REVISION ACIDS & BASES. MODELS ARRHENIUS THEORY A n acid is a substance that produces hydrogen ions (H + )/hydronium ions (H 3 O + ) when it dissolves.

Slides:

Advertisements

Similar presentations

ACIDS AND BASES

Advertisements

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

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 Chapter 19. Acids pH less than 7 Sour taste Conduct electricity Reacts with metals to produce hydrogen gas Higher [H + ] concentration.

Conjugate acids and bases. When a substance loses ONE hydrogen ion, the species produced is called a “conjugate base” What’s the conjugate base of H 2.

Slide 1 of 52  Ch.16. Acids and Bases (the fundamentals)

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

ACIDS AND BASES. Acids  Acidic solutions contain water and hydrogen ions (H+)

1 Acids and Bases ICS Madrid. 2 Revision l When an acid reacts with a base, which compound(s) are formed? l What is the name of H 2 SO 4 ? l What is the.

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.

Chapter 14 Acids and Bases in the Environment. Acids and Bases Acids and Bases (video)Acids and Bases H + ions - ? OH - ions - ? Soapy slippery - ? Taste.

Acids and Bases Chemistry 2013.

Acids and Bases. Acids: Compounds that dissociate (give off) one or more hydrogen ions (H+) when dissolved in water (proton donors) Bases: Compounds that.

Volumetric Analysis Titration Dr.Riham Hazzaa

Chapter 9 Charge-Transfer Reactions: Acids and Bases and Oxidation-Reduction Copyright  The McGraw-Hill Companies, Inc. Permission required for reproduction.

The Chemistry of Acids and Bases

19.1 Acid-Base Theories> 1 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. LAB: COMPLETE EQUATION: KSCN (aq) + FeCl 3(aq)

Chapter 14 – Acids and Bases. History of Acids & Bases Vinegar was probably the only known acid in ancient times. Strong acids such as sulfuric, nitric.

Acids and Bases. Acids are substances that turn blue litmus red, and usually react with metals such as zinc, releasing hydrogen. Examples: hydrochloric.

Acids and Bases Chapter 14 – One step closer to the AP Test.

Acids and Bases.

Acids - Ionisation All acids ionise in solution to give ………ions. HCl  H+ H+ H+ H+ + Cl - Cl - (100%) HCl (+ H 2 O) H 2 O)  H 3 O + (aq) H 3 O + (aq)

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.

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

 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.

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

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

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

REVISION ACIDS & BASES. MODELS ARRHENIUS THEORY A n acid is a substance that produces hydrogen ions (H + )/hydronium ions (H 3 O + ) when it dissolves.

pH What is the pH of an ACID? Which type of OXIDE forms an ALKALI? Which type of OXIDE forms an ACID? What happens to the pH of an ACID when it is diluted?

Acids and Bases. Common household acids Citric acid Ethanoic acid Lactic acid Stearic acid Acetylsailicylic Acid.

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)

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

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 A More Detailed Look VCE Chemistry Unit 2: Environmental Chemistry Area of Study 1 – Water.

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

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

Water Solutions of Acids Universal Indicator is yellow Turn phenolphthalein colorless Turn litmus paper red React with metals to give off hydrogen gas.

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

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.

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

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.

1 Dr. Marwa Eid. 3 4  An acid is a solution that has an excess of H + (hydrogen ion).  The more H + ions, the more acidic the solution.

Title: Lesson 4 Strong and Weak Acids and Bases

Acids and Bases Chapter 14. Brønsted-Lowry Theory Brønsted-Lowry describes reactions of acids as involving the donation of a hydrogen ion (H + ) Brønsted-Lowry.

Acids and Bases. Brønsted-Lowry Theory Brønsted-Lowry describes reactions of acids as involving the donation of a hydrogen ion (H + ) Brønsted-Lowry describes.

ATB Question of the Day Day

Acids and Bases By Abdul Musawwir Class 2Q. NaCl NaOH A Salt A Base The base is under a salt!! Copyright © 2011 | Abdul Musawwir.

Acids and Bases – Acid Strength and K a.

Acid and base Iman AlAjeyan. Acid-Base Theory Acids in water solutions show certain properties. They taste sour and turn litmus paper red. They react.

Topic 8: Acids and Bases Theories of acids and bases Properties of acids and bases Strong and weak acids and bases The pH-scale.

Topic 8: Acids and Bases Theories of acids and bases Properties of acids and bases Strong and weak acids and bases The pH-scale.

