For a 0.450 mol L-1 solution of formic acid (HCOOH) answer the following questions. The Ka of formic acid is 1.80 x 10-4. The small x assumption is allowed. a) Draw the equation for the dissociation of formic acid in water. b) Complete the ICE table for the above dissociation. c) What are the [H30*], pH, and pOH of this solution. d) What is the percent ionization?

For a 0.450 mol L-1 solution of formic acid (HCOOH) answer the following questions. The Ka of formic acid is 1.80 x 10-4. The small x assumption is allowed. a) Draw the equation for the dissociation of formic acid in water. b) Complete the ICE table for the above dissociation. c) What are the [H30*], pH, and pOH of this solution. d) What is the percent ionization?

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 87AP

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Two students were asked to determine the Kb of an unknown base. They were given a bottle with a solution in it. The bottle was labeled aqueous solution of a monoprotic strong acid. They were also given a pH meter, a buret, and an appropriate indicator. They reported the following data: volume of acid required for neutralization = 21.0 mL pH after 7.00 mL of strong acid added = 8.95 Use the students' data to determme the Kb of the unknown base.
. Strong buses are bases that completely ionize in water to produce hydroxide ion, OH-. The strong bases include the hydroxides of the Group I elements. For example, if 1.0 mole of NaOH is dissolved per liter, the concentration of OH ion is 1.0 M. Calculate the [OH-], pOH, and pH for each of the following strong base solutions. a. 1.10 M NaOH b. 2.0104M KOH c. 6.2103M CsOH d. 0.0001 M NaOH
A solution of formic acid (HCOOH, Ka = 1.8 104) has a pH of 2.70. Calculate the initial concentration of formic acid in this solution.
Find [OH+], [OH-] and the pH of the following solutions. (a) 30.0 mL of a 0.216 M solution of HCI diluted with enough water to make 125 mL of solution. (b) A solution made by dissolving 275 mL of HBr gas at 25C and 1.00 atm in enough water to make 475 mL of solution. Assume that all the HBr dissolves in water.
A 0.365-g sample of HCl is dissolved in enough water to give 2.00 102 mL of solution. What is the pH? (a) 2.000 (b) 0.0500 (c) 1.301 (d) 1.000
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The pH of a 0.10-M solution of caffeine is 11.16. Determine Kb for caffeine from these data: C8H10N4O2(aq)+H2O(l)C8H10N4O2H+(aq)+OH(aq)
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