Chapter 10 - Acids & Bases

Save this PDF as:
 WORD  PNG  TXT  JPG

Size: px
Start display at page:

Download "Chapter 10 - Acids & Bases"

Transcription

1 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 acids Which subatomic particles are present in H +? (Why called protic?) Bases: substances that produce hydroxide ions when dissolved in H 2 O Common Strong Bases: Common Weak Bases Page1

2 Bronsted-Lowry Acids & Bases Acid: Proton donor Base: Proton acceptor Implications of the Bronsted-Lowry definition: 1) Free H + does not actually exist in H 2 O 2) Reactions between an acid and base involve proton transfer. i. NH 3 + HCl à ii. HO - + HCN à Conjugated acid/base pair: In an acid/base reaction an acid loses a H + to become its conjugated base and a base gains a H + to become its conjugated acid. The formula for a conjugate acid/base pair differ by Page2

3 Problem: Write the conjugate base for HClO 3. Problem: Write the conjugate acid for HS -. Problem: Identify the following conjugate pairs: a) The conjugated base of hydrogen sulfate ion is. b) The conjugated acid of a cyanide ion is. c) The conjugated base of a bicarbonate ion is. d) The conjugated acid of a bicarbonate ion is. A substance that has a conjugate acid is a: A substance that has a conjugate base is an: A substance that can act as both an acid and a base is: Other amphoteric substances: Identify the conjugate acid-base pairs in the following reactions. HC 2 H 3 O 2(aq) + H 2 O (l) D H 3 O + (aq) + C 2 H 3 O 2 - (aq) NH 3(aq) + H 2 O (l) D NH 4 + (aq) + OH - (aq) Page3

4 What do you notice that is different about the previous reactions? Problem:: Write a balanced acid/base reaction between hydrochloric acid and the phosphate ion. Identify the conjugate acid base pairs Acids and Base Strength When describing the strength of acids and bases, we are referring to the degree of dissociation of the H + or OH - ions. Strong acids and bases completely dissociate. Weak acids and bases only partially dissociate. Strong Acids & Bases. Strong Acids Strong Bases HCl LiOH HBr NaOH HI KOH H 2 SO 4 * Ca(OH) 2 HNO 3 Ba(OH) 2 HClO 4 * Sr(OH) 2 ** HClO 3 OH - are insoluble except 1A ions, Ba 2+. NH4OH is a weak base; *Ca(OH)2 and Sr(OH)2 are slightly soluble in water (depends on temp). **HClO3 is borderline; only about 99% dissociated. Page4

5 - - - Problem: Use the table above to identify the stronger acid in each pair. + a) H 2 O or NH 4 b) HCN or H 2 CO 3 Problem: Use the above table to identify the weaker base in each pair. a) OH - or NH 3 b) CN - - or HCO 3 Page5

6 Equilibrium of Acid-Base Reactions Proton transfer ALWAYS favors reaction of the stronger acid and base to FORM the weaker acid and base. (lies to the side of the weaker ones) In General: Problem: Write a balanced equation for the Rxn between HPO 4 2- and OH -. Identify each acid-base conjugate pair, and determine in which direction the equilibrium is favored Acid Dissociation Constants Do ALL weak acid dissociate the same amount? (Or is there only 1 level of weak?) How do we compare weak acid strengths? Since it is based on the extent of the equilibrium, we need to compare their equilibrium constants! Acid dissociation constant, Ka Page6

7 Problem: Write the Ka expression for phosphoric acid. What is the relationship between the value of Ka and the degree of dissociation? Comparing Weak Acids Because there are different strengths of weak acids, we can compare their Ka values. However, Ka values are awkward (they span large orders of magnitude), so we look at the power of the Ka or by taking log of the Ka to simplify the numerical expression. Compound Name Ka pka H 3 O + Hydronium ion H 3 PO 4 Phosphoric acid 7.5 x HF Hydrofluoric acid 3.5x CH 3 COOH Acetic acid 1.8 x H 2 CO 3 Carbonic acid 4.3 x H 2 PO 4 Dihydrogen phosphate ion 6.2 x NH 4 Ammonium ion 5.6 x HCN Hydrocyanic acid 4.9 x HCO 3 Bicarbonate ion 5.6 x HPO 4 Hydrogen phosphate ion 2.2 x H 2 O Water 1.0 x Page7

