Calculate the pH and the equilibrium concentrations of H₂PO4, HPO42- and PO4³- in a 0.0960 M aqueous phosphoric acid solution. For H3PO4, Ka1 = 7.5x10-3, Ka2 = 6.2x10-8, and Ka3 = 3.6x10-13 pH = [H₂PO4] = [HPO4²-] = [PO4³-] = 3 M M
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.
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Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
![Calculate the pH and the equilibrium concentrations of H₂PO4, HPO42- and PO4³- in a 0.0960 M
aqueous phosphoric acid solution.
For H3PO4, Ka1 = 7.5x10-3, Ka2 = 6.2x10-8, and Ka3 = 3.6x10-13
pH =
[H₂PO4] =
[HPO4²-] =
[PO4³-] =
3
M
M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9aca1772-1e0c-4e24-86a8-736d39b6760d%2Fa170c0f7-861b-4315-8c2e-aca4345d3b9a%2F2vyea4m_processed.jpeg&w=3840&q=75)
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