Suppose 100.0 mL of a 0.3750 M solution of the strong base Ba(OH)2 is titrated with a 0.4540 M solution of the strong acid HCIO4. The neutralization reaction is Ba(OH)2(aq) + 2 HCIO,(aq) - → Ba(CIO4)2 (aq) + 2 H2O(€) Compute the pH of the titration solution before any acid is added, when the titration is 1.00 mL short of the equiv- alence point, when the titration is at the equivalence point, and when the titration is 1.00 mL past the equivalence point. (Note: Each mole of Ba(OH), gives two moles of OH- in solution.)

Suppose 100.0 mL of a 0.3750 M solution of the strong base Ba(OH)2 is titrated with a 0.4540 M solution of the strong acid HCIO4. The neutralization reaction is Ba(OH)2(aq) + 2 HCIO,(aq) - → Ba(CIO4)2 (aq) + 2 H2O(€) Compute the pH of the titration solution before any acid is added, when the titration is 1.00 mL short of the equiv- alence point, when the titration is at the equivalence point, and when the titration is 1.00 mL past the equivalence point. (Note: Each mole of Ba(OH), gives two moles of OH- in solution.)

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter4: Reactions In Aqueous Solution

Section: Chapter Questions

Problem 75QAP: A student is given 0.930 g of an unknown acid, which can be either oxalic acid, H2C2O4, or citric...

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