Ch Acids and Bases. Arrhenius Definition Acids produce hydrogen ions in aqueous solution. Bases produce hydroxide ions when dissolved in water.

Size: px
Start display at page:

Download "Ch Acids and Bases. Arrhenius Definition Acids produce hydrogen ions in aqueous solution. Bases produce hydroxide ions when dissolved in water."

Transcription

1 Ch Acids and Bases 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 base. NH 3 ammonia could not be an Arrhenius base. Bronsted-Lowry Definitions And acid is an proton (H + ) donor and a base is a proton acceptor. Acids and bases always come in pairs. HCl is an acid.. When it dissolves in water it gives its proton to water. HCl(g) + H 2 O(l) H 3 O + + Cl - Water is a base makes hydronium ion 1

2 Conjugate Acid Base Pairs General equation HA(aq) + H 2 O(l) H 3 O + (aq) + A - (aq) Acid + Base Conjugate acid +Conjugate base This is an equilibrium. Competition for H + between H 2 O and A - The stronger base controls direction. If H 2 O is a stronger base it takes the H + Equilibrium moves to right. Acid dissociation constant K a The equilibrium constant for the general equation. HA(aq) + H 2 O(l) H 3 O + (aq) + A - (aq) K a = [H 3 O + ][A - ] [HA] H 3 O + is often written H + ignoring the water in equation (it is implied). Acid dissociation constant K a HA(aq) + H 2 O(l) H 3 O + (aq) + A - (aq) means the same as HA(aq) K a = [H + ][A - ] [HA] H + (aq) + A - (aq) Strong acids dissociate completely. Equilibrium far to right. Conjugate base must be weak. What about weak acids? 2

3 Back to Pairs Strong acids K a is large [H + ] is equal to [HA] A - is a weaker base than water Weak acids K a is small [H + ] <<< [HA] A - is a stronger base than water Types of Acids Oxyacids (Ternary Acids) Polyprotic Acids Carboxylic Acids Binary Acids Structure and Acid Properties Any molecule with an H in it is a potential acid. The stronger the X-H bond the less acidic (compare bond dissociation energies). The more polar H-O-X bond -stronger acid. 3

4 Types of Acids Oxyacids - Proton is attached to the oxygen of an ion. The more polar the acid, the easier the H + comes off, the stronger the acid Strength of oxyacids The more oxygen hooked to the central atom, the more acidic the hydrogen. HClO 4 > HClO 3 > HClO 2 > HClO Remember that the H is attached to an oxygen atom. The oxygens are electronegative Pull electrons away from hydrogen Strength of oxyacids Electron Density Cl O H 4

5 Strength of oxyacids Electron Density O Cl O H Strength of oxyacids Electron Density O O Cl O H Strength of oxyacids Electron Density O O O Cl O H 5

6 Polyprotic Acids Types of acids Always dissociate stepwise. The first H + comes of much easier than the second. Ka for the first step is much bigger than Ka for the second. Denoted Ka 1, Ka 2, Ka 3 Types of Acids Polyprotic Acids- more than 1 acidic hydrogen (diprotic, triprotic). Strength of Polyprotic acids? Types of Acids Organic acids contain the Carboxyl group -COOH with the H attached to O Generally very weak. 6

7 Binary Acids In a covalent bond, the electrons from one atom attracted to the nucleus of the the other atom Bigger the molecule, the weaker the bond, the stronger the acid Binary Acids Amphoteric DEF Behave as both an acid and a base. Water autoionizes 2H 2 O(l) H 3 O + (aq) + OH - (aq) K W = [H 3 O + ][OH - ]=[H + ][OH - ] At 25ºC K W = 1.0 x10-14 This occurs in EVERY aqueous solution. Neutral solution [H + ] = [OH - ]= 1.0 x10-7 Acidic solution [H + ] > [OH - ] Basic solution [H + ] < [OH - ] 7

8 Identify the Amphoteric substance H 2 CO 3 H + + HCO - 3 Ka 1 = 4.3 x 10-7 HCO - 3 H + + CO -2 3 Ka 2 = 4.3 x ph= -log[h + ] ph and poh Used because [H + ] is usually very small As ph decreases, [H + ] increases exponentially Sig figs only the digits after the decimal place of a ph are significant Example [H + ] = 1.0 x sig figs total ph= sig figs to the right of the decimal point poh= -log[oh - ] Relationships K W = [H + ][OH - ]= 1.0 x = ph + poh [H + ],[OH - ],ph and poh Given any one of these we can find the other three. 8

9 [H + ] ph Acidic Neutral Basic poh Basic [OH - ] Equilibrium and Calculating ph of Solutions Always write down the major ions in solution. Remember these are equilibria. Remember the chemistry. Don t try to memorize there is no one way to do this. Strong Acids HBr, HI, HCl, HNO 3, H 2 SO 4, HClO 4 ALWAYS WRITE THE MAJOR SPECIES Completely dissociated [H + ] = [HA] [OH - ] is going to be small because of equilibrium = [H + ][OH - ] If [HA]< 10-7 water contributes H + 9

10 Calculate the ph of a strong acid With a high concentration super acid, ph <0 Ka will be small. Weak Acids ALWAYS WRITE THE MAJOR SPECIES. It will be an equilibrium problem from the start. Determine whether most of the H + will come from the acid or the water. Compare Ka or Kw Rest is just like last chapter. Calculate the ph of a weak acid Calculate the ph of 2.0 M acetic acid HC 2 H 3 O 2 with a Ka 1.8 x10-5 Calculate poh, [OH - ], [H + ] 10

