Chemistry VSEPR Theory Quiz
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Questions and Answers

The electron-pair arrangement of ozone, O3, is ___ and the molecular geometry is ___.

tetrahedral, bent

Which of the following is not a strong acid in aqueous solution?

  • HClO2 (correct)
  • HCl
  • HBr
  • HI

    • What is the pH of a 0.07 M solution of KOH?

    12.85 ± 0.02

    Classify CsOH as a type of acid or base.

    <p>strong base</p> Signup and view all the answers

    Give the conjugate base of H3PO4.

    <p>H2PO4-</p> Signup and view all the answers

    Which of the following acids has the strongest conjugate base?

    <p>NH3</p> Signup and view all the answers

    Use a table of Ka or Kb values to determine whether Kc for the reaction OH- + CH3OH ⇌ H2O + CH3O- is less than, equal to or greater than 1.

    <p>Kc &lt; 1</p> Signup and view all the answers

    Consider the reaction H3PO4(aq) + HSO4- ⇌ H2PO4-(aq) + H2SO4(aq). Determine the size of Kc.

    <p>Kc &lt; 1</p> Signup and view all the answers

    Calculate the pH of a 0.20 M solution of aniline (C6H5NH2, Kb = 3.8 x 10-10).

    <p>8.94</p> Signup and view all the answers

    Calculate the pH of a 0.400 M solution of propanoic acid, for which the Ka value is 1.30 x 10-5.

    <p>2.64</p> Signup and view all the answers

    Is an aqueous solution of NH4Cl acidic, basic or neutral?

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

    What is the pH of 0.354 M trimethylammonium iodide, (CH3)3NHI?

    <p>5.13 ± 0.02</p> Signup and view all the answers

    Calculate the pH of a 0.50 M solution of sodium acetate (NaCH3COO).

    <p>9.26</p> Signup and view all the answers

    Use VSEPR theory to predict the molecular geometry of the bromate ion, BrO3-.

    <p>Trigonal-pyramidal</p> Signup and view all the answers

    Which of the following is not a strong acid in aqueous solution?

    <p>H2SO3</p> Signup and view all the answers

    What is the pH of a 0.284 M solution of HBr?

    <p>0.55 ± 0.02</p> Signup and view all the answers

    Classify H2Se as a type of acid or base.

    <p>Weak acid</p> Signup and view all the answers

    Match each substance with the correct designation for the reaction equation H2O + HS- ⇌ OH- + H2S.

    <p>H2S = B HS- = A OH- = C H2O = D</p> Signup and view all the answers

    Which of the following acids has the weakest conjugate base?

    <p>Iodic acid, Ka = 1.7 x 10-1</p> Signup and view all the answers

    Use a table of Ka or Kb values to determine whether Kc for the reaction NH4+ + HCO3- ⇌ H2CO3 + NH3 is less than, equal to or greater than 1.

    <p>Kc &lt; 1</p> Signup and view all the answers

    Consider the reaction H3SbO4(aq) + HTeO4- ⇌ H2SbO4-(aq) + H2TeO4(aq). Determine the size of Kc.

    <p>Kc &lt; 1</p> Signup and view all the answers

    Calculate the pH of a 0.50 M solution of ammonia (NH3, Kb = 1.8 x 10-5).

    <p>11.48</p> Signup and view all the answers

    Calculate the pH of a 0.100 M solution of lactic acid, for which the Ka value is 1.40 x 10-4.

    <p>2.43</p> Signup and view all the answers

    Is an aqueous solution of NaCN acidic, basic or neutral?

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

    What is the pH of 0.58 M ethylammonium iodide, C2H5NH3I?

    <p>5.43 ± 0.02</p> Signup and view all the answers

    Calculate the pH of a 0.10 M solution of sodium benzoate (NaC6H5COO).

    <p>8.59</p> Signup and view all the answers

    Use VSEPR theory to predict the electron-pair arrangement and molecular geometry of tetrahydroborate ion, BH4-.

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

    Which of the following is not a strong acid in aqueous solution?

    <p>H2SO3</p> Signup and view all the answers

    What is the pH of a 0.061 M solution of NaOH?

    <p>12.79 ± 0.02</p> Signup and view all the answers

    Classify H2TeO4 as a type of acid or base.

    <p>Weak acid</p> Signup and view all the answers

    Give the conjugate base of HPO32-.