8 What is the relationship between acid strength and pka values? Problem: Which acid is stronger? aspirin, pka = 3.49 or vitamin C, pka = 4.1 Problem: The Ka for benzoic acid is 6.5 x What is the pka? Problem: The pka of lactic acid is 3.9. What is the Ka? Problem: Use pka values to predict the direction of the equilibrium in the following reactions. Strategy: 1) Identify the conjugate acid-base pairs. 2) Compare pka values to determine the strongest acid. HC 2 H 3 O 2(aq) + H 2 O (l) D H 3 O + (aq) + C 2 H 3 O 2 - (aq) HC 2 H 3 O 2(aq) + NH 3(aq) D NH 4 + (aq) + C 2 H 3 O 2 - (aq) Page8

9 10.4 Water as Both an Acid and a Base Identify the conjugate acid/base pairs in the following reactions. HF (aq) + H 2 O (l) H 3 O + (aq) + F - (aq) NH 3(aq) + H 2 O (l) D OH - (aq) + NH 4 + (aq) Water is amphoteric, it can be both as an acid or a base. Self-ionization of water: H 2 O (l) + H 2 O (l) D OH - (aq) + H 3 O + (aq) Ion-product constant for water: 2 H 2 O (l) «H 3 O + (aq) + OH - (aq) Neutral: [H 3 O + ] = 10-7 M [OH - ] = 10-7 M Acidic: [H 3 O + ] > 10-7 M [OH - ] < 10-7 M Basic: [H 3 O + ] < 10-7 M [OH - ] > 10-7 M Page9

10 Problem: Is water an acid or a base in the following reaction? H 2 CO 3(aq) + H 2 O (l) «HCO 3 - (aq) + H 3 O + (aq) Problem: Are the following solutions acidic, basic or neutral? Beer; [H 3 O + ] = 3.2 x 10-5 M Milk of Magnesia; [H 3 O + ] = 1.0 x 10-9 M Problem: What is the [OH - ] in a solution of 0.10 M HBr? 10.5 Measuring Acidity with ph Scale Once again, we have encountered awkward large and small numbers. We will use logarithms to simplify the numerical values. ph = power of the hydrogen or hydronium ion concentration. ph= [H 3 O + ] = [H 3 O + ] > 1.0 x 10-7 [H 3 O + ] = 1.0 x 10-7 [H 3 O + ] < 1.0 x 10-7 Page10

11 In H 2 O: ph ranges from Remember: Logarithms are powers of ph unit change Þ 3 ph unit change Þ As ph goes, Acidity goes: We can also work with the [OH - ] on a log scale. poh= [OH - ] = As [H 3 O + ] goes, the [OH - ] goes ph + poh = As [H 3 O + ] goes, the acidity goes At the ph goes, the acidity goes As [OH - ] goes, the alkalinity goes and the acidity goes. As the poh goes up, the alkalinity goes and the acidity goes. Page11

12 Problem: Which solution has a higher H 3 O + concentration, one with a ph of 5 or one with a ph of 9? Which one has the higher OH - concentration? Measuring ph Early measurements were made with indicators, which we still use today. Indicators Indicators are substances (dyes) that change color at various ph values. They are usually weak acids. HA + H 2 O D H 3 O + + A - Early scientists discovered the fiber litmus. The most common acid/base indicator: phenolphthalein. Page12

13 Picture above shows universal indicator: ph Meter A more accurate way to measure ph is with an electronic ph meter Working with ph Page13

14 Problem: What is the ph of a solution with a [H 3 O + ] = 1 x 10-5 M? Problem: What is the ph of a solution with a [H 3 O + ] = 4.3 x 10-3 M? Problem: What is the ph of a solution with a [OH - ] = 2.4 x 10-8 M? Problem: a)what is the H 3 O + concentration of saliva, with a ph of 6.70? b)is it acidic or basic? Problem: What is the ph of a M solution of HCl? Problem: What is the H 3 O + concentration of saliva, with a poh of 3.42? Is it acidic or basic? Problem: What is the poh of a 0.024M solution of Ba(OH) 2? Page14

