Acids and Bases: Acid/Base Theory

Slides:



Advertisements
Similar presentations
Acid-Base Theories Section 20.3
Advertisements

There are 3 theories… Arrhenius (most common) Bronsted-Lowry Lewis.
Acids bases & salts.
Acids & Bases. Properties of Acids & Bases  Acids Aqueous solutions of acids have a sour taste Turn blue litmus paper to red React with metals to produce.
Year 12 Chemistry. He classified all chemicals into three categories – acids, bases and salts He classified all chemicals into three categories – acids,
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. What are acids and bases?  Arrhenius Acids Hydrogen-containing compounds that ionize to yield hydrogen ions (H + ) in aqueous solutions.
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.
Chem-To-Go Lesson 38 Unit 10.  Both acids and bases ionize or dissociate in water  Acids: taste sour, conduct electricity, cause certain indicators.
Chemistry 121/122 Acids, Bases and Salts. Properties of Acids Acids, in foods, give a sour or tart taste Aqueous solutions of acids are electrolytes (conduct.
Acids and Bases Acid-Base Theories.  Objectives  Define and recognize Brønsted-Lowry acids and bases  Define a Lewis acid and a Lewis base  Name compounds.
6.1 – Introduction to Acids and Bases Unit 6 – Acids and Bases.
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+
NOTES: 19.1 – Acid-Base Theories
ACIDS, BASES & SALTS The Arrhenius Theory of Acids and Bases.
The Brønsted-Lowry Theory of Acids Two important theories have been developed to explain the properties of acids, bases, and salts. These are the Arrhenius.
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.
Pg ◦ Tastes sour ◦ Corrosive to metals ◦ Electrolytes: break into ions when dissolved in water ◦ React with blue litmus and indicators.
Lesson 1 Arrhenius Theory Bronsted-Lowry Theory ACIDS AND BASES.
Acid-Base Theories. In 1887, a Swedish chemist, Svante Arrhenius, published a paper concerning acids and bases. In 1887, a Swedish chemist, Svante Arrhenius,
Acids and Just the Bases Mrs. Herrmann Concentrations of Solutions Concentration—quantitive; a measure of the amount of solute in a given amount of solvent.
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.
Acids and Bases: Acid/Base Theory Mrs. Crowley’s Chemistry Class
Mrs. Howland Chemistry 10 Rev. April Learners will be able to… Identify acids and bases by chemical formula Compare and contrast acids and bases.
Properties of Acids and Bases
Today’s lesson is brought to you by 7, 14, and the letters Kw, pH
Acids, Bases and Salts.
Acids and Bases.
Chapter 19 Notes: Part II Acid/Base Theories.
Bellringer MULTIPLE CHOICE
Theories Acids and Bases.
Ways of Understanding Acids and Bases
Ways of Understanding Acids and Bases
Which of the following is a conjugate pair? A.H+ and OH−
Ionic Equilibrium in Solutions
Section 1 Properties of Acids and Bases
Chapter 14 Preview Lesson Starter Objectives Acids Bases
Chapter 8.1 The Nature of Acids and Bases
Acids Bases.
Acid-Base Theories.
UNIT 6 INTRODUCTION TO CHEMISTRY
Acid/Base Chemistry.
Acids & Bases Chapter 16.
Chemistry 19.1.
Acids and Bases.
Acids & Bases.
Acids Bases.
Acids and Bases Mr. Sonaji V. Gayakwad Asst. professor
Acids and Bases.
Prentice-Hall Chapter 19.1 Dr. Yager
Ch. 14 Acids And Bases.
Acids and Bases.
ACIDS and BASES Chapter 19
Acids & Bases.
Acids, Bases, Salts An introduction.
Section 1 Properties of Acids and Bases
Acids Bases.
Chapter 10 Acids, Bases, and Salts
Chapter 8 Acids and Bases
Acids & Bases Vocabulary.
Chapter 19 Notes, Part II Acid/Base Theories.
Acids & Bases Chapters 20 & 21.
Strong Acids Ch
Acids & Bases.
Acids and Bases Acids Bases Sour Taste React with metal to form H2.
Chapter 19.1 Acid-Base Theories
Introduction to Acids and Bases
Descriptions & Reactions
Presentation transcript:

