Reactions in Aqueous Solution: Acids (section 4.3)

Slides:

Advertisements

Similar presentations

CHAPTER 9 CONCURRENT ENROLLMENT. ACIDS AND BASES WEAK ACIDS AND BASES ONLY A FEW IONS ARE FORMED DEFINITIONS –Arrhenius - Acid contains H + ions and Bases.

Advertisements

Chapter 14 Acids and Bases 2006, Prentice hall.

Acids & Bases Acids: acids are sour tasting

UNIT 5 Aqueous Reactions and Solution Stoichiometry Acid-Base Neutralization.

Acid-Base Reactions. Review Acids are proton (H +1 ion) donors. ◦ H 2 SO 4 (aq) + H 2 O(l)  HSO 4 -1 (aq) + H 3 O +1 (aq)  In this reaction, H 2 SO.

 Topic 10 Correlates to Topic 10 in review book, pages

ACIDS AND BASES TOPIC 8 1. ARRHENIUS MODEL OF ACIDS AND BASES Acid is a substance that contains hydrogen and ionizes to produce a hydrogen ion in an aqueous.

Arrhenius Definition of Acids Bases - Substances that produce hydrogen ions, H + when dissolved in water - Substances that produce hydroxide ions, OH -

Acids and Bases. What are acids and bases?  Arrhenius Acids Hydrogen-containing compounds that ionize to yield hydrogen ions (H + ) in aqueous solutions.

Chem-To-Go Lesson 38 Unit 10.  Both acids and bases ionize or dissociate in water  Acids: taste sour, conduct electricity, cause certain indicators.

Acids and Bases Chapter 15.

Chapter 10 Acids and Bases.

Acid-Base Theories pH Reactions Indicators Titration Q $100 Q $200 Q $300 Q $400 Q $500 Q $100 Q $200 Q $300 Q $400 Q $500 Final JeopardyJeopardy.

Chapter 19 More about ACID-BASES. Self-Ionization of Water Two water molecules produce a hydronium ion & a hydroxide ion by the transfer of a proton.

Acid/Base. Properties of Acids ·Sour taste, Change color of dyes, Conduct electricity in solution, React with many metals, React with bases to form salts.

1A + 2B  1C + 1D Calculate the equilibrium concentrations of each species when 150 mL 2.5 M A is mixed with mL 2.5 M B. K c = 2.0 x

THIS IS With Host... Your Misc.Acid misc.Base misc.Acid base definitions Titration pH/pOH.

Chapter 4. Solution: -> Any homogeneous mixture. All parts of the mixture have the identical composition. Solvent – The substance in a solution that causes.

Chapter 19 More about ACID-BASES. Self-Ionization of Water Two water molecules produce a hydronium ion & a hydroxide ion by the transfer of a proton.

1A + 1B  1C + 1D Calculate the equilibrium concentrations of each species when 150 ml 2.0 M A is mixed with ml 2.0 M B. K c = 0.25.

1 Some Properties of Acids þ Produce H + (as H 3 O + ) ions in water (the hydronium ion is a hydrogen ion attached to a water molecule) þ Taste sour þ.

Acids, Bases, and Salts Chapter Acids – Taste sour – React with metals to form H 2 gas – Will change the color of and acid-base indicator Turns.

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.

Arrhenius acid - any HA, H 2 A, H 3 A, or RCOOH substance with an H + to donate Examples include HCl, H 2 SO 4, H 3 PO 4, and CH 3 COOH.

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.

Chapter Arrhenius Concept: Acids produce H + in solution, bases produce OH  ion. In aqueous solutions. Brønsted-Lowry: Acids are H + donors, bases.

Acids and Bases. These are acids….. HNO 3 HCl H 2 SO 4 HC 2 H 2 OOH H 3 PO 4 What do they all have in common?

 Brønsted-Lowry – proton donor  Arrhenius – acids produce H + ions in water  HCl  H + + Cl -  HCl, HBr, HI, H 2 SO 4, HC 2 H 3 O 2.

 Strong and Weak Acids  Titration  Common Acid Names Textbook section 4.3.

There are several ways to define acids and bases: Arrhenius ( narrowest/most common definition ) –a–acids – produce H + ions in water –b–bases – produce.

