Chemistry Notes Acid/Base Theories. There are three ways to define acids and bases. This reflects the fact that science is always revising itself.

Slides:

Advertisements

Similar presentations

Acid-Base Theories Section 20.3

Advertisements

 Brønsted/Lowry acid: a proton donor proton donor?... a proton is also an H + ion  in water, H 2 O + donated H +  H 3 O +  H 3 O + = “hydronium ion”

There are 3 theories… Arrhenius (most common) Bronsted-Lowry Lewis.

HOBr is a weaker acid than HBrO3. Account for this fact.

Brønsted-Lowry theory of acids and bases An acid is a H + donorHCl A base is a H + acceptorNH 3 H + Cl - + NH 3 Cl - + NH 4 + H + is transferred Note:We.

Modern Theories of Acids & Bases The Arrhenius and Bronsted-Lowry Theories.

1. Comments on Test 2. Section 16.1A – Acids and Bases 3. Homework: pg 589, #2, 3, 7, 8, 9, 10 Wednesday, March 12, 2008.

Acids and Bases Chapter 19 Section 19.1.

ACIDS AND BASES.

Properties of Acids and Bases Acids taste sour, will change the color of an acid base indicator, and can be strong or weak electrolytes in aqueous solution.

Bronsted-Lowry Acid – Base Reactions Chemistry. Bronsted – Lowry Acid Defined as a molecule or ion that is a hydrogen ion donor Defined as a molecule.

Acids and Bases: Introduction Section Objectives Identify the physical and chemical properties of acids and bases Classify solutions as acidic,

Year 12 Chemistry. He classified all chemicals into three categories – acids, bases and salts He classified all chemicals into three categories – acids,

Aim: What are acids and bases?. Acids 1.Acids can be strong or weak electrolytes in aqueous solutions. 2.Acids (ex: HCl) react with certain metals to.

What are Acids and Bases ? There are three main theories to describe what acids and bases are In general each theory widens what chemical reactions can.

Acid-Base Theories The “Boyz”. Acid and Base Theories2 Arrhenius Theory of Acids Acid: molecular substances that breaks-ups in aqueous solution into H+

Unit 18 Acids and Bases. I. Defining Acids & Bases A. Properties Acids Bases 1. Taste sour bitter (not in lab) ex: Citrus ex: soap fruits, yogurt vinegar.

Acids and Bases Unit 12. Properties of an Acid  Sour taste  Turns litmus paper red (and responds uniquely to other indicators)  Reacts with:  Hydroxide.

NOTES: 19.1 – Acid-Base Theories

1 The Chemistry of Acids and Bases Chapter Some Properties of Acids þ Produce H + ions in water þ Taste sour þ Corrode metals þ Electrolytes þ React.

Podcast 18.1 Introduction to Acid-Base Chemistry.

ACIDS, BASES & SALTS The Arrhenius Theory of Acids and Bases.

Acids and Bases. Acids from the Latin word acere  “ sharp ” or “ sour ” taste sour (but you wouldn ’ t taste an acid to see) change litmus paper red.

Acids and Bases: Introductory Concepts Arrhenius...acids increase the ______ when dissolved in H 2 O....bases increase the ______ when dissolved in H 2.

Acids, Bases, and Salts - Acids taste sour, will change the color of an indicators (chemical dyes), and can be strong or weak electrolytes (aqueous solutions.

Acid-Base Equilibrium According to Arrhenius theory, substances were acids if they contained hydrogen ion (H + ), and bases if they contained hydroxide.

Review: Arrhenius Definition of Acids and Bases Acids produce H + in aqueous (water) solutions Acids produce H + in aqueous (water) solutions water water.

ACID/BASE Theories & Review

Acid and Bases: An Introduction. Properties of Acids 1. Sour taste 2. Can produce H + (hydrogen) ions (protons) 3. Change the color of litmus from blue.

Tonight’s homework: Read pages Do practice problems 1 & 2.

Acids and Bases Chemistry 12. Arrhenius Definition of an Acid An acid has a sour taste (ex: vinegar, citric acid) and when placed in water to become an.

Acid/Base Properties In the past, we have classified acids and bases according to their observed properties ACIDS BASES Sour tastebitter taste Watery.

Acid and Base Definitions Objectives: 1. State the Bronsted-Lowry definition of acids and bases. 2. Identify the common physical and chemical properties.

Pg ◦ Tastes sour ◦ Corrosive to metals ◦ Electrolytes: break into ions when dissolved in water ◦ React with blue litmus and indicators.

Chapter 20 Section 3 monoprotic acid- contains one ionizable H ex- HNO 3 diprotic acid- contains two ionizable H ex- H 2 SO 4 triprotic acid- contains.

Conjugate Acid-Base Pairs. Acid Dissociation Kelter, Carr, Scott, Chemistry A World of Choices 1999, page 280 HCl Conjugate base Acid Conjugate pair +

Acid-Base Theories The “Boyz”. Acid and Base Theories2 Arrhenius Theory of Acids Acid: molecular substances that breaks-ups in aqueous solution into H+

8.4 Acid-Base Theories. Recall: Arrhenius’ TheoryAcids:  Arrhenius theory  Arrhenius theory: Any substance that, when dissolved in water, increases.

