1 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 used in industry and the laboratory, and give two properties of each. Define acid and base according to Arrhenius s theory of ionization. Explain the differences between strong and weak acids and bases.
2 Section 1 Properties of Acids and Bases Acids 1. Aqueous solutions of acids have a sour taste. 2. Acids change the color of acid-base indicators. 3. Some acids react with active metals and release hydrogen gas, H 2. Ba(s) + H 2 SO 4 (aq) BaSO 4 (s) + H 2 (g) 4. Acids react with bases to produce salts and water. 5. Acids conduct electric current.
3 Section 1 Properties of Acids and Bases Acids, continued Acid Nomenclature A binary acid is an acid that contains only two different elements: hydrogen and one of the more electronegative elements. HF, HCl, HBr, and HI Binary Acid Nomenclature 1. The name of a binary acid begins with the prefix hydro-. 2. The root of the name of the second element follows this prefix. 3. The name then ends with the suffix -ic.
4 Section 1 Properties of Acids and Bases Acids, continued Acid Nomenclature, continued
5 Section 1 Properties of Acids and Bases Acids, continued Acid Nomenclature, continued An oxyacid is an acid that is a compound of hydrogen, oxygen, and a third element, usually a nonmetal. HNO 3, H 2 SO 4 The names of oxyacids follow a pattern. The names of their anions are based on the names of the acids.
6 Section 1 Properties of Acids and Bases Acids, continued Acid Nomenclature, continued
7 Section 1 Properties of Acids and Bases Some Common Industrial Acids Sulfuric Acid Sulfuric acid is the most commonly produced industrial chemical in the world. Nitric Acid Phosphoric Acid Hydrochloric Acid Concentrated solutions of hydrochloric acid are commonly referred to as muriatic acid. Acetic Acid Pure acetic acid is a clear, colorless, and pungent-smelling liquid known as glacial acetic acid.
8 Section 1 Properties of Acids and Bases Bases 1. Aqueous solutions of bases taste bitter. 2. Bases change the color of acid-base indicators. 3. Dilute aqueous solutions of bases feel slippery. 4. Bases react with acids to produce salts and water. 5. Bases conduct electric current.
9 Section 1 Properties of Acids and Bases Arrhenius Acids and Bases An Arrhenius acid is a chemical compound that increases the concentration of hydrogen ions, H +, in aqueous solution. An Arrhenius base is a substance that increases the concentration of hydroxide ions, OH, in aqueous solution.
10 Section 1 Properties of Acids and Bases Arrhenius Acids and Bases, continued Aqueous Solutions of Acids Arrhenius acids are molecular compounds with ionizable hydrogen atoms. Their water solutions are known as aqueous acids. All aqueous acids are electrolytes.
11 Section 1 Properties of Acids and Bases Arrhenius Acids and Bases, continued Aqueous Solutions of Acids, continued Common Aqueous Acids
12 Section 1 Properties of Acids and Bases Arrhenius Acids and Bases, continued Strength of Acids A strong acid is one that ionizes completely in aqueous solution. a strong acid is a strong electrolyte HClO 4, HCl, HNO 3 A weak acid releases few hydrogen ions in aqueous solution. hydronium ions, anions, and dissolved acid molecules in aqueous solution HCN Organic acids ( COOH), such as acetic acid
13 Section 1 Properties of Acids and Bases Arrhenius Acids and Bases, continued Aqueous Solutions of Bases Most bases are ionic compounds containing metal cations and the hydroxide anion, OH. dissociate in water s HO 2 NaOH( ) Na ( aq ) + OH ( aq) Ammonia, NH 3, is molecular Ammonia produces hydroxide ions when it reacts with water molecules. NH 3( aq ) + H2O( l ) NH 4( aq ) + OH ( aq)
14 Section 1 Properties of Acids and Bases Arrhenius Acids and Bases, continued Strength of Bases The strength of a base depends on the extent to which the base dissociates. Strong bases are strong electrolytes
15 Section 1 Properties of Acids and Bases Relationship of [H 3 O + ] to [OH ]
16 Section 2 Acid-Base Theories Objectives Define and recognize Brønsted-Lowry acids and bases. Define a Lewis acid and a Lewis base. Name compounds that are acids under the Lewis definition but are not acids under the Brønsted-Lowry definition.
