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1. Classify these ionic compounds as soluble or insoluble in water: a. Na2S03 b. PbS04 c. (NH4)2S

1. Classify these ionic compounds as soluble or insoluble in water: a. Na2S03 b. PbS04 c. (NH4)2S

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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1. Classify these ionic compounds as soluble or insoluble in water: a. Na2SO3 b. PbSO4 c. (NH4)2S 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 parentheses): 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 c. KOH d. C2H5OH (ethanol) e. HCOOH (formic acid) 4. For the reaction between aqueous solutions of acetic acid (CH3COOH) and barium hydroxide: a. 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 ➔ Sn^4+ + 4 e^- b. Fe^3+ + 1 e^- ➔ Fe^2+ c. Cl2 + 2 e^- ➔ 2 Cl^- 6. In light-sensitive sunglasses, light initiates an oxidation-reduction reaction that causes them to darken. Ag^+ + Cl^- ➔ Ag (s) + Cl (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. PCl3 c. NO3^- 8. Write the oxidation and reduction half reactions for the following: 2 Cs (s) + F2 (g) ➔ 2 CsF (aq) 9. Determine the oxidation number of each of the following: a. C in CO2 b. Cl in Cl2O7 c. P in H3PO4 d. Mn in MnO4^2- 10. Determine the oxidizing and reducing agent in each of the following:
Transcribed Image Text:1. Classify these ionic compounds as soluble or insoluble in water: a. Na2SO3 b. PbSO4 c. (NH4)2S 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 parentheses): 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 c. KOH d. C2H5OH (ethanol) e. HCOOH (formic acid) 4. For the reaction between aqueous solutions of acetic acid (CH3COOH) and barium hydroxide: a. 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 ➔ Sn^4+ + 4 e^- b. Fe^3+ + 1 e^- ➔ Fe^2+ c. Cl2 + 2 e^- ➔ 2 Cl^- 6. In light-sensitive sunglasses, light initiates an oxidation-reduction reaction that causes them to darken. Ag^+ + Cl^- ➔ Ag (s) + Cl (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. PCl3 c. NO3^- 8. Write the oxidation and reduction half reactions for the following: 2 Cs (s) + F2 (g) ➔ 2 CsF (aq) 9. Determine the oxidation number of each of the following: a. C in CO2 b. Cl in Cl2O7 c. P in H3PO4 d. Mn in MnO4^2- 10. Determine the oxidizing and reducing agent in each of the following:
**Chemistry Problem Set** This worksheet focuses on various chemistry concepts such as oxidation-reduction reactions, stoichiometry, and thermochemistry. --- **8. Oxidation and Reduction Half Reactions** For the following reaction, identify the oxidation and reduction half reactions: \[ \text{2 Cs (s) + F}_2 \text{(g) } \rightarrow \text{2 CsF (aq)} \] --- **9. Determining Oxidation Numbers** Determine the oxidation number for each of the following elements in their respective compounds: a. C in CO₂ b. Cl in Cl₂O₇ c. P in H₃PO₄ d. Mn in MnO₄²⁻ --- **10. Oxidizing and Reducing Agents** Determine the oxidizing and reducing agent in each of the following reactions: a. \( \text{Zn (s) + 2 HBr (aq)} \rightarrow \text{ZnBr}_2 \text{(aq) + H}_2 \text{(g)} \) b. \( \text{Mn (s) + Pb(NO}_3\text{)}_2 \text{(aq)} \rightarrow \text{Pb (s) + Mn(NO}_3\text{)}_2 \text{(aq)} \) --- **11. Reaction Analysis** For the following reaction: \[ \text{2 Na + 2 H}_2\text{O} \rightarrow \text{2 NaOH + H}_2 \] a. Write the oxidation number for each element in the reaction. b. Write the reduction and oxidation half reactions. c. Identify the reducing and oxidizing agents. --- **12. Hydrogen Gas Production** Calculate the amount of \( \text{H}_2 \) gas produced when 6.25 g of Zn reacts with 20.0 mL of a 1.50 M HCl solution: \[ \text{Zn (s) + 2 HCl (aq)} \rightarrow \text{ZnCl}_2 \text{(aq) + H}_2 \text{(g)} \] --- **13. Oxygen Reaction Energetics** How many grams of \( \text{O}_2 \) react if 1280 kJ was released in the following reaction? \[ \text{CH}_4 +
Transcribed Image Text:**Chemistry Problem Set** This worksheet focuses on various chemistry concepts such as oxidation-reduction reactions, stoichiometry, and thermochemistry. --- **8. Oxidation and Reduction Half Reactions** For the following reaction, identify the oxidation and reduction half reactions: \[ \text{2 Cs (s) + F}_2 \text{(g) } \rightarrow \text{2 CsF (aq)} \] --- **9. Determining Oxidation Numbers** Determine the oxidation number for each of the following elements in their respective compounds: a. C in CO₂ b. Cl in Cl₂O₇ c. P in H₃PO₄ d. Mn in MnO₄²⁻ --- **10. Oxidizing and Reducing Agents** Determine the oxidizing and reducing agent in each of the following reactions: a. \( \text{Zn (s) + 2 HBr (aq)} \rightarrow \text{ZnBr}_2 \text{(aq) + H}_2 \text{(g)} \) b. \( \text{Mn (s) + Pb(NO}_3\text{)}_2 \text{(aq)} \rightarrow \text{Pb (s) + Mn(NO}_3\text{)}_2 \text{(aq)} \) --- **11. Reaction Analysis** For the following reaction: \[ \text{2 Na + 2 H}_2\text{O} \rightarrow \text{2 NaOH + H}_2 \] a. Write the oxidation number for each element in the reaction. b. Write the reduction and oxidation half reactions. c. Identify the reducing and oxidizing agents. --- **12. Hydrogen Gas Production** Calculate the amount of \( \text{H}_2 \) gas produced when 6.25 g of Zn reacts with 20.0 mL of a 1.50 M HCl solution: \[ \text{Zn (s) + 2 HCl (aq)} \rightarrow \text{ZnCl}_2 \text{(aq) + H}_2 \text{(g)} \] --- **13. Oxygen Reaction Energetics** How many grams of \( \text{O}_2 \) react if 1280 kJ was released in the following reaction? \[ \text{CH}_4 +
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