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.
Strong acids and strong bases ionize 100% in aqueous solution.
- HCl is a strong acid. In solution we write it as H+(aq) + Cl -(aq).
- HF is a weak acid. In solution we write it as HF(aq).
- KOH is a strong base. In solution we write it as K+(aq) + OH -(aq).
- NH3 is a weak base. In solution we write it as NH3(aq).
Exception: Since Ca(OH)2 is only slightly soluble we write it as Ca(OH)2(s).
Below is a list of the 6 strong acids and 6 strong bases you should know. All other acids and bases are considered weak.
| Strong Acids | Strong Bases |
| HCl, HBr, HI | LiOH, NaOH, KOH |
| HNO3 | Ca(OH)2 (slightly soluble) |
| HClO4 | Ba(OH)2 |
| H2SO4 | Sr(OH)2 |
Question 1)
What is the hydronium ion concentration in an aqueous hydrobromic acid solution that has a pOH of 10.200?
[H3O+] = M
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