Acid and Base Strength. Weak Acid-Base Equilibrium. Acid and Base Strength 1. Acid and Base Strength. Dissociation Constants
|
|
- Bethany Cannon
- 6 years ago
- Views:
Transcription
1 Weak AcidBase Equilibrium A molecule with negligible acidity contains hydrogen but does not demonstrate any acidic behavior in water. Its conjugate base is extremely strong. Possibly explained by Lewis theory. No measurable H A strong acid completely transfers its protons to water leaving no undissociated (ionized) molecules. Its conjugate base is extremely weak. Easily explained by Arrhenius Concentration of H + is defined stoichometrically by initial acid concentration 2. A weak acid only partially dissociates in aqueous solution and therefore exists in the solution as a mixture of the acid and its conjugate base. Its conjugate base is fairly strong. Explained by Arrhenius but better explained by BL. Concentration of H + must be determined applying equilibrium calculations. Dissociation Constants For a generalized acid dissociation, HA(aq) + H 2 O(l) the equilibrium expression would be K c = [H 3 O + ] [A ] [HA] A (aq) + H 3 O + (aq) This equilibrium constant is called the aciddissociation constant, K a. 1
2 Weak AcidBase Equilibrium For the weak acid acetic acid, the equilibrium exists as: CH 3 CO 2 H + H 2 O CH 3 CO 2 + H 3 O + Therefore, we can define K as K = [CH 3 CO 2 ] [H 3 O + ] / [CH 3 CO 2 H] = K a Where: K a = acid dissociation constant for Acetic Acid The aciddissociation constant (K a ) describes the ratio of H + and acid anion to acid molecules for weak acid dissociation using the Law of Mass Action. Using what we now know about equilibrium, we can calculate the concentrations of dissociated ions and undissociated acid molecules at equilibrium, thereby allowing us to find K a for any acid. (AP equation Sheet) Calculating K a from the ph The ph of a 0.10 M solution of formic acid, HCOOH, at 25 C is Calculate K a for formic acid at this temperature. We know that K a = [H 3 O + ] [HCOO ] [HCOOH] Two things to note: A. We neglected the [H + ] due to the autoionization of water in aqueous solutions only one source of H + is dominant. Even weak acids have a much higher H + concentration than water B. Given the number of significant figures, 1. Niacin, one of the B vitamins, has the following molecular structure: [RCO 2 H] o [RCO 2 Weak acids usually have very little dissociation (K<<1). We will learn to make this assumption as long as we do not affect the H + concentration by more than 5% A M solution of niacin has a ph of 3.26, What is the K a for Niacin? 2
3 Dissociation Constants The greater the value of K a, the stronger the acid. Percent Ionization Another measure of acid strength, besides Ka, is the acid percent ionization (dissociation) The percent dissociation of an acid,or base, is the percent of initial concentration that is dissociated in a weak acidbase solution. As the weak acid/base concentration increases, the percent ionization decreases Calculating Percent Ionization [HCOOH], M [H 3O + ], M [HCOO ], M Initially Weak Bases Change At equilibrium = = [H 3 O + ] eq Percent ionization = [HA] 100 initial From our earlier example, [H 3 O + ] eq = M [HCOOH] initial = 0.10 M Percent ionization = = 4.2% Bases react with water to produce hydroxide ion Pearson Education, Inc. Weak Bases The equilibrium constant expression for this reaction is K b = [HB] [OH ] [B ] 3. For base reactions, K b can be determined following the same equilibrium guidelines. Calculate the K b for a M CO 3 2 solution having a ph of where K b is the basedissociation constant Pearson Education, Inc. (AP equation Sheet) 3
