Calculate the pH of 50.0 mL of 0.250 M oxalic acid (HOOCCOOH) upon addition of 31.9 mL of 0.500 M NaOH. Round your calculated value for pH to two figures to the right of the decimal point. Significant constants: Ka1 of oxalic acid = 5.60 x 10-2 and Ka2 of oxalic acid = 5.42 x 10-5
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.
pH calculation after the first equivalence point:
Calculate the pH of 50.0 mL of 0.250 M oxalic acid (HOOCCOOH) upon addition of 31.9 mL of 0.500 M NaOH. Round your calculated value for pH to two figures to the right of the decimal point. Significant constants: Ka1 of oxalic acid = 5.60 x 10-2 and Ka2 of oxalic acid = 5.42 x 10-5
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