Determine the value of Ksp for Cu(10), by constructing an ICE table, writing the solubility constant expression, and solving the expression. The molar solubility of Cu(10), is 2.7 x 10³ M at this temperature. Complete Parts 1-2 before submitting your answer. NEXT > Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products at this temperature.. Initial (M) Change (M) Equilibrium (M) 4.00 8.1 x 10³ 0 -2.00 1 1.5 x 10 Cu(10),(s) 2.7 x 10³ -1.00 -1.4 x 10° -2.7 x 10³ -4.00 -7.3 x 10° 5.4 x 10³ 1.4 x 10³ -2.0 x 10° 2 Cu²+ (aq) -5.4 x 10° 7.3 x 10° + 1.00 2.0 x 10* 210, (aq) RESET 2.00 9.0 × 10*
Determine the value of Ksp for Cu(10), by constructing an ICE table, writing the solubility constant expression, and solving the expression. The molar solubility of Cu(10), is 2.7 x 10³ M at this temperature. Complete Parts 1-2 before submitting your answer. NEXT > Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products at this temperature.. Initial (M) Change (M) Equilibrium (M) 4.00 8.1 x 10³ 0 -2.00 1 1.5 x 10 Cu(10),(s) 2.7 x 10³ -1.00 -1.4 x 10° -2.7 x 10³ -4.00 -7.3 x 10° 5.4 x 10³ 1.4 x 10³ -2.0 x 10° 2 Cu²+ (aq) -5.4 x 10° 7.3 x 10° + 1.00 2.0 x 10* 210, (aq) RESET 2.00 9.0 × 10*
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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![**Exercise: Calculating Ksp for Cu(IO₃)₂**
To determine the value of the solubility product constant (Ksp) for Cu(IO₃)₂, perform the following steps:
1. **Construct an ICE Table**: Use the solubility data provided to fill in the Initial, Change, and Equilibrium concentrations for each species.
2. **Write the Solubility Constant Expression**: Formulate based on the dissolution of Cu(IO₃)₂.
3. **Solve the Expression**: Use the equilibrium concentrations to calculate Ksp.
**Data Provided:**
- Molar solubility of Cu(IO₃)₂: 2.7 × 10⁻³ M
**Reaction:**
\[ \text{Cu(IO}_3\text{)}_2(s) \rightleftharpoons \text{Cu}^{2+}(aq) + 2 \text{IO}_3^{-}(aq) \]
**ICE Table:**
| | Cu(IO₃)₂(s) | Cu²⁺(aq) | 2 IO₃⁻(aq) |
|------------------------------|-------------|----------|------------|
| **Initial (M)** | | | |
| **Change (M)** | | | |
| **Equilibrium (M)** | | | |
**Instructions:**
- **Initial Concentration (M)**: Begin with the starting concentrations.
- **Change (M)**: Determine the changes during dissolution.
- **Equilibrium (M)**: Calculate the concentrations at equilibrium.
**Interactive Buttons:**
- Values provided can be used to fill in the tables.
- A **RESET** button is available to clear entries and start again if needed.
**Note:** Ensure your solution satisfies the stoichiometry of the reaction when calculating the changes and equilibrium concentrations.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa91f799b-1b33-41a5-8f4e-af83231854b4%2Fc63fd0d7-e451-4305-9c33-d305d46fea47%2Fumjc15o_processed.png&w=3840&q=75)
Transcribed Image Text:**Exercise: Calculating Ksp for Cu(IO₃)₂**
To determine the value of the solubility product constant (Ksp) for Cu(IO₃)₂, perform the following steps:
1. **Construct an ICE Table**: Use the solubility data provided to fill in the Initial, Change, and Equilibrium concentrations for each species.
2. **Write the Solubility Constant Expression**: Formulate based on the dissolution of Cu(IO₃)₂.
3. **Solve the Expression**: Use the equilibrium concentrations to calculate Ksp.
**Data Provided:**
- Molar solubility of Cu(IO₃)₂: 2.7 × 10⁻³ M
**Reaction:**
\[ \text{Cu(IO}_3\text{)}_2(s) \rightleftharpoons \text{Cu}^{2+}(aq) + 2 \text{IO}_3^{-}(aq) \]
**ICE Table:**
| | Cu(IO₃)₂(s) | Cu²⁺(aq) | 2 IO₃⁻(aq) |
|------------------------------|-------------|----------|------------|
| **Initial (M)** | | | |
| **Change (M)** | | | |
| **Equilibrium (M)** | | | |
**Instructions:**
- **Initial Concentration (M)**: Begin with the starting concentrations.