Acids and Bases: Acid/Base Theory Mrs. Crowley’s Chemistry Class

Measuring pH How do we measure pH? Own a pool? Own a spa? How do you check the water quality? Look at my poster. Also…pH meters can do the trick, too:

This is an example of an “equilibrium” Indicators Acid-base indicators: This is usually a solution that you add to a solution that will undergo a chemical reaction at a certain pH. The reaction is called “dissociation.” This type of reaction is an equilibrium. Remember, equilibriums go from reactants to products and products to reactants (back and forth). H2O H+ + OH- This is an example of an “equilibrium” The rate of flow towards products is the same as the rate to reactants.

Check out my poster! There are many different indicators available for chemists. Sometimes, we can combine these indicators to make a broad spectrum of color changes. This is how traditional pH paper is made.

Acid-Base Theories Well, now it’s time to learn what his theory of acids and bases were. Arrhenius’s main contribution to physical chemistry was his theory (1887) that electrolytes, certain substances that dissolve in water to yield a solution that conducts electricity, are separated, or dissociated, into electrically charged particles, or ions, even when there is no current flowing through the solution

Svante Arrhenius Svante said that acids are hydrogen-containing compounds that ionize to yield hydrogen ions (H+) in aqueous solution. He also said that bases are compounds that ionize to yield hydroxide ions (OH-) in aqueous solution.

Acids – further explaination Not all compounds that contain hydrogen are acids! (poor Arrhenius!...he didn’t know this…YET) Also, not all hydrogens in an acid are released as hydrogen ions. Only the hydrogens in very polar bonds are ionizable. EXAMPLE: HCl + H2O  H3O+ + Cl- Highly Polar molecule

Bronsted-Lawry Acids and Bases The next theory on acids and bases came from these two men around the year 1923.

Bronsted-Lowry Theory These guys re-defined an acid as a hydrogen-ion donor. They also re-defined a base as a hydrogen ion acceptor. Let me explain:

Explanation When ammonia (a well known base) combines with water, the ammonia will act as a base. But ammonia doesn’t have an OH! How can it possibly be a base if there is no OH ion? The OH ion will come from the water! Yes…that’s right. The water will donate a hydrogen to the ammonia. Poor Arrehenius thought ammonia’s formula was NH4OH! But the molar mass of ammonia was discovered to be MUCH less than that of NH4OH!

Further Explanation Does that mean that the water is an acid? Well, according to the Bronsted-Lowry theory…YES! Water acts like a Bronsted-Lowry base. HOW? Look at that “double arrow.”

Equilibriums If the reaction between water and ammonia goes in the reverse direction, NH4+ will react with OH- to form NH3 and H2O. acid = hydrogen-ion donor. base = hydrogen ion acceptor.

Conjugate Acids and Bases If the reaction goes in the reverse direction, NH4+ gives up a hydrogen ion. That makes it an Bronsted-Lowry ACID! OH- will accept that hydrogen ion from NH4+. That makes it a Bronsted-Lowry BASE! Since NH4+ is on the right side of the equation, it is called a conjugate acid. Since OH- is on the right side of the equation, it is called a conjugate base.

Definitions Conjugate acids are the particles formed when a base gains a hydrogen ion. A conjugate base is the particle that remains when an acid has donated a hydrogen ion.

Extra Examples

Lewis Acids and Bases The last theory for acids and bases came from Gilbert Lewis (1875-1946).

Lewis Acids-Bases A lewis acid is a substance that can accept a pair of electrons to form a covalent bond. A lewis base is a substance that can donate a pair of electrons to form a covalent bond.

In this reaction, the ammonia is a lewis base. The ammonia will give the extra pair of electrons to the other substance to form an additional bond with it.

RECAP: Arrhenious: Acids make H+ and Bases make OH- Acids have H+ ion in front of formula, bases have OH- ion in back of formula. Brønsted–Lowry: Acids are proton donors and Bases are proton acceptors Conjugate acid/base pairs Lewis: Acids accepts a pair of electrons, Bases donates a pair of electrons

STOP HERE