Determine the molar solubility for Cr(OH); (Ksp = 6.3 × 10-31") in an aqueous solution that has a pH of 11.90 at 25 °C. PREV 3 NEXT Based on your ICE table, set up the expression for Ksp in order to determine the unknown. Do not combine or simplify terms. Ksp = 6.3 × 1031 [x] %3D [3x]°
Determine the molar solubility for Cr(OH); (Ksp = 6.3 × 10-31") in an aqueous solution that has a pH of 11.90 at 25 °C. PREV 3 NEXT Based on your ICE table, set up the expression for Ksp in order to determine the unknown. Do not combine or simplify terms. Ksp = 6.3 × 1031 [x] %3D [3x]°
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Please help me fix the ICE table
![### Molar Solubility of Cr(OH)₃
**Objective:**
Determine the molar solubility for Cr(OH)₃ (Ksp = 6.3 x 10⁻³¹) in an aqueous solution with a pH of 11.90 at 25 °C.
---
**Instructions:**
Based on your ICE table, set up the expression for Ksp to determine the unknown. Do not combine or simplify terms.
**Expression:**
\[ K_{sp} = [x][3x]^3 = 6.3 \times 10^{-31} \]
---
**Options:**
Below are the possible expressions or values you might use when setting up your expression:
- [0]
- [11.90]
- [11.90]³
- [1.3 × 10⁻¹²]
- [7.9 × 10⁻³]
- [7.9 × 10⁻³]³
- [x]
- [3x]
- [3x]³
- [11.90 + x]
- [11.90 - 3x]
- [1.3 × 10⁻¹² + x]
- [11.90 + 3x]³
- [1.3 × 10⁻¹² - 3x]³
- [7.9 × 10⁻³ + 3x]³
---
**Reset:**
If needed, you can reset your entries and start over by selecting the reset option.
---
By setting up the correct solubility expression using these inputs, you can solve for the unknown molar concentration of Cr(OH)₃ in the solution.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Faeef920a-b7fc-42c4-a405-16f92aebf3b1%2Ff2929843-3c50-42da-b528-6ea9e2961c3a%2F70l6zn3_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Molar Solubility of Cr(OH)₃
**Objective:**
Determine the molar solubility for Cr(OH)₃ (Ksp = 6.3 x 10⁻³¹) in an aqueous solution with a pH of 11.90 at 25 °C.
---
**Instructions:**
Based on your ICE table, set up the expression for Ksp to determine the unknown. Do not combine or simplify terms.
**Expression:**
\[ K_{sp} = [x][3x]^3 = 6.3 \times 10^{-31} \]
---
**Options:**
Below are the possible expressions or values you might use when setting up your expression:
- [0]
- [11.90]
- [11.90]³
- [1.3 × 10⁻¹²]
- [7.9 × 10⁻³]
- [7.9 × 10⁻³]³
- [x]
- [3x]
- [3x]³
- [11.90 + x]
- [11.90 - 3x]
- [1.3 × 10⁻¹² + x]
- [11.90 + 3x]³
- [1.3 × 10⁻¹² - 3x]³
- [7.9 × 10⁻³ + 3x]³
---
**Reset:**
If needed, you can reset your entries and start over by selecting the reset option.
---
By setting up the correct solubility expression using these inputs, you can solve for the unknown molar concentration of Cr(OH)₃ in the solution.
![### Determining Molar Solubility of Cr(OH)₃
In this exercise, we aim to determine the molar solubility of Chromium(III) hydroxide, Cr(OH)₃, given a solubility product constant (Ksp) of \(6.3 \times 10^{-31}\) at 25 °C in an aqueous solution with a pH of 11.90.
#### ICE Table Setup
**ICE Table Components:**
- **Cr(OH)₃ (s) ⇌ Cr³⁺ (aq) + 3 OH⁻ (aq)**
1. **Initial Concentrations (Molarity, M):**
- Cr(OH)₃ (solid): Not applicable.
- Cr³⁺: 0 M
- OH⁻: 0 M
2. **Change in Concentrations (M):**
- Cr(OH)₃: Not applicable
- Cr³⁺: +x M
- OH⁻: +3x M
3. **Equilibrium Concentrations (M):**
- Cr(OH)₃: Not applicable
- Cr³⁺: x M
- OH⁻: 3x M
#### Exploring pH and Hydroxide Ion Concentration
- Given pH: 11.90
- Calculating pOH: \(14 - 11.90 = 2.10\)
- Hydroxide ion concentration, [OH⁻]: \(10^{-2.10}\)
#### Selection Area
1. **Variable Value Selections:**
- Cr³⁺ concentration: 1.3 × 10⁻¹² M
- OH⁻ concentration options include values such as \(7.9 \times 10^{-3}\) M and adjustments for \(3x\) relationship, etc.
By inputting these values and calculations appropriately, you will determine the molar solubility of Cr(OH)₃ using the ICE table and correlation with Ksp.
**Note:** The diagram offers options to reset and assemble different concentrations to solidify conceptual understanding of how changes in pH and concentration affect solubility equilibrium.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Faeef920a-b7fc-42c4-a405-16f92aebf3b1%2Ff2929843-3c50-42da-b528-6ea9e2961c3a%2Funfs3n_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Determining Molar Solubility of Cr(OH)₃
In this exercise, we aim to determine the molar solubility of Chromium(III) hydroxide, Cr(OH)₃, given a solubility product constant (Ksp) of \(6.3 \times 10^{-31}\) at 25 °C in an aqueous solution with a pH of 11.90.
#### ICE Table Setup
**ICE Table Components:**
- **Cr(OH)₃ (s) ⇌ Cr³⁺ (aq) + 3 OH⁻ (aq)**
1. **Initial Concentrations (Molarity, M):**
- Cr(OH)₃ (solid): Not applicable.
- Cr³⁺: 0 M
- OH⁻: 0 M
2. **Change in Concentrations (M):**
- Cr(OH)₃: Not applicable
- Cr³⁺: +x M
- OH⁻: +3x M
3. **Equilibrium Concentrations (M):**
- Cr(OH)₃: Not applicable
- Cr³⁺: x M
- OH⁻: 3x M
#### Exploring pH and Hydroxide Ion Concentration
- Given pH: 11.90
- Calculating pOH: \(14 - 11.90 = 2.10\)
- Hydroxide ion concentration, [OH⁻]: \(10^{-2.10}\)
#### Selection Area
1. **Variable Value Selections:**
- Cr³⁺ concentration: 1.3 × 10⁻¹² M
- OH⁻ concentration options include values such as \(7.9 \times 10^{-3}\) M and adjustments for \(3x\) relationship, etc.
By inputting these values and calculations appropriately, you will determine the molar solubility of Cr(OH)₃ using the ICE table and correlation with Ksp.
**Note:** The diagram offers options to reset and assemble different concentrations to solidify conceptual understanding of how changes in pH and concentration affect solubility equilibrium.
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