Chemistry: Acids and Bases Fundamentals
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Chemistry: Acids and Bases Fundamentals

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Questions and Answers

Which statement accurately defines a Lewis acid?

  • A molecule that combines with water.
  • A molecule that produces hydroxide ions.
  • A molecule that accepts an electron pair. (correct)
  • A molecule that donates protons.

    • What is the correct expression for the equilibrium constant K in the context of proton transfer?

  • K = a H2O / a Acid * a H3O
  • K = a H3O * a Base / a Acid * a H2O (correct)
  • K = a Acid * a H2O / a H3O * a Base
  • K = a Acid / a H3O * a Base

    • A strong acid is characterized by which of the following?

  • High pKa and low Ka
  • Equal pKa and Ka values
  • Low pKa and high Ka (correct)
  • Dependent on concentration only

    • In the context of acid-base equilibria, what role does water generally play?

    <p>It serves as a neutral solvent.</p> Signup and view all the answers

    Which of the following compounds has the highest acidity based on pKa values?

    <p>H3O+</p> Signup and view all the answers

    What is true about conjugate acids and bases?

    <p>A conjugate acid can also function as a base.</p> Signup and view all the answers

    Which statement is incorrect regarding the relationship between pH and hydronium ion concentration?

    <p>A pH of 0 is a neutral solution.</p> Signup and view all the answers

    What describes a polyprotic acid?

    <p>An acid that can donate two or more protons.</p> Signup and view all the answers

    Which of the following statements about activities in dilute solutions is true?

    <p>Activities can be approximated by concentrations.</p> Signup and view all the answers

    How would you describe the primary function of a Brønsted base?

    <p>It acts as a proton acceptor.</p> Signup and view all the answers

    Study Notes

    Acids and Bases

    • Acids donate protons (H+)
    • Bases accept protons (H+)
    • Brønsted-Lowry definition: acids donate, bases accept protons
    • Lewis acids and bases: broader definition - acids accept electron pairs, bases donate electron pairs

    Protons in Water

    • Protons in water are highly solvated
    • Represented by the hydronium ion (H3O+)

    Conjugates

    • When an acid loses a proton, it forms its conjugate base
    • When a base gains a proton, it forms its conjugate acid
    • Acids can be neutral, cationic, or anionic
    • Bases can be anionic, neutral, or cationic

    General Equilibrium for Proton Transfer

    • An acid transferring a proton to a base in water can be represented by a general equilibrium equation
    • Equilibrium constant (K) is determined by the activities of the components

    Activity and Concentration

    • Activities in dilute solutions can be approximated by concentrations
    • Water activity is considered constant in dilute solutions

    Acidity of Aqueous Solutions

    • Depends on the concentration of hydronium ions (H3O+)
    • Sørensen defined pH: pH = -log10 [H3O+]
    • pX = -log10 X for many functions

    Acid Dissociation in Water

    • The acidity constant (Ka) measures the strength of an acid
    • Ka is determined by the equilibrium constant for the dissociation in water

    pKa

    • pKa = -log10 Ka
    • Measure of acid strength
    • High Ka = low pKa = strong acid
    • Low Ka = high pKa = weak acid

    Polyprotic Acids

    • Have multiple ionizable protons
    • Can donate protons in steps, each with a different pKa value

    Examples

    • Water (H2O) can act as an acid or a base
    • H3O+ is a strong acid
    • Acetic acid (CH3CO2H) is a weak acid
    • Ammonium ion (NH4+) is a weak acid

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    Description

    This quiz covers essential concepts related to acids and bases, including definitions and characteristics as per the Brønsted-Lowry and Lewis theories. It also explores the behavior of protons in water, the formation of conjugate pairs, and the principles of chemical equilibrium. Test your understanding of these fundamental chemistry topics!

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