What is the correct relationship between Ka and Kb for a weak acid and its conjugate base (temperature = 25 oC)? a. Ka × Kb = 1014 b. Ka × Kb = 1.0 × 10−14 c. Ka / Kb = 1.0 d. Ka / Kb = 1.0 × 10−1
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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.
What is the correct relationship between Ka and Kb for a weak acid and its conjugate base (temperature = 25 oC)?
| a. |
Ka × Kb = 1014 |
|
| b. |
Ka × Kb = 1.0 × 10−14 |
|
| c. |
Ka / Kb = 1.0 |
|
| d. |
Ka / Kb = 1.0 × 10−1 |
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