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Consider the titration of 40.0 mL of 0.18 M H3A (Kal = 1.9 × 10-4, Ka₂ = 1.2 × 10-8, Kaz KOH. a. Calculate the pH of the resulting solution at 100. mL of KOH added. pH = b. At what volume of KOH added does pH = 3.72? Volume = mL c. At 60.0 mL of KOH added, is the pH acidic or basic? O acidic basic Submit Answer Retry Entire Group 9 more group attempts remaining = 1.1 x 10-¹¹) titrated by 0.18 M

Consider the titration of 40.0 mL of 0.18 M H3A (Kal = 1.9 × 10-4, Ka₂ = 1.2 × 10-8, Kaz KOH. a. Calculate the pH of the resulting solution at 100. mL of KOH added. pH = b. At what volume of KOH added does pH = 3.72? Volume = mL c. At 60.0 mL of KOH added, is the pH acidic or basic? O acidic basic Submit Answer Retry Entire Group 9 more group attempts remaining = 1.1 x 10-¹¹) titrated by 0.18 M

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
Chapter15: Acid-base Equilibria
Section: Chapter Questions
Problem 88AE: Consider die titration of 50.0 mL of 0.10 M H3A (Ka1 = 5.0 104, Ka2 = 1.0 108, Ka3 = 1.0 1012)...
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Consider the titration of 40.0 mL of 0.18 M H3A (K₁₁ = 1.9 × 10−4, K₂₂ = 1.2 × 10−8, Kaş = 1.1 × 10-¹¹) titrated by 0.18 M Ka 11 KOH. a. Calculate the pH of the resulting solution at 100. mL of KOH added. pH b. At what volume of KOH added does pH = 3.72? Volume = mL = c. At 60.0 mL of KOH added, is the pH acidic or basic? O acidic basic Submit Answer Retry Entire Group 9 more group attempts remaining
Transcribed Image Text:Consider the titration of 40.0 mL of 0.18 M H3A (K₁₁ = 1.9 × 10−4, K₂₂ = 1.2 × 10−8, Kaş = 1.1 × 10-¹¹) titrated by 0.18 M Ka 11 KOH. a. Calculate the pH of the resulting solution at 100. mL of KOH added. pH b. At what volume of KOH added does pH = 3.72? Volume = mL = c. At 60.0 mL of KOH added, is the pH acidic or basic? O acidic basic Submit Answer Retry Entire Group 9 more group attempts remaining
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