0.1 mL of 1.0 M Cd(NO3)2 is added to 1.0 L of 0.5 M NH3. Relevant equilibria in the solution are: Cd(OH) 2 (s) ⇌ Cd 2+ (aq) + 2OH- (aq) Ksp = 5.9 x 10-15 Cd 2+ (aq) + 4NH 3 (aq) ⇌ Cd(NH3) 4 2+ Kf = = 1.0 x 107 NH 3 (aq) + H 2 O ⇌ NH 4+ + OH- Kb = 1.8 x 10-5 a) What is [OH-] in the ammonia solution (before addition of cadmium nitrate). What is the concentration of NH3 considering that by 0.5 M NH3 solution is meant the sum of the concentrations of NH3 and NH4+? b) Will the OH concentration change significantly when you add to the solution that contains Cd(NO3)2. A good justification in words is enough. c) Calculate the equilibrium constant for the reaction where Cd(OH)2(s) is converted to Cd(NH3) 42+
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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.
0.1 mL of 1.0 M Cd(NO3)2 is added to 1.0 L of 0.5 M NH3. Relevant equilibria in the solution are:
Cd(OH) 2 (s) ⇌ Cd 2+ (aq) + 2OH- (aq) Ksp = 5.9 x 10-15
Cd 2+ (aq) + 4NH 3 (aq) ⇌ Cd(NH3) 4 2+ Kf = = 1.0 x 107
NH 3 (aq) + H 2 O ⇌ NH 4+ + OH- Kb = 1.8 x 10-5
a) What is [OH-] in the ammonia solution (before addition of cadmium nitrate). What is
the concentration of NH3 considering that by 0.5 M NH3 solution is meant
the sum of the concentrations of NH3 and NH4+?
b) Will the OH concentration change significantly when you add to the solution that
contains Cd(NO3)2. A good justification in words is enough.
c) Calculate the equilibrium constant for the reaction where Cd(OH)2(s) is converted to
Cd(NH3) 42+
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