88 Using the eyumu page 81, calculate the pH after the additioll UI UUIUI Neutial When a strong base is added to a buffer solution it will react with the weak acid to produce weak base without dramatically changing the mol ratio (mol A/mol HA). Complete the ICE table below to show the change occurring and calculate the equilibrium for the addition of 0.10 mol of OH added to a buffer consisting of 10 mel HA and 1.0 mol A (with a pKa = 9.00 and initial buffer pH of 9.00) The initial values %3D have already been included in the table. HA + OH A+ H2O mol HA mol OH mol A Initial 1.0 0.10 1.0 Change Equilibrium Using the equilibrium values from the table above and the Henderson-Hasselbalch equation on page 81, calculate the pH after the addition of acid.

88 Using the eyumu page 81, calculate the pH after the additioll UI UUIUI Neutial When a strong base is added to a buffer solution it will react with the weak acid to produce weak base without dramatically changing the mol ratio (mol A/mol HA). Complete the ICE table below to show the change occurring and calculate the equilibrium for the addition of 0.10 mol of OH added to a buffer consisting of 10 mel HA and 1.0 mol A (with a pKa = 9.00 and initial buffer pH of 9.00) The initial values %3D have already been included in the table. HA + OH A+ H2O mol HA mol OH mol A Initial 1.0 0.10 1.0 Change Equilibrium Using the equilibrium values from the table above and the Henderson-Hasselbalch equation on page 81, calculate the pH after the addition of acid.

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter16: Acids And Bases

Section: Chapter Questions

Problem 10ALQ

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Similar questions

A 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in enough water to make 100.0 mL of solution and was then titrated with 0.100 M HCl. After 500.0 mL HCl was added, the pH was 5.00. The experimenter found that 1.00 L of 0.100 M HCl was required to reach the stoichiometric point of the titration. a. What is the molar mass of NaA? b. Calculate the pH of the solution at the stoichiometric point of the titration.
Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.
What mass of NH4Cl must be added to 0.750 L of a 0.100-M solution of NH3 to give a buffer solution with a pH of 9.26? (Him: Assume a negligible change in volume as the solid is added.)
How much solid NaCH3CO23H2O must be added to 0300 L of a 0.50-M acetic acid solution to give a buffer with a pH of 5.00? (Him: Assume a negligible change in volume as the solid is added.)
Consider a 10.0% (by mass) solution of hypochlorous acid. Assume the density of the solution to be 1.00 g/mL. A 30.0-mL sample of the solution is titrated with 0.419 M KOH. Calculate the pH of the solution (a) before titration. (b) halfway to the equivalence point. (c) at the equivalence point.
Calculate the pH after 0.15 mole of solid NaOH is added to 1.00 L of each of the following solutions: a. 0.050 M propanoic acid (HC3H5O2, Ka = 1.3 105) and 0.080 M sodium propanoate b. 0.50 M propanoic acid and 0.80 M sodium propanoate c. Is the solution in part a still a buffer solution after the NaOH has been added? Explain.
A certain indicator HIn has a pKa of 3.00 and a color change becomes visible when 7.00% of the indicator has been convened to In. At what pH is this color change visible?
When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
. Which component of a buffered solution is capable of combining with an added strong acid? Using your example from Exercise 60, show how this component would react with added HC1.