Chemistry Chapter on Solubility and Electrolytes
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Questions and Answers

Which of the following compounds is classified as soluble in water?

  • Ba(NO3)2 (correct)
  • CaCrO4
  • AgI
  • Mg(OH)2

    • What characterizes a strong electrolyte?

  • It contains only molecular compounds.
  • It partially ionizes in solution.
  • It does not produce ions in solution.
  • It completely dissociates into ions. (correct)

    • What is the primary factor that affects the electrical conductivity of an electrolyte solution?

  • Volume of solvent used.
  • Total concentration of the electrolyte. (correct)
  • The color of the solution.
  • Temperature of the solution.

    • What process describes the separation of ionic compounds into ions when dissolved?

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

    Which of the following would be classified as a nonelectrolyte?

    <p>CH3OH</p> Signup and view all the answers

    How would you classify Mg(OH)2 in terms of solubility?

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

    When Ba(NO3)2 is dissolved in water, what are the expected ions in solution?

    <p>Ba2+ and NO3-</p> Signup and view all the answers

    In the context of an aqueous solution, what is meant by stoichiometric calculations?

    <p>Calculating concentrations of ions based on total moles.</p> Signup and view all the answers

    In a redox reaction, which statement is true regarding the transfer of electrons?

    <p>One species loses electrons while another species gains electrons.</p> Signup and view all the answers

    Which species acts as the reducing agent in the reaction of zinc with HCl represented by Zn(s) + H+(aq) → Zn2+(aq) + H2(g)?

    <p>Zinc metal</p> Signup and view all the answers

    What does the abbreviation OIL stand for in the context of redox reactions?

    <p>Oxidation Is Loss</p> Signup and view all the answers

    If zinc is oxidized to Zn2+, what half-equation represents this process?

    <p>Zn(s) → Zn2+(aq) + 2e</p> Signup and view all the answers

    In the reaction 2Mg(s) + O2(g) → 2MgO(s), which statement describes magnesium?

    <p>It is oxidized by losing electrons.</p> Signup and view all the answers

    What occurs during the reduction half-reaction involving H+ ions according to the provided equations?

    <p>H+ ions gain electrons to form H2 molecules.</p> Signup and view all the answers

    Which of the following best describes the relationship between oxidation and reduction?

    <p>Both processes must occur simultaneously in a reaction.</p> Signup and view all the answers

    What is the role of an oxidizing agent in a redox reaction?

    <p>It gains electrons and gets reduced.</p> Signup and view all the answers

    What is a half-reaction?

    <p>A reaction that only shows one of either reduction or oxidation.</p> Signup and view all the answers

    In the reaction Ag+ (aq) + Cu(s) → Ag(s) + Cu2+ (aq), which species is reduced?

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

    Which of the following best describes how to balance charges in half-reactions?

    <p>Add electrons to the more positive side.</p> Signup and view all the answers

    Which half-reaction is correctly balanced for both mass and charge: Sn → Sn2+?

    <p>Sn + 2e- → Sn2+</p> Signup and view all the answers

    What is the oxidation state of chlorine in the half-reaction Cl2 → Cl-?

    <p>-1</p> Signup and view all the answers

    When balancing half-reactions in acidic solution, which species is NOT typically involved?

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

    Which of the following represents a correct balanced half-reaction for the reduction of MnO4- to Mn2+ in acid?

    <p>MnO4- + 8H+ + 5e- → Mn2+ + 4H2O</p> Signup and view all the answers

    How does the oxidation state of copper change in the half-reaction Cu → Cu2+?

    <p>It decreases from 0 to +2.</p> Signup and view all the answers

    What is the last step in balancing a half-reaction?

    <p>Adding electrons to balance charge</p> Signup and view all the answers

    In a basic solution, which species is primarily used to balance hydrogen?

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

    When balancing the redox reaction PbO2(s) to PbO(s), what is the first step?

    <p>Balance the atom being reduced/oxidized</p> Signup and view all the answers

    Why is adding electrons to the more positive side important in a half-reaction?

    <p>To achieve charge balance</p> Signup and view all the answers

    What must be done to the half-reaction when converting all H+ to H2O?

    <p>Add hydroxide ions (OH-) to both sides</p> Signup and view all the answers

    What type of ions are primarily available for balancing reactions in basic solutions?

    <p>H2O, OH-, and e-</p> Signup and view all the answers

    During the balancing process, when should water molecules be added?