15 10.7 presented later 10.8 Common Acid-Base Reactions 1) Acid Base Neutralization reactions: Acid + Base salt + water 2) Acids with active Metals (single replacement reaction) Mg (s) + 2 HCl (aq) MgCl 2(aq) + H 2(g) 3) Acids with Carbonates and Bicarbonates Similar result for bicarbonate: Can also be written with hydronium Page15

16 4) Acids with Amines + HCl (aq) + RNH 2(aq) RNH 3 (aq) + Cl - (aq) Amines react with acids in the same way that ammonia would: 10.9 Acidity and Basicity of Salt solution: ions of strong acids and strong bases do not react with water (don t undergo hydrolysis) and therefore have no effect on the ph of a solution. ions of weak acids react with water to form OH - ions, forming basic soln. e.g. F- from the weak acid HF ions of weak bases react with water to form H 3 O + ions, forming acidic soln. e.g. NH 4 + from the weak base NH 4 OH Examples in salts. Salt of strong acid and weak base : Salt of strong base and weak acid : Salt of strong acid and strong base : Salt of weak acid and weak base : Page16

Acids, Bases, and ph. ACIDS, BASES, & ph

Acids, 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 information

Chem 1046 Lecture Notes Chapter 17

Chem 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 information

Strong and Weak. Acids and Bases

Strong 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 information

Contents and Concepts

Contents 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 information

ACID BASE EQUILIBRIUM

ACID 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 information

Acids - Bases in Water

Acids - Bases in Water more equilibrium Dr. Fred Omega Garces Chemistry, Miramar College 1 Acids-Bases Characteristics Acids (Properties) Taste Sour Dehydrate Substances Neutralizes bases Dissolves metals Examples: Juices: TJ,

More information

Chapter 7 Acids and Bases

Chapter 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 information

Chemistry 400 Homework #3, Chapter 16: Acid-Base Equilibria

Chemistry 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 information

In 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 +.

In 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 information

Unit 6: ACIDS AND BASES

Unit 6: ACIDS AND BASES Unit 6: Acids and Bases Honour Chemistry Unit 6: ACIDS AND BASES Chapter 16: Acids and Bases 16.1: Brønsted Acids and Bases Physical and Chemical Properties of Acid and Base Acids Bases Taste Sour (Citric

More information

Acid/Base Definitions

Acid/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 information

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

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 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 information

Chap 16 Chemical Equilibrium HSU FUYIN

Chap 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

Unit Nine Notes N C U9

Unit Nine Notes N C U9 Unit Nine Notes N C U9 I. AcidBase Theories A. Arrhenius Acids and Bases 1. Acids contain hydronium ions (H O ) commonly referred to as hydrogen ions (H ) that dissociate in water a. Different acids release

More information

A) Arrhenius Acids produce H+ and bases produce OH not always used because it only IDs X OH as basic species

A) 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 information

CHAPTER 19. Acids, Bases, and Salts Acid Base Theories

CHAPTER 19. Acids, Bases, and Salts Acid Base Theories CHAPTER 19 Acids, Bases, and Salts 19.1 Acid Base Theories ACIDS tart or sour taste Electrolytes Strong acids are corrosive Acid Facts... indicators will change color Blue litmus paper turns pink react

More information

THE BIG IDEA: REACTIONS. 1. Review nomenclature rules for acids and bases and the formation of acids and bases from anhydrides. (19.

THE BIG IDEA: REACTIONS. 1. Review nomenclature rules for acids and bases and the formation of acids and bases from anhydrides. (19. HONORS CHEMISTRY - CHAPTER 19 ACIDS, BASES, AND SALTS OBJECTIVES AND NOTES - V14 NAME: DATE: PAGE: THE BIG IDEA: REACTIONS Essential Questions 1. What are the different ways chemists define acids and bases?

