A certain weak acid, HA, with a Ka value of 5.61 × 10- is titrated with NaOH. Part A A solution is made by titrating 8.00 mmol (millimoles) of HA and 3.00 mmol of the strong base. What is the resulting pH? Express the pH numerically to two decimal places. femplates Symbols uAdo redo reset keyboard shortcuts help pH = Submit Request Answer Part B More strong base is added until the equivalence point is reached. What is the pH of this solution at the equivalence point if the total volume is 74.0 mL ? Express the pH numerically to two decimal places. femplates Symbols uado redo reset keyboard shortcuts help, pH =

A certain weak acid, HA, with a Ka value of 5.61 × 10- is titrated with NaOH. Part A A solution is made by titrating 8.00 mmol (millimoles) of HA and 3.00 mmol of the strong base. What is the resulting pH? Express the pH numerically to two decimal places. femplates Symbols uAdo redo reset keyboard shortcuts help pH = Submit Request Answer Part B More strong base is added until the equivalence point is reached. What is the pH of this solution at the equivalence point if the total volume is 74.0 mL ? Express the pH numerically to two decimal places. femplates Symbols uado redo reset keyboard shortcuts help, pH =

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 191MP

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H2Z is a diprotic acid with Ka1 = 3.0 × 10^-3 and Ka2 = 8.0 x 10^-8. Suppose you start with 1.00 L of 1.00 M H2Z(aq) and add 1.00 M KOH (aq) gradually. Calculate the pH at the following volumes of added strong base: a) 0.00 L; b) 0.50 L; c) 1.00 L; d) 1.50 L; e) 2.00 L. Report the pH values with 2 decimal places after dot. Write relevant chemical equations and show work on every part of this problem. f. Sketch the titration curve g. How many liters of 1.00 M KOH(ag) should be added to 1.00 L of 1.00 M H2Z to obtain a buffered solution with pH = 7.50? Hint to part g: you may calculate the moles of two salts in the buffer, then moles of K* ions in the salt, and finally consider that all K* ions come from KOH(ag).
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