Determine the pH of a buffer formed by dissolving 21.5 g HC-HsO2 and 37.7 g of NaC-H:O2 in 200.0 mL of solution. The value of Ka for HC-H:O2 is 6.3 x 10-5. 2 3 NEXT > Based on the given values, set up ICE table in order to determine the unknown. НС-Н.О-(аq) + H:O(I) H:O“(aq) + C-HsO: (aq) Initial (M) Change (M) Equilibrium (M) 5 RESET 21.5 37.7 0.176 0.261 0.880 1.31 0.178 0.888 -- 21.5 - x 37.7 +x 0.176 - x 0.261 +x 0.880 - x 1.31 + x 0.178 +x 0.888 + x
Determine the pH of a buffer formed by dissolving 21.5 g HC-HsO2 and 37.7 g of NaC-H:O2 in 200.0 mL of solution. The value of Ka for HC-H:O2 is 6.3 x 10-5. 2 3 NEXT > Based on the given values, set up ICE table in order to determine the unknown. НС-Н.О-(аq) + H:O(I) H:O“(aq) + C-HsO: (aq) Initial (M) Change (M) Equilibrium (M) 5 RESET 21.5 37.7 0.176 0.261 0.880 1.31 0.178 0.888 -- 21.5 - x 37.7 +x 0.176 - x 0.261 +x 0.880 - x 1.31 + x 0.178 +x 0.888 + x
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Chapter1: Chemical Foundations
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![The image depicts a step-by-step approach to determine the pH of a buffer solution. Here's a transcription and explanation of the ICE table setup:
**Title:** Determine the pH of a buffer.
**Introduction:**
A buffer is prepared by dissolving 21.5 g of HC₇H₅O₂ and 37.7 g of NaC₇H₅O₂ in 200.0 mL of solution. The value of Ka for HC₇H₅O₂ is 6.3 × 10⁻⁵.
**Instructions:**
Based on the given values, set up an ICE (Initial, Change, Equilibrium) table in order to determine the unknown.
**ICE Table:**
The reaction is as follows:
\[ \text{HC}_7\text{H}_5\text{O}_2(\text{aq}) + \text{H}_2\text{O}(\text{l}) \rightleftharpoons \text{H}_3\text{O}^+(\text{aq}) + \text{C}_7\text{H}_5\text{O}_2^-(\text{aq}) \]
- **Initial (M):**
- HC₇H₅O₂(aq): blank
- H₂O(l): not applicable
- H₃O⁺(aq): blank
- C₇H₅O₂⁻(aq): blank
- **Change (M):**
- HC₇H₅O₂(aq): blank
- H₂O(l): not applicable
- H₃O⁺(aq): blank
- C₇H₅O₂⁻(aq): blank
- **Equilibrium (M):**
- HC₇H₅O₂(aq): blank
- H₂O(l): not applicable
- H₃O⁺(aq): blank
- C₇H₅O₂⁻(aq): blank
**Values Provided Below the Table:**
- **HC₇H₅O₂(aq):**
- Initial: 0.178 M
- Change: \( -x \)
- Equilibrium: \( 0.880 - x \)
- **NaC₇H](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcf18891e-a57f-4755-b1e7-859ef1938a42%2F4086cefe-ebae-4431-9af7-7aa32f576bbc%2Fnn8f32_processed.png&w=3840&q=75)
Transcribed Image Text:The image depicts a step-by-step approach to determine the pH of a buffer solution. Here's a transcription and explanation of the ICE table setup:
**Title:** Determine the pH of a buffer.
**Introduction:**
A buffer is prepared by dissolving 21.5 g of HC₇H₅O₂ and 37.7 g of NaC₇H₅O₂ in 200.0 mL of solution. The value of Ka for HC₇H₅O₂ is 6.3 × 10⁻⁵.
**Instructions:**
Based on the given values, set up an ICE (Initial, Change, Equilibrium) table in order to determine the unknown.