4 The relationship between K a and K b conj. is described by the ionproduct constant of water (K w ) 4. Calculate K b for the fluoride ion, using Appendix D. K b for F is not given, but its conjugate acid is. K a x K b conj. = K w The product of the aciddissociation constant and basedissociation constant for the conjugate acidbase pair equals the ionproduct constant of water Recall the autoionizatoin of water: Where: K w = [H 3 O + ][OH ] = K w = 1.0 x (@ 25.0 o C) This only describes the concentration of hydronium and hydroxide ions in water, not the acid or base strength of water. You may also recall that the concentration of a solid or pure liquid, not a solution, is equal to its density(g/cm 3 ) divided by its molecular weight (g/mol); for water this is g/mol. From: K a = [H 3 O + ][OH ] / [H 2 O] = K w = 1.0 x We get: K a H20 = K b H20 = (1.0 e 7 )(1.0 e 7 ) / (55.556) = 1.8 e 16 And from: K ah2o K boh = K w We get: K boh = K ah+ = K w / K ah2o = 1.0 e14 / 1.8 e 16 = Looking at the relative acid base strengths, this should make since: K a H20 = K b H20 = 1.8 e 16 K b OH = K a H+ = The magnitude of K a describes the weak acid strength, just as K eq described the magnitude of a reaction. The larger the value of K a, the greater the dissociation, the further to the right the equilibrium is shifted, meaning the greater the acid strength. Examine the Acetic acid equilibrium again. 4
5 CH 3 CO 2 H + H 2 O CH 3 CO 2 + H 3 O + A 1 B 1 B 2 A 2 Look Up K a values for both acids We know that K<<1; so, the equilibrium favors the reactants. But what does that say about the rest of the species in equilibrium? Because H 3 O + is a stronger BL acid than acetic the reaction lies to the left. This brings us to an important observation: In every acidbase reaction, equilibrium favors the transfer of the proton from the stronger acid to the stronger base to form the weaker acid and the weaker base. 2. Write the dissociation (ionization) reaction for each of the following and label as acid/base or conjugate acid/base. Then determine if the equilibrium will lie to the right or the left using what you know about acid/base strengths. a. NH 3 + H 2 O b.hso 4 + CO 3 2 c. PO H 2 O 5
Lecture Presentation. Chapter 16. Acid Base Equilibria. John D. Bookstaver St. Charles Community College Cottleville, MO Pearson Education, Inc.
Lecture Presentation Chapter 16 Acid Base Equilibria John D. Bookstaver St. Charles Community College Cottleville, MO Some Definitions Arrhenius An acid is a substance that, when dissolved in water, increases
More informationChapter 16. Chemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., and Bruce E. Bursten
Chemistry, The Central Science, 11th edition Theodore L. Brown, H. Eugene LeMay, Jr., Bruce E. Bursten Chapter 16 John D. Bookstaver St. Charles Community College Cottleville, MO Some Definitions Arrhenius
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 information19.3 Strengths of Acids and Bases > Chapter 19 Acids, Bases, and Salts Strengths of Acids and Bases
Chapter 19 Acids, Bases, and Salts 19.1 Acid-Base Theories 19.2 Hydrogen Ions and Acidity 19.3 Strengths of Acids and Bases 19.4 Neutralization Reactions 19.5 Salts in Solution 1 Copyright Pearson Education,
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 informationChapter 16 Acid Base Equilibria
Chapter 16 Acid Base Equilibria 2015 Pearson Education, Inc. Acid Base Equilibria 16.1 : A Brief Review 16.2 Brønsted Lowry 16.3 The Autoionization of Water 16.4 The ph Scale 16.5 Strong Balsamic Vinegar
More informationChpt 16: Acids and Bases
Chpt 16 Acids and Bases Defining Acids Arrhenius: Acid: Substances when dissolved in water increase the concentration of H+. Base: Substances when dissolved in water increase the concentration of OH- Brønsted-Lowry:
More information1. Strengths of Acids and Bases 2. K a, K b 3. Ionization of Water 4. Relative Strengths of Brønsted-Lowry Acids and Bases
Chemistry 12 Acid-Base Equilibrium II Name: Date: Block: 1. Strengths of Acids and Bases 2. K a, K b 3. Ionization of Water 4. Relative Strengths of Brønsted-Lowry Acids and Bases Strengths of Acids and
More informationChapter 16 Acid-Base Equilibria
Chapter 16 Acid-Base Equilibria Learning goals and key skills: Understand the nature of the hydrated proton, represented as either H + (aq) or H 3 O + (aq) Define and identify Arrhenuis acids and bases.
More informationWeak acids are only partially ionized in aqueous solution: mixture of ions and un-ionized acid in solution.
