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The final part asks for molar solubility.

The final part asks for molar solubility.

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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The final part asks for molar solubility.

**Title: Calculating Molar Solubility of Lead Iodide (PbI₂)** **Objective:** Determine the molar solubility for Lead Iodide (PbI₂) with a given solubility product constant (Ksp = 7.9 × 10⁻⁹). **Instructions:** Use the ICE (Initial, Change, Equilibrium) table to solve for the unknown molar concentrations at equilibrium. **Procedure:** 1. **Balanced Equation:** PbI₂(s) ⇌ Pb²⁺(aq) + 2 I⁻(aq) 2. **ICE Table Setup:** | | PbI₂(s) | Pb²⁺(aq) | 2 I⁻(aq) | |----------------|---------|----------|-----------| | Initial (M) | | | | | Change (M) | | | | | Equilibrium (M)| | | | **Steps:** - Start by identifying initial concentrations. For Pb²⁺ and I⁻, initial values are usually zero in pure water. - Apply changes to concentrations based on the stoichiometry of the dissolution reaction. - Calculate equilibrium concentrations and use them to solve for solubility using the Ksp expression. **Interactive Controls:** - Use the buttons to input changes and calculate equilibrium concentrations. - Reset any changes using the provided reset button if necessary. **Conclusion:** This exercise helps in understanding the relationship between solubility product constants and molar solubility, using the systematic approach of an ICE table. By completing this task, you will appreciate the quantitative analysis of equilibrium in chemical reactions.
Transcribed Image Text:**Title: Calculating Molar Solubility of Lead Iodide (PbI₂)** **Objective:** Determine the molar solubility for Lead Iodide (PbI₂) with a given solubility product constant (Ksp = 7.9 × 10⁻⁹). **Instructions:** Use the ICE (Initial, Change, Equilibrium) table to solve for the unknown molar concentrations at equilibrium. **Procedure:** 1. **Balanced Equation:** PbI₂(s) ⇌ Pb²⁺(aq) + 2 I⁻(aq) 2. **ICE Table Setup:** | | PbI₂(s) | Pb²⁺(aq) | 2 I⁻(aq) | |----------------|---------|----------|-----------| | Initial (M) | | | | | Change (M) | | | | | Equilibrium (M)| | | | **Steps:** - Start by identifying initial concentrations. For Pb²⁺ and I⁻, initial values are usually zero in pure water. - Apply changes to concentrations based on the stoichiometry of the dissolution reaction. - Calculate equilibrium concentrations and use them to solve for solubility using the Ksp expression. **Interactive Controls:** - Use the buttons to input changes and calculate equilibrium concentrations. - Reset any changes using the provided reset button if necessary. **Conclusion:** This exercise helps in understanding the relationship between solubility product constants and molar solubility, using the systematic approach of an ICE table. By completing this task, you will appreciate the quantitative analysis of equilibrium in chemical reactions.
**Question 7 of 30** **Determine the molar solubility for PbI₂ (Ksp = 7.9 × 10⁻⁹).** Based on your ICE table, set up the expression for Ksp in order to determine the unknown. Do not combine or simplify terms. \[ K_{sp} = \_\_\_\_ = 7.9 \times 10^{-9} \] **Available Expressions:** - \([0]\) - \([7.9 \times 10^{-1}]\) - \([1.58 \times 10^{-7}]\) - \([7.9 \times 10^{-7}]\) - \([1.58 \times 10^{-4}]\) - \([x]\) - \([x]^2\) - \([2x]\) - \([2x]^2\) - \([7.9 \times 10^{-7} + x]\) - \([7.9 \times 10^{-7} - x]\) - \([1.58 \times 10^{-4} + x]\) - \([1.58 \times 10^{-4} - x]\) - \([7.9 \times 10^{-7} + 2x]\) - \([7.9 \times 10^{-7} - 2x]\) - \([1.58 \times 10^{-4} + 2x]\) - \([1.58 \times 10^{-4} - 2x]\) **Reset Button:** Allows clearing the current selection to start afresh. To answer, the user must select the appropriate expressions to fill in the blank for the \( K_{sp} \) equation.
Transcribed Image Text:**Question 7 of 30** **Determine the molar solubility for PbI₂ (Ksp = 7.9 × 10⁻⁹).** Based on your ICE table, set up the expression for Ksp in order to determine the unknown. Do not combine or simplify terms. \[ K_{sp} = \_\_\_\_ = 7.9 \times 10^{-9} \] **Available Expressions:** - \([0]\) - \([7.9 \times 10^{-1}]\) - \([1.58 \times 10^{-7}]\) - \([7.9 \times 10^{-7}]\) - \([1.58 \times 10^{-4}]\) - \([x]\) - \([x]^2\) - \([2x]\) - \([2x]^2\) - \([7.9 \times 10^{-7} + x]\) - \([7.9 \times 10^{-7} - x]\) - \([1.58 \times 10^{-4} + x]\) - \([1.58 \times 10^{-4} - x]\) - \([7.9 \times 10^{-7} + 2x]\) - \([7.9 \times 10^{-7} - 2x]\) - \([1.58 \times 10^{-4} + 2x]\) - \([1.58 \times 10^{-4} - 2x]\) **Reset Button:** Allows clearing the current selection to start afresh. To answer, the user must select the appropriate expressions to fill in the blank for the \( K_{sp} \) equation.
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