More information

Chem 30A. Ch 14. Acids and Bases

Chem 30A. Ch 14. Acids and Bases Chem 30A Ch 14. Acids and Bases Acids and Bases Acids and Bases Acids Sour taste Dissolve many metals Turn litmus paper red. Egs. Ace9c acid (vinegar), citric acid (lemons) Bases Bi>er taste, slippery

More information

Part One: Acid-Base Concepts. 1. Sour taste. (Examples: vinegar = acetic acid; lemons - citric acid) yellow

Part One: Acid-Base Concepts. 1. Sour taste. (Examples: vinegar = acetic acid; lemons - citric acid) yellow CHAPTER 15: ACIDS AND BASES Part One: Acid-Base Concepts A. Properties of Aqueous Solutions of Acids. 1. Sour taste. (Examples: vinegar = acetic acid; lemons - citric acid) 2. Change the colors of many

More information

10.1 Acids and Bases in Aqueous Solution

10.1 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 information

Chem 105 Tuesday March 8, Chapter 17. Acids and Bases

Chem 105 Tuesday March 8, Chapter 17. Acids and Bases Chem 105 Tuesday March 8, 2011 Chapter 17. Acids and Bases 1) Define Brønsted Acid and Brønsted Base 2) Proton (H + ) transfer reactions: conjugate acid-base pairs 3) Water and other amphiprotic substances

More information

UNIT 14 - Acids & Bases

UNIT 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 information

Acids and Bases. Feb 28 4:40 PM

Acids and Bases. Feb 28 4:40 PM Acids and Bases H O s O Cl H O O H H N H Na O H H Feb 28 4:40 PM Properties of Acids 1. Taste sour 2. Conduct electrical current 3. Liberate H 2 gas when reacted with a metal. 4. Cause certain dyes to

More information

Chapters 15 & 16 ACIDS & BASES ph & Titrations

Chapters 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 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

1. Strengths of Acids and Bases 2. K a, K b 3. Ionization of Water 4. Relative Strengths of Brønsted-Lowry Acids and Bases

1. 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 information

SCH4U Chapter 8 review

SCH4U Chapter 8 review Name: Class: Date: SCH4U Chapter 8 review Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Which statement does not describe a characteristic of acidic

More information

Proton Transfer Acids - Base. Dr. Fred Omega Garces Chemistry 201. Miramar College

Proton Transfer Acids - Base. Dr. Fred Omega Garces Chemistry 201. Miramar College 16.2 Acids Base Proton Transfer Dr. Fred Omega Garces Chemistry 201 Miramar College Important Notes: K a when H 3 O + is produced, K b when OH is produced 1 Acids Bases; Proton Transfer BrønstedLowry AcidsBases

More information

Section 32 Acids and Bases. Copyright (c) 2011 by Michael A. Janusa, PhD. All rights reserved.

Section 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 information

CHAPTER Acid & Base

CHAPTER Acid & Base CHAPTER 19 19.1 Acid & Base Common Reactions with Acids Dilute: small amount of solute 1-M Concentrated: large amount of solute Indicator: changes color to show the presence of acids or bases : eat or

More information

Chapter 14 Properties of Acids and Bases

Chapter 14 Properties of Acids and Bases Section 14.1 Defining Acids and Bases Properties of acids and bases Chapter 14 Properties of Acids and Bases taste sour Acids taste bitter Bases conduct electricity no characteristic feel react with metals

More information

Equations. M = n/v. M 1 V 1 = M 2 V 2 if the moles are the same n 1 n 2 you can cancel out the n s. ph = -log [H + ] poh = -log [OH - ] ph + poh = 14

Equations. M = n/v. M 1 V 1 = M 2 V 2 if the moles are the same n 1 n 2 you can cancel out the n s. ph = -log [H + ] poh = -log [OH - ] ph + poh = 14 Equations M = n/v M 1 V 1 = M 2 V 2 if the moles are the same n 1 n 2 you can cancel out the n s. ph = -log [H + ] poh = -log [OH - ] ph + poh = 14 [H 3 O + ] = 10^-pH [OH - ] = 10^-pOH [H 3 O + ] [OH

More information

Duncan. UNIT 14 - Acids & Bases. COMMON ACIDS NOTES lactic acetic phosphoric NAMING ACIDS NOTES

Duncan. 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 information

Dynamic equilibrium: rate of evaporation = rate of condensation II. In a closed system a solid obtains a dynamic equilibrium with its dissolved state

Dynamic equilibrium: rate of evaporation = rate of condensation II. In a closed system a solid obtains a dynamic equilibrium with its dissolved state CHEMISTRY 111 LECTURE EXAM III Material PART 1 CHEMICAL EQUILIBRIUM Chapter 14 I Dynamic Equilibrium I. In a closed system a liquid obtains a dynamic equilibrium with its vapor state Dynamic equilibrium:

More information

Acid and Bases. Physical Properties. Chemical Properties. Indicators. Corrosive when concentrated. Corrosive when concentrated.

