CHAPTER 7 Acid Base Equilibria
|
|
- Marylou Hines
- 5 years ago
- Views:
Transcription
1 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 2 ACID BASE THEORIES Arrhenius theory: H + and OH Theory of solvent systems: solvent cations and anions Brønsted-Lowry theory: taking and giving protons (conjugate pairs) Lewis theory: taking and giving electrons In general: Acid is a substance that increases the concentration of H 3 O + (hydronium ion). Conversely, a base decreases the concentration of H 3 O + in aqueous solution. A more general definition of acids and bases given by Brønsted and Lowry is that an acid is a proton donor and a base is a proton acceptor.
3 3 ACID BASE EQUILIBRIA IN WATER Hydrochloric acid is a strong acid, and in water, its ionization is complete: Acetic acid is a weak acid, which ionizes only partially in water (a few percent): We can write an equilibrium constant for this reaction:
4 4 ACID BASE EQUILIBRIA IN WATER Pure water ionizes slightly, or undergoes autoprotolysis: The equilibrium constant for this is
5 5 THE ph SCALE ph = - Log [H + ] In general, panything = log Anything, and it is a mathematical function to express the very low quantities.
6 6 THE ph SCALE Blood ph is 7.4 at 37 C. The ph of blood must be measured at body temperature to accurately reflect the status of blood buffers.
7 7 Weak Acids and Bases, K a and K b Salts of weak acids are bases (conjugate bases) and have K b = K w / K a Also salt of weak base is a conjugate acid and has K a = K w / K b For a diprotic acid base pair like ethylenediamine, NH 2 C 2 H 4 NH 2, K b1 = K w /K a2 and K b2 = K w /K a1
8 8 Weak Acids and Bases, K a and K b
9 9 Buffers Buffer is a solution that resists changes in ph when a small amount of acid or base is added or when the solution is diluted. Buffer solution is usually made of (weak acid with its conjugated base) or (weak base with its conjugated acid). Examples: CH 3 COO - and CH 3 COOH HCN and CN - C 6 H 5 COOH and C 6 H 5 COONa NH 3 and NH 4 Cl (C 2 H 5 ) 3 N and (C 2 H 5 ) 3 NH +
10 10 Buffers, Henderson-Hasselbalch equation
11 11 Buffers, Henderson-Hasselbalch equation
12 12 Buffers, Henderson-Hasselbalch equation
13 13 Buffers, Henderson-Hasselbalch equation Calculating the ph of a buffer when strong acid or base is added when strong acid is added to the buffer: when strong base is added to the buffer:
14 14 Buffers, Henderson-Hasselbalch equation Example: Find the ph of a solution of M HA (Ka =8.4x10-9 ) plus M NaA? Answer: ph=8.614 Example: For 1L of the above solution, calculate the ph after addition of 12mL of 1.0M HCl. HCl is an acid, it will react with the basic content (A - ) of the buffer solution and forming more of HA, so it will affect the acid/base content of the solution, NaA will decrease and HA will increase. Amount of change is equal to the moles of HCl (0.012Lx1.0M) - mol. A (1x0.1026) - (0.012x1.0) ph pka Log Log mol. HA (1x ) (0.012x1.0) ph Log Log(2.1757)
15 15 Buffers, Henderson-Hasselbalch equation Added base will react with the acid content of the buffer, this will decrease the concentration (or moles) of acid and increase the concentration (or moles) of base content of the buffer. Example: For 1L of the previous buffer solution, calculate the ph after addition of 12mL of 1.0M NaOH. NaOH will affect the acid/base content of the solution, HA will decrease and NaA will increase. Amount of change is equal to the moles of NaOH (0.012Lx1.0M) ph pk a - mol. A (1x0.1026) (0.012x1.0) Log Log mol. HA (1x ) - (0.012x1.0) ph Log Log(6.4966)
16 16 Acid-Base Titration Titration is used to determine the concentration of analyte volumetrically, depending on the stoichiometric ratio between analyte and titrant. Examples: HCl + NaOH NaCl + H 2 O (ratio 1:1) H 2 SO 4 + 2NaOH Na 2 SO 4 + 2H 2 O (ratio 1:2) 2CH 3 COOH +Ca(OH) 2 (CH 3 COO) 2 Ca + 2H 2 O (ratio 2:1) H 2 SO 4 + Ca(OH) 2 CaSO 4 + 2H 2 O (ratio 1:1)
17 17 ph curve During the acid-base titration, the ph will change. If the analyte is acid, ph will be low and start increasing through titrant addition (base). Example: (titration 50 ml of 0.10M HCl with 0.10M NaOH) Volume of NaOH added ph equiv. point Acid excess [H][OH]=K w Base excess
18 18 ph curve Titration strong base with strong acid Titration diprotic acid with strong base
19 19 ph curve Question 50 ml of 0.10M HCl was titrated with 0.24M NaOH. Calculate the ph after addition of 0, 5, 20, 25 and 30 ml of NaOH. Question 17.4mL of M HCl was needed to titrate 25.0mL of NaOH with unknown concentration. Calculate the concentration of NaOH.
