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Determine the pH of a 0.10 M solution of HNC-H.SO3 (pKa = 2.32). %3D 1 2 NEXT > Based on the given values, set up ICE table in order to determine the unknown. HNC-H.SO:(aq) + Н.О() H.O“(aq) + NC-H.SOs-(aq) Initial (M) Change (M) Equilibrium (M)

Determine the pH of a 0.10 M solution of HNC-H.SO3 (pKa = 2.32). %3D 1 2 NEXT > Based on the given values, set up ICE table in order to determine the unknown. HNC-H.SO:(aq) + Н.О() H.O“(aq) + NC-H.SOs-(aq) Initial (M) Change (M) Equilibrium (M)

Chemistry
Chemistry
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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
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**Determine the pH of a 0.10 M solution of HNC₇H₄SO₃ (pKa = 2.32).** ### Step 1: Introduction Based on the given values, set up an ICE table in order to determine the unknown. ### ICE Table Setup | | HNC₇H₄SO₃(aq) | + | H₂O(l) | ⇌ | H₃O⁺(aq) | + | NC₇H₄SO₃⁻(aq) | |------------------|---------------|---|--------|----|----------|---|---------------| | **Initial (M)** | | | | | | | | | **Change (M)** | | | | | | | | | **Equilibrium (M)** | | | | | | | | ### Values to Choose From - \(-\) - \(0\) - \(0.10\) - \(2.32\) - \(0.20\) - \(+x\) - \(-x\) - \(-2x\) - \(0.10 + x\) - \(0.10 - x\) - \(0.10 + 2x\) - \(0.10 - 2x\) - \(0.20 + x\) - \(0.20 - x\) - \(0.20 + 2x\) Use these values to fill in the ICE table. **Note:** Click the "RESET" button if you need to clear your current selections. ---
Transcribed Image Text:**Determine the pH of a 0.10 M solution of HNC₇H₄SO₃ (pKa = 2.32).** ### Step 1: Introduction Based on the given values, set up an ICE table in order to determine the unknown. ### ICE Table Setup | | HNC₇H₄SO₃(aq) | + | H₂O(l) | ⇌ | H₃O⁺(aq) | + | NC₇H₄SO₃⁻(aq) | |------------------|---------------|---|--------|----|----------|---|---------------| | **Initial (M)** | | | | | | | | | **Change (M)** | | | | | | | | | **Equilibrium (M)** | | | | | | | | ### Values to Choose From - \(-\) - \(0\) - \(0.10\) - \(2.32\) - \(0.20\) - \(+x\) - \(-x\) - \(-2x\) - \(0.10 + x\) - \(0.10 - x\) - \(0.10 + 2x\) - \(0.10 - 2x\) - \(0.20 + x\) - \(0.20 - x\) - \(0.20 + 2x\) Use these values to fill in the ICE table. **Note:** Click the "RESET" button if you need to clear your current selections. ---
**Determine the pH of a 0.10 M solution of HNC₇H₄SO₃ (pKₐ = 2.32).** **Instruction:** Based on your ICE (Initial, Change, Equilibrium) table and the definition of Kₐ (acid dissociation constant), set up the expression for Kₐ in order to determine the unknown. Do not combine or simplify terms. **Kₐ Expression:** \[ K_a = \frac{[ \text{H}^+ ][ \text{C}_7\text{H}_4\text{SO}_3^- ]}{[ \text{HNC}_7\text{H}_4\text{SO}_3 ]} \] **Available Options:** - \([0]\) - \([0.10]\) - \([2.32]\) - \([0.20]\) - \([x]\) - \([2x]\) - \([0.10 + x]\) - \([0.10 - x]\) - \([0.20 + x]\) - \([0.20 - x]\) - \([0.20 + 2x]\) - \([0.20 - 2x]\) - \(2.32\) - \(0.098\) - \(4.8 \times 10^{-3}\) - \(2.1 \times 10^{-12}\) **Interface Elements:** - Input boxes for Kₐ expression setup - A RESET button for clearing inputs Explore each option and construct the appropriate Kₐ expression without simplifying the terms.
Transcribed Image Text:**Determine the pH of a 0.10 M solution of HNC₇H₄SO₃ (pKₐ = 2.32).** **Instruction:** Based on your ICE (Initial, Change, Equilibrium) table and the definition of Kₐ (acid dissociation constant), set up the expression for Kₐ in order to determine the unknown. Do not combine or simplify terms. **Kₐ Expression:** \[ K_a = \frac{[ \text{H}^+ ][ \text{C}_7\text{H}_4\text{SO}_3^- ]}{[ \text{HNC}_7\text{H}_4\text{SO}_3 ]} \] **Available Options:** - \([0]\) - \([0.10]\) - \([2.32]\) - \([0.20]\) - \([x]\) - \([2x]\) - \([0.10 + x]\) - \([0.10 - x]\) - \([0.20 + x]\) - \([0.20 - x]\) - \([0.20 + 2x]\) - \([0.20 - 2x]\) - \(2.32\) - \(0.098\) - \(4.8 \times 10^{-3}\) - \(2.1 \times 10^{-12}\) **Interface Elements:** - Input boxes for Kₐ expression setup - A RESET button for clearing inputs Explore each option and construct the appropriate Kₐ expression without simplifying the terms.
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