Ka1, Ka2 and Ka3 are the respective ionization constants for the following reactions (a),(b), and (c).
(a) H2C2O4⇌H++HC2O4−
(b) HC2O4−⇌H++HC2O42−
(c) H2C2O4⇌2H++C2O42−
The relationship between Ka1,Ka2 and Ka3 is given as
(a) H2C2O4⇌H++HC2O4−
(b) HC2O4−⇌H++HC2O42−
(c) H2C2O4⇌2H++C2O42−
The relationship between Ka1,Ka2 and Ka3 is given as
Ka3=Ka1+Ka2
Ka3=Ka1−Ka2
Ka3=\(\frac{Ka_1}{Ka_2}\)
Ka3=Ka1×Ka2
The Correct Option is D
Solution and Explanation
H2C2O4⇌H++HC2O4− Ka1
H2C2O4−⇌H++C242− Ka2
H2C2O4⇌2H++C2O42− Ka2 
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Concepts Used:
Ionic Equilibrium
In Ionic equilibrium, the ionic substance dissociates into its ions in polar solvents. The ions formed are always in equilibrium with their undissociated solute in the solution.
⇒ Representation of Ionic Equilibrium: Xa Yb ⇌ aXb+ + bYa-
Reactants and products coexist in equilibrium so that reactant conversion to product is always less than 100%. Equilibrium reactions may involve the decomposition of a covalent (non-polar) reactant or ionization of ionic compounds into their ions in polar solvents.
In this section, we will learn about the ionic equilibrium in ionic solutions. Substances in Ionic Equilibrium can be classified into two categories on the basis of their ability to conduct electricity given as under,
Non-Electrolytes:
These are substances that consist of molecules that bear no electric charge, do not dissociate into their constituent ions and thus do not conduct electricity in their aqueous solution or molten state. For example sugar solution.
Electrolytes:
These are substances that dissociate into their constituent ions in their aqueous solution and thus conduct electricity in their aqueous solutions or molten state. For example, salt solution, acid solution, base solution etc.