16.6 Weak Acids Weak acids are only partially ionized in aqueous solution: mixture of ions and un-ionized acid in solution. Therefore, weak acids are in equilibrium: HA(aq) + H 2 O(l) H 3 O + (aq) + A
More informationHA(aq) H + (aq) + A (aq) We can write an equilibrium constant expression for this dissociation: [ ][ ]
16.6 Weak Acids Weak acids are only partially ionized in aqueous solution. There is a mixture of ions and un-ionized acid in solution. Therefore, weak acids are in equilibrium: Or: HA(aq) + H 2 O(l) H
More informationTalk n Acids & Bases... Lady Dog! Definitions
Talk n Acids & Bases... Lady Dog! Definitions So far in this course, we have looked at processes in chemistry that deal with, or are best explained by, ionic salts or molecules. Now we will turn our attention
More informationCHEMISTRY. Chapter 16 Acid-Base Equilibria
CHEMISTRY The Central Science 8 th Edition Chapter 16 Acid-Base Equilibria Kozet YAPSAKLI Why study acids bases? bases are common in the everyday world as well as in the lab. Some common acidic products
More informationACID BASE EQUILIBRIUM
ACID BASE EQUILIBRIUM Part one: Acid/Base Theories Learning Goals: to identify acids and bases and their conjugates according to Arrhenius and Bronstead Lowry Theories. to be able to identify amphoteric
More informationAP Chemistry CHAPTER 16 STUDY GUIDE Acid-Base Equilibrium
AP Chemistry CHAPTER 16 STUDY GUIDE AcidBase Equilibrium 16.1 Acids and Bases: A Brief Review Acids taste sour and cause certain dyes to change color. Bases taste bitter and feel soapy. Arrhenius concept
More informationAqueous Equilibria: Acids and Bases
Slide 1 Chapter 14 Aqueous Equilibria: Acids and Bases Slide 2 Acid Base Concepts 01 Arrhenius Acid: A substance which dissociates to form hydrogen ions (H + ) in solution. HA(aq) H + (aq) + A (aq) Arrhenius
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 informationAcid-Base Chemistry & Organic Compounds. Chapter 2
Acid-Base Chemistry & Organic Compounds Chapter 2 Brønsted Lowry Acids & Bases! Brønsted-Lowry Acid: Proton (H + ) Donor! Brønsted-Lowry Base: Proton (H + ) Acceptor! General reaction: HA + B: A - + BH
More informationChapter 16: Acid Base Equilibria Chapter 16 Acid-Base Equilibria Learning Standards & Objectives;
Chapter 16: Acid Base Equilibria Chapter 16 Acid-Base Equilibria Learning Standards & Objectives; Chapter 16 AP16-1,2-01 AP16-1,2-02 AP16-1,2-03 AP16-3,4-01 AP16-3,4-02 AP16-5-01 AP16-6,7-01 AP16-6,7-02
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 informationChem12 Acids : Exam Questions M.C.-100
Chem12 Acids : Exam Questions M.C.-100 1) Given : HPO 4 2- (aq) + NH 4 + (aq) H 2 PO 4 - (aq) + NH 3 (aq), the strongest acid in the above equation is : a) NH 4 + b) HPO 4 2- c) NH 3 d) H 2 PO 4-2)
More informationChapter 16. Acid-Base Equilibria
Chapter 16. Acid-Base Equilibria 16.1 Acids and Bases: A Brief Review Acids taste sour and cause certain dyes to change color. Bases taste bitter and feel soapy. Arrhenius concept of acids and bases: An
More informationACIDS AND BASES CONTINUED
ACIDS AND BASES CONTINUED WHAT HAPPENS WHEN AN ACID DISSOLVED IN WATER? Water acts as a Brønsted Lowry base and abstracts a proton (H+) from the acid. As a result, the conjugate base of the acid and a
More informationPrinciples of Reactivity: The Chemistry of Acids and Bases. Acids, Bases and Arrhenius
Principles of Reactivity: The Chemistry of Acids and Bases **a lot of calculations in this chapter will be done on the chalkboard Do not rely on these notes for all the material** Acids, Bases and Arrhenius
More informationChap 16 Chemical Equilibrium HSU FUYIN
