3) Buffer C: 100.0 mL at pH = 12.000, [conj. base]: = 0.500 M %3D a) What conjugate pair should be chosen? Conjugate acid: Conjugate base: b) Calculate the molarity of the conjugate acid necessary to obtain the desired pH using the Henderson-Hasselbalch equation. Show the variable equation with specific species and Ka values.
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.
Part A B and C
We need to an acid whose pKa is close to 12. then we make a solution of the acid and its conjugate base.
The acid pKa colse to 12 are H3PO4 and ascorbic acid (H2C2H6O2)
pKa3 of H3PO4 = 12.32
pKa2 of H2C2H6O2 = 11.79
The solution of Na2HPO4 and NaOH can be used make buffer solution:
let the Buffer solution Na3PO4(PO4-3) and Na2HPO4(HPO4-2).
molar mass of Na3PO4 = 163.94 g/mol
molar mass of Na2HPO4 = 141.96 g/mol
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