17 Section 2 Acid-Base Theories Brønsted-Lowry Acids and Bases A Brønsted-Lowry acid is a molecule or ion that is a proton donor. Hydrogen chloride acts as a Brønsted-Lowry acid when it reacts with ammonia. HCl NH NH + Cl 3 4 Water can act as a Brønsted-Lowry acid. H2O( l ) + NH 3( aq ) NH 4( aq ) + OH ( aq)
18 Section 2 Acid-Base Theories Brønsted-Lowry Acids and Bases, continued A Brønsted-Lowry base is a molecule or ion that is a proton acceptor. Ammonia accepts a proton from the hydrochloric acid. It acts as a Brønsted-Lowry base. HCl NH3 NH4 + Cl The OH ion produced in solution by Arrhenius hydroxide bases (NaOH) is the Brønsted-Lowry base. The OH ion can accept a proton
19 Section 2 Acid-Base Theories Brønsted-Lowry Acids and Bases, continued In a Brønsted-Lowry acid-base reaction, protons are transferred from one reactant (the acid) to another (the base). HCl NH NH + Cl acid base 3 4
20 Section 2 Acid-Base Theories Monoprotic and Polyprotic Acids A monoprotic acid is an acid that can donate only one proton (hydrogen ion) per molecule. HClO 4, HCl, HNO 3 only one ionization step HCl( g ) + H O( l) H O ( aq ) + Cl ( aq) 2 3
21 Section 2 Acid-Base Theories Monoprotic and Polyprotic Acids, continued A polyprotic acid is an acid that can donate more than one proton per molecule. H 2 SO 4, H 3 PO 4 Multiple ionization steps (1) (2) H SO ( l ) + H O( l ) H O ( aq ) + HSO ( aq) HSO aq + l aq + 2 4( ) H2O( ) H3O ( ) SO 4 ( l) Sulfuric acid solutions contain H 3 O +, 2 HSO4 and SO4 ions
22 Section 2 Acid-Base Theories Monoprotic and Polyprotic Acids, continued A diprotic acid is the type of polyprotic acid that can donate two protons per molecule H 2 SO 4 A triprotic acid is the type of polyprotic acid that can donate three protons per molecule. H 3 PO 4
23 Section 2 Acid-Base Theories Lewis Acids and Bases A Lewis acid is an atom, ion, or molecule that accepts an electron pair to form a covalent bond. The Lewis definition is the broadest of the three acid definitions. A bare proton (hydrogen ion) is a Lewis acid H ( aq ) + :NH ( aq) [H NH ] ( aq ) or [NH ] ( aq) 3 3 4
24 Section 2 Acid-Base Theories Lewis Acids and Bases, continued The formula for a Lewis acid need not include hydrogen. The silver ion can be a Lewis acid Ag ( aq ) + 2 :NH ( aq ) [H N Ag NH ] ( aq ) or [Ag(NH ) ] Any compound in which the central atom has three valence electrons and forms three covalent bonds can react as a Lewis acid. BF ( aq ) F ( aq ) BF ( aq) 3 4
25 Section 2 Acid-Base Theories Lewis Acids and Bases, continued Acid Base Definitions
26 Section 3 Acid-Base Reactions Objectives Describe a conjugate acid, a conjugate base, and an amphoteric compound. Explain the process of neutralization. Define acid rain, give examples of compounds that can cause acid rain, and describe effects of acid rain.
