The acid dissociation Ka of acetic acid HCH3CO2 is ×1.810−5. Calculate the pH of a ×6.610−1M aqueous solution of acetic acid. Round your answer to 2 decimal places.
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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.
The acid dissociation Ka of acetic acid HCH3CO2 is ×1.810−5. Calculate the pH of a ×6.610−1M aqueous solution of acetic acid. Round your answer to 2 decimal places.
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