Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
Given data :
Molar concentraion of Formic Acid = 0.050 M .
Molar concentraion of Nitric Acid = 0.10 M .
Ka = 1.8 x 10-4
Formate ion concentration = ?
Explanation :
- HCOOH is a weak acid and HNO3 is a strong acid, the major species in solution are H+ and HCOO-.
- The problem asks for [HCOO-] , which is formed by ionization of HCOOH.
- Thus, the important equilibrium is The common ion in this problem is the hydrogen ion.
- Now we can calculate the initial and equilibrium concentrations of each species involved in this equilibrium.
- The equilibrium constant for the ionization of HCOOH =1.8 x 10-4
Substituting the equilibrium-constant concentrations into the equilibrium expression gives :
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