Acid and Bases. Physical Properties. Chemical Properties. Indicators. Corrosive when concentrated. Corrosive when concentrated. Physical Properties Acid and Bases Chemistry 30 Acids Corrosive when concentrated Have a sour taste Bases Corrosive when concentrated Have a bitter taste Often have a sharp odour Chemical Properties Indicators

More information

Grace King High School Chemistry Test Review

Grace 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 information

Chapter 10. Acids, Bases, and Salts

Chapter 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 information

Name Date Class ACID-BASE THEORIES

Name 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 information

Chemistry 40S Acid-Base Equilibrium (This unit has been adapted from

Chemistry 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 information

Reactions in Aqueous Solutions I: Acids, Bases & Salts

Reactions in Aqueous Solutions I: Acids, Bases & Salts 10 Reactions in Aqueous Solutions I: Acids, Bases & Salts CHAPTER GOALS 1. Properties of Aqueous Solutions of Acids and Bases 2. The Arrhenius Theory 3. The Hydronium Ion (Hydrated Hydrogen Ion) 4. The

More information

Amount of substance dissolved in 1 L of water

Amount of substance dissolved in 1 L of water Chapter 7: Phenomena Phenomena: Scientists dissolved different substances in water and then measured the [H + ] and [OH - ] concentrations in each solution. What patterns do you notice about the substances?

More information

Chapter 16. Dr Ayman Nafady

Chapter 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 information

Chapter 7: Phenomena. Chapter 7 Acids and Bases. Acids and Bases. Acids and Bases. Acids and Bases

Chapter 7: Phenomena. Chapter 7 Acids and Bases. Acids and Bases. Acids and Bases. Acids and Bases Chapter 7: Phenomena Phenomena: Scientists dissolved different substances in water and then measured the [H + ] and [OH - ] concentrations in each solution. What patterns do you notice about the substances?

More information

Chapter 10. Acids and Bases

Chapter 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 information

What is an acid? What is a base?

What 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 information

Chemistry 102 Chapter 15 ACID-BASE CONCEPTS

Chemistry 102 Chapter 15 ACID-BASE CONCEPTS General Properties: ACID-BASE CONCEPTS ACIDS BASES Taste sour Bitter Change color of indicators Blue Litmus turns red no change Red Litmus no change turns blue Phenolphtalein Colorless turns pink Neutralization

More information

Unit 9. Acids, Bases, & Salts Acid/Base Equilibrium

Unit 9. Acids, Bases, & Salts Acid/Base Equilibrium Unit 9 Acids, Bases, & Salts Acid/Base Equilibrium Properties of Acids sour or tart taste strong acids burn; weak acids feel similar to H 2 O acid solutions are electrolytes acids react with most metals

More information

Acids and Bases. Bases react with acids to form water and a salt. Bases do not commonly with metals.

Acids and Bases. Bases react with acids to form water and a salt. Bases do not commonly with metals. Acids and Bases Properties of Acids and Bases Acids taste. Lemon juice and, for example, are both aqueous solutions of acids. Acids conduct electricity; they are. Some are strong electrolytes, while others

More information

CHAPTER 13: ACIDS & BASES. Section Arrhenius Acid & Bases Svante Arrhenius, Swedish chemist ( ).

