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Acids & Bases & Equilibrium
Acid- Base Strength & Dissociation Recall: Strong acids and bases dissociate quantitatively (>99.9%) in water Weak acids and bases dissociate partially in water When a weak acid or base is added to water dynamic equilibrium is established
The Acid-Dissociation Constant, K a
Determine the K a of propanoic acid (C 2 H 5 COOH (aq) ) given that a 0.10 mol/L solution has a pH of 2.96
Determine the pH of a 0.050 mol/L solution of nitrous acid (HNO 2(aq) ). K a = 5.6 X 10 -4
The Base-Ionization Constant, K b
A 5.0 g/L solution of aniline (C 6 H 5 NH 2(aq) ) has a pH of 8.68. Determine the K b of aniline.
Calculate the pH of a 3.6 X 10 -3 mol/L solution of quinine (C 20 H 24 N 2 O 2(aq). K b = 3.3 X 10 -6
Practice Problems P. 554 #1, 2 P. 556 #3-5 P. 568-570 #7-10 P. 574 #12, 13
Relationship between K a, K b, & K w Worksheet (Benzoic Acid)
Lecture 122/12/07. pH What is it? How do you measure it?
8.2 – Equilibrium of Weak Acids and Bases Acids and bases dissociate in aqueous solutions to form ions that interact with water. pH of a solution is determined.
Lecture 142/19/06. Strong Bases: What is the pH of 0.01 M solution of each of the strong bases? NaOH CaO.
Acid and Base Dissociation Constants. How do we calculate [H + ] for a weak acid? We know that strong acids dissociate 100% and that, therefore, the [H.
IIIIIIIVV Ch. 19 – Strengths of Acids & Bases 19.3 pp. 602 – 611.
The pK a Scale. Acid Dissociation Constant, K a K a, is a measure of how readily H + ions are released HA (aq) + H 2 O (aq) H 3 O + (aq) + A - (aq) K.
Acids & Bases Part 2. Acid & Base Ionization Constants A weak acid or base produces a reaction that only partially goes forward. The acid or base ionization.
Chemistry Chapter Acids and Bases. (Self-Ionization of Water) H 2 O + H 2 O H 3 O + + OH - Two water molecules collide to form Hydronium and.
Acids and Bases Part 3. Strong and Weak Acids and Bases Consider the acid dissociation reaction: HA H + + A - If this equilibrium lies to the right,
Equilibrium – Acids and Bases. Review of Acids and Bases Arrhenius Theory of Acids and Bases ▫An acid is a substance that dissociates in water to produce.
Acid-Base Equilibrium Learning Goal: I will understand the Bronsted-Lowry Theory of acids and bases, be able to identify conjugate acid/base pairs, understand.
PH. Definitions and Formulas The pH scale is defined as the negative log of the concentration of H + : pH = -log[H + ] The pOH scale is defined as the.
Lecture 152/22/06 Topics due. Neutralization: Acid + Base = Water + Salt pH of neutralized solution? Strong Acid + Strong Base HCl (aq) + NaOH (aq)
Ch.15: Acid-Base and pH Part 1. Self-Ionization of Water Pure water is a VERY weak electrolyte It undergoes self-ionization H 2 O (l) + H 2 O (l) H 3.
PH. Hydrogen Ions and Acidity Water molecules go through self ionization to form hydrogen ion and hydroxide ions. In aqueous solution, hydrogen ions H.
Finding the pH of Weak Acids. Strengths of Acids and Bases “Strength” refers to how much an acid or base ionizes in a solution. STRONGWEAK Ionize completely.
Review 1: Written the conjugate base and acid for the following acids and bases.
General Chemistry II Acid and Base Equilibria Lecture 2
1 The Chemistry of Acids and Bases –Finding pH and pOH.
Strong Acids Strong acids fully dissociate so: They are fully separated into their ions They are good conductors of electricity Are not in a state of equilibrium.
Acids and Bases Calculating Excess. Calculations involving strong acids and bases During an experiment, a student pours 25.0 mL of 1.40 mol/L nitric acid.
BUFFERS Mixture of an acid and its conjugate base. Buffer solution resists change in pH when acids or bases are added or when dilution occurs. Mix: A.