27 Section 3 Acid-Base Reactions Conjugate Acids and Bases The species that remains after a Brønsted-Lowry acid has given up a proton is the conjugate base of that acid. HF( aq ) + H2O( l ) F ( aq ) + H3O ( aq) acid conjugate base
28 Section 3 Acid-Base Reactions Conjugate Acids and Bases, continued Brønsted-Lowry acid-base reactions involve two acid-base pairs, known a conjugate acid-base pairs. HF( aq ) + H2O( l ) F ( aq ) + H3O ( aq) acid 1 base 2 base 1 acid 2
30 Section 3 Acid-Base Reactions Conjugate Acids and Bases, continued Strength of Conjugate Acids and Bases The stronger an acid is, the weaker its conjugate base The stronger a base is, the weaker its conjugate acid HCl( g ) + H O( l ) H O ( aq ) + Cl ( aq) 2 3 strong acid base acid weak base
31 Section 3 Acid-Base Reactions Conjugate Acids and Bases, continued Strength of Conjugate Acids and Bases, continued Proton transfer reactions favor the production of the weaker acid and the weaker base. HClO ( aq ) + H O( l ) H O ( aq ) + ClO ( aq) stronger acid stronger base weaker acid weaker base The reaction to the right is more favorable CH COOH( aq ) + H O( l ) H O ( aq ) + CH COO ( aq) weaker acid weaker base stronger acid stronger base The reaction to the left is more favorable
32 Section 3 Acid-Base Reactions Relative Strengths of Acids and Bases Relative Strengths of Acids and Bases
33 Section 3 Acid-Base Reactions Amphoteric Compounds Any species that can react as either an acid or a base is described as amphoteric. example: water water can act as a base H SO ( aq ) + H O( l ) H O ( aq ) + HSO ( aq) acid 1 base 2 acid 2 base 1 water can act as an acid NH 3( g ) + H2O( l ) NH 4( aq ) OH ( aq) base 1 acid 2 acid 1 base 2
34 Section 3 Acid-Base Reactions Amphoteric Compounds, continued OH in a Molecule The covalently bonded IOH group in an acid is referred to as a hydroxyl group. Molecular compounds containing OH groups can be acidic or amphoteric. The behavior of a compound is affected by the number of oxygen atoms bonded to the atom connected to the OH group.
35 Section 3 Acid-Base Reactions Oxyacids of Chlorine
36 Section 3 Acid-Base Reactions Neutralization Reactions Strong Acid-Strong Base Neutralization In aqueous solutions, neutralization is the reaction of hydronium ions and hydroxide ions to form water molecules. A salt is an ionic compound composed of a cation from a base and an anion from an acid. HCl( aq ) + NaOH( aq ) NaCl( aq ) H O( l) 2
37 Section 3 Acid-Base Reactions Acid Rain NO, NO 2, CO 2, SO 2, and SO 3 gases from industrial processes can dissolve in atmospheric water to produce acidic solutions. example: SO ( g ) + H O( l ) H SO ( aq) Very acidic rain is known as acid rain. Acid rain can erode statues and affect ecosystems.
Chemistry I Notes Unit 10: Acids and Bases Acids 1. Sour taste. 2. Acids change the color of acid- base indicators (turn blue litmus red). 3. Some acids react with active metals and release hydrogen gas,
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
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
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
Assessment Chapter Test B Chapter: Acids and Bases PART I In the space provided, write the letter of the term or phrase that best completes each statement or best answers each question. 1. Which of the
Chapter 6 Acids, Bases, and Acid-Base Reactions Chapter Map Arrhenius Acid Definition Anacid is a substance that generates hydronium ions, H 3 O + (often described as H + ), when added to water. An acidic
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,
Chapter 15 Aqueous Equilibria: Acids and Bases Properties of Acids and Bases Generally, an acid is a compound that releases hydrogen ions, H +, into water. Blue litmus is used to test for acids. Blue litmus
Acids and bases Properties of Acids and Bases SECTION 1 Many foods have acid in them Sour milk lactic acid Vinegar acetic acid Citrus fruits citric acid Apples malic acid Grape juice tartaric acid Many
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
Chemistry: The Central Science Chapter 16: Acid-Base Equilibria 16.1: Acids and Bases: A Brief Review Acids have a sour taste and cause certain dyes to change color Base have a bitter taste and feel slippery
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
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
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
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.