CHAPTER 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 information

INTRODUCTION TO ACIDS AND BASES

INTRODUCTION TO ACIDS AND BASES INTRODUCTION TO ACIDS AND BASES ALIGNED STANDARDS S.C. 912.P.8.11 Relate acidity and basicity to hydronium and hydroxide concentration and ph. S.C.912.N.1.2 Describe and explain what characterizes science

More information

Acid / Base Properties of Salts

Acid / Base Properties of Salts Acid / Base Properties of Salts n Soluble ionic salts produce may produce neutral, acidic, or basic solutions depending on the acidbase properties of the individual ions. n Consider the salt sodium nitrate,

More information

Mr. Storie 40S Chemistry Student Acid and bases Unit. Acids and Bases

Mr. Storie 40S Chemistry Student Acid and bases Unit. Acids and Bases Acids and Bases 1 UNIT 4: ACIDS & BASES OUTCOMES All important vocabulary is in Italics and bold. Outline the historical development of acid base theories. Include: Arrhenius, BronstedLowry, Lewis. Write

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

(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

CHEMISTRY. Chapter 16 Acid-Base Equilibria

CHEMISTRY. 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 information

Unit 2 Acids and Bases

Unit 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 information

-a base contains an OH group and ionizes in solutions to produce OH - ions: Neutralization: Hydrogen ions (H + ) in solution form

-a base contains an OH group and ionizes in solutions to produce OH - ions: Neutralization: Hydrogen ions (H + ) in solution form NOTES Acids, Bases & Salts Arrhenius Theory of Acids & Bases: an acid contains hydrogen and ionizes in solutions to produce H+ ions: a base contains an OH group and ionizes in solutions to produce OH ions:

More information

Aqueous solutions of acids have a sour Aqueous solutions of bases taste bitter

Aqueous solutions of acids have a sour Aqueous solutions of bases taste bitter Acid and Bases Exam Review Honors Chemistry 3 April 2012 Chapter 14- Acids and Bases Section 14.1- Acid and Base Properties List five general properties of aqueous acids and bases Properties of Acids Properties

More information

Acids & Bases. Strong Acids. Weak Acids. Strong Bases. Acetic Acid. Arrhenius Definition: Classic Definition of Acids and Bases.

Acids & 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 information

Part 01 - Assignment: Introduction to Acids &Bases

Part 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 information

Chapter Menu Chapter Menu

Chapter 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 information

Acids and Bases. Properties, Reactions, ph, and Titration

Acids and Bases. Properties, Reactions, ph, and Titration Acids and Bases Properties, Reactions, ph, and Titration C-19 2017 Properties of acids 1. Taste Sour (don t try this except with foods). 2. Are electrolytes (conduct electricity). Some are strong, some

More information

Acids and Bases. Acid. Acid Base 2016 OTHS. Acid Properties. A compound that produces H + ions when dissolved in water. Examples!

Acids and Bases. Acid. Acid Base 2016 OTHS. Acid Properties. A compound that produces H + ions when dissolved in water. Examples! Acids and Bases Acid A compound that produces H + ions when dissolved in water. Examples! Vinegar Acetic acid Lemon Juice Citric acid Sour Candy Malic acid (and others) Milk Lactic acid HCl(aq) Acid Properties

More information

Name. Academic Chemistry. Acid Base. Notes. Unit #14 Test Date: cincochem.pbworks.com

Name. Academic Chemistry. Acid Base. Notes. Unit #14 Test Date: cincochem.pbworks.com Periodic Table Name Academic Chemistry Acids & Bases Notes Unit #14 Test Date: 20 cincochem.pbworks.com Acid Base cincochem.pbworks.com Notes Find ph To go from [H 3 O + ] to ph EXAMPLE: [H 3 O + ] = 3.23

More information

Acids and Bases. A strong base is a substance that completely ionizes in aqueous solutions to give a cation and a hydroxide ion.

Acids 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 information

Unit 9: Acid and Base Multiple Choice Practice

Unit 9: Acid and Base Multiple Choice Practice Unit 9: Acid and Base Multiple Choice Practice Name June 14, 2017 1. Consider the following acidbase equilibrium: HCO3 H2O H2CO3 OH In the reaction above, the BrönstedLowry acids are: A. H2O and OH B.