    <p>PO33-</p> Signup and view all the answers

    Which of the following acids has the weakest conjugate base?

    <p>Chloroacetic acid, Ka = 1.4 x 10-3</p> Signup and view all the answers

    Use a table of Ka or Kb values to determine whether Kc for the reaction OH- + CH3OH ⇌ H2O + CH3O- is less than, equal to or greater than 1.

    <p>Kc &lt; 1</p> Signup and view all the answers

    Consider the reaction HOCl(aq) + ClO3-(aq) ⇌ OCl-(aq) + HClO3(aq). Determine the size of Kc.

    <p>Kc &lt; 1</p> Signup and view all the answers

    Calculate the pH of a 0.40 M solution of aniline (C6H5NH2, Kb = 3.8 x 10-10).

    <p>9.09</p> Signup and view all the answers

    Calculate the pH of a 0.100 M solution of benzoic acid, for which the Ka value is 6.50 x 10-5.

    <p>2.59</p> Signup and view all the answers

    Is an aqueous solution of CuCl2 acidic, basic or neutral?

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

    What is the pH of 0.51 M diethylammonium chloride, (C2H5)2NH2Cl?

    <p>5.57 ± 0.02</p> Signup and view all the answers

    Calculate the pH of a 0.20 M solution of sodium formate (NaHCOO).

    <p>8.52</p> Signup and view all the answers

    Study Notes

    VSEPR Theory & Molecular Geometry

    • Ozone (O3) exhibits tetrahedral electron-pair arrangement with a bent molecular geometry.
    • Bromate ion (BrO3-) has a trigonal-pyramidal molecular geometry according to VSEPR theory.
    • Tetrahydroborate ion (BH4-) shows a tetrahedral electron-pair arrangement and molecular geometry.

    Acids and Bases

    • HClO2 is identified as a weak acid in aqueous solution, unlike the other strong acids listed (HI, HBr, HCl, HNO3).
    • The conjugate base of H3PO4 is H2PO4-.
    • The strongest conjugate base among the given options is NH3.
    • An aqueous solution of NH4Cl is classified as acidic (A), while NaCN and KCN are classified as basic (B).

    pH Calculations

    • The pH of a 0.07 M KOH solution is approximately 12.85.
    • For a 0.20 M solution of aniline (C6H5NH2), the pH is calculated to be 8.94.
    • A 0.400 M solution of propanoic acid (Ka = 1.30 x 10-5) results in a pH of 2.64.
    • The pH of a 0.061 M NaOH solution is around 12.79.
    • Calculate the pH of a 0.100 M benzoic acid solution (Ka = 6.50 x 10-5); the result is 2.59.

    Equilibrium and Reaction Constants

    • For the reaction OH- + CH3OH ⇌ H2O + CH3O-, the equilibrium constant (Kc) is less than 1.
    • For H3PO4(aq) + HSO4-(aq) ⇌ H2PO4-(aq) + H2SO4(aq), Kc is also less than 1.
    • In the reaction NH4+ + HCO3- ⇌ H2CO3 + NH3, Kc is less than 1, indicating the reactants are favored.
    • The equilibrium constant (Kc) for HOCl(aq) + ClO3-(aq) ⇌ OCl-(aq) + HClO3(aq) is less than 1.

    Weak Acids and Bases

    • Weak acids in the given choices include H2Se and H2SO3.
    • The weakest conjugate base corresponds to H2Te and Iodic acid (Ka = 1.7 x 10-1) has the weakest conjugate base.
    • An aqueous solution of diethylamine (C2H5)2NH results in a pH of approximately 5.54.

    Summary of Acid Strength

    • The selection of stronger acids from pairs: HI over HBr, H2SeO3 over H3AsO3, and HNO3 over HNO2.
    • Classifications for acids: H2TeO4 is a weak acid, and H2S is also classified as a weak acid.

    Other Key Points

    • Conjugate bases include HS- for H2S, PO33- for HPO32-, and relevant calculations yield pH results for sodium formate (8.52) and related compounds.
    • The pH of ethylammonium iodide (C2H5NH3I) is 5.13, indicating a mildly acidic solution.
    • Kb values for various compounds play a crucial role in assessing the basicity and corresponding pH of their solutions.

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    Description

    Test your understanding of VSEPR theory by predicting the electron-pair arrangement and molecular geometry for ozone and other related molecules. This quiz will challenge your knowledge about molecular shapes and electron configurations.

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