11 A mixture of Weak Acids The process is the same. Determine the major species. The stronger will predominate. Bigger Ka if concentrations are comparable Calculate the ph of a mixture 1.20 M HF (Ka = 7.2 x 10-4 ) and 3.4 M HOC 6 H 5 (Ka = 1.6 x ) A mixture of Weak Acids Calculate the ph of a mixture 1.20 M HF (Ka = 7.2 x 10-4 ) and 3.4 M HOC 6 H 5 (Ka = 1.6 x ) Percent dissociation of an Acid = amount dissociated x 100 initial concentration For a weak acid percent dissociation increases as acid becomes more dilute. As [HA] 0 decreases [H + ] decreases but % dissociation increases. Le Chatelier 11

12 Percent dissociation of an Acid Calculate the % dissociation of 1.00 M Acetic acid (Ka = 1.8 x 10-5 ) Working Backwards What is the Ka of a weak acid that is 8.1 % dissociated as M solution? Bases The OH - is a strong base. Hydroxides of the alkali metals are strong bases because they dissociate completely when dissolved. The hydroxides of alkaline earths Ca(OH) 2 etc. are strong dibasic bases, but they don t dissolve well in water. Used as antacids because [OH - ] can t build up. 12

13 Bases without OH - Bases are proton acceptors. NH 3 + H 2 O NH OH - It is the lone pair on nitrogen that accepts the proton. Many weak bases contain N B(aq) + H 2 O(l) K b = [BH + ][OH - ] [B] BH + (aq) + OH - (aq) Strength of Bases Hydroxides are strong. Others are weak. Smaller K b weaker base. Calculate the ph of a solution of 4.0 M pyridine (Kb = 1.7 x 10-9 ) N: K a tells us K b The anion of a weak acid is a weak base. Calculate the ph of a solution of 1.00 M NaCN. Ka of HCN is 6.2 x The CN - ion competes with OH - for the H + 13

14 Anion of weak acid, cation of weak base K a > K b K a < K b K a = K b acidic basic Neutral 14

Chapter 14 - Acids and Bases

Chapter 14 - Acids and Bases Chapter 14 - Acids and Bases 14.1 The Nature of Acids and Bases A. Arrhenius Model 1. Acids produce hydrogen ions in aqueous solutions 2. Bases produce hydroxide ions in aqueous solutions B. Bronsted-Lowry

More information

Since we will be dealing with aqueous acid and base solution, first we must examine the behavior of water.

Since we will be dealing with aqueous acid and base solution, first we must examine the behavior of water. Acids and Bases Know the definition of Arrhenius, Bronsted-Lowry, and Lewis acid and base. Autoionization of Water Since we will be dealing with aqueous acid and base solution, first we must examine the

More information

Acids and Bases: A Brief Review

Acids and Bases: A Brief Review Acids and : A Brief Review Acids: taste sour and cause dyes to change color. : taste bitter and feel soapy. Arrhenius: acids increase [H ] bases increase [OH ] in solution. Arrhenius: acid base salt water.

More information

Chapter 16 Acid-Base Equilibria

Chapter 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 information

Chapter 14: Acids and Bases

Chapter 14: Acids and Bases Ch 14 Page 1 Chapter 14: Acids and Bases Properties of Acids Sour taste React with some metals Turns blue litmus paper red React with bases Some Common Acids HCl, hydrochloric acid H 2 SO 4, sulfuric acid

More information

NH 3 + H 2 O + OH - NH 4. Acid-Base Concepts -- Chapter 15 + H + Conjugate Acid-Base Pairs: - H + base. acid

NH 3 + H 2 O + OH - NH 4. Acid-Base Concepts -- Chapter 15 + H + Conjugate Acid-Base Pairs: - H + base. acid Acid-Base Concepts -- Chapter 15 1. Arrhenius Acid-Base Concept (last semester) Acid: H+ supplier Base: OH- supplier 2. Brønsted-Lowry Acid-Base Concept (more general) (a) Definition (H+ transfer) Acid:

More information

Chapter 15 Acids and Bases. Fu-Yin Hsu

Chapter 15 Acids and Bases. Fu-Yin Hsu Chapter 15 Acids and Bases Fu-Yin Hsu Stomach Acid and Heartburn The cells that line your stomach produce hydrochloric acid. To kill unwanted bacteria To help break down food To activate enzymes that break

More information

Chapter 17. How are acids different from bases? Acid Physical properties. Base. Explaining the difference in properties of acids and bases

Chapter 17. How are acids different from bases? Acid Physical properties. Base. Explaining the difference in properties of acids and bases Chapter 17 Acids and Bases How are acids different from bases? Acid Physical properties Base Physical properties Tastes sour Tastes bitter Feels slippery or slimy Chemical properties Chemical properties

More information

An acid is a substance that produces H + (H 3 O + ) Ions in aqueous solution. A base is a substance that produces OH - ions in aqueous solution.

An acid is a substance that produces H + (H 3 O + ) Ions in aqueous solution. A base is a substance that produces OH - ions in aqueous solution. Chapter 8 Acids and Bases Definitions Arrhenius definitions: An acid is a substance that produces H + (H 3 O + ) Ions in aqueous solution. A base is a substance that produces OH - ions in aqueous solution.