More information

Chpt 16: Acids and Bases

Chpt 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 information

Acids & Bases. Properties. Definitions Arrhenius acid (1880 s)

Acids & Bases. Properties. Definitions Arrhenius acid (1880 s) Name Date Properties Acid Base Taste sour/tart bitter Feel burn slippery Metal rxn yes no Litmus red blue Conductivity yes yes Definitions Arrhenius acid (1880 s) Acids & Bases In actuality the reaction

More information

Chapter 15: Acids and Bases Arrhenius Definitions:

Chapter 15: Acids and Bases Arrhenius Definitions: Chapter 15: Acids and Bases Arrhenius Definitions: Acids and Bases s - compounds that produce an increase in [H + ] when dissolved in water bases - compounds that produce an increase in [OH ] when dissolved

More information

ACIDS AND BASES CONTINUED

ACIDS 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 information

ACIDS, BASES, AND SALTS

ACIDS, 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 information

Unit 4a Acids, Bases, and Salts Theory

Unit 4a Acids, Bases, and Salts Theory Unit 4a Acids, Bases, and Salts Theory Chemistry 12 Arrhenius Theory of Acids and Bases The first theory that was proposed to explain the actions of acids and bases was by Svante Arrhenius. It is still

More information

Chapter 16 Acid-Base Equilibria

Chapter 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 information

Name: Per: Date: Unit 11 - Acids, Bases and Salts Chemistry Accelerated Chemistry I Define each of the following: 1. Acidic hydrogens.

Name: Per: Date: Unit 11 - Acids, Bases and Salts Chemistry Accelerated Chemistry I Define each of the following: 1. Acidic hydrogens. Name: Per: Date: Unit 11 - Acids, Bases and Salts Chemistry Accelerated Chemistry I Define each of the following: 1. Acidic hydrogens 2. Binary acids 3. Oxyacids 4. Carboxylic acid 5. Amines Name the following

More information

What is an acid? What is a base?

What 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 information

1. Properties of acids: 1. Contain the ion Bases: 1. Contain the ion. 4. Found on Table 4. Found on table

1. Properties of acids: 1. Contain the ion Bases: 1. Contain the ion. 4. Found on Table 4. Found on table For each word, provide a short but specific definition from YOUR OWN BRAIN! No boring textbook definitions. Write something to help you remember the word. Explain the word as if you were explaining it

More information

Acids and Bases Written Response

Acids 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 information

Unit 9: Acids and Bases Chapter 19

Unit 9: Acids and Bases Chapter 19 Unit 9: Acids and Bases Chapter 19 I. Introduction In aqueous solutions, the solvent is. Aqueous solutions contain. In the self-ionization of water, the hydrogen ion (H+) exists in solution as the ion.

More information

Chapter 14 Acid- Base Equilibria Study Guide

Chapter 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 information

Worksheet 4.1 Conjugate Acid-Base Pairs

Worksheet 4.1 Conjugate Acid-Base Pairs Worksheet 4.1 Conjugate AcidBase Pairs 1. List five properties of acids that are in your textbook. Acids conduct electricity, taste sour, neutralize bases, change the color of indicators, and react with

More information

Acids and Bases Review Worksheet II Date / / Period. Molarity. moles L. Normality [H 3 O +1 ] [OH -1 ] ph poh

Acids and Bases Review Worksheet II Date / / Period. Molarity. moles L. Normality [H 3 O +1 ] [OH -1 ] ph poh Honors Chemistry Name Acids and Bases Review Worksheet II Date / / Period Solute Name of Solute Molar Mass grams mole Molarity moles L Normality [H 3 O +1 ] [OH ] ph poh Acidic or Basic 1. HCl Hydrochloric

More information

Unit 10: Acids and Bases

Unit 10: Acids and Bases Unit 10: Acids and Bases PROPERTIES OF ACIDS & BASES Properties of an Acid: a Tastes sour substance which dissociates (ionizes, breaks apart in solution) in water to form hydrogen ions Turns blue litmus

More information

Chapter 16. Acid-Base Equilibria

Chapter 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 information

Acids and Bases. Unit 10

Acids and Bases. Unit 10 Acids and Bases Unit 10 1 Properties of Acids and Bases Acids Bases Taste Sour Turns Litmus Dye Red Reacts with Metals to give H 2 (g) Taste Bitter Turns Litmus Dye Blue Do Not React with Metals Reacts

More information

Chapter 14: Acids and Bases

Chapter 14: Acids and Bases Chapter 14: Acids and Bases Properties of Acids and Bases What is an acid? Some examples of common items containing acids: Vinegar contains acetic acid; lemons and citrus fruits contain citric acid; many

More information

ACID-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. 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 information

Aqueous Reactions and Solution Stoichiometry (continuation)

