2. What would be the pH of a 0.642M solution ofN_(2)H_(5)CI? The K_(b) of N_(2)H(4) is 9.5\times 10^(-7).3. What would be the concentration.of oxalate ions(C_(2)0_(4)^(2-)) in a 0.500MH_(2)C_(2)0_(4) ?K_(a1) = 5.9\times 10^(-2)K_(a2) = 6.4\times 10^(-5)

2. pH of a 0.642 M solution of N₂H₅ClGiven:Concentration of N₂H₅Cl = 0.642 MKb of N₂H₄ = 9.5 ×…

Answered: 2. What would be the pH of a 0.642 M…

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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2. What would be the pH of a 0.642 M solution of N_(2)H_(5)CI? The K_(b) of N_(2)H (4) is 9.5\times 10^(-7). 3. What would be the concentration . of oxalate ions (C_(2)0_(4)^(2-)) in a 0.500MH_(2) C_(2)0_(4) ? K_(a1) = 5.9\times 10^(-2) K_(a2) = 6.4\times 10^(-5)