Consider the titration of 40.0 mL of 0.200 mol/L HCOONa (aq) with 0.300 mol/L HCl (aq). Ka for HCOOH is 1.8×10⁻⁴. Given: Kb = [x][x] / [0.200 - x] Based on your ICE table and Kb expression, determine the [OH⁻] in the solution.
Consider the titration of 40.0 mL of 0.200 mol/L HCOONa (aq) with 0.300 mol/L HCl (aq). Ka for HCOOH is 1.8×10⁻⁴. Given: Kb = [x][x] / [0.200 - x] Based on your ICE table and Kb expression, determine the [OH⁻] in the solution.
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter15: Additional Aqueous Equilibria
Section: Chapter Questions
Problem 111QRT: Consider the nanoscale-level representations for Question 111 of the titration of the aqueous strong...
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Consider the titration of 40.0 mL of 0.200 mol/L HCOONa (aq) with 0.300 mol/L HCl (aq). Ka for HCOOH is 1.8×10⁻⁴. Given: Kb = [x][x] / [0.200 - x] Based on your ICE table and Kb expression, determine the [OH⁻] in the solution.
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