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: Ksp Mg3(PO4)2 = 5.2 * 10-24
Concnentration of Na3PO4= 0.25 M
To Calculate: Molar solubility of Mg3(PO4)2 in 0.25 M Na3PO4
Na3PO4 ionize as follows
Na3PO4 ---------> 3 Na+ + PO43-
So 0.25 M Na3PO4 will give 0.25 M PO43- ions.
Mg3(PO4)2 disociates as follows:
Mg3(PO4)2 <--------->3Mg2+ + 2PO43-
The solubility product constant, Ksp is the equilibrium constant for a solid substance dissolving in an aqueous solution.
For the given reaction Ksp = [3 Mg2+]3 [2PO43- ]2
Mg3(PO4)2 <--------->3Mg2+ + 2PO43-
3x 2x+0.25M
Ksp = [3 x]3 [2x+0.25]2
5.2 * 10-24 = [3 x]3 [2x+0.25]2
Since Ksp is small, so x will be small, we can neglect 2x in comparison to 0.25
So,
5.2 * 10-24 = [3 x]3 [0.25]2
5.2 * 10-24 = 1.6875 * x3
3.081 * 10-24 = x3
x =1.455 * 10-8
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