Determine the pH of a solution of HCIO₂ by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-3 before submitting your answer. 1 2 3 NEXT > A 0.020 M aqueous solution of HCIO2 is prepared. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products.. Initial (M) Change (M) Equilibrium (M) -2x 1.2 x 10-²-2x 0 0.020 + x HCIO₂(aq) 0.020 0.020 - x + H₂O(l) 1.2 x 10-² 0.020 + 2x 0.010 0.020 - 2x H3O+ (aq) +X 1.2 x 10-2 + x + CIO₂ (aq) 1.2 x 10-2-x RESET +2x 1.2 x 10-² + 2x
Determine the pH of a solution of HCIO₂ by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-3 before submitting your answer. 1 2 3 NEXT > A 0.020 M aqueous solution of HCIO2 is prepared. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products.. Initial (M) Change (M) Equilibrium (M) -2x 1.2 x 10-²-2x 0 0.020 + x HCIO₂(aq) 0.020 0.020 - x + H₂O(l) 1.2 x 10-² 0.020 + 2x 0.010 0.020 - 2x H3O+ (aq) +X 1.2 x 10-2 + x + CIO₂ (aq) 1.2 x 10-2-x RESET +2x 1.2 x 10-² + 2x
Chemistry
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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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Question
![**Determining the pH of an HClO₂ Solution Using an ICE Table**
To determine the pH of a 0.020 M aqueous solution of HClO₂, follow these steps:
1. **Construct an ICE Table:**
- Write the balanced chemical equation: HClO₂(aq) + H₂O(l) ⇌ H₃O⁺(aq) + ClO₂⁻(aq).
- Prepare an ICE (Initial, Change, Equilibrium) table to organize and calculate concentrations.
2. **Fill in the ICE Table:**
| | HClO₂(aq) | | H₃O⁺(aq) | | ClO₂⁻(aq) |
|:-------------:|:--------:|:-----------:|:--------:|:-----------:|:--------:|
| **Initial (M)** | 0.020 | | 0 | | 0 |
| **Change (M)** | -x | | +x | | +x |
| **Equilibrium (M)** | 0.020-x | | x | | x |
3. **Select Values to Determine Concentrations:**
- Use the provided values for calculating equilibrium concentrations:
- `0.020` for initial HClO₂.
- `0` for initial H₃O⁺ and ClO₂⁻.
- Changes: `-x`, `+x` for H₃O⁺ and ClO₂⁻.
4. **Equilibrium Constant Expression:**
- Calculate equilibrium concentrations using selected expressions:
- `HClO₂`: `0.020 - x`
- `H₃O⁺` and `ClO₂⁻`: `x`
5. **Calculate the pH:**
- Use the expression \( \text{pH} = -\log [\text{H}_3\text{O}^+] \) with equilibrium concentration of \( [\text{H}_3\text{O}^+] = x \).
**Explanation of Included Elements:**
- **Reset Button:** Allows resetting current values for recalculations.
- **Editable Fields and Buttons:** Help select different initial, change, and equilibrium concentrations for](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F53fad175-5b35-4951-b14a-e374468693f0%2Ffc899e77-2f06-4c63-904d-78fe591745c5%2F18f01ln_processed.png&w=3840&q=75)
Transcribed Image Text:**Determining the pH of an HClO₂ Solution Using an ICE Table**
To determine the pH of a 0.020 M aqueous solution of HClO₂, follow these steps:
1. **Construct an ICE Table:**
- Write the balanced chemical equation: HClO₂(aq) + H₂O(l) ⇌ H₃O⁺(aq) + ClO₂⁻(aq).
- Prepare an ICE (Initial, Change, Equilibrium) table to organize and calculate concentrations.
2. **Fill in the ICE Table:**
| | HClO₂(aq) | | H₃O⁺(aq) | | ClO₂⁻(aq) |
|:-------------:|:--------:|:-----------:|:--------:|:-----------:|:--------:|
| **Initial (M)** | 0.020 | | 0 | | 0 |
| **Change (M)** | -x | | +x | | +x |
| **Equilibrium (M)** | 0.020-x | | x | | x |
3. **Select Values to Determine Concentrations:**
- Use the provided values for calculating equilibrium concentrations:
- `0.020` for initial HClO₂.
- `0` for initial H₃O⁺ and ClO₂⁻.
- Changes: `-x`, `+x` for H₃O⁺ and ClO₂⁻.
4. **Equilibrium Constant Expression:**
- Calculate equilibrium concentrations using selected expressions:
- `HClO₂`: `0.020 - x`
- `H₃O⁺` and `ClO₂⁻`: `x`
5. **Calculate the pH:**
- Use the expression \( \text{pH} = -\log [\text{H}_3\text{O}^+] \) with equilibrium concentration of \( [\text{H}_3\text{O}^+] = x \).
**Explanation of Included Elements:**
- **Reset Button:** Allows resetting current values for recalculations.
- **Editable Fields and Buttons:** Help select different initial, change, and equilibrium concentrations for
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