This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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Here are the solutions for both questions. Question 1: Degree of ionization To calculate the degree of ionization () for a weak acid, we can use the approximation = sqrt((K_a)/(C)), where K_a is the acid dissociation constant and C is the initial concentration of the acid. Step 1: Identify the given values. The initial concentration of the acid is C = 0.01 M. The acid dissociation constant is K_a = 10^-4. Step 2: Apply the approximation formula for the degree of ionization. = sqrt((K_a)/(C)) = sqrt(10^-4)0.01 Step 3: Calculate the degree of ionization. = sqrt(10^-4)10^-2 = sqrt(10^-2) = 10^-1 = 0.1 The degree of ionization is 0.1. The final answer is 0.1. --- Question 2: Neutralization reaction statements The given hypothetical neutralization reaction is: H_2X(aq) + 2BOH(aq) B_2X(aq) + 2H_2O(l) Let's analyze each statement based on Brønsted-Lowry acid-base theory: A Brønsted-Lowry acid donates protons (H^+). A Brønsted-Lowry base accepts protons (H^+). A conjugate acid is formed when a base accepts a proton. A conjugate base is formed when an acid donates a proton. In the reaction: H_2X donates protons to BOH (specifically, its OH^- part). Thus, H_2X acts as an acid. BOH (or OH^- from BOH) accepts protons from H_2X. Thus, BOH acts as a base. When H_2X donates protons, its conjugate base is X^2- (which forms B_2X with B^+). When OH^- accepts a proton, its conjugate acid is H_2O. Now, let's evaluate each statement: I. B_2X is conjugate acid. B_2X is a salt formed from the cation B^+ and the