U2 S2 L4 Ka and Kb calculations p : pH and Ka of a Weak Acid p : The Base Dissociation Constant, Kb Homework: p 591: # 5, 6, 7, 8, 9 and.
Acids, Bases, and pH Part 2. Properties of Acids Acids: –Taste Sour (never use taste to test the presence of an acid) –Are Electrolytes –Are Corrosive.
Chapter 19 Self-Ionization of Water and pH. Strong vs. Weak Strong: 100% dissociation of H + or OH – – Strong electrolytes (conduct electricity very well)
Acid – Base Equilibrium Problem #13. Example: Calculate the number of grams of NH 4 Br that have to be dissolved in 1.00L of water at 25 o C to have a.
1 Chapter 10 Acids and Bases 10.3 Strengths of Acids and Bases 10.4 Dissociation Constants.
Lecture 122/18/05 There is class on Monday. Strong Bases: What is the pH of 0.01 M solution of each of the strong bases? Oxide (O 2- : CaO, Na 2 O) O.
The pH Scale. Arrange the substances in order of increasing pH. Match the pH and [H + ] to each substance Try to work out the relationship between pH.
The Ionic Product of Water KwKw. Ionic Product of water, K w Just because a solution contains [H + ] it doesn’t necessarily mean it’s acidic. All aqueous.
SWBAT Learn about The Common Ion Effect. SWBAT Work out Common Ion Effect icebox problems.
Be able to write the chemical equation for a chemical species acting as an acid: HX(aq) H + (aq) + X - (aq) Example Write the equation showing the bicarbonate.
Example 15.6: Find the pH of M HNO 2 (aq) 25 °C 9 Tro, Chemistry: A Molecular Approach, 2/e.
BASE IONIZATION Section 8.3. Base-Ionization Constant - K b ■The following equation represents a weak base, B, dissolving in water: ■B (aq) + H 2 O (l)
Section 18-3 Section 18.3 Hydrogen Ions and pH Explain pH and pOH. Relate pH and pOH to the ion product constant for water. Calculate the pH and pOH of.
Ch. 19 – Acids & Bases II. pH (p. 644 – 658). A. Ionization of Water H 2 O + H 2 O H 3 O + + OH - Self-Ionization of Water.
TEKS 10I: Define pH and use the hydrogen or hydroxide ion concentrations to calculate the pH of a solution. How is pH defined? The pH of a solution is.
Chapter 17: Additional Aspects of Aqueous Equilibria Section 1: The Common Ion Effect.
Acids and Bases. Ionization of Water H 2 O + H 2 O H 3 O + + OH - K w = [H 3 O + ][OH - ] = 1.0
Applications of Aqueous Equilibria Common Ions When we dissolve acetic acid in water, the following equilibrium is established: –CH 3 COOH CH 3 COO -
16.1b: Acid strength and equilibrium position. Strong acids ionize completely, strong electrolyte reacts completely with water to form H 3 O +
Dissociation Constant or Ionization Constant for Weak Acids & Bases When a weak acid, HX, is placed into water some of it reacts with water to form H 3.
Relationship Between Ka and Kb. Consider the dissociation of a weak acid: CH 3 COOH (aq) + H 2 O (l) H 3 O + (aq) + CH 3 COO - (aq) K a = [H 3 O + ][CH.
Acid/Base Indicators Substance that changes color in the presence of an acid or a base – Red or Blue Litmus – Phenolphthalein (phth) – Bromothymol blue.
19.3 Strengths of Acids and Bases > 1 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved. Chapter 19 Acids, Bases, and Salts 19.1.
Chemistry 1011 Slot 51 Chemistry 1011 TOPIC Acids and Bases TEXT REFERENCE Masterton and Hurley Chapter 4.2 (Review), 13, 14.1, 15.1 (page 427), 21.2 (page589)
Chapter 16: Equilibrium in Acid-Base Systems 16.1a: Self-ionization of Water K w pH and pOH.
Weak Acids and Bases. “WEAK” Acids and bases that ionize less (much less) than 100% The amount of H 3 O + or OH - in solution is MUCH smaller than the.
CHAPTER 13 Acids and Bases 13.3 Acid-Base Equilibria.
PH (potential of Hydrogen). According to the Bronsted-Lowry theory, both acids and bases are related to the concentration of hydrogen ions. Acids will.
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