The pOH of an aqueous solution of 0.532 M caffeine (a weak base with the formula \( \text{C}_8\text{H}_{10}\text{N}_4\text{O}_2 \)) is \(\_\_\_\_\_\_\_\_\_\_\_\_\_\). (Assume that \( K_b (\text{C}_8\text{H}_{10}\text{N}_4\text{O}_2) = 4.10 \times 10^{-4} \).) The text reads:"The pH of an aqueous solution of 0.0959 M ammonium perchlorate, \( \text{NH}_4\text{ClO}_4 \, (\text{aq}), \) is [_____]. (Assume that \( K_b(\text{NH}_3) = 1.80 \times 10^{-5}. \))This solution is [dropdown menu]."Explanation:- The question asks for the pH calculation of a 0.0959 M ammonium perchlorate solution.- It provides the base dissociation constant (\( K_b \)) for ammonia (\( \text{NH}_3 \)) as \( 1.80 \times 10^{-5} \).- There is a blank space to fill in the pH value.- There is a dropdown menu indicating the nature of the solution (likely options such as acidic, neutral, or basic).

Answered: The pOH of an aqueous solution of 0.532…

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

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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The pOH of an aqueous solution of 0.532 M caffeine (a weak base with the formula C8 H10 N4O2) is (Assume that Kb (C8H10N4O2) = 4.10 × 10-4.)