From the equilibrium concentrations given, calculate Ka for each of the weak acids and Kb for each of the weak bases.(a) NH3: [OH−] = 3.1 × 10−3 M;[NH4+] = 3.1 × 10−3 M;[NH3] = 0.533 M;(b) HNO2: [H3 O+] = 0.011 M;[NO2−] = 0.0438 M;[HNO2] = 1.07 M;(c) (CH3)3N: [(CH3)3N] = 0.25 M;[(CH3)3NH+] = 4.3 × 10−3 M;[OH−] = 4.3 × 10−3 M;(d) NH4 + : [NH4 +] = 0.100 M;[NH3] = 7.5 × 10−6 M;[H3O+] = 7.5 × 10−6 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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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.
From the equilibrium concentrations given, calculate Ka for each of the weak acids and Kb for each of the weak bases.
(a) NH3: [OH−] = 3.1 × 10−3 M;
[NH4+] = 3.1 × 10−3 M;
[NH3] = 0.533 M;
(b) HNO2: [H3 O+] = 0.011 M;
[NO2−] = 0.0438 M;
[HNO2] = 1.07 M;
(c) (CH3)3N: [(CH3)3N] = 0.25 M;
[(CH3)3NH+] = 4.3 × 10−3 M;
[OH−] = 4.3 × 10−3 M;
(d) NH4 + : [NH4 +] = 0.100 M;
[NH3] = 7.5 × 10−6 M;
[H3O+] = 7.5 × 10−6 M
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