20 20 CHAPTER 8 Acid Base Titrations Learning Objectives Calculating acid base titration curves Indicators Mixtures of Acids or Bases Derivatives of a Titration Curve
21 21 TITRATION Strong acid with strong base (monoprotic acid with monohydroxy base) Four stages a, b, c, d At the beginning (a) only acid is present, concentration if [H + ] = [acid] Before the equivalence point (b), acid in excess [H ] mole of acid - mole of base totalsolution volume (L) At the equivalence point (c), base reacts completely with the acid and H + comes only from water hydrolysis [H + ] = 1x10-7 After the equivalence point (d), base in excess [OH - mole of base - mole of acid ] totalsolution volume (L) [H Kw ] [OH - ]
22 22 TITRATION Strong base with strong acid (monohydroxy base with monoprotic acid ) Four stages a, b, c, d At the beginning (a) only base is present, concentration if [H + ] = K w /[base] Before the equivalence point (b), base in excess [OH - ] mole of base - mole of acid totalsolution volume (L) [H Kw ] [OH - ] At the equivalence point (c), acid reacts completely with the base and H + comes only from water hydrolysis [H + ] = 1x10-7 After the equivalence point (d), acid in excess mole of acid - mole of base [H ] totalsolution volume (L)
23 23 TITRATION
24 24 TITRATION Detection of the End Point: Indicators The point at which the reaction is observed to be complete is called the end point. The difference between the equivalence point and the end point is referred to as the titration error. Indicator is added to the solution for visual detection of color change which indicates a ph change. An indicator for an acid base titration is a weak acid or weak base that is highly colored. Choose an indicator with a pka near the equivalence point ph.
25 25 TITRATION Weak Acid versus Strong Base Weak Base versus Strong Acid
26 26 TITRATION Weak acid HA with strong base (monoprotic acid with monohydroxy base) Four stages a, b, c, d At the beginning (a) only acid is present, concentration of [H ] [HA].K a Before the equivalence point (b), buffer is formed ph pk a - moles of A ( moles of base added) Log moles of HA ( started moles of HA- moles of base added) Special case: in the middle region of (b) when volume of NaOH =1/2 equivalence volume, ph=pk a At the equivalence point (c), hydrolysis of A Kw [OH ] [A ].K b [H ] - [OH ], - started moles of HA [A ] total volume (L) After the equivalence point (d) - mole of base - mole of acid [OH ] totalsolution volume (L) [H Kw ] [OH - ]
27 27 TITRATION Weak-acid titrations require careful selection of the indicator.
28 28 TITRATION
29 29 TITRATION Mixtures of Acids or Bases One acid should be at least 10 4 times weaker than the other to titrate separately. The stronger acid will titrate first and will give a ph break at its equivalence point. If two strong acids are titrated together, there will be no differentiation between them, and only one equivalence point break will occur. For H 2 SO 4, the first proton is completely dissociated and the second proton has a Ka of about Therefore, the second proton is ionized sufficiently to titrate as a strong acid, and only one equivalence point break is found. For Phosphoric acid, the first proton titrates as a strong acid, followed by titration of the second proton to give a second equivalence point; the third proton is too weakly ionized to be titrated.