Chap 16 Chemical Equilibrium HSU FUYIN 1 Definitions: Arrhenius & Brønsted Lowry acid and base Arrhenius theory: An acid is a substance that, when dissolved in water, increases the concentration of hydrogen
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 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 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 informationChapter 14: Acids and Bases
Chapter 14: Acids and Bases 14.1 The Nature of Acids and Bases Bronsted-Lowry Acid-Base Systems Bronsted acid: proton donor Bronsted base: proton acceptor Bronsted acid base reaction: proton transfer from
More informationAqueous Equilibria, Part 1 AP Chemistry Lecture Outline
Aqueous Equilibria, Part 1 AP Chemistry Lecture Outline Name: Acids and Bases Arrhenius...acids increase the when dissolved in H 2 O....bases increase the when dissolved in H 2 O. e.g., HCl and NaOH Bronsted-Lowry
More informationChapter 16 exercise. For the following reactions, use figure 16.4 to predict whether the equilibrium lies predominantly. - (aq) + OH - (aq)
1 Chapter 16 exercise Q1. Practice exercise page 671 Write the formula for the conjugate acid of the following, HSO 3, F, PO 4 3 and CO. HSO 3 H H 2 SO 4 F H HF PO 4 3 H HPO 4 2 CO H HCO Q2. Practice exercise
More informationChapter 14. Acids and Bases
Chapter 14 Acids and Bases Section 14.1 The Nature of Acids and Bases Models of Acids and Bases Arrhenius: Acids produce H + ions in solution, bases produce OH - ions. Brønsted Lowry: Acids are proton
More informationChapter 16: Acids and Bases I. Chem 102 Dr. Eloranta
Chapter 16: Acids and Bases I Chem 102 Dr. Eloranta Acids and Bases Acids Sour taste (vinegar) Dissolve many metals Ability to neutralize bases Strong or Weak Bases Bitter taste (caffeine, poisons from
More information1.10 Structural formulas
1.10 Structural formulas It shows which atoms are bonded to which. There are two types of structural formulas, complete Lewis structures and condensed structural formulas. In addition, there are several
More informationChapter 14 Acids and Bases
Properties of Acids and Bases Chapter 14 Acids and Bases Svante Arrhenius (1859-1927) First to develop a theory for acids and bases in aqueous solution Arrhenius Acids Compounds which dissolve (dissociate)
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 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 informationEXAM 2 PRACTICE KEY. Leaders: Deborah Course: CHEM 178
Leaders: Deborah Course: CHEM 178 EXAM 2 PRACTICE KEY Instructor: Bonaccorsi/Vela Date: 3/6/18 Make sure you (also) know: Acid-base definitions Arrhenius Bronsted-Lowry Lewis Autoionization process of
More informationChapter 7 Acids and Bases
Chapter 7 Acids and Bases 7.1 The Nature of Acids and Bases 7.2 Acid Strength 7.3 The ph Scale 7.4 Calculating the ph of Strong Acid Solutions 7.5 Calculating the ph of Weak Acid Solutions 7.6 Bases 7.7
More informationAcids. Names of Acids. Naming Some Common Acids. Solution. Learning Check Acids and Bases. Arrhenius acids Produce H + ions in water.
Chapter 10 Acids and Bases Acids 10.1 Acids and Bases Arrhenius acids Produce H + ions in water. H 2 O HCl(g) H + (aq) + Cl (aq) Are electrolytes. Have a sour taste. Turn litmus red. Neutralize bases.
More informationAcids and Bases. Slide 1 / 208. Slide 2 / 208. Slide 3 / 208. Table of Contents: Acids and Bases
Slide 1 / 208 Slide 2 / 208 Acids and Bases Table of Contents: Acids and Bases Click on the topic to go to that section Slide 3 / 208 Properties of Acids and Bases Conjugate Acid and Base Pairs Amphoteric
More informationAcids & Bases. Strong Acids. Weak Acids. Strong Bases. Acetic Acid. Arrhenius Definition: Classic Definition of Acids and Bases.