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
SCHOOL YEAR 2017-18 NAME: CH- 13 IONS IN AQUEOUS SOLUTIONS AND COLLIGATIVE PROPERTIES SUBJECT: CHEMISTRY GRADE : 11 TEST A Choose the best answer from the options that follow each question. 1. A solute
Acids and Bases Chapter 15 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Acids Have a sour taste. Vinegar owes its taste to acetic acid. Citrus fruits contain
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
Unit 12: Acids & Bases Aim: What are the definitions and properties of an acid and a base? Mar 23 12:08 PM Properties of an Acid 3. Are electrolytes. (Dissociate and conduct electricity when aq) 2. Turns
May 09, 2013 Properties of Acids AcidAcid Base Chemistry Base Chemistry Taste sour Are strong or weak electrolytes React with bases to form water and salts React with active metals to produce H2 Turn litmus
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),
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.
Acids Bases and Salts Acid ph less than 7.0 Sour taste Electrolyte Names of Acids Binary acids Contain only 2 elements Begin with hydro; end with ic Ternary acids Ex: H 2 S = hydrosulfuric Contain a polyatomic
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
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
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,
Section 2 Main Ideas rønstedlowry acids and bases donate or accept protons. A Lewis acid or base accepts or donates a pair of electrons. define acids and bases and distinguish between Arrhenius and ronstedlowry
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
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
NAME: UNIT #11: Acids and Bases ph and poh Neutralization Reactions Oxidation and Reduction 1. SELF-IONIZATION OF WATER a) Water molecules collide, causing a very small number to ionize in a reversible
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
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
AcidBase Reactions Key Terms conjugate base conjugate acid amphoteric neutralization salt In the previous sections, you learned about three acidbase theories: Arrhenius, BrønstedLowry, and Lewis. The BrønstedLowry
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.
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
7.6: Properties of Acids & Bases and Acid Nomenclature Remember: Have your 7.6 notesheet ready! You can pause the video anytime. You can rewind the video anytime. Write down questions/comments as you go
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
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
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
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
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
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
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
ACIDS AND BASES Acids and Bases Two important classification of compounds - Acids and Bases Properties of ACIDS Taste Sour/Tart Stings and burns the skin Reacts with bases Turns blue litmus paper red Reacts
Acids and Bases Chapter 11 Acids and Bases in our Lives Acids and bases are important substance in health, industry, and the environment. One of the most common characteristics of acids is their sour taste.
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
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).
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
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
P a g e 1 Chapter 16 ACID-BASE EQUILIBRIA Nature of Acids and Bases Before we formally define acids and bases, let s examine their properties. Properties of Acids Sour taste Ability to dissolve many metals
Acids and Bases Chapter 11 Acids and Bases in our Lives Acids and bases are important substance in health, industry, and the environment. One of the most common characteristics of acids is their sour taste.
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
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
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
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
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
Chapter 15 Acid and Bases Properties of Acids! Sour taste! React with active metals! React with carbonates, producing CO 2! Change color of vegetable dyes!blue litmus turns red! React with bases to form
8.1 Explaining the Properties of Acids & Bases SCH4U - Chemistry, Gr. 12, University Prep Equilibrium & Acids & Bases 2 So far, we have looked at equilibrium of general chemical systems: We learned about
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
Acids, Bases and ph Preliminary Course Steffi Thomas firstname.lastname@example.org 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?
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
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
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
!! www.clutchprep.com CONCEPT: ACID IDENTIFICATION The most common feature of an acid is that many possess an H + ion called the. When it comes to acids there are 2 MAJOR TYPES that exist: are acids where
Reading Assignments: Chapter 15 in R. Chang, Chemistry, 8th Ed., McGraw-Hill, 2005 Or Related topics in other textbooks. Acids and Bases Consultation outside lecture room: Office Hours: Tuesday & Thursday
Acids and Bases Chapter 11 Acids and Bases in our Lives We produce lactic acid in our muscles when we exercise. Acid from bacteria turns milks sour in the products of yogurt and cottage cheese. We have
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
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
Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) The effect of a catalyst on a chemical reaction is to. A) increase the entropy change
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
As you work through the chapter, you should be able to: Advanced Placement Chemistry Chapters 14 16 Syllabus Chapter 14 Acids and Bases 1. Describe acid and bases using the Bronsted-Lowry, Arrhenius, and
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
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