-5 Ionic solubility Sect 6-7 Complex Formation 3//011 1 The net ionic equation for the reaction of KOH(aq) and
More informationAP Chemistry: Acid-Base Chemistry Practice Problems
Name AP Chemistry: Acid-Base Chemistry Practice Problems Date Due Directions: Write your answers to the following questions in the space provided. For problem solving, show all of your work. Make sure
More informationBrønsted-Lowry Acid-Base Model. Chapter 13 Acids and Bases. The Nature of H + Outline. Review from Chapter 4. Conjugate Pairs
Brønsted-Lowry Acid-Base Model William L Masterton Cecile N. Hurley Edward J. Neth cengage.com/chemistry/masterton Chapter 13 Acids and Bases Brønsted-Lowry Johannes Brønsted (1879-1947) Thomas Lowry (1874-1936)
More information( 1 ) Concept of acid / base
Section 6.2 Ionic Equilibrium Unit 628 ( 1 ) Concept of acid / base The best definition of acids and bases is that proposed by T.M. Lowry and also, independently by J.N. Bronsted in 1923. BronstedLowry
More informationIn the Brønsted-Lowry system, a Brønsted-Lowry acid is a species that donates H + and a Brønsted-Lowry base is a species that accepts H +.
16.1 Acids and Bases: A Brief Review Arrhenius concept of acids and bases: an acid increases [H + ] and a base increases [OH ]. 16.2 BrønstedLowry Acids and Bases In the BrønstedLowry system, a BrønstedLowry
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 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 information