Arrhenius Definition: Classic Definition of Acids and Bases Acid: A substance that increases the hydrogen ion concetration, [H ], (also thought of as hydronium ion, H O ) when dissolved in water. Acids
More information11/14/10. Properties of Acids! CHAPTER 15 Acids and Bases. Table 18.1
11/14/10 CHAPTER 15 Acids and Bases 15-1 Properties of Acids! Sour taste React with active metals i.e., Al, Zn, Fe, but not Cu, Ag, or Au 2 Al + 6 HCl 2 AlCl3 + 3 H2 corrosive React with carbonates, producing
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 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. Properties of Acids. Properties of Bases. Slide 1 / 174. Slide 2 / 174. Slide 3 / 174
Slide 1 / 174 Acids and Bases PSI Chemistry covers the material approximately up to slide 75. Properties of Acids Slide 2 / 174 Acids release hydrogen ion(s) into (aqueous) solution Acids neutralize bases
More informationAcids, Bases, and ph. ACIDS, BASES, & ph
I. Arrhenius Acids and Bases ACIDS, BASES, & ph Acid any substance which delivers hydrogen ion (H + ) _ to the solution. Base any substance which delivers hydroxide ion (OH ) to the solution. II ph ph
More informationAcid-Base Equilibrium Solving ph Problems for Weak Acids and Bases
Solving ph Problems for Weak Acids and Bases How do we classify a compound as an acid or base? Recall that the word acid is from the Latin word acidus which means sour. The word alkali is an Arabic word
More informationCu 2+ (aq) + 4NH 3(aq) = Cu(NH 3) 4 2+ (aq) I (aq) + I 2(aq) = I 3 (aq) Fe 3+ (aq) + 6H 2O(l) = Fe(H 2O) 6 3+ (aq) Strong acids
There are three definitions for acids and bases we will need to understand. Arrhenius Concept: an acid supplies H + to an aqueous solution. A base supplies OH to an aqueous solution. This is the oldest
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 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 informationDuncan. UNIT 14 - Acids & Bases. COMMON ACIDS NOTES lactic acetic phosphoric NAMING ACIDS NOTES
COMMON ACIDS NOTES lactic acetic phosphoric citric malic PROPERTIES OF ACIDS 1. 1. PROPERTIES OF BASES 2. 2. 3. 3. 4. 4. 5. 5. NAMING ACIDS NOTES Binary acids (H + one element) 1. hydro- - HF 2. root of
More informationChemical Equilibrium
Chemical Equilibrium Equilibrium Constants For a generic chemical reaction, the equilibrium constant is defined as: aa + bb cc + dd (1) The equilibrium constant, K eq, for a chemical reaction indicates
More informationChapter 16 Acid-Base Equilibria
Page 1 of 20 Chapter 16 Acid-Base Equilibria 16.1 Acids and Bases: A Brief Review Acids: taste sour and cause certain dyes to change color. Bases: taste bitter and feel soapy. Arrhenius concept o acids
More informationContents and Concepts
Chapter 16 1 Learning Objectives Acid Base Concepts Arrhenius Concept of Acids and Base a. Define acid and base according to the Arrhenius concept. Brønsted Lowry Concept of Acids and Bases a. Define acid
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 informationChem 1046 Lecture Notes Chapter 17
Chem 1046 Lecture Notes Chapter 17 Updated 01-Oct-2012 The Chemistry of Acids and Bases These Notes are to SUPPLIMENT the Text, They do NOT Replace reading the Text Book Material. Additional material that
More informationCHEMISTRY 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 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 information5 Acid Base Reactions
Aubrey High School AP Chemistry 5 Acid Base Reactions 1. Consider the formic acid, HCOOH. K a of formic acid = 1.8 10 4 a. Calculate the ph of a 0.20 M solution of formic acid. Name Period Date / / 5.2
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 informationCOMPARISON OF STRONG AND WEAK ACIDS (of the same concentration, eg mol/l) Characteristic Strong Acid Weak Acid. Equal to Solution Concentration
1 COMPARISON OF STRONG AND WEAK ACIDS (of the same concentration, eg. 0.10 mol/l) Characteristic Strong Acid Weak Acid % reaction with water (%dissociation/ionization) 100% Less than 50% for most Hydronium
More informationChemistry 40S Acid-Base Equilibrium (This unit has been adapted from
Chemistry 40S Acid-Base Equilibrium (This unit has been adapted from https://bblearn.merlin.mb.ca) Name: 1 Lesson 1: Defining Acids and Bases Goals: Outline the historical development of acid base theories.