30 30 TITRATION Equivalence Points from Derivatives of a Titration Curve Bases In general, derivatives reveal subtle features that are not always observable on the original plots. The rate at which ph changes with added titrant is the greatest at the equivalence point. For an acid sample, titrated with a base, this rate of change is the first derivative of the ph vs. V B plot, or d ph /d VB
Acid 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 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 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 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 informationTitration a solution of known concentration, called a standard solution
Acid-Base Titrations Titration is a form of analysis in which we measure the volume of material of known concentration sufficient to react with the substance being analyzed. Titration a solution of known
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 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 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 informationTitration Of A Weak Acid With Strong Base. BCH 312 [Practical]
Titration Of A Weak Acid With Strong Base BCH 312 [Practical] Weak Acid : Weak acids or bases do not dissociate completely, therefore an equilibrium expression with Ka must be used. The Ka is a quantitative
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 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 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 informationI. Acids & Bases. A. General ideas:
Acid-Base Equilibria 1. Application of equilibrium concepts. 2. Not much else new in the way of theory is presented. 3. Specific focus on aqueous (H O is 2 solvent) systems. 4. Assume we are at equilibrium
More informationChapter 14. Objectives
Section 1 Properties of Acids and Bases Objectives List five general properties of aqueous acids and bases. Name common binary acids and oxyacids, given their chemical formulas. List five acids commonly
More informationChapter 15 Acid-Base Equilibria
Chapter 15 Acid-Base Equilibria Acid-Base Equilibria 15.1 Solutions of Acids or Bases Containing a Common Ion A. Common Ion 1. Ion provided in solution by an aqueous acid (or base) as well as a salt 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 informationGrace King High School Chemistry Test Review
CHAPTER 19 Acids, Bases & Salts 1. ACIDS Grace King High School Chemistry Test Review UNITS 7 SOLUTIONS &ACIDS & BASES Arrhenius definition of Acid: Contain Hydrogen and produce Hydrogen ion (aka proton),
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. 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 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 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 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 information10.1 Acids and Bases in Aqueous Solution
10.1 Acids and Bases in Aqueous Solution Arrhenius Definition of Acids and Bases An acid is a substance that gives hydrogen ions, H +, when dissolved in water. In fact, H + reacts with water and produces
More informationACIDS AND BASES. Note: For most of the acid-base reactions, we will be using the Bronsted-Lowry definitions.
DEFINITIONS: ACIDS AND BASES Arrhenius Definition An acid in aqueous solution produces H + ions. A base in aqueous solution produces OH - ions. Bronsted Lowry Theory An acid is a proton donor A base is
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 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 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 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 informationChemistry I Notes Unit 10: Acids and Bases
Chemistry I Notes Unit 10: Acids and Bases Acids 1. Sour taste. 2. Acids change the color of acid- base indicators (turn blue litmus red). 3. Some acids react with active metals and release hydrogen gas,
More 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 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 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 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 informationAcids and Bases. A strong base is a substance that completely ionizes in aqueous solutions to give a cation and a hydroxide ion.
Acid-Base Theories Arrhenius Acids and Bases (1884) Acids and Bases An acid is a substance that, when dissolved in water, increases the concentration of hydrogen ions. A base is a substance that, when
More 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 informationChapter 16 Aqueous Ionic Equilibrium Buffer Solutions
Chapter 16 Aqueous Ionic Equilibrium 16.1-16.2 Buffer Solutions Why? While a weak acid will partially ionize to produce its conjugate base, it will not produce enough conjugate base to be considered a
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 informationChapter 10. Acids and Bases
Chapter 10 Acids and Bases 1 Properties of Aqueous Solutions of Acids and Bases Aqueous acidic solutions have the following properties: 1. They have a sour taste.. They change the colors of many indicators.
More 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 information5/10/2017. Chapter 10. Acids, Bases, and Salts
Chapter 10. Acids, Bases, and Salts Introduction to Inorganic Chemistry Instructor Dr. Upali Siriwardane (Ph.D. Ohio State) E-mail: upali@latech.edu Office: 311 Carson Taylor Hall ; Phone: 318-257-4941;
More informationThe Common Ion Effect
Chapter 17 ACID BASE EQUILIBRIA (Part I) Dr. Al Saadi 1 17.1 The Common Ion Effect A phenomenon known as the common ion effect states that: When a compound containing an ion in common with an already dissolved
More informationWhat is an acid? What is a base?