More information

3/6/2014. Chapter 15. Acids and Bases. Stomach Acid and Heartburn GERD. Curing Heartburn. Common Acids. Properties of Acids. Lecture Presentation

3/6/2014. Chapter 15. Acids and Bases. Stomach Acid and Heartburn GERD. Curing Heartburn. Common Acids. Properties of Acids. Lecture Presentation Lecture Presentation Chapter 15 Acids and Bases Sherril Soman Grand Valley State University Stomach Acid and Heartburn The cells that line your stomach produce hydrochloric acid. To kill unwanted bacteria

More information

CHAPTER 16: ACIDS AND BASES

CHAPTER 16: ACIDS AND BASES CHAPTER 16: ACIDS AND BASES Active Learning: 4, 6, 14; End-of-Chapter Problems: 2-25, 27-58, 66-68, 70, 75-77, 83, 90-91, 93-104 Chapter 15 End-of-Chapter Problems: 69-74, 125, 129, 133 16.1 ACIDS AND

More information

Acid-Base Chemistry. Brønsted-Lowry Acids & Bases

Acid-Base Chemistry. Brønsted-Lowry Acids & Bases Acid-Base Chemistry ν There are a couple of ways to define acids and bases ν Brønsted-Lowry acids and bases ν Acid: H + ion donor ν Base: H + ion acceptor ν Lewis acids and bases ν Acid: electron pair

More information

Chapter 16: Acid-Base and Solubility Equilibria: Reactions in Soil and Water

Chapter 16: Acid-Base and Solubility Equilibria: Reactions in Soil and Water Chapter 16: Acid-Base and Solubility Equilibria: Reactions in Soil and Water Problems: 16.2-16.86 16.1 ACIDS AND BASES: THE BRØNSTED-LOWRY MODEL PROPERTIES OF ACIDS & BASES Acids produce hydrogen ions,

More information

Acids and Bases HW PSI Chemistry

Acids and Bases HW PSI Chemistry Acids and Bases HW PSI Chemistry Name 1) According to the Arrhenius concept, an acid is a substance that. A) is capable of donating one or more H + B) causes an increase in the concentration of H + in

More information

Q.1 Classify the following according to Lewis theory and Brønsted-Lowry theory.

Q.1 Classify the following according to Lewis theory and Brønsted-Lowry theory. Acid-base A4 1 Acid-base theories ACIDS & BASES - IONIC EQUILIBRIA 1. LEWIS acid electron pair acceptor H, AlCl 3 base electron pair donor NH 3, H 2 O, C 2 H 5 OH, OH e.g. H 3 N: -> BF 3 > H 3 N BF 3 see

More information

Acid-Base (Proton-Transfer) Reactions

Acid-Base (Proton-Transfer) Reactions Acid-Base (Proton-Transfer) Reactions Chapter 17 An example of equilibrium: Acid base chemistry What are acids and bases? Every day descriptions Chemical description of acidic and basic solutions by Arrhenius

More information

Write the acid-base equilibria connecting all components in the aqueous solution. Now list all of the species present.

Write the acid-base equilibria connecting all components in the aqueous solution. Now list all of the species present. Chapter 16 Acids and Bases Concept Check 16.1 Chemists in the seventeenth century discovered that the substance that gives red ants their irritating bite is an acid with the formula HCHO 2. They called

More information

Ch 15: Acids and Bases

Ch 15: Acids and Bases Ch 15: Acids and Bases A c i d s a n d B a s e s C h 1 5 P a g e 1 Homework: Read Chapter 15 Work out sample/practice exercises in the sections, Bonus problems: 39, 41, 49, 63, 67, 83, 91, 95, 99, 107,

More information

Chapter 19: Acids and Bases Homework Packet (50 pts) Name: Score: / 50

Chapter 19: Acids and Bases Homework Packet (50 pts) Name: Score: / 50 Chapter 19: Acids and Bases Homework Packet (50 pts) Topic pg Section 19.1 1-3 Section 19.2 3-6 Section 19.3 6-7 Section 19.4 8 Naming Acids 9 Properties of Acids/Bases 10-11 Conjugate Acid/Base Pairs

More information

Q.1 Classify the following according to Lewis theory and Brønsted-Lowry theory.

Q.1 Classify the following according to Lewis theory and Brønsted-Lowry theory. Acid-base 2816 1 Acid-base theories ACIDS & BASES - IONIC EQUILIBRIA LEWIS acid electron pair acceptor H +, AlCl 3 base electron pair donor NH 3, H 2 O, C 2 H 5 OH, OH e.g. H 3 N: -> BF 3 > H 3 N + BF

More information

AP*Chemistry The Chemistry of Acids and Bases

AP*Chemistry The Chemistry of Acids and Bases AP*Chemistry The Chemistry of Acids and Bases "ACID"--Latin word acidus, meaning sour. (lemon) "ALKALI"--Arabic word for the ashes that come from burning certain plants; water solutions feel slippery and

More information

Chem101: General Chemistry Lecture 9 Acids and Bases

Chem101: General Chemistry Lecture 9 Acids and Bases : General Chemistry Lecture 9 Acids and Bases I. Introduction A. In chemistry, and particularly biochemistry, water is the most common solvent 1. In studying acids and bases we are going to see that water

More information

Name period Unit 9: acid/base equilibrium

Name period Unit 9: acid/base equilibrium Name period Unit 9: acid/base equilibrium 1. What is the difference between the Arrhenius and the BronstedLowry definition of an acid? Arrhenious acids give H + in water BronstedLowry acids are proton

More information

CHEMISTRY 101 EXAM 3 (FORM B) DR. SIMON NORTH

CHEMISTRY 101 EXAM 3 (FORM B) DR. SIMON NORTH 1. Is H 3 O + polar or non-polar? (1 point) a) Polar b) Non-polar CHEMISTRY 101 EXAM 3 (FORM B) DR. SIMON NORTH 2. The bond strength is considerably greater in HF than in the other three hydrogen halides

More information

6) Which compound is manufactured in larger quantities in the U.S. than any other industrial chemical?

