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Acid rain is a major environmental problem throughout the industrialized world. A major source of acid rain is the burning of fossil fuels containing sulfur (coal, oil and natural gas). The sulfur dioxide released into the air dissolves in water or. more seriously, it may be oxidized to sulfur trioxide which then dissolves in water to form the acid. The net effect is to decrease the pH of rain, damaging trees, killing fish, dissolving stone and corroding metal. 1. Write the hydrolysis reactions for the sulfur trioxide in water and for sulfur dioxide in water. 2. The pH of acid rain can range down to 3 or even lower in heavily polluted areas. Calculate the concentrations of H3O+ and OH" in a raindrop at pH 3.30 at 25°C. 3. When sulfur dioxide dissolves in water to form sulfurous acid, that acid can donate a hydrogen ion into water. Write a balanced chemical equation for this reaction and identify the stronger Brønste-Lowry acid and bse in the equation.

Acid rain is a major environmental problem throughout the industrialized world. A major source of acid rain is the burning of fossil fuels containing sulfur (coal, oil and natural gas). The sulfur dioxide released into the air dissolves in water or. more seriously, it may be oxidized to sulfur trioxide which then dissolves in water to form the acid. The net effect is to decrease the pH of rain, damaging trees, killing fish, dissolving stone and corroding metal. 1. Write the hydrolysis reactions for the sulfur trioxide in water and for sulfur dioxide in water. 2. The pH of acid rain can range down to 3 or even lower in heavily polluted areas. Calculate the concentrations of H3O+ and OH" in a raindrop at pH 3.30 at 25°C. 3. When sulfur dioxide dissolves in water to form sulfurous acid, that acid can donate a hydrogen ion into water. Write a balanced chemical equation for this reaction and identify the stronger Brønste-Lowry acid and bse in the equation.

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
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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Acid rain is a major environmental problem throughout the industrialized world. A major source of acid rain is the burning of fossil fuels containing sulfur (coal, oil and natural gas). The sulfur dioxide released into the air dissolves in water or. more seriously, it may be oxidized to sulfur trioxide which then dissolves in water to form the acid. The net effect is to decrease the pH of rain, damaging trees, killing fish, dissolving stone and corroding metal. 1. Write the hydrolysis reactions for the sulfur trioxide in water and for sulfur dioxide in water. 2. The pH of acid rain can range down to 3 or even lower in heavily polluted areas. Calculate the concentrations of H3O+ and OH in a raindrop at pH 3.30 at 25°C. 3. When sulfur dioxide dissolves in water to form sulfurous acid, that acid can donate a hydrogen ion into water. Write a balanced chemical equation for this reaction and identify the stronger Brønste-Lowry acid and bse in the equation. 4. Calculate the pH of a solution with an initial concentration of sulfurous acid of 1.5x10-4. For any approximation that you use (if any) , be sure to check if it is properly valid. pka1=1.92 pka2=7.18 5. Suppose that all the dissolved SO2 from the previous part has been further oxidized to SO3, so that 1.5x10-4 mol of H2SO4 is dissolved per liter. Calculate the pH in this case. pka1=strong, pka2=1.92.
Transcribed Image Text:Acid rain is a major environmental problem throughout the industrialized world. A major source of acid rain is the burning of fossil fuels containing sulfur (coal, oil and natural gas). The sulfur dioxide released into the air dissolves in water or. more seriously, it may be oxidized to sulfur trioxide which then dissolves in water to form the acid. The net effect is to decrease the pH of rain, damaging trees, killing fish, dissolving stone and corroding metal. 1. Write the hydrolysis reactions for the sulfur trioxide in water and for sulfur dioxide in water. 2. The pH of acid rain can range down to 3 or even lower in heavily polluted areas. Calculate the concentrations of H3O+ and OH in a raindrop at pH 3.30 at 25°C. 3. When sulfur dioxide dissolves in water to form sulfurous acid, that acid can donate a hydrogen ion into water. Write a balanced chemical equation for this reaction and identify the stronger Brønste-Lowry acid and bse in the equation. 4. Calculate the pH of a solution with an initial concentration of sulfurous acid of 1.5x10-4. For any approximation that you use (if any) , be sure to check if it is properly valid. pka1=1.92 pka2=7.18 5. Suppose that all the dissolved SO2 from the previous part has been further oxidized to SO3, so that 1.5x10-4 mol of H2SO4 is dissolved per liter. Calculate the pH in this case. pka1=strong, pka2=1.92.
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