What is the approximate concentration of free Ag+ ion at equilibrium when 1.79x10-2 mol silver nitrate is added to 1.00 L of solution that is 1.100 M in S₂03²-. For [Ag (S₂03)₂]³-, K₁= 2.9x10¹³ [Ag+] = M
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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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![**Question:**
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What is the approximate concentration of free Ag\(^+\) ion at equilibrium when 1.79 x 10\(^{-2}\) mol silver nitrate is added to 1.00 L of solution that is 1.100 M in S\(_2\)O\(_3^{2-}\). For [Ag(S\(_2\)O\(_3\))\(_2\)]\(^{3-}\), K\(_f\) = 2.9 x 10\(^{13}\).
\[[\text{Ag}^+] =\] \_\_\_\_\_\_ M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9d65d074-1570-4831-8dec-170f6bb6e3ab%2F25fb9468-0985-49be-8384-1e81709edd4c%2Fe23mlxi_processed.jpeg&w=3840&q=75)
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