6) Which compound is manufactured in larger quantities in the U.S. than any other industrial chemical? MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which statement concerning Arrhenius acid-base theory is not correct? A) Acid-base reactions must

More information

Chapter 16 Acid-Base Equilibria. Most solutions that occur in nature are slightly acidic. One reason for this is that when carbon

Chapter 16 Acid-Base Equilibria. Most solutions that occur in nature are slightly acidic. One reason for this is that when carbon Chapter 16 Acid-Base Equilibria Most solutions that occur in nature are slightly acidic. One reason for this is that when carbon dioxide dissolves in water, it forms carbonic acid, H 2 CO 3. Basic solutions

More information

p3 Recognizing Acid/Base Properties when p11 Recognizing Basic versus Nonbasic

p3 Recognizing Acid/Base Properties when p11 Recognizing Basic versus Nonbasic General Chemistry II Jasperse Acid-Base Chemistry. Extra Practice Problems 1 General Types/Groups of problems: Conceptual Questions. Acids, Bases, and p1 K b and pk b, Base Strength, and using K b or p7-10

More information

Topic 5. Acid and Bases

Topic 5. Acid and Bases Topic 5 5-1 Acid and Bases Acid and Bases 5-2 There are a number definitions for aicd and bases, depending on what is convenient to use in a particular situation: Arrhenius and Ostwald: Theory of electrolyte

More information

Acids and Bases. Chapter 16

Acids and Bases. Chapter 16 Acids and Bases Chapter 16 The Arrhenius Model An acid is any substance that produces hydrogen ions, H +, in an aqueous solution. Example: when hydrogen chloride gas is dissolved in water, the following

More information

CHEM 1212 Test II. MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

CHEM 1212 Test II. MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. CHEM 1212 Test II MULTIPLE CHOICE. Choose the one alternative that est completes the statement or answers the question. 1) At 1000 K, the equilirium constant for the reaction is K p = 0.013. 2NO (g) +

More information

Acids and Bases. An Introduction. David A Katz Department of Chemistry Pima Community College, Tucson, AZ, USA

Acids and Bases. An Introduction. David A Katz Department of Chemistry Pima Community College, Tucson, AZ, USA Acids and Bases An Introduction David A Katz Department of Chemistry Pima Community College, Tucson, AZ, USA Properties of Acids 1. Sour taste (examples: vinegar, citric acid, lemon juice) 2. Turns litmus

More information

Notes on Unit 4 Acids and Bases

Notes on Unit 4 Acids and Bases Ionization of Water DEMONSTRATION OF CONDUCTIVITY OF TAP WATER AND DISTILLED WATER Pure distilled water still has a small conductivity. Why? There are a few ions present. Almost all the pure water is H

More information

Acid-Base Equilibrium

Acid-Base Equilibrium AcidBaseEquil 1 Acid-Base Equilibrium See AqueousIons in Chemistry 1110 online notes for review of acid-base fundamentals! Acid- Base Reaction in Aqueous Salt Solutions Recall that use [ ] to mean concentration

More information

ACID-BASE REACTIONS/ THE PH CONCEPT.

ACID-BASE REACTIONS/ THE PH CONCEPT. Dr Mike Lyons School of Chemistry Trinity College Dublin. melyons@tcd.ie ACID-BASE REACTIONS/ THE PH CONCEPT. Chemistry Preliminary Course 2011 1 Lecture topics. 2 lectures dealing with some core chemistry

More information

CHAPTERS 15 FAKE TEST QUESTIONS. 1. According to the Brønsted Lowry definition, which species can function both as an acid and as a base?

CHAPTERS 15 FAKE TEST QUESTIONS. 1. According to the Brønsted Lowry definition, which species can function both as an acid and as a base? You might need to know the following K values: CHAPTERS 15 FAKE TEST QUESTIONS CH 3 COOH K a = 1.8 x 10 5 Benzoic Acid K a = 6.5 x 10 5 HNO 2 K a = 4.5 x 10 4 NH 3 K b = 1.8 x 10 5 HF K a = 7.2 x 10 4

More information

Acid/base Definitions. Acid/Base Definitions. Acid / Base Chemistry. Acid/Base Definitions. Identifying Acids and Bases

Acid/base Definitions. Acid/Base Definitions. Acid / Base Chemistry. Acid/Base Definitions. Identifying Acids and Bases Acids Identifying Acids and Bases Acid (anhydrides) contains H+ ions as the cation, with and other element as the anion Non-metal oxide H2SO4 HI P2O5 Bases Base (anhydrides) Contains OH- as the anion Combined

More information

TOPIC 11: Acids and Bases

TOPIC 11: Acids and Bases TOPIC 11: Acids and Bases ELECTROLYTES are substances that when dissolves in water conduct electricity. They conduct electricity because they will break apart into Ex. NaCl(s)! Na + (aq) + Cl - (aq), and

More information

AP Chemistry Summary Acids, Bases and Buffers Definitions:

AP Chemistry Summary Acids, Bases and Buffers Definitions: AP Chemistry Summary Acids, Bases and Buffers Definitions: Arrhenius: Acid - Produces H + ions in solution HCl H + (aq) + Cl - (aq) Base - Produces OH - ions in solution NaOH Na + (aq) + OH - (aq) Dissociation

More information

Unit Two: Acids and Bases

Unit Two: Acids and Bases Section One: Theoretical Stuff Unit Two: Acids and Bases The concept of acids and bases has existed for centuries. We can discuss them two ways, operational definitions and theoretical definitions. 1.

More information

Chem 116 POGIL Worksheet - Week 10 - Solutions Weak Acid and Base Equilibria

Chem 116 POGIL Worksheet - Week 10 - Solutions Weak Acid and Base Equilibria Chem 116 POGIL Worksheet - Week 10 - Solutions Weak Acid and Base Equilibria Key Questions 1. A 0.0100 M solution of a weak acid HA has a ph of 2.60. What is the value of K a for the acid? [Hint: What

More information

QUESTION (2012:3) (a) (i) Complete the table below showing the conjugate acids and bases. CO 3 H 2 O OH HCN CN -

QUESTION (2012:3) (a) (i) Complete the table below showing the conjugate acids and bases. CO 3 H 2 O OH HCN CN - QUESTION (2012:3) (i) Complete the table below showing the conjugate acids and bases. Conjugate acid Conjugate base - HCO 3 2 CO 3 H 2 O OH HCN CN - (ii) HPO 4 2 (aq) Write equations for the reactions

