Calculate the pH of 0.1 M NaHC2O4. Your solution should involve a system of equations that simultaneously describes the dissociation of HC2O4- and formation of H+, H2C2O4, and C2O42-.
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.
Calculate the pH of 0.1 M NaHC2O4. Your solution should involve a system of equations that simultaneously describes the dissociation of HC2O4- and formation of H+, H2C2O4, and C2O42-.
![Oxalic acid (H₂C2O4) is a diprotic acid, meaning that a single H₂C2O4 molecule can dissociate twice following the equilibrium
reactions presented by Equations 2.1 to 2.2.
H₂C₂O4 (aq) → H¹+ (aq) + HC₂O4 (aq)
(2.1)
(2.2)
HC₂04 (aq) → H+ (aq) + C₂0² (aq)
The acid dissociation constants (equilibrium constants) of the reactions are K₁₁=5.4 x 10-² and K₁2 = 5.2 × 10-5,
respectively. The acid dissociation constants are related to the molar concentrations of each ion by Equations 2.3 and 2.4.
Ка1
[H*][HC,O4]
[H₂C₂04]
(2.3)
[H+][C₂0²-]
[HC₂04]
(2.4)
Kaz
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