Introductory Chemistry II: Acids and Bases
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Questions and Answers

Which acid-base theory emphasizes the role of proton donors and acceptors?

  • Arrhenius Theory
  • Lux-Flood Theory
  • Lewis Theory
  • Brønsted-Lowry Theory (correct)

    • What characterizes Lewis acids and bases?

  • They require an aqueous solution to operate.
  • They involve electron pair acceptors and donors. (correct)
  • They are defined based on proton transfer.
  • They strictly follow Arrhenius definitions.

    • What type of substances does the self-ionizing definition of acids and bases apply to?

  • Nonaqueous media (correct)
  • Protic substances only
  • Only aqueous solutions
  • Ionic compounds

    • Which theory is considered the most general in defining acids and bases?

    <p>Lewis Theory</p> Signup and view all the answers

    In which of the following reactions would a Lewis base be characterized as donating an electron pair?

    <p>A substance combining with a Lewis acid</p> Signup and view all the answers

    What does HSAB stand for in the classification of metal ions and ligands?

    <p>Hard and Soft Acids and Bases</p> Signup and view all the answers

    Which of the following compounds is an example of a strong acid in liquid solutions?

    <p>H2SO4</p> Signup and view all the answers

    Which type of oxides typically exhibit acidic properties according to trends in acid-base properties?

    <p>Non-metallic oxides</p> Signup and view all the answers

    What does an Arrhenius acid release when dissolved in water?

    <p>H+ ions</p> Signup and view all the answers

    Which of the following is a strong acid according to the Arrhenius definition?

    <p>HClO4</p> Signup and view all the answers

    Why is NH3 (ammonia) not classified as an Arrhenius base?

    <p>It does not contain hydroxide groups.</p> Signup and view all the answers

    An Arrhenius base is characterized by producing which ion when dissolved in water?

    <p>OH-</p> Signup and view all the answers

    How does a strong acid behave in an aqueous solution according to the Arrhenius theory?

    <p>It completely ionizes.</p> Signup and view all the answers

    Which of the following substances is considered a strong base?

    <p>LiOH</p> Signup and view all the answers

    What happens when HCl gas is dissolved in water according to the Arrhenius definition?

    <p>It increases the concentration of H3O+ ions.</p> Signup and view all the answers

    Which statement about Arrhenius acids is true?

    <p>They are only defined in terms of water.</p> Signup and view all the answers

    What is a characteristic of acids?

    <p>They turn blue litmus red.</p> Signup and view all the answers

    Which of the following definitions pertains to acids and bases?

    <p>Solvent System Definition</p> Signup and view all the answers

    What happens to the pH level of a solution when it is more acidic?

    <p>The pH decreases.</p> Signup and view all the answers

    What taste is primarily associated with bases?

    <p>Bitter</p> Signup and view all the answers

    Which statement correctly describes a base's effect on litmus paper?

    <p>It turns it blue.</p> Signup and view all the answers

    What do both Arrhenius and Brønsted-Lowry definitions focus on regarding acids and bases?

    <p>The production of hydroxide or hydrogen ions.</p> Signup and view all the answers

    What is the typical pH range of a basic solution?

    <p>Greater than 7</p> Signup and view all the answers

    Which of the following is a common reaction of acids?

    <p>Reacting with bases to form salts.</p> Signup and view all the answers

    Which statement correctly describes weak acids?

    <p>Weak acids undergo reversible reactions with corresponding ions.</p> Signup and view all the answers

    What characterizes a weak base, such as ammonium hydroxide?

    <p>It exists in both ionized and un-ionized forms in solution.</p> Signup and view all the answers

    Which of the following describes a limitation of the Arrhenius concept of acids and bases?

    <p>It considers only H+ and OH- ions in aqueous solutions.</p> Signup and view all the answers

    In an Arrhenius acid-base reaction, what are the products of the reaction between hydrochloric acid and sodium hydroxide?

    <p>Sodium chloride and water</p> Signup and view all the answers

    Which of the following best describes a strong Arrhenius base?

    <p>It completely dissociates in water to produce OH- ions.</p> Signup and view all the answers

    How can you differentiate between strong and weak Arrhenius acids?

    <p>By their level of ionization in water.</p> Signup and view all the answers

    Which ion would be produced by the dissociation of calcium hydroxide in water?

    <p>OH- and Ca2+</p> Signup and view all the answers

    What is one characteristic difference between the definitions of Bronsted-Lowry acids and bases compared to Arrhenius acids and bases?