More information

Topic 8 Acids and bases 6 hours

Topic 8 Acids and bases 6 hours Topic 8 Acids and bases 6 hours Hydronium ion (H3O + ) = more stable form of hydrogen ion (H + ) H + + H2O H3O + 8.1 Theories of acids and bases 2 hours 1. Arrhenius H-X / M-OH ACID a substance that dissociates

More information

CHAPTER 18 ACID-BASE EQUILIBRIA

CHAPTER 18 ACID-BASE EQUILIBRIA CHAPTER 18 ACID-BASE EQUILIBRIA 18.1 The Arrhenius definition classified substances as being acids or bases by their behavior in the solvent water. 18. All Arrhenius acids contain hydrogen and produce

More information

Acid/Base Definition. Acid/Base Reactions. Major vs. Minor Species. Terms/Items you Need to Know. you need to memorize these!!

Acid/Base Definition. Acid/Base Reactions. Major vs. Minor Species. Terms/Items you Need to Know. you need to memorize these!! Acid/Base Reactions some covalent compounds have weakly bound H atoms and can lose them to water (acids) some compounds produce OH in water solutions when they dissolve (bases) acid/base reaction are very

More information

Note: (H 3 O + = hydronium ion = H + = proton) Example: HS - + H 2 O H 3 O + + S 2-

Note: (H 3 O + = hydronium ion = H + = proton) Example: HS - + H 2 O H 3 O + + S 2- AcidBase Chemistry Arrhenius acid: Substance that dissolves in water and provides H + ions Arrhenius base: Substance that dissolves in water and provides OH ions Examples: HCl H + and Cl Acid NaOH Na +

More information

UNIT (6) ACIDS AND BASES

UNIT (6) ACIDS AND BASES UNIT (6) ACIDS AND BASES 6.1 Arrhenius Definition of Acids and Bases Definitions for acids and bases were proposed by the Swedish chemist Savante Arrhenius in 1884. Acids were defined as compounds that

More information

Chemistry 52. Reacts with active metals to produce hydrogen gas. Have a slippery, soapy feeling. React with carbonates to produce CO 2

Chemistry 52. Reacts with active metals to produce hydrogen gas. Have a slippery, soapy feeling. React with carbonates to produce CO 2 ACID AND BASE STRENGTH Experiment #2 PURPOSE: 1. To distinguish between acids, bases and neutral substances, by observing their effect on some common indicators. 2. To distinguish between strong and weak

More information

Titrations. Acid-Base Indicators and Titration Curves. Shapes of Titration Curves. A titration curve is a graphical history of a titration

Titrations. Acid-Base Indicators and Titration Curves. Shapes of Titration Curves. A titration curve is a graphical history of a titration Acid-Base Indicators and Titration Curves Titrations In a titration a solution of accurately known concentration is added gradually added to another solution of unknown concentration until the chemical

More information

Classification of Reagents in Chemistry I: Acids and Bases

Classification of Reagents in Chemistry I: Acids and Bases University of Califnia, Davis F use with UC Davis Chem 8 and 118 Series Classification of Reagents in Chemistry I: Acids and Bases There are 3 definitions of acids and bases. All three are used in both

More information

Answer Key, Problem Set 5 (With explanations)--complete

Answer Key, Problem Set 5 (With explanations)--complete Chemistry 122 Mines, Spring 2016 Answer Key, Problem Set 5 (With explanations)complete 1. NT1; 2. NT2; 3. MP; 4. MP (15.38); 5. MP (15.40); 6. MP (15.42); 7. NT3; 8. NT4; 9. MP; 10. NT5; 11. NT6; 12. MP;

More information

Ch 8.5 Solution Concentration Units % (m/m or w/w) = mass of solute x 100 total mass of solution mass of solution = mass solute + mass solvent

Ch 8.5 Solution Concentration Units % (m/m or w/w) = mass of solute x 100 total mass of solution mass of solution = mass solute + mass solvent 1 Ch 8.5 Solution Concentration Units % (m/m or w/w) = mass of solute x 100 total mass of solution mass of solution = mass solute + mass solvent % (v/v) = volume of solute x 100 volume of solution filled

More information

Chapter 9 Lecture Notes: Acids, Bases and Equilibrium

Chapter 9 Lecture Notes: Acids, Bases and Equilibrium Chapter 9 Lecture Notes: Acids, Bases and Equilibrium Educational Goals 1. Given a chemical equation, write the law of mass action. 2. Given the equilibrium constant (K eq ) for a reaction, predict whether

More information

4. Acid Base Chemistry

4. Acid Base Chemistry 4. Acid Base Chemistry 4.1. Terminology: 4.1.1. Bronsted / Lowry Acid: "An acid is a substance which can donate a hydrogen ion (H+) or a proton, while a base is a substance that accepts a proton. B + HA

More information

Chemistry 3202. Unit 2 Acids and Bases

Chemistry 3202. Unit 2 Acids and Bases Chemistry 3202 Unit 2 Acids and Bases Definitions of Acids and Bases An operational definition is one that is based on the observable properties, behaviours or uses of an entity. The earliest definitions

More information

CHM1 Review for Exam 12

CHM1 Review for Exam 12 Topics Solutions 1. Arrhenius Acids and bases a. An acid increases the H + concentration in b. A base increases the OH - concentration in 2. Strong acids and bases completely dissociate 3. Weak acids and

More information

Chapter 13 & 14 Practice Exam

Chapter 13 & 14 Practice Exam Name: Class: Date: Chapter 13 & 14 Practice Exam Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Acids generally release H 2 gas when they react with a.