What is an acid? What is a base? Properties of an acid Sour taste Turns litmus paper red Conducts electric current Some acids are strong and some are weak Properties of a base Bitter taste Slippery to
More informationIntroduction to Acids & Bases II. Packet #26
Introduction to Acids & Bases II Packet #26 1 Review I Svante Arrhenius was the first person to recognize the essential nature of acids and bases. 2 Review II Arrhenius postulated that: Acids produce hydrogen
More informationbattery acid the most widely used industrial chemical Hydrochloric acid, HCl muriatic acid stomach acid Nitric acid, HNO 3
BRCC CHM 101 Chapter 9 Notes (Chapter 8 in older text versions) Page 1 of 9 Chapter 9: Acids and Bases Arrhenius Definitions more than 100 years old Acid a substance that produces H + in water (H + is
More informationChemical Equilibria Part 2
Unit 1 - Inorganic & Physical Chemistry 1.4 Chemical Equilibria Part 2 Acid / Base Equilibria Indicators ph Curves Buffer Solutions Pupil Notes Learning Outcomes Questions & Answers KHS ChemistrySept 2015
More informationg. Looking at the equation, one can conclude that H 2 O has accepted a proton from HONH 3 HONH 3
Chapter 14 Acids and Bases I. Bronsted Lowry Acids and Bases a. According to Brønsted- Lowry, an acid is a proton donor and a base is a proton acceptor. Therefore, in an acid- base reaction, a proton (H
More informationAcids and bases. for it cannot be But I am pigeon-liver d and lack gall To make oppression bitter Hamlet. Different concepts Calculations and scales
Acids and bases for it cannot be But I am pigeon-liver d and lack gall To make oppression bitter Hamlet Different concepts Calculations and scales Learning objectives You will be able to: Identify acids
More information11/15/11. Chapter 16. HA(aq) + H 2 O(l) H 3 O + (aq) + A (aq) acid base conjugate conjugate
Chapter 16 Table of Contents Chapter 16 16.1 16.2 16.3 16.4 16.5 16.6 Buffered Solutions Copyright Cengage Learning. All rights reserved 2 Models of Arrhenius: Acids produce H + ions in solution, bases
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 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 informationAcids, Bases, & Neutralization Chapter 20 & 21 Assignment & Problem Set
Acids, Bases, & Neutralization Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Acids, Bases, & Neutralization 2 Study Guide: Things You Must Know
More informationChapter 14 Acid- Base Equilibria Study Guide
Chapter 14 Acid- Base Equilibria Study Guide This chapter will illustrate the chemistry of acid- base reactions and equilibria, and provide you with tools for quantifying the concentrations of acids and
More informationACIDS AND BASES. for it cannot be But I am pigeon-liver d and lack gall To make oppression bitter Hamlet
ACIDS AND BASES for it cannot be But I am pigeon-liver d and lack gall To make oppression bitter Hamlet Learning objectives Name and write formulae for common acids and bases Describe acids and bases according
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 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 informationIntroduction to Acids & Bases. Packet #26
Introduction to Acids & Bases Packet #26 Review I Svante Arrhenius was the first person to recognize the essential nature of acids and bases. Review II Arrhenius postulated that: Acids produce hydrogen
More informationBuffer Effectiveness, Titrations & ph curves. Section
Buffer Effectiveness, Titrations & ph curves Section 16.3-16.4 Buffer effectiveness Buffer effectiveness refers to the ability of a buffer to resist ph change Effective buffers only neutralize small to
More informationChapter 16. Acids and Bases. Copyright Cengage Learning. All rights reserved 1
Chapter 16 Acids and Bases Copyright Cengage Learning. All rights reserved 1 Section 16.1 Acids and Bases Models of Acids and Bases Arrhenius: Acids produce H + ions in solution, bases produce OH ions.