    <p>Bronsted-Lowry bases can accept protons, not just produce OH- ions.</p> Signup and view all the answers

    Study Notes

    Course Information

    • Course Title: Introductory Chemistry II
    • Course Code: CHEM 1820
    • Instructor: Dr. Joyann Marks
    • Email: [email protected]
    • Lecture Topic: Acids and Bases
    • Lecture Number: 1

    Office Hours

    • Mondays: 2-3 PM
    • Wednesdays: 2-3 PM
    • Thursdays: 1-2 PM
    • Virtual appointments available via calendly.com/joyannmarks/uwichem
    • Email for scheduling outside of these times: [email protected]
    • Tutorials not available Tuesdays and Fridays at 10 AM due to scheduling conflicts

    Learning Outcomes

    • Discuss acid-base properties of protic and aprotic substances and explain why the Lewis definition is most general.
    • Describe reactions in liquid NH3, HF, H2SO4, and BrF3.
    • Classify metal ions and ligands according to HSAB concepts.
    • Account for trends in acid-base properties of oxides, metal ions, and ligands.

    Objectives for Acids and Bases

    • Review Arrhenius and Brønsted-Lowry theories of acids and bases.
    • Discuss solvent-oriented definitions of acids and bases.
    • Discuss self-ionizing and non-self-ionizing non-aqueous media.
    • Discuss Brønsted Lowry as a special case.
    • Discuss acidic and basic oxides (Lux-Flood definition).
    • Discuss trends in acid-base properties of oxides.
    • Discuss Lewis acid-base theory.
    • Discuss water as a Lewis base.
    • Discuss HSAB (Hard and Soft Acid and Base) concepts.
    • Discuss reactions of Lewis acids and bases.

    Acids

    • Acid properties: sour taste, turning blue litmus red, reaction with bases to form salts.
    • Aqueous solutions have a pH less than 7. Lower pH means higher acidity and concentration of hydrogen ions (using Arrhenius/Brønsted-Lowry definitions).

    Bases

    • Base properties: bitter taste, slippery to the touch, turning red litmus blue, react with acids to form salts.
    • Aqueous solutions have a pH greater than 7. Higher pH means higher basicity and concentration of hydroxide ions (using Arrhenius/Brønsted-Lowry definitions).

    Definitions of Acids and Bases

    • Arrhenius acid and bases
    • Brønsted-Lowry Definition
    • Solvent System Definition
    • Lewis Definition
    • Lux-Flood Definition

    Arrhenius Acids and Bases

    • Acid: substance that ionizes in water to produce H+ ions.
    • Base: substance that ionizes in water to produce OH- ions.
    • Limitations: Only applicable to aqueous solutions; doesn't account for bases like NH3.

    Arrhenius Acids

    • An Arrhenius acid, when dissolved in water, increases the concentration of H3O+ (hydronium) ions.
    • Chemists often use H+(aq) as shorthand for H3O+(aq); this representation is for hydrogen ion in water.
    • Example: HCl(aq) → H+(aq) + Cl-(aq), where H+(aq) is actually H3O+(aq).

    Arrhenius Bases

    • An Arrhenius base, when dissolved in water, increases the concentration of OH-(aq) hydroxide ions.
    • Example: NaOH(aq) → Na+(aq) + OH-(aq)

    Strong Acids and Bases

    • Strong acid: ionizes completely in water.
    • Some strong acids (HCl, HBr, HI, HNO3, HClO4, H2SO4).
    • Strong base: dissociates completely in water.
    • Some strong bases (NaOH, LiOH, KOH, Ca(OH)2, Sr(OH)2, Ba(OH)2)

    Weak Acids and Bases

    • Weak acid/base: partially/incomplete ionization in water
    • Example: acetic acid, HC2H3O2)(or CH3COOH) is a weak acid

    Limitations of the Arrhenius Concept

    • Limited to aqueous solutions
    • Doesn’t account for properties of substances not involving OH⁻ or H⁺ ions.
    • The OH⁻ ion is singled out as the source of basicity when other species play a similar role in reactions.
    • Broader definitions of acids/bases are needed.

    Arrhenius Acid-Base Reaction

    • Involves the reaction of an Arrhenius acid and an Arrhenius base.
    • Produces water and a salt.
    • Example: HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)

    Additional Information

    • Relevant textbooks and online resources provided for further study.

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    Description

    Test your understanding of the properties and behaviors of acids and bases in chemistry. This quiz will cover topics such as the Lewis definition, Arrhenius and Brønsted-Lowry theories, and reactions involving various substances. Perfect for students enrolled in CHEM 1820.

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