More information

ph: Measurement and Uses

ph: Measurement and Uses ph: Measurement and Uses One of the most important properties of aqueous solutions is the concentration of hydrogen ion. The concentration of H + (or H 3 O + ) affects the solubility of inorganic and organic

More information

Arrhenius Definition. Chapter 15 Acids and Bases. Brønsted-Lowry Concept. Brønsted-Lowry Concept. Conjugate Acid-Base Pairs

Arrhenius Definition. Chapter 15 Acids and Bases. Brønsted-Lowry Concept. Brønsted-Lowry Concept. Conjugate Acid-Base Pairs John W. Moore Conrad L. Stanitski Peter C. Jurs http://academic.cengage.com/chemistry/moore Chapter 15 Acids and Bases Arrhenius Definition Arrhenius: any substance which ionizes in water to produce: Protons

More information

Brønsted-Lowry Acids and Bases

Brønsted-Lowry Acids and Bases Brønsted-Lowry Acids and Bases 1 According to Brønsted and Lowry, an acid-base reaction is defined in terms of a proton transfer. By this definition, the reaction of Cl in water is: Cl(aq) + Cl (aq) +

More information

Required Reading Material.

Required Reading Material. JF Chemistry 1101 2014-2015 Introduction to Physical Chemistry: Acid Base and Solution Equilibria. Professor Mike Lyons School of Chemistry melyons@tcd.ie Required Reading Material. Kotz, Treichel and

More information

Aqueous Ions and Reactions

Aqueous Ions and Reactions Aqueous Ions and Reactions (ions, acids, and bases) Demo NaCl(aq) + AgNO 3 (aq) AgCl (s) Two clear and colorless solutions turn to a cloudy white when mixed Demo Special Light bulb in water can test for

More information

CHAPTER 5: MOLECULES AND COMPOUNDS

CHAPTER 5: MOLECULES AND COMPOUNDS CHAPTER 5: MOLECULES AND COMPOUNDS Problems: 1-6, 9-13, 16, 20, 31-40, 43-64, 65 (a,b,c,e), 66(a-d,f), 69(a-d,f), 70(a-e), 71-78, 81-82, 87-96 A compound will display the same properties (e.g. melting

More information

Chapter 17. The best buffer choice for ph 7 is NaH 2 PO 4 /Na 2 HPO 4. 19)

Chapter 17. The best buffer choice for ph 7 is NaH 2 PO 4 /Na 2 HPO 4. 19) Chapter 17 2) a) HCl and CH 3 COOH are both acids. A buffer must have an acid/base conjugate pair. b) NaH 2 PO 4 and Na 2 HPO 4 are an acid/base conjugate pair. They will make an excellent buffer. c) H

More information

Q1: What is the ph Scale? Q6: As acids become more acidic, their ph values

Q1: What is the ph Scale? Q6: As acids become more acidic, their ph values Q1: What is the ph Scale? Q6: As acids become more acidic, their ph values increase or decrease? Q2: The range of values of the ph scale is: Q7: As bases become more alkaline, their ph values increase

More information

I N V E S T I C E D O R O Z V O J E V Z D Ě L Á V Á N Í CHEMICAL REACTIONS

I N V E S T I C E D O R O Z V O J E V Z D Ě L Á V Á N Í CHEMICAL REACTIONS Chemical reaction = process during which original substances change to new substances, reactants turn to... The bonds of reactants... and new bonds are... The classification of reactions: 1. Classification

More information

10. Acids, Bases, and Salts. Acids and bases. 10.1 Arrhenius Acid-Base Theory. 10.2 Bronsted-Lowry Acid-Base Theory

10. Acids, Bases, and Salts. Acids and bases. 10.1 Arrhenius Acid-Base Theory. 10.2 Bronsted-Lowry Acid-Base Theory 10. Acids, Bases, and Salts Acids and bases For centuries people have known acids are in vinegar, lemon juice and many other foods taste sour. Only few hundred years ago that it was discovered that acids

More information

ORGANIC CHEMISTRY I PRACTICE PROBLEMS FOR BRONSTED-LOWRY ACID-BASE CHEMISTRY

ORGANIC CHEMISTRY I PRACTICE PROBLEMS FOR BRONSTED-LOWRY ACID-BASE CHEMISTRY RGANIC CHEMISTRY I PRACTICE PRBLEMS FR BRNSTED-LWRY ACID-BASE CHEMISTRY 1. For each of the species below, identify the most acidic proton and provide the structure of the corresponding conjugate base.

More information

Topic 18 Acids and Bases. 18.1 Exercises

Topic 18 Acids and Bases. 18.1 Exercises Topic 18 Acids and Bases 18.1 Exercises 1. Define: (a) ph The negative log of the hydrogen ion concentration in a solution. i.e. ph = log[h 3 O + ] (b) poh The negative log of hydroxide ion concentration

More information

Properties of Aqueous Solutions of Acids and Bases. CHAPTER 10 Acids, Bases and Salts. Properties of Aqueous Solutions of Acids and Bases

Properties of Aqueous Solutions of Acids and Bases. CHAPTER 10 Acids, Bases and Salts. Properties of Aqueous Solutions of Acids and Bases CAPTER Acids, Bases and Salts Properties of Aqueous Solutions of Acids and Bases Strong and Weak Acids Acids are substances that generate in aqueous solutions. Strong acids ionize 0% in water. That is,

More information

Suggested Problems: p. 625-627 #58, 59, 65, 69, 74, 80, 85, 86, 90, 92, 93, 98, 99

Suggested Problems: p. 625-627 #58, 59, 65, 69, 74, 80, 85, 86, 90, 92, 93, 98, 99 Chemistry I Accelerated Study Guideline - Chapter 19 Acids, Bases and Salts ------------------------------------------------------------------------------ By the end of this unit, the skills you should

More information

Review for Solving ph Problems:

Review for Solving ph Problems: Review for Solving ph Problems: Acid Ionization: HA H 2 O A - H 3 O CH 3 COOH H 2 O CH 3 COO - H 3 O Base Ionization: B H 2 O BH OH - 1) Strong Acid complete dissociation [H ] is equal to original [HA]

