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Consider the following infermation about sulfurous acid, a diprotic id (11,SO) ELS03= HSO," + 1I* pK1-1.81 HSO=S0,+ H pK-691 The titration curve for sodim sulfite, Na SO, with standard HCl is shown below PH VI 2 ml, HO added What ure the majoK species present al point 3? 30

Consider the following infermation about sulfurous acid, a diprotic id (11,SO) ELS03= HSO," + 1I* pK1-1.81 HSO=S0,+ H pK-691 The titration curve for sodim sulfite, Na SO, with standard HCl is shown below PH VI 2 ml, HO added What ure the majoK species present al point 3? 30

Chemistry
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
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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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### Understanding Sulfurous Acid and its Titration Curve #### Chemical Properties of Sulfurous Acid Sulfurous acid (H2SO3) is a diprotic acid, meaning it can donate two protons (H+ ions). The dissociation occurs in two steps: 1. **First dissociation:** \( \text{H}_2\text{SO}_3 (aq) \rightleftharpoons \text{HSO}_3^− (aq) + \text{H}^+ (aq) \) - **pKa1 = 1.81** 2. **Second dissociation:** \( \text{HSO}_3^− (aq) \rightleftharpoons \text{SO}_3^{2−} (aq) + \text{H}^+ (aq) \) - **pKa2 = 6.91** #### Titration Curve Explanation The provided titration curve depicts the titration of sodium sulfite (Na2SO3) with standard hydrochloric acid (HCl). - **X-axis:** Volume of HCl added (mL) - **Y-axis:** pH of the solution Key Points on the Curve: - **Point 1:** Initial pH before any HCl is added, showing the basic nature of the sodium sulfite solution. - **Point 2:** The first equivalence point where enough HCl has been added to neutralize one mole of the base (conversion of SO3²⁻ to HSO3⁻). - **Point 3:** A buffer region where HSO3⁻ and SO3²⁻ coexist, displaying resistance to pH change. - **Point 4:** The second equivalence point where enough HCl has been added to neutralize another mole of the base (conversion of HSO3⁻ to H2SO3). - **Point 5:** Final pH after all the sodium sulfite has been neutralized. #### Question: What are the major species present at point 3 on the titration curve? - **Point 3 represents a buffer region, so the major species present would be \( \text{HSO}_3^− \) and \( \text{SO}_3^{2−} \).** This example illustrates the titration process and how the pH changes as HCl is added, neutral
Transcribed Image Text:### Understanding Sulfurous Acid and its Titration Curve #### Chemical Properties of Sulfurous Acid Sulfurous acid (H2SO3) is a diprotic acid, meaning it can donate two protons (H+ ions). The dissociation occurs in two steps: 1. **First dissociation:** \( \text{H}_2\text{SO}_3 (aq) \rightleftharpoons \text{HSO}_3^− (aq) + \text{H}^+ (aq) \) - **pKa1 = 1.81** 2. **Second dissociation:** \( \text{HSO}_3^− (aq) \rightleftharpoons \text{SO}_3^{2−} (aq) + \text{H}^+ (aq) \) - **pKa2 = 6.91** #### Titration Curve Explanation The provided titration curve depicts the titration of sodium sulfite (Na2SO3) with standard hydrochloric acid (HCl). - **X-axis:** Volume of HCl added (mL) - **Y-axis:** pH of the solution Key Points on the Curve: - **Point 1:** Initial pH before any HCl is added, showing the basic nature of the sodium sulfite solution. - **Point 2:** The first equivalence point where enough HCl has been added to neutralize one mole of the base (conversion of SO3²⁻ to HSO3⁻). - **Point 3:** A buffer region where HSO3⁻ and SO3²⁻ coexist, displaying resistance to pH change. - **Point 4:** The second equivalence point where enough HCl has been added to neutralize another mole of the base (conversion of HSO3⁻ to H2SO3). - **Point 5:** Final pH after all the sodium sulfite has been neutralized. #### Question: What are the major species present at point 3 on the titration curve? - **Point 3 represents a buffer region, so the major species present would be \( \text{HSO}_3^− \) and \( \text{SO}_3^{2−} \).** This example illustrates the titration process and how the pH changes as HCl is added, neutral
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