Copyright © Cengage Learning. All rights reserved.15 | 1 Brønsted–Lowry Concept of Acids and Bases The Brønsted–Lowry concept expands the compounds that.

Brønsted-Lowry Model Acids - proton (H + ) donors Bases – accepts proton (H + )

1 - Alternate Acid Base Theory Mr. ShieldsRegents Chemistry U15 L02.

Aim: How did Bronsted describe acids and bases? Do Now: 1.Take out a calculator and reference tables. 2.How did Arrehnius define an acid and a base?

Acids and Bases Chapter 19. Ants use formic acid to alert each other of danger. Citrus acid gives OJ it’s flavor. Limestone is carved away by acid in.

Acids and Bases. Acid and Base Overview Acids and bases are a group of compounds that combine to form a salt. A salt is an ionic solid made from a metal.

Classifying Acids and Bases. Acid and Base Theories  There are different ways of defining what an acid and base is 1. Arrhenius 2. Bronstead Lowry.

19.1 Acid-Base Theories> 1 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Chapter 19 Acids, Bases, and Salts 19.1 Acid-Base.

What makes an acid an acid or a base a base can vary depending on definition being used. The first definition was created by Svante Arrhenius in 1883.

Theories of Acids and Bases

Chapter 19 Notes: Part II Acid/Base Theories.

Bellringer MULTIPLE CHOICE

ACIDS, BASES and SALTS Definitions Acid Base

Acid Base Reactions & Theories

Acids and Bases.

Acid and Bases: An Introduction

Aim: What are acids and bases?

Acids and Bases.

Neutralization Reactions

Prentice-Hall Chapter 19.1 Dr. Yager

Acids and Bases.

Aim: What are acids and bases?

ACIDS and BASES Chapter 19

Acids and Bases Chapter 12.

Definitions of acids and bases

Acid & Bases Review Notes

Introduction to Acids and Bases

Chapter 19 Notes, Part II Acid/Base Theories.

Acids and Bases SWBAT – Analyze strong/weak acids and bases.

Conjugate Acid-Base Pairs

Descriptions & Reactions

Presentation transcript:

Chemistry Notes Acid/Base Theories

There are three ways to define acids and bases. This reflects the fact that science is always revising itself.

Arrhenius Acids/Bases An acid is a chemical that gives off hydrogen ions in solution. A base is a chemical that gives off hydroxide ions in solution. Example: HCl + NaOH  NaCl + H2O **BASICALLY…acids start with H+ and bases end with OH-!!!

There are three ways to describe an acid: Monoprotic-gives off one H + in solution Diprotic-gives off two H + Triprotic-gives off three H +

Bronsted-Lowry Acids/Bases The Arrhenius definition is a good one, but does not encompass everything that shows acidic/basic qualities. To account for this, Johannes Bronsted and Thomas Lowry proposed a new idea.

Bronsted-Lowry Acids/Bases An acid is a hydrogen-ion (proton) donor. A base is a hydrogen-ion (proton) acceptor.

Conjugate Acids/Bases A conjugate acid is the particle that is formed when a base gains a hydrogen ion. A conjugate base is the particle that is formed when an acid donates a hydrogen ion.

Conjugate Acids/Bases A conjugate acid/base pair consist of two substances related by the loss of a single hydrogen ion.

NH 3 + H 2 O  NH OH - Which is the initial acid? Which is the initial base? What is the conjugate acid? What is the conjugate base?

NH 3 + H 2 O  NH OH - Which is the initial acid? H 2 O Which is the initial base? What is the conjugate acid? What is the conjugate base?

NH 3 + H 2 O  NH OH - Which is the initial acid? H 2 O Which is the initial base? NH 3 What is the conjugate acid? What is the conjugate base?

NH 3 + H 2 O  NH OH - Which is the initial acid? H 2 O Which is the initial base? NH 3 What is the conjugate acid? NH 4 + What is the conjugate base?

NH 3 + H 2 O  NH OH - Which is the initial acid? H 2 O Which is the initial base? NH 3 What is the conjugate acid? NH 4 + What is the conjugate base? OH -

HCl + H 2 O  H 3 O + + Cl - Which is the initial acid? Which is the initial base? What is the conjugate acid? What is the conjugate base?

HCl + H 2 O  H 3 O + + Cl - Which is the initial acid? HCl Which is the initial base? What is the conjugate acid? What is the conjugate base?

HCl + H 2 O  H 3 O + + Cl - Which is the initial acid? HCl Which is the initial base? H 2 O What is the conjugate acid? What is the conjugate base?

HCl + H 2 O  H 3 O + + Cl - Which is the initial acid? HCl Which is the initial base? H 2 O What is the conjugate acid? H 3 O + What is the conjugate base?

HCl + H 2 O  H 3 O + + Cl - Which is the initial acid? HCl Which is the initial base? H 2 O What is the conjugate acid? H 3 O + What is the conjugate base? Cl -

Amphoteric Substances Note that in one of the previous examples water was acidic and basic in the other. A substance that can act as an acid or a base is called amphoteric.