More information

ph. Weak acids. A. Introduction

ph. Weak acids. A. Introduction ph. Weak acids. A. Introduction... 1 B. Weak acids: overview... 1 C. Weak acids: an example; finding K a... 2 D. Given K a, calculate ph... 3 E. A variety of weak acids... 5 F. So where do strong acids

More information

Acids and Bases. but we will use the term Lewis acid to denote only those acids to which a bond can be made without breaking another bond

Acids and Bases. but we will use the term Lewis acid to denote only those acids to which a bond can be made without breaking another bond Acids and Bases. Brønsted acids are proton donors, and Brønsted bases are proton acceptors. Examples of Brønsted acids: HCl, HBr, H 2 SO 4, HOH, H 3 O +, + NH 4, NH 3, CH 3 CO 2 H, H CH 2 COCH 3, H C CH,

More information

Upon completion of this lab, the student will be able to: H3O + (aq) + A (aq) BH + (aq) + OH (aq) O + ] [H 3. ph = log[h 3.

Upon completion of this lab, the student will be able to: H3O + (aq) + A (aq) BH + (aq) + OH (aq) O + ] [H 3. ph = log[h 3. 1 Learning Outcomes EXPERIMENT B5: ACID/BASE DISSOCIATION CONSTANT Upon completion of this lab, the student will be able to: 1) Estimate the dissociation constant for a weak acid and a weak base. 2) Relate

More information

Sketch the model representation of the first step in the dissociation of water. H 2. O (l) H + (aq) + OH- (aq) + H 2. OH - (aq) + H 3 O+ (aq)

Sketch the model representation of the first step in the dissociation of water. H 2. O (l) H + (aq) + OH- (aq) + H 2. OH - (aq) + H 3 O+ (aq) Lesson Objectives Students will: Create a physical representation of the autoionization of water using the water kit. Describe and produce a physical representation of the dissociation of a strong acid

More information

Acids and Bases CHAPTER 12. Opening Essay

Acids and Bases CHAPTER 12. Opening Essay CHAPTER 12 Acids and Bases Opening Essay Formerly there were rather campy science-fiction television shows in which the hero was always being threatened with death by being plunged into a vat of boiling

More information

6 Reactions in Aqueous Solutions

6 Reactions in Aqueous Solutions 6 Reactions in Aqueous Solutions Water is by far the most common medium in which chemical reactions occur naturally. It is not hard to see this: 70% of our body mass is water and about 70% of the surface

More information

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. CHE 1400 - Spring 2015 - Chapter 7 Homework 7 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1)According to Arrhenius, an acid and a base will react

More information

Auto-ionization of Water

Auto-ionization of Water 2H 2 O H 3 O + + OH Hydronium ion hydroxide ion Q: But how often does this happen? This is the fundamental concept of all acid-base chemistry In pure water, how much of it is water and how much is ions?

More information

Chapter 2 Polar Covalent Bonds; Acids and Bases

Chapter 2 Polar Covalent Bonds; Acids and Bases John E. McMurry http://www.cengage.com/chemistry/mcmurry Chapter 2 Polar Covalent Bonds; Acids and Bases Javier E. Horta, M.D., Ph.D. University of Massachusetts Lowell Polar Covalent Bonds: Electronegativity

More information

Lecture 22 The Acid-Base Character of Oxides and Hydroxides in Aqueous Solution

Lecture 22 The Acid-Base Character of Oxides and Hydroxides in Aqueous Solution 2P32 Principles of Inorganic Chemistry Dr. M. Pilkington Lecture 22 The Acid-Base Character of Oxides and Hydroxides in Aqueous Solution Oxides; acidic, basic, amphoteric Classification of oxides - oxide

More information

NAME PER DATE DUE ACTIVE LEARNING IN CHEMISTRY EDUCATION "ALICE" CHAPTER 21 ACIDS AND BASES. Behavior In Water. 21-1 1997, A.J.

NAME PER DATE DUE ACTIVE LEARNING IN CHEMISTRY EDUCATION ALICE CHAPTER 21 ACIDS AND BASES. Behavior In Water. 21-1 1997, A.J. NAME PER DATE DUE ACTIVE LEARNING IN CEMISTRY EDUCATIN "ALICE" CAPTER 21 ACIDS AND BASES Behavior In Water 21-1 1997, A.J. Girondi NTICE F RIGTS All rights reserved. No part of this document may be reproduced

More information

Equilibrium Constants The following equilibrium constants will be useful for some of the problems.

Equilibrium Constants The following equilibrium constants will be useful for some of the problems. 1 CH302 Exam 4 Practice Problems (buffers, titrations, Ksp) Equilibrium Constants The following equilibrium constants will be useful for some of the problems. Substance Constant Substance Constant HCO

More information

3 The Preparation of Buffers at Desired ph

3 The Preparation of Buffers at Desired ph 3 The Preparation of Buffers at Desired ph Objectives: To become familiar with operating a ph meter, and to learn how to use the Henderson-Hasselbalch equation to make buffer solutions at a desired ph

More information

Chemistry 201. Practical aspects of buffers. NC State University. Lecture 15

Chemistry 201. Practical aspects of buffers. NC State University. Lecture 15 Chemistry 201 Lecture 15 Practical aspects of buffers NC State University The everyday ph scale To review what ph means in practice, we consider the ph of everyday substances that we know from experience.

More information

Aqueous Solutions. Water is the dissolving medium, or solvent. Some Properties of Water. A Solute. Types of Chemical Reactions.

