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.
Polyprotic acid Titration.
Consider the titration of 50.00 mL of a solution that is 0.0800 M oxalic acid. Calculate the pH after addition of 1.00 mL, 20.00 mL, and 21.00 ml of 0.2000 M KOH.
Note: This has two equivalence regions.
Ka1 = 5.4 x 10-2
Ka2 = 5.4 x 10-5
| KOH volume added (mL) | pH | H+ | OH | [H2A] | [HA-] | [A2-] |
| 1.00 (first pre-equivalence point) | ||||||
| 20.00 (first equivalence point) | ||||||
| 21.00 (second pre-equivalence point) |
Formula:
First Pre -Equivalence
H2A = MH2AVH2A - MOHVOH/ Vtotal
HA- = MOHVOH/Vtotal
pH = pKa1 + log [HA-]/[H2A]
First equivalence point
HA- = MH2AVH2A/Vtotal
H+ = √Ka1Ka2[HA-] + Ka1Kw/Ka1+ [HA-]
Second pre-equivalence point
HA- = MH2AVH2A - MOHVOH/ Vtotal
A2- = MOH(VOH-Veq1)/Vtotal
pH = pKa2+ log [A2-]/{HA-]
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