HO -OH Oxalic Acid, H₂C₂O₁ PK₁₁ = 1.27 pka2 = 4.266 H₂Ox→ HOX → Ox ²- H₂A → HA → A²- pH = ? Adding 0.20 mole of NaOH to 0.40 mole of NaHC₂O4 (s) with total volume of 500 mL. pH = ? 150 g of NaHC₂O4 (s) dissolved in DI water total volume of 500 mL. pH = ? Adding 0.20 mole of HCI to 0.40 mole of NaHC₂O4 (s) with total volume of 500 mL. pH = ? 0.40 Adding 0.20 mole of HCI mole of Na₂C₂O4 (s) with total volume of 500 mL. pH = ? Adding 0.40 mole of HCI to 0.40 mole of Na₂C₂O4 (s) with total volume of 500 mL. pH = ? Important Key Concept Exercise
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.
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