Aqueous Solutions. Water is the dissolving medium, or solvent. Some Properties of Water. A Solute. Types of Chemical Reactions. Aqueous Solutions and Solution Stoichiometry Water is the dissolving medium, or solvent. Some Properties of Water Water is bent or V-shaped. The O-H bonds are covalent. Water is a polar molecule. Hydration

More information

Worksheet 23 Strong Acid/Strong Base Titrations

Worksheet 23 Strong Acid/Strong Base Titrations Worksheet 2 Strong Acid/Strong Base Titrations A. Initial ph This is always determined based solely on the initial concentration of the acid or base being titrated. Every mole of acid or base will produce

More information

4.1 Aqueous Solutions. Chapter 4. Reactions in Aqueous Solution. Electrolytes. Strong Electrolytes. Weak Electrolytes

4.1 Aqueous Solutions. Chapter 4. Reactions in Aqueous Solution. Electrolytes. Strong Electrolytes. Weak Electrolytes Chapter 4 Reactions in Aqueous Solution 4.1 Aqueous Solutions Solution homogeneous mixture of 2 or more substances Solute the substance present in a smaller amount (usually solid in Chap. 4) Solvent the

More information

INTI COLLEGE MALAYSIA A? LEVEL PROGRAMME CHM 111: CHEMISTRY MOCK EXAMINATION: DECEMBER 2000 SESSION. 37 74 20 40 60 80 m/e

INTI COLLEGE MALAYSIA A? LEVEL PROGRAMME CHM 111: CHEMISTRY MOCK EXAMINATION: DECEMBER 2000 SESSION. 37 74 20 40 60 80 m/e CHM111(M)/Page 1 of 5 INTI COLLEGE MALAYSIA A? LEVEL PROGRAMME CHM 111: CHEMISTRY MOCK EXAMINATION: DECEMBER 2000 SESSION SECTION A Answer ALL EIGHT questions. (52 marks) 1. The following is the mass spectrum

More information

Copyright 2009 by Pearson Education, Inc. Upper Saddle River, New Jersey 07458 All rights reserved.

Copyright 2009 by Pearson Education, Inc. Upper Saddle River, New Jersey 07458 All rights reserved. Sample Exercise 17.1 Calculating the ph When a Common Ion is Involved What is the ph of a solution made by adding 0.30 mol of acetic acid and 0.30 mol of sodium acetate to enough water to make 1.0 L of

More information

1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436 #1, 7, 8, 11

1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436 #1, 7, 8, 11 SCH3U- R.H.KING ACADEMY SOLUTION & ACID/BASE WORKSHEET Name: The importance of water - MAKING CONNECTION READING 1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436

More information

RESONANCE, USING CURVED ARROWS AND ACID-BASE REACTIONS

RESONANCE, USING CURVED ARROWS AND ACID-BASE REACTIONS RESONANCE, USING CURVED ARROWS AND ACID-BASE REACTIONS A STUDENT SHOULD BE ABLE TO: 1. Properly use curved arrows to draw resonance structures: the tail and the head of every arrow must be drawn in exactly

More information

EXPERIMENT 20: Determination of ph of Common Substances

EXPERIMENT 20: Determination of ph of Common Substances Materials: ph paper and color chart (ph range 3 to 12) or ph meter distilled water white vinegar household ammonia (or baking soda) spot plate test or 3 small test tubes stirring rod solutions / fruits

More information

3.4 BRØNSTED LOWRY ACIDS AND BASES

3.4 BRØNSTED LOWRY ACIDS AND BASES 96 CAPTER 3 ACIDS AND BASES. TE CURVED-ARROW NOTATION and that the unshared electron pair (and negative charge) is shared equally by the two terminal carbons. C L C A C 1 allyl anion (c) Using the curved-arrow

More information

CHEMISTRY BONDING REVIEW

CHEMISTRY BONDING REVIEW Answer the following questions. CHEMISTRY BONDING REVIEW 1. What are the three kinds of bonds which can form between atoms? The three types of Bonds are Covalent, Ionic and Metallic. Name Date Block 2.

More information

Acid Dissociation Constants and the Titration of a Weak Acid

Acid Dissociation Constants and the Titration of a Weak Acid Acid Dissociation Constants and the Titration of a Weak Acid One of the most important applications of equilibria is the chemistry of acids and bases. The Brønsted-Lowry acid-base theory defines an acid

More information

We remember that molarity (M) times volume (V) is equal to moles so this relationship is the definition of the equivalence point.

We remember that molarity (M) times volume (V) is equal to moles so this relationship is the definition of the equivalence point. Titrations Titration - a titration is defined as the determination of the amount of an unknown reagent (analyte) through the use of a known amount of another reagent (titrant) in an essentially irreversible

More information

Chemical Reactions in Water Ron Robertson

Chemical Reactions in Water Ron Robertson Chemical Reactions in Water Ron Robertson r2 f:\files\courses\1110-20\2010 possible slides for web\waterchemtrans.doc Properties of Compounds in Water Electrolytes and nonelectrolytes Water soluble compounds

More information

Acids and Bases. Problem Set: Chapter 17 questions 5-7, 9, 11, 13, 18, 43, 67a-d, 71 Chapter 18 questions 5-9, 26, 27a-e, 32

Acids and Bases. Problem Set: Chapter 17 questions 5-7, 9, 11, 13, 18, 43, 67a-d, 71 Chapter 18 questions 5-9, 26, 27a-e, 32 Acids and Bases Problem Set: Chapter 17 questions 5-7, 9, 11, 13, 18, 43, 67a-d, 71 Chapter 18 questions 5-9, 26, 27a-e, 32 Arrhenius Theory of Acids An acid base reaction involves the reaction of hydrogen

More information

Experiment 1 Chemical Reactions and Net Ionic Equations

Experiment 1 Chemical Reactions and Net Ionic Equations Experiment 1 Chemical Reactions and Net Ionic Equations I. Objective: To predict the products of some displacement reactions and write net ionic equations. II. Chemical Principles: A. Reaction Types. Chemical

More information