Acids-Bases Arrhenius: Acid…. A substance that increases the hydrogen ion, H +, concentration when dissolved in H 2 O. Eg. HCl, H 2 SO 4, HC 2 H 3 O 2.

Slides:

Advertisements

Similar presentations

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

Advertisements

Chapter 17 Acid–Base (Proton Transfer) Reactions

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.

Introduction to Acids and Bases AP Chemistry

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 AND BASES Topic Reactions of acids and bases Acids with metals Produces a salt and hydrogen gas Mg + 2HCl  MgCl 2 + H 2 Acids with carbonates.

Acids and Bases Chemistry 2013.

Acids & Bases Acids: acids are sour tasting

Chapter 19 Acids and Bases.

ACID AND BASES Definition and properties of Acid: Acid is defined as a substance whose aqueous solution possesses the following characteristic properties:

Chapter 16 Acids and Bases. © 2009, Prentice-Hall, Inc. Some Definitions Arrhenius – An acid is a substance that, when dissolved in water, increases the.

Acids-Bases Arrhenius:

Acids-Bases Arrhenius: Acid…. A substance that increases the hydrogen ion, H +, concentration when dissolved in H 2 O. Eg. HCl, H 2 SO 4, HC 2 H 3 O 2.

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

I. Introduction to Acids & Bases

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.

Acids-Bases Part I Arrhenius: Acid…. A substance that increases the hydrogen ion, H +, concentration when dissolved in H 2 O. Eg. HCl, H 2 SO 4, HC 2 H.

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.

Chapter 19 DHS Chemistry.

Acids and Bases. Properties of Acids and Bases Pg 236.

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

Introduction to Acids and Bases IB Chemistry Power Points Topic 08 Acids and Bases

ACIDS, BASES, AND pH. 2 The solutions conduct electricity! They are called ELECTROLYTES HCl, MgCl 2, and NaCl are strong electrolytes. They dissociate.

THE CHEMISTRY OF ACIDS AND BASES. ACID AND BASES.

Chapter 14 Acids and Bases. Chapter 14 Table of Contents Copyright © Cengage Learning. All rights reserved The Nature of Acids and Bases 14.2Acid.

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

Chapter 19: Acids and Bases Sections 19.1 to 19.4.

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.

1 Acids, Bases and PH. 2 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)

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 Arrhenius: Acid…. A substance that increases the hydrogen ion, H +, concentration when dissolved in H 2 O. Eg. HCl, H 2 SO 4, HC 2 H 3 O 2.

  Sour Taste  Electrolytes  Identified by the presence of H + ions (Arrhenius).  Proton (H + ) donor (Bronsted-Lowry).  Common Acids: vinegar, citric.

Acids and Bases Chapter 15. Acids Have a sour taste. Vinegar owes its taste to acetic acid. Citrus fruits contain citric acid. React with certain metals.

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 and Base Equilibria The concept of acidic and basic solutions is perhaps one of the most important topics in chemistry. Acids and bases affect the.

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

Acids and Bases. Acids & Bases ● There are 3 common definitions of acids and bases. – Arrhenius definition – acids increase H+ concentration, bases increase.

Acids and Bases.

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 and Bases!  Acids and Bases (and calculations involving them) are essential to all areas of analytical chemistry!

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.

Acids and Bases: Qualitative and Quantitative Approaches SCH4U1 Unit 5.

Acids-Bases Part I Arrhenius: Acid…. A substance that increases the hydrogen ion, H +, concentration when dissolved in H 2 O. Eg. HCl, H 2 SO 4, HC 2 H.

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.

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

ACIDS & BASES. ACID/BASE THEORY Acids and bases are solutions which can be described differently by multiple theories. So far, we have treated everything.

SURVEY OF CHEMISTRY I CHEM 1151 CHAPTER 9 DR. AUGUSTINE OFORI AGYEMAN Assistant professor of chemistry Department of natural sciences Clayton state university.

Acids, Bases, and pH Chapters 14/15. 1.Aqueous solutions of acids have a sour taste. 2.Acids change the color of acid-base indicators. 3.Some acids react.

Acids and Bases Ch 16. I. Properties of Acids and Bases A. Acids –1. Taste sour (think lemons: citric acid) –2. React with metals to produce hydrogen.

I. Introduction to Acids & Bases (p ) Ch. 15 & 16 - Acids & Bases.

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,

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

Acids and Bases. Three Definitions Arrhenius  acid – produces H + in soln  base – produces OH - in soln Bronsted-Lowry  acid – H + donor  base – H.