Section 16.1 Properties of Acids and Bases 1. To learn about two models of acids and bases 2. To understand the relationship of conjugate acid-base pairs.

Characteristics of Acids: Table K  Electrolytes  pH scale: less than 7  Litmus: RED  Phenolphthelein: colorless  Contains a high concentration of.

Section 2Acids, Bases, and Salts Section 2: Reactions of Acids with Bases Preview Key Ideas Bellringer Acid-Base Reaction Neutralization Reaction Titration.

Acids and bases.

Acid – Base Theory Definitions: Arrhenius: An acid is a substance that increases the H + (or H 3 O + ) concentration in an aqueous solution. HCl + H.

11111 Chemistry 132 NT A man is rich in proportion to the number of things he can let alone. Henry David Thoreau.

1 Reactions in Aqueous Solutions I. 2 Properties of Aqueous Solutions of Acids & Bases Acidic properties taste sour change the colors of indicators turn.

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.

Acids & Bases Chemistry 6.0. Naming Acids Review: A. Binary – H +one anion Prefix “hydro”+ anion name +“ic”acid Ex) HCl hydrochloric acid Ex) H 3 P hydrophosphoric.

ACID-BASE EQUILIBRIUM. Arrhenius Theory  Acids – are solutes that produce hydrogen ions H + in aqueous solutions ex. HCl (aq)  H + (aq) + Cl - (aq)

Acids & Bases Acids:  acids are sour tasting  Arrhenius acid  Arrhenius acid: Any substance that, when dissolved in water, increases the concentration.

19.1 Acid-Base Theories> 1 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Day The pH for a 0.10 M solution of a.

I. Introduction to Acids & Bases Acids & Bases. A. Properties  electrolytes  turn litmus red  sour taste  react with metals to form H 2 gas  slippery.

Acids –Sour Taste –Change the color of an acid-base indicator –React with metals to form H 2 gas –React with bases to produce salts and water –Conduct.

ACIDS and BASES Chapter 18. Acids and Bases: An Introduction Acidic solution – contains more hydrogen ions than hydroxide ions. [H + ]>[OH - ] Acidic.

Acids, Bases, & Salts. Properties  Taste Sour.  Can sting skin if open (cut).  React with metals to produce H 2 gas.  Disassociate in water to produce.

Acids  Arrhenius definition  Produces H + ions in aqueous solutions  Some completely dissociate, others partially dissociate in solutions.

Acids/Bases. Properties of Acids pp 186 Properties of Bases pp 186.

19.1 Acid-Base Theories> 1 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. 1.What can you say about the K a value of a strong.

Acids and Bases All you ever wanted to know, and more!

Acids and Bases Topic 8 General Properties Definitions pH Scale.

Acids & Bases. Acids and Bases an Introduction A. Properties of Acids and Bases –1. Acids Ionize when put into water React with active metals (Group I,

Acids/Base. Acids Acids- form H + ions when dissolved. Strong acids fall apart completely.  many ions Weak acids- don’t dissociate completely. There.

Types of Chemical Reactions and Solution Stoichiometry.

ACID-BASE REACTIONS.

Acids and Bases – Acid Strength and K a.

Definition of Acids Traditional (Arrhenius)- a chemical compound that contains hydrogen and ionizes in aqueous solutions to form hydrogen ions Examples:

Chapter 17 Acids and Bases. Necessary Terminology to Begin Hydronium = H 3 O + (aq) or H + (aq) Hydroxide = OH - (aq) Neutral Water = Equal amounts of.

1A + 2B  1C + 1D Calculate the equilibrium concentrations of each species when 150 mL 2.5 M A is mixed with mL 2.5 M B. K c = 2.0 x

Chapter 15 Acids bases acids Sour Turns litmus red Reacts with some metals to produce H 2 Phenolphthalein-clear Corrosive Conducts electricity bases Bitter.

Acids and Bases Chapter 19. Naming Acids Binary Acids- two different elements in the formula, H is one of them Prefix= hydro Root= second element ends.

Acids and Bases HW: read CH 16. Acids and Bases Importance Commonly found in all aspects of daily life: car batteries, cleaners, fertilizers, detergents,

Objectives Learn the properties and definitions of acids / bases.

