Q3 Calculate the pH after 0.020 mol of HCl is added to 1.00L ofa) 0.100 M propionic acid (HC3H502, K₁= 1.3x10-5)b) 0.100 M sodium propanoate (NaC3H5O₂)c) 0.100 M HONH₂ (K=1.1x10-8)d) 0.100 M KOH

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Q3 Calculate the pH after 0.020 mol of HCl is added to 1.00L of a) 0.100 M propionic acid (HC3H5O2, K₁= 1.3x10-5) b) 0.100 M sodium propanoate (NaC3H5O₂) c) 0.100 M HONH₂ (Kb-1.1x10-8) d) 0.100 M KOH

Q3 Calculate the pH after 0.020 mol of HCl is added to 1.00L of a) 0.100 M propionic acid (HC3H5O2, K₁= 1.3x10-5) b) 0.100 M sodium propanoate (NaC3H5O₂) c) 0.100 M HONH₂ (Kb-1.1x10-8) d) 0.100 M KOH

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 30QRT

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Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

Q3 Calculate the pH after 0.020 mol of HCl is added to 1.00L of
a) 0.100 M propionic acid (HC3H502, K₁= 1.3x10-5)
b) 0.100 M sodium propanoate (NaC3H5O₂)
c) 0.100 M HONH₂ (K=1.1x10-8)
d) 0.100 M KOH

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