Taste sour Taste sour Form solution that conduct electricity Form solution that conduct electricity React with metals React with metals Turn blue litmus.

When we think of acids and bases we tend to think of chemistry lab acids and bases like But we are surrounded by acids and bases in the world. Most of.

Chapter 15 Acids and Bases. Some Properties of Acids þ Produce H + (_______) ions in water (the ________ ion is a hydrogen ion attached to a water molecule)

Introduction to Acids and Bases Chapter 19. What is and Acid? Arrhenius Acid Defined as any chemical that increases the concentration of hydrogen ions.

Ch. 15 & 16 - Acids & Bases II. pH (p ) C. Johannesson.

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

ERT 207 ANALYTICAL CHEMISTRY ACIDS AND BASES THEORIES ACID BASE EQUILIBRIA IN WATER pH SCALE 27 Jan 2011 (MISS NOORULNAJWA DIYANA YAACOB) 1.

Acids and Bases. Drill – 4/23/08 Write everything you know about acids and bases!

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.

Objectives Learn the properties and definitions of acids / bases.

Unit 8 Acids and Bases. Naming acids 1)Acids not containing oxygen: hydro______ ic acid HF, HCl, HBr, HI, HCN, H 2 S 2)Acids containing polyatomic ions.

Acids and Bases Chapter 19. Arrhenius Acids- hydrogen containing compounds that ionize to yield H + ions in an aqueous solution Begins with H Bases- compounds.

Intro to Acids & Bases.

Acid-Base Equilibria Review: In pure water & all aqueous solutions:

Acids-Bases Arrhenius:

Presentation transcript:

Acids-Bases Arrhenius: Acid…. A substance that increases the hydrogen ion, H +, concentration when dissolved in H 2 O. Eg. HCl, H 2 SO 4, HC 2 H 3 O 2 (CH 3 COOH), etc. Base…. A substance that increases hydroxide ion, OH -, concentration. Eg. NaOH, NH 4 OH, etc. Bronsted-Lowry (1923) (not worried about increasing/decreasing H + or OH - concentrations) Acid … a “proton donor”, p + = H +, any formula HA. Eg. HCl, H 2 SO 4, HC 2 H 3 O 2 (CH 3 COOH), etc. Base …. A “proton acceptor” Eg. OH -, NH 3 ; Cl -

Acid solutions: HCl (g) + H 2 O (l) H 3 O + (aq) + Cl - (aq) H 3 O + (aq) = H + (aq) H:Cl:.. + :O::O: H H H H :O::O: H + + :Cl:.. - Hydrogen ion, H +, or hydronium ion, H 3 O + has formed HCl (g) + H 2 O (l) H + (aq) + Cl - (aq)

Strength of an acid can be determined by conductivity. 12 M HCl Good or poor electrolyte? Large or small # of ions? HCl (g) + H 2 O (l) H 3 O + (aq) + Cl - (aq)

Strength of an acid can be determined by conductivity. Good or poor electrolyte?Large or small # of ions? Pure HC 2 H 3 O 2 Diluted HC 2 H 3 O 2

Properties of Acids:

More Bronsted-Lowry Acid/Base info: General acid/base reaction: HA + B = A - + HB +

Basic Solutions: Strong Arrhenius bases: 1.Group IA hydroxides. Eg. NaOH, KOH 2.Lower Group IIA hydroxides. Eg. Sr(OH) 2, Ba(OH) 2

Lewis Acid/Base Lewis acid: electron pair acceptor Lewis base: electron pair donor H+H+ + :N:.. H H H H H H H ::N + “adduct” … the product of a L.acid/base rxn

Acid-Base Equilibria Review: In pure water & all aqueous solutions: H 2 O + H 2 O = H 3 O + + OH -

Solutions of Strong Acids/ Bases: 0.10 M HNO 3 actually consists of 0.10 M H 3 O + or [H + ] = 0.10 M 0.10 M NaOH…. Adds 0.10 OH - to the water solution

pH A simple scale for ranking the H 3 O + concentrations of dilute acid/base solutions. (Sorenson). The logarithm of a number is that number expressed as an exponent of the base 10. For example, the logarithm of 1 is 0, 1 x 10 0.

pH Scale [H 3 O + ][OH - ]= 1x pH = - log[H 3 O] pH + pOH = 14 Formulas to remember

Given a 3.25 x M HNO 3, solve for: a.[H 3 O + ] a.pH = a.[OH - ] = More About the pH Scale