Fundamental Inorganic Chemistry Quiz
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Questions and Answers

What describes the relationship between pKa and acid strength?

  • The concentration of the acid solution determines strength.
  • Stronger acids have lower pKa values. (correct)
  • Higher pKa values indicate stronger acids.
  • Acids with pKa values below 0 are classified as weak.

    • What happens to the phosphate buffer equilibrium if H3O+ concentration increases?

  • The concentration of H2PO4- decreases. (correct)
  • The pH of the buffer solution increases.
  • The equilibrium shifts to produce more HPO4 2-.
  • H3O+ concentration remains constant.

    • What is the primary measure that pH represents in solution?

  • The hydronium ion concentration. (correct)
  • The overall molecular concentration of the solution.
  • The concentration of hydroxide ions.
  • The total number of water molecules present.

    • Which of the following statements about strong and weak acids is true?

    <p>Weak acids have higher pKa values than strong acids.</p> Signup and view all the answers

    At which pH level can aqueous solutions not exceed?

    <p>pH 14</p> Signup and view all the answers

    What are the positively charged ions called?

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

    Which statement about salts is correct?

    <p>Salts consist of two ions forming a neutral compound.</p> Signup and view all the answers

    What is the oxidation state of Iron in Iron (III) Sulphate?

    <p>+3</p> Signup and view all the answers

    What happens when an acid deprotonates?

    <p>It loses a hydrogen ion.</p> Signup and view all the answers

    Which of the following compounds is an example of a polyprotic acid?

    <p>Acetic Acid</p> Signup and view all the answers

    What is formed when hydrochloric acid ionizes in water?

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

    What is the relationship between anions and their conjugate acids?

    <p>Anions are created when acids donate protons.</p> Signup and view all the answers

    Which of the following is a correct name for FeSO4?

    <p>Iron (II) Sulphate</p> Signup and view all the answers

    What is the implication of acetic acid having a pK of 4.756?

    <p>At pH 4.756, there are equal concentrations of acetic acid and acetate.</p> Signup and view all the answers

    Which compound predominantly exists at physiological pH (7.2) when considering succinic acid?

    <p>Succinic anion</p> Signup and view all the answers

    How does the Brønsted-Lowry definition categorize acids and bases?

    <p>Acids donate protons and bases accept protons.</p> Signup and view all the answers

    What happens to water at a neutral pH of 7?

    <p>It can act as both an acid and a base.</p> Signup and view all the answers

    Which statement about the deprotonization of acids is true?

    <p>It varies with pH levels.</p> Signup and view all the answers

    What defines the conjugate base of acetic acid?

    <p>Acetate ion.</p> Signup and view all the answers

    What is the relationship between sulfuric acid and its ionized forms?

    <p>Both bisulfate and sulfate ions can exist in solution.</p> Signup and view all the answers

    Which statement best describes the formation of ammonium ions?

    <p>Ammonium is formed when ammonia accepts a proton.</p> Signup and view all the answers

    Study Notes

    Fundamental Inorganic Chemistry

    • Inorganic chemistry studies non-carbon-based compounds and carbon compounds less oxidized than carbon dioxide.
    • Yellow is a color found in all living organisms.
    • Salts are formed from two ions.
    • Ions are atoms with a positive or negative electric charge.
    • Cations are positively charged ions.
    • Anions are negatively charged ions.
    • The charge of an ion is its valence.
    • A 2+ ion is a divalent cation, a 3- ion is a trivalent anion.
    • Salt names consist of the cation first, then the anion.
    • Examples include Sodium Chloride and Potassium Nitrate.
    • Some cations are formed from their conjugate bases. Ammonia (NH3), for example, forms Ammonium (NH4+).
    • Oxidation state of a cation (like Iron) is indicated using Roman numerals. Iron(II) Sulphate is FeSO4; Iron(III) Sulphate is Fe2(SO4).

    Acids

    • Acids deprotonate (lose hydrogen ions) when they ionize or deprotonate.
    • HCl + H2O → H3O+ + Cl- (shorthand: HCl → H+ + Cl-)
    • Polyprotic acids have more than one proton to lose, which creates a wide range of anions with varying pH values.
    • Organic acids work similarly. Acetic acid (CH3COOH), for example, forms acetate (CH3COO-) and H3O+.

    Acids and Bases

    • Multiple definitions exist for acids and bases.
      • Arrhenius: Acids form H3O+ ions; bases form OH- ions.
      • Brønsted-Lowry: Acids donate H+ ions; bases accept H+ ions.
      • Lewis: Acids donate electron pairs; bases accept electron pairs.
    • Water has a neutral pH (7) and reacts with itself (forming H3O+ and OH-).
    • Acidic solutions (pH < 7) have more H3O+ than OH-.
    • Basic/Alkaline solutions (pH > 7) have more OH- than H3O+.
    • pH measures H3O+ concentration (pH = -log10[H+]).

    Strong and Weak Acids

    • Acid strength depends on pKa. A lower pKa indicates a stronger acid.
    • Organic acids are always weak acids.
    • Hydrochloric and Nitric acids are strong acids.
    • Nitrous acid and Acetic acid are weak acids.

    Buffers

    • Buffers maintain a narrow pH range around a pKa value, preventing drastic pH changes.
    • Phosphate buffers, for example, are used at physiological pH (7.2) to prevent pH changes.

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    Fundamental Inorganic Chemistry PDF

    Description

    Test your knowledge of fundamental concepts in inorganic chemistry. This quiz covers topics such as ions, salts, acids, and the properties of cations and anions. Perfect for students looking to solidify their understanding of non-carbon-based compounds.

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