Reaction 2: Bicarbonate (acting as an acid) reacts with water (acting as a base). HCO3 + H₂O = acid base Reaction 1 is more favorable. Reaction 2 is more favorable. Key Which statement correctly describes the relative favorability of these reactions in an aqueous solution of bicarbonate? Both reactions are equally favorable. Favorability cannot be determined. =
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.
![This
example demonstrates how pk, can be used to help determine the favorability of a reaction.
Keq is the equilibrium constant and is usually referred to as K₁ in acid-base reactions. Given the pK, of an acid, you can
calculate K by taking its antilog.
Species
H₂O
HCO3
H₂CO3
H₂O+
HCO3 + H₂O =
base
acid
pK₁
15.74
10.33
6.35
-1.74
Complete the balanced equations for the equilibria given in reaction 1 and reaction 2. Then use the pK₂ values in the table to
calculate Keq for each reaction, where the Keq expression includes [H₂O]. Be sure to enter Keq in proper scientific notation.
Reaction 1: Bicarbonate (acting as a base) reacts with water (acting as an acid).
Kca
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