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 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 informationDr. Zellmer Chemistry 1220 Monday Time: 18 mins Spring Semester 2019 February 11, 2019 Quiz IV. Name KEY Rec. TA/time. 0 mol gas 2 mol gas
Dr. Zellmer Chemistry 1220 Monday Time: 18 mins Spring Semester 2019 February 11, 2019 Quiz IV Name KEY Rec. TA/time 1. (9 pts) For the following reaction answer the questions below. NH 4 HS (s) W NH 3
More informationExam Practice. Chapters
Exam Practice Chapters 16.6 17 1 Chapter 16 Chemical Equilibrium Concepts of: Weak bases Percent ionization Relationship between K a and K b Using structure to approximate strength of acids Strength of
More informationACID-BASE EQUILIBRIA (Part One) A Competition for Protons ADEng. PROGRAMME Chemistry for Engineers Prepared by M. J. McNeil, MPhil.
ACID-BASE EQUILIBRIA (Part One) A Competition for Protons ADEng. PROGRAMME Chemistry for Engineers Prepared by M. J. McNeil, MPhil. Department of Pure and Applied Sciences Portmore Community College Main
More informationCHAPTER 17: ACIDS AND BASES
INTRODUCTION CHAPTER 17: ACIDS AND BASES In this chapter you will learn about the properties of acids and bases. You know about some of the properties of acids already. Substances such as lemon juice and
More informationChemistry 132 NT. Acid-Base Equilibria. The face of a child can say it all. Especially the mouth part of the face.
Chemistry 1 NT The face of a child can say it all. Especially the mouth part of the face. Jack Handey 1 Chem 1 NT AcidBase Equilibria Module 1 Solutions of a Weak Acid AcidIonization Equilibria Polyprotic
More informationCHEMISTRY 1220 CHAPTER 16 PRACTICE EXAM
CHEMISTRY 1220 CHAPTER 16 PRACTICE EXAM 1. The ph of a 0.10 M solution of NH3 containing 0.10 M NH 4 Cl is 9.20. What is the [H3O + ]? a) 1.6 x 10-5 b) 1.0 x 10-1 c) 6.3 x 10-10 d) 1.7 x 10-10 e) 2.0 x
More informationAcid-Base Chemistry. Brønsted-Lowry Acids & Bases. Conjugate Acids & Bases. Conjugate Acids & Bases 7/6/12
AcidBase Chemistry BrønstedLowry Acids & Bases n There are a couple of ways to define acids and bases n BrønstedLowry acids and bases n Acid: H + ion donor n Base: H + ion acceptor n Lewis acids and bases
More informationChapter 6 Acids and Bases
Chapter 6 Acids and Bases Introduction Brønsted acid-base reactions are proton transfer reactions. Acids donate protons to bases. In the process, the acid is converted into its conjugate base and the base
More informationUNIT 14 - Acids & Bases
COMMON ACIDS NOTES lactic sour milk, sore muscles acetic vinegar phosphoric soft drinks citric citrus fruits malic apples PROPERTIES OF ACIDS PROPERTIES OF BASES 1. Taste sour 1. Taste bitter 2. react
More informationCHAPTER 13: ACIDS & BASES. Section Arrhenius Acid & Bases Svante Arrhenius, Swedish chemist ( ).
CHAPTER 13: ACIDS & BASES Section 13.1 Arrhenius Acid & Bases Svante Arrhenius, Swedish chemist (1839-1927). He understood that aqueous solutions of acids and bases conduct electricity (they are electrolytes).
More 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 informationContents and Concepts
Learning Objectives Chapter 15 Acid Base Concepts Arrhenius Concept of Acids and Base a. Define and according to the Arrhenius concept. Brønsted Lowry Concept of Acids and Bases a. Define and according
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 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 informationThe Chemistry of Acids and Bases
The Chemistry of 1 Acids and Bases 2 Acid and Bases 3 Acid and Bases 4 Acid and Bases 5 Strong and Weak Acids/Bases Generally divide acids and bases into STRONG or WEAK ones. STRONG ACID: HNO 3 (aq) +
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 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 informationChem 40S Notes: Indicators What makes an acid/base strong?
