An analytical chemist is titrating 130.0 mL of a 0.7300M solution of ammonia (NH,) with a 0.4800M solution of HNO3. The pK, of ammonia is 4.74. Calculate the pH of the base solution after the chemist has added 82.8 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH- X 5
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
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
![**Calculating the pH of a Weak Base Titrated with a Strong Acid**
An analytical chemist is titrating 130.0 mL of a 0.7300 M solution of ammonia (NH₃) with a 0.4800 M solution of HNO₃. The \( pK_b \) of ammonia is 4.74. Calculate the pH of the base solution after the chemist has added 82.8 mL of the HNO₃ solution to it.
*Note for advanced students*: You may assume the final volume equals the initial volume of the solution plus the volume of HNO₃ solution added.
Round your answer to 2 decimal places.
**pH = [Input Box]**
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