**ICE Table:**
The reaction is as follows:
\[ \text{HC}_7\text{H}_5\text{O}_2(\text{aq}) + \text{H}_2\text{O}(\text{l}) \rightleftharpoons \text{H}_3\text{O}^+(\text{aq}) + \text{C}_7\text{H}_5\text{O}_2^-(\text{aq}) \]
- **Initial (M):**
- HC₇H₅O₂(aq): blank
- H₂O(l): not applicable
- H₃O⁺(aq): blank
- C₇H₅O₂⁻(aq): blank
- **Change (M):**
- HC₇H₅O₂(aq): blank
- H₂O(l): not applicable
- H₃O⁺(aq): blank
- C₇H₅O₂⁻(aq): blank
- **Equilibrium (M):**
- HC₇H₅O₂(aq): blank
- H₂O(l): not applicable
- H₃O⁺(aq): blank
- C₇H₅O₂⁻(aq): blank
**Values Provided Below the Table:**
- **HC₇H₅O₂(aq):**
- Initial: 0.178 M
- Change: \( -x \)
- Equilibrium: \( 0.880 - x \)
- **NaC₇H
![**Buffer pH Determination**
To determine the pH of a buffer formed by dissolving 21.5 g of HC₇H₅O₂ and 37.7 g of NaC₇H₅O₂ in 200.0 mL of solution, we use the given value of the acid dissociation constant (\( K_a \)) for HC₇H₅O₂, which is \( 6.3 \times 10^{-5} \).
**ICE Table and Expression for \( K_a \):**
Based on the ICE (Initial, Change, Equilibrium) table and definition of \( K_a \), set up the expression for \( K_a \) to determine the unknown. Do not combine or simplify terms.
\[
K_a = \boxed{\_\_\_} = 6.3 \times 10^{-5}
\]
**Options for Values in Expression Setup:**
- [0]
- [21.5]
- [37.7]
- [0.176]
- [0.261]
- [0.880]
- [1.31]
- [0.178]
- [0.888]
- [x]
- [2x]
- [21.5 - x]
- [37.7 + x]
- [0.176 - x]
- [0.261 + x]
- [0.880 - x]
- [1.31 + x]
- [0.178 + x]
- [0.888 + x]
**Instructions:**
- Choose the appropriate values for the expression.
- Do not combine or simplify the terms when setting up the equation.
**User Interaction:**
- Use the provided buttons to select values for the expression.
- Press "RESET" to clear selections and start over.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcf18891e-a57f-4755-b1e7-859ef1938a42%2F4086cefe-ebae-4431-9af7-7aa32f576bbc%2Fh6wvfs_processed.png&w=3840&q=75)
Transcribed Image Text:**Buffer pH Determination**
To determine the pH of a buffer formed by dissolving 21.5 g of HC₇H₅O₂ and 37.7 g of NaC₇H₅O₂ in 200.0 mL of solution, we use the given value of the acid dissociation constant (\( K_a \)) for HC₇H₅O₂, which is \( 6.3 \times 10^{-5} \).
**ICE Table and Expression for \( K_a \):**
Based on the ICE (Initial, Change, Equilibrium) table and definition of \( K_a \), set up the expression for \( K_a \) to determine the unknown. Do not combine or simplify terms.
\[
K_a = \boxed{\_\_\_} = 6.3 \times 10^{-5}
\]
**Options for Values in Expression Setup:**
- [0]
- [21.5]
- [37.7]
- [0.176]
- [0.261]
- [0.880]
- [1.31]
- [0.178]
- [0.888]
- [x]
- [2x]
- [21.5 - x]
- [37.7 + x]
- [0.176 - x]
- [0.261 + x]
- [0.880 - x]
- [1.31 + x]
- [0.178 + x]
- [0.888 + x]
**Instructions:**
- Choose the appropriate values for the expression.
- Do not combine or simplify the terms when setting up the equation.
**User Interaction:**
- Use the provided buttons to select values for the expression.
- Press "RESET" to clear selections and start over.
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