    <p>When oxygen needs to be balanced</p> Signup and view all the answers

    What is the purpose of canceling duplicate molecules or ions in a balanced equation?

    <p>To simplify the equation</p> Signup and view all the answers

    What is the oxidation half-equation for the reaction provided?

    <p>SO32-(aq) → SO42-(aq)</p> Signup and view all the answers

    Which species is being reduced in the half-equation?

    <p>MnO4-(aq)</p> Signup and view all the answers

    How many electrons are needed to balance the reduction half-equation?

    <p>5</p> Signup and view all the answers

    What is the final simplified overall redox equation?

    <p>5SO32-(aq) + 2MnO4-(aq) + 6H+(aq) → 5SO42-(aq) + 2Mn2+(aq) + 3H2O(l)</p> Signup and view all the answers

    What is the purpose of adding H2O in the balancing process?

    <p>To balance hydrogen and oxygen atoms</p> Signup and view all the answers

    Which step involves ensuring that the charges on both sides of each half-equation are equal?

    <p>Balance in terms of electric charge</p> Signup and view all the answers

    In the complete reaction, what happens to the H+ ions?

    <p>They are eliminated completely.</p> Signup and view all the answers

    What is the first step in balancing the redox reaction?

    <p>Identify oxidation and reduction</p> Signup and view all the answers

    Study Notes

    Solubility Rules

    • Phosphates (PO43-), carbonates (CO32-) and chromates (CrO42-) are insoluble, except for those of alkali metals and ammonium salts.

    Electrolytes

    • Electrolyte: substance that dissolves in water to produce a solution that conducts electricity; contains ions.
    • Nonelectrolyte: substance that dissolves in water to produce a solution that does not conduct electricity; does not contain ions.

    Strong and Weak Electrolytes

    • Dissociation: ionic compounds separate into constituent ions when dissolved in solution.
    • Ionization: molecular compounds form/generate ions when dissolved in solution.
    • Strong Electrolytes: Undergo complete dissociation/ionization.
    • Weak Electrolytes: Partially ionized in solution.

    Stoichiometry of Aqueous Reactions

    • When making stoichiometric calculations for aqueous reactions, one must know:
      • The nature of the reacting species and the product — net ionic equation.
      • The amount of the chemical species present — concentration, e.g. Molarity.

    Oxidation-Reduction Reactions

    • Oxidation-reduction reactions (redox reactions) involve the transfer of electrons between two species.
    • Oxidation is the loss of electrons.
    • Reduction is the gain of electrons.
    • Oxidizing agent: gains electrons and gets reduced.
    • Reducing agent: loses electrons and gets oxidized.
    • Oxidation and reduction always occur together in the same reaction.

    Half Reactions

    • A half-reaction shows reduction or oxidation, but not both.
    • To identify half-reactions, oxidation numbers of the atoms involved must be determined.

    Balancing Half Reactions

    • A half-reaction is balanced when both the atoms and the total charge are equal on both sides of the equation.
    • Add electrons to the more positive side to balance the charge.

    Balancing Half-Reactions in Acid Solution

    • Available chemical species in acidic solution include H2O, H+, and e-.
    • Balance the atom being reducedor oxidized
    • Balance O atoms by adding H2O molecules
    • Balance H atoms by adding H+ ions
    • Balance the total charge by adding electrons to the more positive side.

    Balancing Half-Reactions in Basic Solution

    • Available chemical species in basic solution include H2O, OH-, and e-.
    • Balance the atom being reduced or oxidized.
    • Balance O atoms by adding H2O molecules.
    • Balance H atoms by adding H+ ions.
    • Balance the total charge by adding electrons to the more positive side.
    • Convert all H+ to H2O by adding OH- ions to both sides and canceling duplicate molecules or ions.

    Balancing Redox Reactions

    • Split the equation into half-equations, one for oxidation and one reduction.
    • Balance each half-equation for atoms and charge.
    • Combine the half-equations to get the overall equation.
    • Multiply the different half-equations by the appropriate factors to ensure electron loss and gain are balanced.
    • Simplify the final equation by canceling species that occur on both sides and reducing coefficients.
    • Make sure that electrons do not appear in the final equation.

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    Test your knowledge on solubility rules, electrolytes, and stoichiometry of aqueous reactions. This quiz covers important concepts such as strong and weak electrolytes as well as the nature of ionic compounds in solutions. Prepare to evaluate your understanding of these key chemistry principles!

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