T08+-+Acid-Base


 * Topics 8&18 - Acids and Bases (SL/HL 2)**

** 8.1 Theories of acids and bases - **** 2 hours ** 8.1.1 Define acids and bases according to the Brønsted–Lowry and Lewis theories.(1) 8.1.2 Deduce whether or not a species could act as a Brønsted–Lowry and/or a Lewis acid or base. (3) 8.1.3 Deduce the formula of the conjugate acid (or base) of any Brønsted–Lowry base (or acid). (3)
 * Topic 8: Acids and bases (6 hours) **
 * Power Point Presentation: || Note Guide: ||
 * [[file:T08D01 - 05.04.11 - 8.1 Acid Base Theories.pdf]] || [[file:T08D01 - 05.04.11 - 8.1 AB Theories Notes.pdf]] ||

** 8.2 Properties of acids and bases - **** 1 hour ** 8.2.1 Outline the characteristic properties of acids and bases in aqueous solution. (2)
 * Power Point Presentation: || Note Guide: ||
 * [[file:T08D01 - 05.04.11 - 8.2 Acid Base Properties.pdf]] || [[file:T08D01 - 05.04.11 - 8.2 AB Properties Notes.pdf]] ||

** 8.3 Strong and weak acids and bases - **** 2 hours ** 8.3.1 Distinguish between strong and weak acids and bases in terms of the extent of dissociation, reaction with water and electrical conductivity. (2) 8.3.2 State whether a given acid or base is strong or weak. (1) 8.3.3 Distinguish between strong and weak acids and bases, and determine the relative strengths of acids and bases, using experimental data. (2)
 * Power Point Presentation: || Note Guide: ||
 * [[file:T08D02 - 05.06.11 - 8.3 Strong Week Acid Base.pdf]] || [[file:T08D02 - 05.06.11 - 8.3 Strong and Weak AB Notes.pdf]] ||

** 8.4 The pH scale - **** 1 hour ** 8.4.1 Distinguish between aqueous solutions that are acidic, neutral or alkaline using the pH scale. (2) 8.4.2 Identify which of two or more aqueous solutions is more acidic or alkaline using pH values. (2) 8.4.3 State that each change of one pH unit represents a 10-fold change in the hydrogen ion concentration [H+(aq)]. (1) 8.4.4 Deduce changes in [H+(aq)] when the pH of a solution changes by more than one pH unit. (3)
 * Power Point Presentation: || Note Guide: ||
 * [[file:T08D03 - 05.10.11 - 8.4 pH Scale.pdf]] || [[file:T08D03 - 05.10.11 - 8.4 pH Scale Notes.pdf]] ﻿ ||

** Topic 18: Acids and bases (10 hours) ** ** 18.1 Calculations involving acids and bases - **** 4 hours ** 18.1.1 State the expression for the ionic product constant of water (Kw). (1) 18.1.2 Deduce [H+(aq)] and [OH–(aq)] for water at different temperatures given Kw values. (3) 18.1.3 Solve problems involving [H+(aq)], [OH–(aq)], pH and pOH. (3) 18.1.4 State the equation for the reaction of any weak acid or weak base with water, and hence deduce the expressions for Ka and Kb. (1) 18.1.5 Solve problems involving solutions of weak acids and bases using the expressions: Ka × Kb = Kw, pKa + pKb = pKw, pH + pOH = pKw. (3) 18.1.6 Identify the relative strengths of acids and bases using values of Ka, Kb, pKa and pKb. (2)
 * Power Point Presentation: || Note Guide: ||
 * [[file:T08D04 - 05.12.11 - 18.1 AB Calcs.pdf]] || [[file:T08D04 - 05.12.11 - 18.1 HL AB Calcs Notes.pdf]] ||

** 18.2 Buffer solutions - **** 2 hours ** 18.2.1 Describe the composition of a buffer solution and explain its action. (3) 18.2.2 Solve problems involving the composition and pH of a specified buffer system. (3)
 * Power Point Presentation: || Note Guide: ||
 * [[file:T08D05 - 05.16.11 - 18.2 Buffers.pdf]] || [[file:T08D05 - 05.16.11 - 18.2 HL Buffer Solution Notes.pdf]] ||

** 18.3 Salt hydrolysis - **** 1 hour ** 18.3.1 Deduce whether salts form acidic, alkaline or neutral aqueous solutions. (3)
 * Power Point Presentation: || Note Guide: ||
 * [[file:T08D06 - 05.18.11 - 18.3 Salt Hydrolysis.pdf]] || [[file:T08D06 - 05.18.11 - 18.3 HL Salt Hydrolysis Notes.pdf]] ||

** 18.4 Acid–base titrations - **** 2 hours ** 18.4.1 Sketch the general shapes of graphs of pH against volume for titrations involving strong and weak acids and bases, and explain their important features. (3)
 * Power Point Presentation: || Note Guide: ||

** 18.5 Indicators - **** 1 hour ** 18.5.1 Describe qualitatively the action of an acid–base indicator. (2) 18.5.2 State and explain how the pH range of an acid–base indicator relates to its pKa value. (3) 18.5.3 Identify an appropriate indicator for a titration, given the equivalence point of the titration and the pH range of the indicator. (2)
 * Power Point Presentation: || Note Guide: ||


 * Topic 08/18 Resources: **



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 * Khan Intro to Acids and Bases: **
 * Conjugate Acid Base Pairs: **
 * pH and pOH explanation: **
 * pH and pOH of strong acids and bases: **
 * pH of weak acids: **
 * pH of weak bases: **
 * HL: pKa and pKb relationship: **
 * HL: Buffers: **
 * HL: Strong Acid Titration **
 * HL: Weak Acid Titration: **
 * HL: Half Equivalence Point: **
 * HL: Titration Roundup: **