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A 0.140 mole quantity of NiCl, is added to a liter of 1.20 M NH, solution. What is the concentration of Ni2 + ions at equilibrium? Assume the formation constant of Ni(NH,)+ is 5.5 × 108. -10 9.4 x10¬1 M Incerres

A 0.140 mole quantity of NiCl, is added to a liter of 1.20 M NH, solution. What is the concentration of Ni2 + ions at equilibrium? Assume the formation constant of Ni(NH,)+ is 5.5 × 108. -10 9.4 x10¬1 M Incerres

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
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**Problem Statement:** A 0.140 mole quantity of NiCl₂ is added to a liter of 1.20 M NH₃ solution. What is the concentration of Ni²⁺ ions at equilibrium? Assume the formation constant of Ni(NH₃)₆²⁺ is 5.5 × 10⁸. **Provided Answer:** 9.4 × 10⁻¹⁰ M **Feedback:** Incorrect --- This exercise involves determining the equilibrium concentration of nickel(II) ions in a solution where nickel chloride is mixed with an ammonia solution. The provided answer is marked as incorrect, indicating a review of calculations related to the formation constant of the complex ion is necessary for accuracy.
Transcribed Image Text:**Problem Statement:** A 0.140 mole quantity of NiCl₂ is added to a liter of 1.20 M NH₃ solution. What is the concentration of Ni²⁺ ions at equilibrium? Assume the formation constant of Ni(NH₃)₆²⁺ is 5.5 × 10⁸. **Provided Answer:** 9.4 × 10⁻¹⁰ M **Feedback:** Incorrect --- This exercise involves determining the equilibrium concentration of nickel(II) ions in a solution where nickel chloride is mixed with an ammonia solution. The provided answer is marked as incorrect, indicating a review of calculations related to the formation constant of the complex ion is necessary for accuracy.
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