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You mix 250 mL of 2.1 M HBr with 200 mL of 2.5 M KOH. What is the pH of the resulting solution? Careful! This problem is challenging. Always think about what is in your beaker after the reaction has run to completion: Utilize moles to figure out which is your limiting reactant, HBr or KOH. • How much of your other reactant will be leftover? This will determine your pH. • Note that your pH equation uses the concentration of H3O* (molarity), not moles! You know molarity is moles solute per liter of solution. Think carefully about the total volume of the final solution in your beaker. . 1 12.4 12.7 1.3 1.6

You mix 250 mL of 2.1 M HBr with 200 mL of 2.5 M KOH. What is the pH of the resulting solution? Careful! This problem is challenging. Always think about what is in your beaker after the reaction has run to completion: Utilize moles to figure out which is your limiting reactant, HBr or KOH. • How much of your other reactant will be leftover? This will determine your pH. • Note that your pH equation uses the concentration of H3O* (molarity), not moles! You know molarity is moles solute per liter of solution. Think carefully about the total volume of the final solution in your beaker. . 1 12.4 12.7 1.3 1.6

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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You mix 250 mL of 2.1 M HBr with 200 mL of 2.5 M KOH. What is the pH of the resulting solution? Careful! This problem is challenging. Always think about what is in your beaker after the reaction has run to completion: Utilize moles to figure out which is your limiting reactant, HBr or KOH. • How much of your other reactant will be leftover? This will determine your pH. • Note that your pH equation uses the concentration of H3O* (molarity), not moles! You know molarity is moles solute per liter of solution. Think carefully about the total volume of the final solution in your beaker. . 1 12.4 12.7 1.3 1.6
Transcribed Image Text:You mix 250 mL of 2.1 M HBr with 200 mL of 2.5 M KOH. What is the pH of the resulting solution? Careful! This problem is challenging. Always think about what is in your beaker after the reaction has run to completion: Utilize moles to figure out which is your limiting reactant, HBr or KOH. • How much of your other reactant will be leftover? This will determine your pH. • Note that your pH equation uses the concentration of H3O* (molarity), not moles! You know molarity is moles solute per liter of solution. Think carefully about the total volume of the final solution in your beaker. . 1 12.4 12.7 1.3 1.6
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