Classify these ionic compounds as soluble or insoluble in water

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  1. Classify these ionic compounds as soluble or insoluble in water:
    a. Na2503
    b. PbSO4
    c. (NH4)25
  2. Predict the precipitate that forms when solutions of BaCl2 and K2SO4 are mixed.
    a. Write the balanced molecular formula (with states of matter in parenthesis):
    b. Write the complete ionic equation:
    c. Write the net ionic equation:
  3. Classify these dissolved substances as a strong electrolyte, weak electrolyte, or nonelectrolyte.
    a. CaCl2
    b. HNO3
    с. KOH
    d. C2H5OH (ethanol)
    e. HCOOH (formic acid)
  4. For the reaction between aqueous solutions of acetic acid (CH3COOH) and barium hydroxide:
    Write the balanced molecular equation:
    b. Write the complete ionic equation:
    c. Write the net ionic equation:
  5. Identify each of the following as oxidation or reduction:
    a. Sn à 5n4++40-
    b. Fe3++1 e-à Fe+2
    c. C12+20-20-
  6. In light-sensitive sunglasses, light initiates an oxidation-reduction reaction that causes them to darken
    AgCl-à Ag (s) CI (s)
    a. Which reactant is oxidized?
    b. Which reactant is reduced?
  7. Assign the oxidation numbers to the elements in each of the following:
    a. N2
    b. PC13
    C, NO3-

The Correct Answer and Explanation is :

Let’s break down each of your questions step-by-step.

1. Classification of Ionic Compounds as Soluble or Insoluble in Water:

  • a. Na₂SO₃: Soluble. Sodium (Na⁺) compounds are generally soluble in water.
  • b. PbSO₄: Insoluble. Most sulfate salts are soluble, but lead(II) sulfate is an exception and is insoluble in water.
  • c. (NH₄)₂S: Soluble. Ammonium (NH₄⁺) compounds are typically soluble in water.

2. Precipitation Reaction of BaCl₂ and K₂SO₄:

  • a. Balanced Molecular Formula:
    [ \text{BaCl}_2 (aq) + \text{K}_2\text{SO}_4 (aq) \rightarrow \text{BaSO}_4 (s) + 2 \text{KCl} (aq) ]
  • b. Complete Ionic Equation:
    [ \text{Ba}^{2+} (aq) + 2 \text{Cl}^- (aq) + 2 \text{K}^+ (aq) + \text{SO}_4^{2-} (aq) \rightarrow \text{BaSO}_4 (s) + 2 \text{K}^+ (aq) + 2 \text{Cl}^- (aq) ]
  • c. Net Ionic Equation:
    [ \text{Ba}^{2+} (aq) + \text{SO}_4^{2-} (aq) \rightarrow \text{BaSO}_4 (s) ]

3. Classification of Substances as Electrolytes:

  • a. CaCl₂: Strong Electrolyte. It dissociates completely in water into Ca²⁺ and Cl⁻ ions.
  • b. HNO₃: Strong Electrolyte. Nitric acid is a strong acid and dissociates completely in water.
  • c. KOH: Strong Electrolyte. Potassium hydroxide is a strong base and dissociates completely.
  • d. C₂H₅OH (ethanol): Nonelectrolyte. Ethanol does not dissociate into ions in water.
  • e. HCOOH (formic acid): Weak Electrolyte. Formic acid only partially dissociates in water.

4. Acetic Acid and Barium Hydroxide Reaction:

  • a. Balanced Molecular Equation:
    [ 2 \text{CH₃COOH} (aq) + \text{Ba(OH)}_2 (aq) \rightarrow \text{Ba(CH₃COO)₂} (aq) + 2 \text{H₂O} (l) ]
  • b. Complete Ionic Equation:
    [ 2 \text{CH₃COOH} (aq) + \text{Ba}^{2+} (aq) + 2 \text{OH}^- (aq) \rightarrow \text{Ba}^{2+} (aq) + 2 \text{CH₃COO}^- (aq) + 2 \text{H₂O} (l) ]
  • c. Net Ionic Equation:
    [ 2 \text{CH₃COOH} (aq) + 2 \text{OH}^- (aq) \rightarrow 2 \text{CH₃COO}^- (aq) + 2 \text{H₂O} (l) ]

5. Identify Oxidation or Reduction:

  • a. Sn → Sn⁴⁺ + 4e⁻: Oxidation (loss of electrons).
  • b. Fe³⁺ + 1e⁻ → Fe²⁺: Reduction (gain of electrons).
  • c. Cl₂ → 2Cl⁻: Reduction (gain of electrons).

6. Oxidation-Reduction in Light-Sensitive Sunglasses:

  • a. Oxidized Reactant: AgCl. Silver chloride loses electrons (oxidation) to form metallic silver.
  • b. Reduced Reactant: Cl⁻. The chloride ion gains electrons (reduction) to form chlorine gas.

7. Oxidation Numbers:

  • a. N₂: Each nitrogen atom in molecular nitrogen has an oxidation number of 0.
  • b. PCl₃: Phosphorus (P) has an oxidation number of +3, and chlorine (Cl) has an oxidation number of -1.
  • c. NO₃⁻: The oxidation number of nitrogen (N) in the nitrate ion is +5, and oxygen (O) is -2.

Explanation:

  1. Ionic Solubility: Solubility rules help classify compounds. Group 1 salts (like Na⁺) and ammonium salts are soluble. Lead salts and some sulfates are exceptions.
  2. Precipitation Reactions: When solutions of two ionic compounds mix, the ions may form an insoluble compound (precipitate), following the solubility rules. The complete ionic equation shows all dissolved ions, while the net ionic equation highlights the ions that participate in the reaction.
  3. Electrolytes: Strong electrolytes dissociate completely into ions, weak electrolytes partially dissociate, and nonelectrolytes do not dissociate into ions.
  4. Acid-Base Reaction: Acetic acid reacts with barium hydroxide in a neutralization reaction, forming water and a salt (barium acetate).
  5. Oxidation-Reduction: Oxidation is the loss of electrons, while reduction is the gain of electrons. In reactions, identifying which element undergoes oxidation and which undergoes reduction is crucial for understanding redox processes.

Let me now generate the image for the concept.

Here is the diagram illustrating the precipitation reaction between BaCl₂ and K₂SO₄. It shows the dissociation of ions, the formation of BaSO₄ as a solid precipitate, and includes the complete and net ionic equations. Let me know if you need further clarification or additional details!

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