Calculate either [H,O*] or [OH-] for each of the solutions at 25 °C. Solution A: [OH-1 = 2.55 x 10-7 M Solution A: H,o*] = %3D Solution B: [H,O+] = 9.05 x 10-9 M Solution B: OH = %3D M Solution C: [H,o*] = 0.000677 M Solution C: OH %3D M Which of these solutions are basic at 25 °C? O Solution B: [H,O*] = 9.05 x 10-9 M Solution C: H,O+] = 0.000677 M %3D O Solution A: [OH = 2.55 x 10-7 M %3D
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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.
Calculate either [H3O+] or [OH−] for each of the solutions at 25 °C.
![Calculate either H,0+] or [OH| for each of the solutions at 25 °C.
Solution A: [OH- = 2.55 x 10-7 M
Solution A: [H,0*] =
%3D
%3D
M
Solution B: [H,O+] = 9.05 x 10-9 M
Solution B: [OH-] =
%3D
M
%3D
Solution C: H,0*| = 0.000677 M
Solution C: OH=
%3D
%3D
Which of these solutions are basic at 25 °C?
O Solution B: [H,O*] = 9.05 x 10-9 M
%3D
Solution C: [H,O+] = 0.000677 M
Solution A: [OH- = 2.55 x 10-7 M
%3D
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