More informationProperties of Acids and Bases
Chapter 15 Aqueous Equilibria: Acids and Bases Properties of Acids and Bases Generally, an acid is a compound that releases hydrogen ions, H +, into water. Blue litmus is used to test for acids. Blue litmus
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 informationAcids and Bases. Chapter 15. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Acids and Bases Chapter 15 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Acids Have a sour taste. Vinegar owes its taste to acetic acid. Citrus fruits contain
More informationStrong and Weak. Acids and Bases
Strong and Weak Acids and Bases Strength of Acids H2SO4 HSO4 - + H + HNO3 NO3 - + H + Strong Acids HCl Cl - + H + H3PO4 H2PO4 - + H + Phosphoric acid Moderate Acid CH3COOH CH3COO - + H + Acetic acid HF
More informationANALYTICAL CHEMISTRY - CLUTCH 1E CH.8 - MONOPROTIC ACID-BASE EQUILIBRIA.
!! www.clutchprep.com CONCEPT: ARRHENIUS ACIDS AND BASES The most general definition for acids and bases was developed by Svante Arrhenius near the end of the 19 th century. According to him, the cation
More informationAcids, Bases and ph Preliminary Course. Steffi Thomas 14/09/2017
Acids, Bases and ph Preliminary Course Steffi Thomas ssthomas@tcd.ie 14/09/2017 Outline What are acids and bases? Can we provide a general definition of acid and base? How can we quantify acidity and basicity?
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 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 information1 Chapter 19 Acids, Bases, and Salts
1 Chapter 19 Acids, Bases, and Salts ACID-BASE THEORIES Acids and bases are all around us and part of our everyday life (ex. bodily functions, vinegar, carbonated drinks, citrus fruits, car batteries,
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 informationChapters 15 & 16 ACIDS & BASES ph & Titrations
PROPERTIES OF ACIDS Chapters 15 & 16 ACIDS & BASES ph & Titrations There are 5 main properties of acids: 1. sour taste 2. change the color of acidbase indicators 3. react with metals to produce H2 gas
More informationChapter Menu Chapter Menu
Chapter Menu Chapter Menu Section 18.1 Section 18.3 Section 18.4 Introduction to Acids and Bases Hydrogen Ions and ph Neutralization Section 18.1 Intro to Acids and Bases Objectives: Compare the Arrhenius,
More informationGrade A buffer: is a solution that resists changes in its ph upon small additions of acid or base.sq1
Chapter 15 Lesson Plan Grade 12 402. The presence of a common ion decreases the dissociation. BQ1 Calculate the ph of 0.10M CH 3 COOH. Ka = 1.8 10-5. [H + ] = = ( )( ) = 1.34 10-3 M ph = 2.87 Calculate
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 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 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 informationChemistry 400 Homework #3, Chapter 16: Acid-Base Equilibria
Chemistry 400 Homework #3, Chapter 16: Acid-Base Equilibria I. Multiple Choice (for those with an asterisk, you must show work) These multiple choice (MC) are not "Google-proof", but they were so good
More informationAcids and Bases. CHEM 102 T. Hughbanks. In following equilibrium, will reactants or products be favored? Strong acid (HCl) + Strong base (NaOH)
Acids and Bases According to the Brønsted Lowry theory, all acid base reactions can be written as equilibria involving the acid and base and their conjugates. CEM 102 T. ughbanks All proton transfer reactions
More informationAQA Chemistry A-Level : Acids and Bases
AQA Chemistry A-Level 3.1.12: Acids and Bases Detailed Notes 3.1.12.1 - Brønsted-Lowry Acids and Bases Acid-base equilibria involve the transfer of protons between substances. Therefore substances can
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 informationAcids and Bases. Click a hyperlink or folder tab to view the corresponding slides. Exit
Acids and Bases Section 18.1 Introduction to Acids and Bases Section 18.2 Strengths of Acids and Bases Section 18.3 Hydrogen Ions and ph Section 18.4 Neutralization Click a hyperlink or folder tab to view
More informationChapter 16. Dr Ayman Nafady
Chemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., Bruce E. Bursten Chapter 16 Dr Ayman Nafady John D. Bookstaver St. Charles Community College Cottleville, MO Some Definitions
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 informationChem 1102 Semester 1, 2011 ACIDS AND BASES
Chem 1102 Semester 1, 2011 ACIDS AND BASES 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
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 informationACIDS, BASES, AND SALTS
ACIDS, BASES, AND SALTS Chapter Quiz Choose the best answer and write its letter on the line. 1. A solution in which the hydroxide-ion concentration is 1 10 2 is a. acidic. c. neutral. b. basic. d. none
More informationAqueous Solutions and Chemical Equilibria:
Aqueous Solutions and Chemical Equilibria: Acidbase titration Complexometric titration Separations Electrochemistry Etc., etc. Illustration: acidbase titrations Concepts and determination of ph during
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 9 Aqueous Solutions and Chemical Equilibria
Chapter 9 Aqueous Solutions and Chemical Equilibria At equilibrium, the rate of a forward process or reaction and that of the reverse process are equal. 9A The chemical composition of aqueous solutions
More information1. Know and be capable of applying the Bronsted-Lowery model of acids and bases (inculdig the concepts related to conjugate acid-base pairs.
