Calculation 1: Initial concentration of hexaaquacobalt(II) ion: 0.022M Calculation 2: Initial concentration of Chloride ion: 5.037M Calculation 3: At 293k CoCI4^-4 eq is 9.06x10^-5M| At 315k CoCI4^-4 eq is 3.00x10^-4M At 326k CoCl4^-4 eq is 5.14x10^-4M At 335 CoCI4^-4 eq is 6.88x10^-4M At 346 CoCI4^-4 eq is 1.01x10^-3M 4. [Co(H20)62*]eq and [Cl-]eq - equilibrium concentrations Construct an 1CE table using the initial concentrations hexaaquacobalt(II) and chloride ions from Calculations #1 and # 2, and final (equilibrium) concentration of the tetrachlorocobaltate(Il) ion from Calculation #3. Use the table to determine the final equilibrium concentrations of the hexaaquacobalt(II) and chloride ions.
Calculation 1: Initial concentration of hexaaquacobalt(II) ion: 0.022M Calculation 2: Initial concentration of Chloride ion: 5.037M Calculation 3: At 293k CoCI4^-4 eq is 9.06x10^-5M| At 315k CoCI4^-4 eq is 3.00x10^-4M At 326k CoCl4^-4 eq is 5.14x10^-4M At 335 CoCI4^-4 eq is 6.88x10^-4M At 346 CoCI4^-4 eq is 1.01x10^-3M 4. [Co(H20)62*]eq and [Cl-]eq - equilibrium concentrations Construct an 1CE table using the initial concentrations hexaaquacobalt(II) and chloride ions from Calculations #1 and # 2, and final (equilibrium) concentration of the tetrachlorocobaltate(Il) ion from Calculation #3. Use the table to determine the final equilibrium concentrations of the hexaaquacobalt(II) and chloride ions.
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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![**Educational Content: Concentration and Equilibrium Calculations in Chemistry**
**Calculation 1:**
Initial concentration of hexaquacobalt(II) ion: 0.022 M
**Calculation 2:**
Initial concentration of chloride ion: 5.037 M
**Calculation 3:**
- At 293 K, CoCl₄²⁻ equilibrium concentration is 9.06 × 10⁻⁵ M
- At 315 K, CoCl₄²⁻ equilibrium concentration is 3.00 × 10⁻⁴ M
- At 326 K, CoCl₄²⁻ equilibrium concentration is 5.14 × 10⁻⁴ M
- At 335 K, CoCl₄²⁻ equilibrium concentration is 6.88 × 10⁻⁴ M
- At 346 K, CoCl₄²⁻ equilibrium concentration is 1.01 × 10⁻³ M
**Instructions for Calculation:**
4. **[Co(H₂O)₆]²⁺ and [Cl⁻] - Equilibrium Concentrations**
Construct an ICE (Initial, Change, Equilibrium) table using the initial concentrations of hexaquacobalt(II) and chloride ions from Calculations #1 and #2, and the final (equilibrium) concentration of the tetrachlorocobaltate(II) ion from Calculation #3. Use the table to determine the final equilibrium concentrations of the hexaquacobalt(II) and chloride ions.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ffee03257-cc52-4b96-ab5f-7658a04cd8e4%2F910db584-53cf-4e3f-ba03-b3ad75a4562a%2F9na4zqs_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Educational Content: Concentration and Equilibrium Calculations in Chemistry**
**Calculation 1:**
Initial concentration of hexaquacobalt(II) ion: 0.022 M
**Calculation 2:**
Initial concentration of chloride ion: 5.037 M
**Calculation 3:**
- At 293 K, CoCl₄²⁻ equilibrium concentration is 9.06 × 10⁻⁵ M
- At 315 K, CoCl₄²⁻ equilibrium concentration is 3.00 × 10⁻⁴ M
- At 326 K, CoCl₄²⁻ equilibrium concentration is 5.14 × 10⁻⁴ M
- At 335 K, CoCl₄²⁻ equilibrium concentration is 6.88 × 10⁻⁴ M
- At 346 K, CoCl₄²⁻ equilibrium concentration is 1.01 × 10⁻³ M
**Instructions for Calculation:**
4. **[Co(H₂O)₆]²⁺ and [Cl⁻] - Equilibrium Concentrations**
Construct an ICE (Initial, Change, Equilibrium) table using the initial concentrations of hexaquacobalt(II) and chloride ions from Calculations #1 and #2, and the final (equilibrium) concentration of the tetrachlorocobaltate(II) ion from Calculation #3. Use the table to determine the final equilibrium concentrations of the hexaquacobalt(II) and chloride ions.
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