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A student mixes 50.0 mL of 1.00 M Ba(OH)2 with 72.5 mL of 0.375 M H,So,. 4- Calculate the mass of BaSO, formed. Calculate the pH of the mixed solution.

A student mixes 50.0 mL of 1.00 M Ba(OH)2 with 72.5 mL of 0.375 M H,So,. 4- Calculate the mass of BaSO, formed. Calculate the pH of the mixed solution.

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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**Chemical Reaction and Calculations for Barium Sulfate Precipitation** A student mixes 50.0 mL of 1.00 M Ba(OH)₂ with 72.5 mL of 0.375 M H₂SO₄. 1. **Calculate the mass of BaSO₄ formed.** Enter your answer in the box provided: _____ g 2. **Calculate the pH of the mixed solution.** Enter your answer in the box provided: _____ **Explanation:** In this reaction, Barium hydroxide [Ba(OH)₂] reacts with sulfuric acid [H₂SO₄] to form barium sulfate [BaSO₄] and water [H₂O] as follows: \[ \text{Ba(OH)}_2 \, + \, \text{H}_2\text{SO}_4 \rightarrow \text{BaSO}_4 \, + \, 2\text{H}_2\text{O} \] **Instructions for Calculation:** - Determine the limiting reactant. - Calculate the mass of BaSO₄ precipitated using stoichiometry. - Use the concentrations of the remaining [H⁺] or [OH⁻] ions to calculate the pH of the solution after reaction.
Transcribed Image Text:**Chemical Reaction and Calculations for Barium Sulfate Precipitation** A student mixes 50.0 mL of 1.00 M Ba(OH)₂ with 72.5 mL of 0.375 M H₂SO₄. 1. **Calculate the mass of BaSO₄ formed.** Enter your answer in the box provided: _____ g 2. **Calculate the pH of the mixed solution.** Enter your answer in the box provided: _____ **Explanation:** In this reaction, Barium hydroxide [Ba(OH)₂] reacts with sulfuric acid [H₂SO₄] to form barium sulfate [BaSO₄] and water [H₂O] as follows: \[ \text{Ba(OH)}_2 \, + \, \text{H}_2\text{SO}_4 \rightarrow \text{BaSO}_4 \, + \, 2\text{H}_2\text{O} \] **Instructions for Calculation:** - Determine the limiting reactant. - Calculate the mass of BaSO₄ precipitated using stoichiometry. - Use the concentrations of the remaining [H⁺] or [OH⁻] ions to calculate the pH of the solution after reaction.
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