Complete the table below. Round each of your entries to 2 significant digits. You may assume the temperature is 25 °C. formula HSO4 conjugate acid NH Ka 0 0.012 5.6 x 10 - 10 conjugate base Kb formula CIO 3.3 × 10 0 0 -7 X x10
Ionic Equilibrium
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.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
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.
Completing the table below,
Conjugate acid conjugate base
| Formula | Ka | formula | Kb |
| ? | ? | ClO- | 3.3 × 10-7 |
| HSO4- | 0.012 | ? | ? |
| NH4+ | 5.6 × 10-10 | ? | ? |
Note:
Conjugate acid and conjugate base,
Conjugated acid base pair Can be define as the acid base pair which differ only by proton (H+).
• Acids after losing a proton (H+) forms a corresponding conjugate base.
Acid ➝conjugate base + H+
• Bases after gaining a proton forms corresponding conjugate acid
Base + H+➝ conjugate acid
• Relationship between Ka and Kb,
Ka × Kb = 10-14
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