Consider the following equilibrium occurring at 40°C: 2NO3 - (aq) + 9 H2O(l) + 2 Cr3+(aq) <---> Cr2O72-(aq) + 2NO(g) + 6 H3O+(aq) If a 1.5M solution of Cr(NO3)3 is allowed to react, what will be the pH of the final solution once equilibrium has been reached?
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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.
Consider the following equilibrium occurring at 40°C: 2NO3 - (aq) + 9 H2O(l) + 2 Cr3+(aq) <---> Cr2O72-(aq) + 2NO(g) + 6 H3O+(aq) If a 1.5M solution of Cr(NO3)3 is allowed to react, what will be the pH of the final solution once equilibrium has been reached?
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