Aqueous 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 information

ACID BASE TEST (2 nd half of class) Acid-base titration lab 2 nd half. Chapter 18 Acids and Bases Campbell Chemistry Name

ACID BASE TEST (2 nd half of class) Acid-base titration lab 2 nd half. Chapter 18 Acids and Bases Campbell Chemistry Name Date In Class 3/31 Thurs. Equilibrium Test Homework (to be done that night, or before coming to the next class) Watch Acid Base Video 1. What are Acids and Bases? 4/1 Fri Video 1 discussion: Identifying

More information

Acids & Bases. Chapter 17

Acids & Bases. Chapter 17 Acids & Bases Chapter 17 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 3 O + )

More information

CHEMISTRY 1220 CHAPTER 16 PRACTICE EXAM

CHEMISTRY 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 information

Chapter 16 - Acids and Bases

Chapter 16 - Acids and Bases Chapter 16 - Acids and Bases 16.1 Acids and Bases: The Brønsted Lowry Model 16.2 ph and the Autoionization of Water 16.3 Calculations Involving ph, K a and K b 16.4 Polyprotic Acids 16.1 Acids and Bases:

More information

Unit 9: Acids, Bases, & Salts

Unit 9: Acids, Bases, & Salts STUDENT VERSION Unit 9: Acids, Bases, & Salts Unit Vocabulary: Arrhenius acid Arrhenius base Bronsted-Lowry acid Bronsted-Lowry base Electrolyte hydronium ion hydroxide ion indicator (acid/base) neutralization

More information

Chapter 14. Objectives

Chapter 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 information

Acids and Bases. Chapters 20 and 21

Acids and Bases. Chapters 20 and 21 Acids and Bases Chapters 20 and 21 Acid and Bases Have a sour taste. Vinegar is a solution of acetic acid. Citrus fruits contain citric acid. React with certain metals to produce hydrogen gas. React with

More information

Resources:

Resources: I. A/B General A. Definitions 1. Arrhenius 2. B-L 3. Lewis *H+=H3O+ B. Properties 1. Acid 2. Base II. ACIDS A. Types 1. Binary 2. Ternary 3. Acid Anhydride B. Protic 1. mono 2. di 3. tri C. Strengths 1.

More information

Acids, Bases and ph Preliminary Course. Steffi Thomas 14/09/2017

Acids, 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 information

AP Study Questions

AP Study Questions ID: A AP 16.4-16.7 Study Questions Multiple Choice Identify the choice that best completes the statement or answers the question. 1 What is the ph of an aqueous solution at 25.0 C in which [H + ] is 0.0025

More information

I II III IV. Volume HCl added. 1. An equation representing the reaction of a weak acid with water is

I II III IV. Volume HCl added. 1. An equation representing the reaction of a weak acid with water is 1. An equation representing the reaction of a weak acid with water is A. HCl + H 2 O H 3 O + + Cl B. NH 3 + H 2 O NH 4 + + OH C. HCO 3 H 2 O H 2 CO 3 + OH D. HCOOH + H 2 O H 3 O + + HCOO 2. The equilibrium

More information

Indicator Color in acid (ph < 7) Color at ph = 7 Color in base (ph > 7) Phenolphthalein Bromothymol Blue Red Litmus Blue Litmus

Indicator Color in acid (ph < 7) Color at ph = 7 Color in base (ph > 7) Phenolphthalein Bromothymol Blue Red Litmus Blue Litmus Unit 9: Acids and Bases Notes Introduction and Review 1. Define Acid: 2. Name the following acids: HCl H2SO4 H2SO3 H2S 3. Bases usually contain 4. Name the following bases: NaOH Ca(OH)2 Cu(OH)2 NH4OH Properties

More information

11/14/10. Properties of Acids! CHAPTER 15 Acids and Bases. Table 18.1

11/14/10. 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 information

Chapter 15 - Acids and Bases Fundamental Concepts

Chapter 15 - Acids and Bases Fundamental Concepts Chapter 15 - Acids and Bases Fundamental Concepts Acids and Bases: Basic Definitions Properties of Acids Sour Taste React with active metals (Al, Zn, Fe) to yield H 2 gas: Corrosive React with carbonates

More information