my question is in the screenshot. **Topic: Solubility Product Constant (Ksp) Calculation for Magnesium Cyanide****Text:**The molar solubility of Mg(CN)₂ is \(1.4 \times 10^{-5}\) M at a certain temperature. Determine the value of K\(_{sp}\) for Mg(CN)₂.---**ICE Table Explanation:**The table below illustrates the Initial, Change, and Equilibrium (ICE) concentrations for the dissolution of magnesium cyanide in water:| | Mg(CN)₂(s) | ⇌ | Mg²⁺(aq) | + | 2 CN⁻(aq) ||---------------|------------|---|-------------|----|-------------|| **Initial (M)** | – | | 0 | | 0 || **Change (M)** | – | | \(1.4 \times 10^{-5}\) | | \(2.8 \times 10^{-5}\) || **Equilibrium (M)** | – | | \(1.4 \times 10^{-5}\) | | \(2.8 \times 10^{-5}\) |- **Initial Concentrations:** - Mg²⁺ and CN⁻ ions are initially not present in solution. - **Change in Concentrations:** - As Mg(CN)₂ dissolves, the concentration of Mg²⁺ increases by \(1.4 \times 10^{-5}\) M. - The concentration of CN⁻ ions, due to stoichiometry, increases by \(2 \times (1.4 \times 10^{-5}) = 2.8 \times 10^{-5}\) M.- **Equilibrium Concentrations:** - At equilibrium, the concentration of Mg²⁺ is \(1.4 \times 10^{-5}\) M. - The concentration of CN⁻ is \(2.8 \times 10^{-5}\) M.**Determination of K\(_{sp}\):**To find the \(K_{sp}\), use the expression:\[ K_{sp} = [\text{Mg}^{2+}][\text{CN}^-]^2 \]Substituting at equilibrium:\[ K_{sp} = (1.4 \times ### Question 11 of 11The molar solubility of Mg(CN)₂ is \(1.4 \times 10^{-5}\) M at a certain temperature. Determine the value of \(K_{sp}\) for Mg(CN)₂.---#### Instructions:Based on the setup of your ICE table, construct the expression for \(K_{sp}\) and then evaluate it. Do not combine or simplify terms.\[K_{sp} = \boxed{} \times \boxed{} = 1.1 \times 10^{-14}\]---#### Options for Boxes:[0]\[1.4 \times 10^{-5}\]\[2.8 \times 10^{-5}\]\[(1.4 \times 10^{-5})^2\]\[(2.8 \times 10^{-5})^2\][x]\[2x\]\[x^2\]\[(1.4 \times 10^{-5} + x)\]\[(1.4 \times 10^{-5} - x)\]\[(1.4 \times 10^{-5} + 2x)^2\]\[(2.8 \times 10^{-5} - 2x)^2\]\[(2.8 \times 10^{-5} + x)\]\[2.7 \times 10^{-15}\]\[1.1 \times 10^{-14}\]\[2.2 \times 10^{-14}\]\[3.9 \times 10^{-10}\]\[1.4 \times 10^{-5}\]---#### Reset Button:RESET---This interactive setup allows students to calculate the solubility product constant (\(K_{sp}\)) using given data, building an understanding of how solubility and equilibrium expressions are constructed from an ICE table (Initial, Change, Equilibrium).

Answered: Image /qna-images/answer/6a69a332-6a2d-43b2-b18b-e7962eacbe4e.jpg

Question 11 of 11 The molar solubility of Mg(CN)2 is 1.4 x 10-5 M at a certain temperature. Determine the value of Ksp for Mg(CN)2. PREV 1 2 Based on the set up of your ICE table, construct the expression for Ksp and then evaluate it. Do not combine or simplify terms. Ksp 1.1 x 10-14 %3D

Question 11 of 11 The molar solubility of Mg(CN)2 is 1.4 x 10-5 M at a certain temperature. Determine the value of Ksp for Mg(CN)2. PREV 1 2 Based on the set up of your ICE table, construct the expression for Ksp and then evaluate it. Do not combine or simplify terms. Ksp 1.1 x 10-14 %3D

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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