Consider the titration of 40.0 mL of 0.20 M H3A (K = 3.0 x 10-4,. , K. 4.4 x 10-8, K = 8.0 x 10-11) titrated by 0.20 M KOH. %3D %3D a. Calculate the pH of the resulting solution at 100. mL of KOH added. pH- b. At what volume of KOH added does pH = 3.52? Volume mL c. At 60.0 mL of KOH added, is the pH acidic or basic? O acidic Obasic

Consider the titration of 40.0 mL of 0.20 M H3A (K = 3.0 x 10-4,. , K. 4.4 x 10-8, K = 8.0 x 10-11) titrated by 0.20 M KOH. %3D %3D a. Calculate the pH of the resulting solution at 100. mL of KOH added. pH- b. At what volume of KOH added does pH = 3.52? Volume mL c. At 60.0 mL of KOH added, is the pH acidic or basic? O acidic Obasic

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter7: Neutralization Titrations And Graphical Representations

Section: Chapter Questions

Problem 8P

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The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSeO4, 0.0118 g/100 mL. (b) Ba(BrO3)2H2O, 0.30 g/100 mL. (c) NH4MgAsO46H2O, 0.033 g/100 mL. (d) La2(MoO4)3, 0.00179 g/100 mL
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