Formic acid dissociates reversibly according to the following equation. \HCOOH(aq) ⇌ HCOO-(aq) + H+(aq)Write the law of mass action for this equilibrium.K = Is the equilibrium constant in (a) a Ka? Briefly explain.If a solution is initially 0.20 mol/L HCOOH and the equilibrium constant in (a) is 1.8 × 10-4, what is the concentration of hydrogen ions at equilibrium? Show your work. Use the value obtained in (c) to find the solution’s pH and pOH at 25 °C. If you were unable to complete (c), you may assume a 0.0030 mol/L concentration of hydrogen ions.Would the addition of sodium formate (NaHCOO) to this solution increase pH? Explain.

There are two types of bases/acids. One is strong base/acid which is completely dissociable in into…

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Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.87QE

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Formic acid dissociates reversibly according to the following equation. \

HCOOH(aq) ⇌ HCOO^-(aq) + H⁺(aq)

Write the law of mass action for this equilibrium.

K =
Is the equilibrium constant in (a) a K_a? Briefly explain.
If a solution is initially 0.20 mol/L HCOOH and the equilibrium constant in (a) is 1.8 × 10^-4, what is the concentration of hydrogen ions at equilibrium? Show your work.

Use the value obtained in (c) to find the solution’s pH and pOH at 25 °C. If you were unable to complete (c), you may assume a 0.0030 mol/L concentration of hydrogen ions.

Would the addition of sodium formate (NaHCOO) to this solution increase pH? Explain.

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