Unit 9 Acids, Bases, Salts. Properties of Acids Acids (Table K) Dilute aqueous solutions of acids taste sour Lemons (citric acid) Vinegar (acetic acid)

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.

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

Acids, bases and pH. The Brønsted–Lowry theory of acids and bases involves the transfer of protons (hydrogen ions). Acids are proton donors.

CHALLENGE 1. KEY QUESTIONS How do we define an acid? How do we define a base?

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.

What is the acid concentration if 0.4 moles is dissolved in 150 cm 3 ? Molarity Check.

Acids and Bases Check 1. Define Bronsted-Lowry base; 2. Identify the acid and base; HSO 4 - (aq) + H 2 O(l) ←→ H 3 O + (aq) + SO 4 2- (aq) 3. What is a.

REVISION MATERIAL FOR PHYSICAL SCIENCES DEFINITIONS: ACIDS and BASES

Acids and Bases.

UNDERSTANDING ACIDS and ALKALIS

Objectives To learn about two models of acids and bases

CHAPTER 13 Acids and Bases 13.1 The Chemical Nature of Acids and Bases.

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

Acids and Bases.

Presentation transcript:

REVISION ACIDS & BASES

MODELS ARRHENIUS THEORY A n acid is a substance that produces hydrogen ions (H + )/hydronium ions (H 3 O + ) when it dissolves in water. A base is a substance that produces hydroxide ions (OH - ) when it dissolves in water. LOWRY-BRØNSTED THEORY An acid is a proton (H + ion) donor. A base is a proton (H + ion) acceptor

ACIDS STRONG ACIDS ionise completely in water to form a high concentration of H3O+ ions. Examples of strong acids are hydrochloric acid, sulphuric acid and nitric acid. WEAK ACIDS ionise incompletely in water to form a low concentration of H 3 O + ions. Examples of weak acids are ethanoic acid and oxalic acid. POLYPROTIC ACIDS Acids that can donate more than one proton AMPHOLYTE Can be an acid OR a base

BASES STRONG BASES dissociate completely in water to form a high concentration of OH- ions. Examples of strong bases are sodium hydroxide and potassium hydroxide WEAK BASES dissociate/ionise incompletely in water to form a low concentration of OH ions. Examples of weak bases are ammonia, calcium carbonate, potassium carbonate, calcium carbonate and sodium hydrogen carbonate.

IONISATION HCℓ(g)+H 2 O(ℓ) →H 3 O + (aq) + Cℓ - (aq) NH 3 (g) + H 2 O(ℓ) → NH + 4 (aq)+ OH - (aq) H 2 SO 4 (aq) + 2H 2 O(ℓ) →2H 3 O + (aq) +SO 2 4− (aq)

CONCENTRATED AND DILUTE CONCENTRATED ACIDS/BASES contain a large amount (number of moles) of acid/base in proportion to the volume of water. DILUTE ACIDS/BASES contain a small amount (number of moles) of acid/base in proportion to the volume of water

CONCENTRATED AND DILUTE

DILUTION

CONJUGATE ACID-BASE PAIRS HCℓ(g)+H 2 O(ℓ) →H 3 O + (aq) + Cℓ - (aq) NH 3 (g) + H 2 O(ℓ) → NH + 4 (aq)+ OH - (aq) H 2 SO 4 (aq) + 2H 2 O(ℓ) →2H 3 O + (aq) +SO 2 4− (aq)

NEUTRALISATION REACTIONS HCℓ(aq)+NaOH(aq)→NaCℓ(aq)+ H 2 O(ℓ) HCℓ(aq)+KOH(aq)→KCℓ(aq)+ H 2 O(ℓ) HCℓ(aq)+Na 2 CO 3 (aq)→NaCℓ(aq) +H 2 O(ℓ) + CO 2 (g) HNO 3 (aq) +NaOH(aq)→NaNO 3 (aq) +H 2 O(ℓ) H 2 SO 4 (aq) +2NaOH(aq)→Na 2 SO 4 (aq) +2H 2 O(ℓ) (COOH) 2 (aq) +NaOH(aq)→(COO) 2 Na 2 (aq)+ H 2 O(ℓ) CH 3 COOH(aq) + NaOH(aq) → CH 3 COONa(aq) + H 2 O(ℓ)

PHENOLPHTHALEIN STRONG BASE WITH WEAK ACID STRONG BASE WITH STRONG ACID

BROMOTHYMOL STRONG BASE WITH STRONG ACID

METHYL ORANGE WEAK BASE WITH STRONG ACID

GRADE 11 STOICHIOMETRY