Chemistry Chapter 4: Acids and Bases Quiz
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Questions and Answers

Which represent a base and its conjugate acid (listed in that order)?

  • NH<sub>4</sub><sup>+</sup>, NH<sub>3</sub>
  • CH<sub>3</sub>S<sup>-</sup>, CH<sub>3</sub>SH (correct)
  • CH<sub>3</sub>CH<sub>3</sub>, CH<sub>3</sub>CH<sub>2</sub><sup>-</sup>
  • HCOOH, HCOO<sup>-</sup>
  • A strong acid completely donates H+ to a base.

    True

    A low pKa value indicates a strong acid.

    True

    What is the equilibrium constant (pKeq) of the following reaction?

    <p>4.94</p> Signup and view all the answers

    Which group will lose a proton first (i.e. is most acidic)?

    <p>The alcohol</p> Signup and view all the answers

    Which pair has the stronger acid listed first (on left)? Select all that apply.

    <p>HC≡CH, cyclohexane</p> Signup and view all the answers

    What is the general trend of acidity across a row in the periodic table?

    <p>Acidity increases going from left to right.</p> Signup and view all the answers

    What is the general trend of acidity down a column in the periodic table?

    <p>Acidity decreases going down a column.</p> Signup and view all the answers

    Which carbon atom is most acidic in the molecule below?

    <p>The carbon atom with the sp hybridization.</p> Signup and view all the answers

    Study Notes

    Chapter 4: Acids and Bases

    • Key Concepts: Brønsted-Lowry acids and bases, acid dissociation constants (pKa), acidity trends (electronegativity, atom size, hybridization at carbon, resonance delocalization, inductive effects).
    • Assigned Reading: All of Chapter 4 except sections 4.2B, 4.2C, 4.5, and 4.7.
    • Practice Problems: From the 8th edition textbook, chapter 4, problems 4.1, 2, 5, 6, and end-of-chapter problems 4.10, 11, 13, 15, 26, 29, 38, 47 (45), 54 (48), 55 (49), 58 (52), and 59 (53).

    Chapter 4.1-4.4: Acids, Bases, and pKas

    • pH and Hydrangeas: pH scale relates to acidity and alkalinity, with a lower pH indicating acidity and a higher pH indicating alkalinity. Hydrangeas flower color changes based on pH levels of soil.
    • Reading: Chapter 4.1, 4.2A, 4.3, and 4.4.
    • Textbook Problems: 4.1, 4.2, 4.5, 4.6, 4.10, 4.11, 4.15, 4.26, and 4.29.

    Brønsted-Lowry Acids and Bases

    • Definitions: Acids are proton donors, bases are proton acceptors.
    • Conjugate Pairs: Conjugate base formed when an acid loses a proton; conjugate acid formed when a base accepts a proton.
    • Strong vs. Weak: Strong acids/bases completely donate/accept protons; weak acids/bases don't.

    Acid Dissociation Constants and pKa

    • pKa and Strength: pKa values measure the strength of an acid; lower pKa indicates a stronger acid.
    • Equilibrium Constant (Ka): Used to express the strength of an acid, relates to concentrations of products and reactants during the acid dissociation process.
    • Relationship between pKa and Ka: The lower the pKa value, the stronger the acid, and the higher its Ka value.

    pKa Values for Common Acids

    • A table of pKa values for various common acids. Refer to the provided table (Table 4.1).

    Predicting Equilibria

    • Using pKa values: Determine whether an acid-base reaction will occur by comparing the pKa of the acid to the pKa of the conjugate acid or base.

    iClicker Questions (Ch4#1, #2, #3, #4)

    • Question 1: Select the conjugate acid-base pair.
    • Question 2: Calculate equilibrium constant (pKeq).
    • Question 3: Identify the most acidic proton in a molecule.
    • Question 4: Select the stronger acid from pairs.
    • Factors affecting stability: Electronegativity, atom size, hybridization, resonance, inductive effects, electrostatic stabilization influence stability of anions during acid dissociation.
    • Electronegativity: More electronegative elements stabilize negative charges better (stabilizing conjugate bases, strengthening acids)
    • Atom Size: Larger atoms accommodate the negative charge better (more stable, stronger acid)
    • Hybridization: More s-character, more stable.
    • Resonance: Delocalization of the negative charge (e.g., via resonance) stabilizes conjugate base improving acid strength.
    • Inductive effects: Electron-withdrawing groups stabilize the negative charge (strengthening the acid).
    • Acidity based on functional groups (alcohols, thiols, carboxylic acids, etc.,): Provide details on acid strength trends for these groups based on structure considerations & the pKa values. Refer to the table and examples provided.
    • Organic Acidity examples and trends: Examples and comparative details on different organic acid structures and stability trends; focus on determining the most acidic proton.
    • Cyclic dipeptides: Examples provided.
    • Cholic Acid: example provided

    Additional notes

    • Consider the provided images and tables for specific details and examples.

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    Related Documents

    Chapter 4 Acids and Bases PDF

    Description

    Test your understanding of Chapter 4 on Acids and Bases, focusing on key concepts like Brønsted-Lowry definitions, acid dissociation constants, and pH levels. This quiz covers the assigned readings and practice problems to enhance your grasp of acidity trends and their implications in chemistry.

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