Acids & Bases Chapter 15 & 16. Acids Have a sour taste Affect indicators React with bases to produce salt & water Conduct an electric current Examples.

Chapter 15: Acids & Bases Ridgewood High School

© Houghton Mifflin Harcourt Publishing Company Acids 1.Aqueous solutions of acids have a sour taste. 2.Acids change the color of acid-base indicators.

Unit 14 Acids, Bases, Salts and Titrations. Acids & Bases Acids :  acids are sour tasting  Arrhenius acid: Any substance that, when dissolved in water.

Acid-Base Reactions. Acids Molecules that ionize in water to form hydrogen ions (H + ) Acids donate [GIVE AWAY] hydrogen ions (H + ) (protons). PROTON.

ACIDS AND BASES Chapter 18. Properties of Acids taste SOUR acids change litmus RED their aqueous (water) solutions CONTAIN HYDRONIUM (H 3 O + ) IONS react.

Acid – Base Theory.

Presentation transcript:

Reactions in Aqueous Solution: Acids (section 4.3)

Build the following molecules using the plastic molecular models: Nitric Acid Perchloric Acid Hydrochloric Acid 3 or 4 water molecules

Find meanings for these: Amphoteric Bronsted-Lowry Aqueous Conjugate Hydronium

What is an ACID? Acid Characteristics: Taste: Indicator:

Acid Definitions: Bronsted-Lowry Arrhenius: Acids put H+ into water Bases put OH- into water Bronsted-Lowry Acids: “ADP” Acids donate protons Bases accept protons The Bronsted-Lowry definition is broader (more inclusive) than the Arrhenius definition.

Strong Acids Strong Acids Ionize completely in water. (100%) HCl (aq)  H + (aq) + Cl - (aq) The strong ACIDS are: 1. HCl 2. HBr 3. HI 4. HNO 3 5. H 2 SO 4 6. HClO 4 Give formula and name of the 6 strong acids.

Weak Acids Weak acids ionize partially in water. Less than 10%, usually much less than 1% ionization. General formula: Double arrow means reversible or it does not go to completion. The equilibrium includes both products AND reactants.

Strong Bases Strong Bases Ionize Completely in water. (100%) NaOH  Na + + OH - Always soluble hydroxides and Ca, Ba, Sr hydroxides are strong bases. Including: LiOH KOH Ca(OH) 2 Sr(OH) 2 Ba(OH) 2

Weak Bases Produce OH - ions by reacting with the water. Less than 100% ionized. NH 3 aq + H 2 O aq   NH 4 + aq + OH - aq Include: ammonia NH 3 amides R-NH 2

Acid-Base Reactions 3 TYPES: 1 Strong ACID - Strong BASE 2 Weak ACID – Strong BASE 3 Strong ACID – Weak BASE

Strong ACID + Strong BASE “Neutralization” Reaction The products are water, and an aqueous salt. (ions)

Weak Acid – Strong Base Weak acid only partially ionized. Strong base fully ionized. The H+ and OH- combine to form water. All H + gets “used up” (reacted). The anion (salt of the weak acid is not used up or reacted).

Strong ACID – Weak BASE The weak base gets “protonated” (H + added to the base) Ammonia and Hydrochloric Acid NH 3 + H + + Cl -  NH Cl - Cross out the spectators Methylamine and Nitric Acid CH 3 NH 2 + H + + NO 3 -  CH 3 NH NO 3 - Cross out the spectators

Johnny finding life a bore, drank some H 2 SO 4. Johnny's father, an M.D., gave him CaCO 3. Johnny's neutralized, it's true, But now he's full of CO 2.

Find meanings for these: Amphoteric Bronsted-Lowry Aqueous Conjugate Hydronium

Acid Base Titration An standardized acid (known concentration) may be used to determine the unknown strength of a base. (or visa- versa) Using an indicator (solution that changes color) you can know when the added solution is exactly equal to the unknown. this is known as the EQUILVALENCE POINT.

Acid-Base titration Objective: Determine the equivalence point. Equivalence point n OH - = n H + If 25.00mL of M NaOH is needed to react with mL of HCl. What is the molarity of HCl? 1.Write the reaction 2.Use M 1 V 1 =M 2 V 2 In this case the formula could be written M OH - V OH - = M H + V H +