Chem 40S Notes: Indicators What makes an acid/base strong? What makes an acid or base strong? Complete dissociation into separate ions. HCl à H + + Cl - Meaning that all of HCl will be dissociated into
More informationChem 40S Notes: Indicators What makes an acid/base strong?
Chem 40S Notes: Indicators What makes an acid/base strong? Indicators There are many different types of indicators to indicate the acidity of a solution 1) Litmus and ph paper - Litmus only tells us if
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 192 Problem Set 4 Spring, 2018 Solutions
Chemistry 192 Problem Set 4 Spring, 2018 Solutions 1. The ionization constant of benzoic acid in water associated with the reaction C 6 H 5 COOH (aq) + H 2 O (l) C 6 H 5 COO (aq) + H 3O + (aq) is K a =
More informationChapter 16 ACIDS AND BASES. (Part I) Dr. Al Saadi. Brønsted Acids and Bases
Chapter 16 ACIDS AND BASES (Part I) Dr. Al Saadi 1 Brønsted Acids and Bases A Brønsted acid is a species that donates a proton. (a proton donor). HCl(aq) + H 2 O(l) H 3 O + (aq) + Cl (aq) acid hydronium
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 information+ H + H 2 PO 4. H + + HAsO In the reaction, HClO 3 + N 2 H 4 ClO 3 + N 2 H + 5, which two species are both bases? Acid Base conj base conj acid
Chapter 7 AcidBase 1. The conjugate acid of HPO 4 2 is a. H 2 PO 4 b. H 3 PO 4 c. PO 4 3 d. PO 4 2 * e. H 2 PO 4 HPO 4 2 is base (accept H ) HPO 4 2 H H 2 PO 4 2. The conjugate base of H 2 AsO 4 is a.
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 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 informationSection 32 Acids and Bases. Copyright (c) 2011 by Michael A. Janusa, PhD. All rights reserved.
Section 32 Acids and Bases 1 Copyright (c) 2011 by Michael A. Janusa, PhD. All rights reserved. Acid-Base Concepts Acids and bases are among the most familiar and important of all chemical compounds. You
More informationDiscussion 7 Chapter Key:
Discussion 7 Chapter 14 2018 Key: 1. 2 M of HCN has a K a = 5 10 10. What is the ph at equilibrium and the percent reaction of the acid? HCN H 2 O H 3 O + CN I Q=0
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 informationChapter 4 Acid-Base Equilibrium DRAFT Answer Key. p. 6. BC Science Chemistry 12 Edvantage Interactive
p. 2 p. 3 p. 6 BC Science Chemistry 12 Edvantage Interactive 2012 1 p. 7 p. 8 p. 9 BC Science Chemistry 12 Edvantage Interactive 2012 2 BC Science Chemistry 12 Edvantage Interactive 2012 3 p. 12 p. 14
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 informationFull file at
Essential Organic Chemistry, 2e (Bruice) Chapter 2 Acids and Bases 1) Which of the following is not a conjugate acid-base pair? A) B) C) HSO- 4, H2SO4 D) -OH, O2- E) NO3 -, NO2-2) Which is defined as a
More informationA is capable of donating one or more H+
Slide 1 / 48 1 According to the Arrhenius concept, an acid is a substance that. A is capable of donating one or more H+ B C D E causes an increase in the concentration of H+ in aqueous solutions can accept
More informationDr. Zellmer Chemistry 1220 Wednesday Time: 18 mins Spring Semester 2019 February 13, 2019 Quiz IV. Name KEY Rec. TA/time. 2 mol gas 0 mol gas
Dr. Zellmer Chemistry 1220 Wednesday Time: 18 mins Spring Semester 2019 February 13, 2019 Quiz IV Name KEY Rec. TA/time 1. (9 pts) For the following reaction answer the questions below. PH 3 (g) + BCl
More informationAcids and Bases. Properties of Acids and Bases. Slide 1 / 208 Slide 2 / 208. Slide 3 / 208. Slide 4 / 208. Slide 5 / 208.
Slide 1 / 208 Slide 2 / 208 cids and ases Slide 3 / 208 Slide 4 / 208 Table of ontents: cids and ases lick on the topic to go to that section Properties of cids and ases onjugate cid and ase Pairs mphoteric
More information