Acid-Base Equilibria You have just completed a chapter on equilibrium. That chapter focused primarily on gas phase reactions (with a few exceptions). This section on Acid-Base equilibria (along with the
More informationChapter 15. Acid-Base Equilibria
Chapter 15 Acid-Base Equilibria Section 15.1 Solutions of Acids or Bases Containing a Common Ion Common Ion Effect Shift in equilibrium position that occurs because of the addition of an ion already involved
More informationChapter 10 - Acids & Bases
Chapter 10 - Acids & Bases 10.1-Acids & Bases: Definitions Arrhenius Definitions Acids: substances that produce hydrogen ions when dissolved in H 2 O Common Strong Acids: Common Weak acids: Organic carboxylic
More informationEdexcel Chemistry A-level Topic 12 - Acid-Base Equilibria
Edexcel Chemistry A-level Topic 12 - Acid-Base Equilibria Flashcards Define a Bronsted-Lowry acid Define a Bronsted-Lowry acid Proton donor Define a Bronsted-Lowry base Define a Bronsted-Lowry base Proton
More informationAcid/Base Definitions
Acids and Bases Acid/Base Definitions Arrhenius Model Acids produce hydrogen ions in aqueous solutions Bases produce hydroxide ions in aqueous solutions Bronsted-Lowry Model Acids are proton donors Bases
More informationAcids and bases, as we use them in the lab, are usually aqueous solutions. Ex: when we talk about hydrochloric acid, it is actually hydrogen chloride
Acids and Bases Acids and bases, as we use them in the lab, are usually aqueous solutions. Ex: when we talk about hydrochloric acid, it is actually hydrogen chloride gas dissolved in water HCl (aq) Concentrated
More informationCHAPTER 14 ACIDS AND BASES
CHAPTER 14 ACIDS AND BASES Topics Definition of acids and bases Bronsted-Lowry Concept Dissociation constant of weak acids Acid strength Calculating ph for strong and weak acids and bases Polyprotic acids
More informationBuffer solutions Strong acids and bases dissociate completely and change the ph of a solution drastically. Buffers are solutions that resist changes i
18.3 ph Curves Buffer solutions Strong acids and bases dissociate completely and change the ph of a solution drastically. Buffers are solutions that resist changes in ph even when acids and bases are added
More informationSolutions are aqueous and the temperature is 25 C unless stated otherwise.
Solutions are aqueous and the temperature is 25 C unless stated otherwise. 1. According to the Arrhenius definition, an acid is a substance that produces ions in aqueous solution. A. H C. OH B. H + D.
More 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 informationAqueous Reactions and Solution Stoichiometry (continuation)
Aqueous Reactions and Solution Stoichiometry (continuation) 1. Electrolytes and non-electrolytes 2. Determining Moles of Ions in Aqueous Solutions of Ionic Compounds 3. Acids and Bases 4. Acid Strength
More informationChapter 16 Acids and Bases. Chapter 16 Acids and Bases
. Chapter 16 Acids and Bases 1 Some Definitions Arrhenius Acid: Substance that, when dissolved in water, increases the concentration of hydrogen ions. Base: Substance that, when dissolved in water, increases
More informationMonoprotic Acid/Base Equilibria. Monoprotic Acid/Base Equilibria
Monoprotic Acid/Base Equilibria Strong acids and bases: What is the ph of 0.10 M HCl? How do you calculate it? Why? Concentration (F) 0.10 (10-1 ) 0.01 (10-2 ) 0.001 (10-3 ) 0.0001 (10-4 ) 0.00001 (10-5
More information