- **Change (M)**: Determine the changes during dissolution.
- **Equilibrium (M)**: Calculate the concentrations at equilibrium.
**Interactive Buttons:**
- Values provided can be used to fill in the tables.
- A **RESET** button is available to clear entries and start again if needed.
**Note:** Ensure your solution satisfies the stoichiometry of the reaction when calculating the changes and equilibrium concentrations.
![**Title: Determining the Solubility Product Constant (Ksp) for Copper(I) Iodate**
**Objective:**
Learn how to determine the value of the solubility product constant (Ksp) for Cu(IO₃)₂ by constructing an ICE table, formulating the solubility constant expression, and solving that expression using given data.
**Instructions:**
1. **Problem Overview:**
- Determine the Ksp for Cu(IO₃)₂.
- Molar solubility of Cu(IO₃)₂ at this temperature is 2.7 × 10⁻³ M.
- Complete all parts before submitting your answer.
2. **Steps to Follow:**
- **ICE Table Usage:**
1. Identify the dissolution reaction of Cu(IO₃)₂ in water.
2. Write down the initial concentrations, changes, and equilibrium concentrations (ICE) of each component.
- **Construct Solubility Expression:**
- Use the values from the ICE table to form the solubility constant expression.
- Each species in the reaction should be represented by one tile.
- Do not combine terms.
- **Solve for Ksp:**
- Write the expression for Ksp using the provided values.
- Insert the correct values, representing the concentrations at equilibrium.
- Calculate Ksp.
3. **Interactive Component:**
- **Tiles Provided for Use:**
- `[0]`, `[2.7 × 10⁻³]`, `[5.4 × 10⁻³]`, `[2.7 × 10⁻³]²`, `[5.4 × 10⁻³]²`, `[1.4 × 10⁻³]`, `[7.3 × 10⁻⁴]`, `[2.0 × 10⁻⁸]`
- `[9.0 × 10⁻¹]`, `[8.1 × 10⁻³]`, `[1.5 × 10⁻³]`, `[1.6 ×10⁻⁷]`, `[1.4 × 10⁻¹²]`, `[7.3 × 10⁻¹²]`, `2.0 × 10⁸`
- Additional numbers to ensure a precise calculation.
4. **Graph & Diagram Explanation:](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa91f799b-1b33-41a5-8f4e-af83231854b4%2Fc63fd0d7-e451-4305-9c33-d305d46fea47%2Fl05j5ox_processed.png&w=3840&q=75)
Transcribed Image Text:**Title: Determining the Solubility Product Constant (Ksp) for Copper(I) Iodate**
**Objective:**
Learn how to determine the value of the solubility product constant (Ksp) for Cu(IO₃)₂ by constructing an ICE table, formulating the solubility constant expression, and solving that expression using given data.
**Instructions:**
1. **Problem Overview:**
- Determine the Ksp for Cu(IO₃)₂.
- Molar solubility of Cu(IO₃)₂ at this temperature is 2.7 × 10⁻³ M.
- Complete all parts before submitting your answer.
2. **Steps to Follow:**
- **ICE Table Usage:**
1. Identify the dissolution reaction of Cu(IO₃)₂ in water.
2. Write down the initial concentrations, changes, and equilibrium concentrations (ICE) of each component.
- **Construct Solubility Expression:**
- Use the values from the ICE table to form the solubility constant expression.
- Each species in the reaction should be represented by one tile.
- Do not combine terms.
- **Solve for Ksp:**
- Write the expression for Ksp using the provided values.
- Insert the correct values, representing the concentrations at equilibrium.
- Calculate Ksp.
3. **Interactive Component:**
- **Tiles Provided for Use:**
- `[0]`, `[2.7 × 10⁻³]`, `[5.4 × 10⁻³]`, `[2.7 × 10⁻³]²`, `[5.4 × 10⁻³]²`, `[1.4 × 10⁻³]`, `[7.3 × 10⁻⁴]`, `[2.0 × 10⁻⁸]`
- `[9.0 × 10⁻¹]`, `[8.1 × 10⁻³]`, `[1.5 × 10⁻³]`, `[1.6 ×10⁻⁷]`, `[1.4 × 10⁻¹²]`, `[7.3 × 10⁻¹²]`, `2.0 × 10⁸`
- Additional numbers to ensure a precise calculation.
4. **Graph & Diagram Explanation:
Expert Solution
Step 1: Determine the solubility product of the solid from the given data:
Given,
The molar solubility of Cu(IO3)2 (s) = 2.7 x 10-3 M
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