Buffer Solutions and pH Concepts

The video tutorial covers the preparation and analysis of a buffer solution containing NH3 and H4 plus. It explains the pH change when 50 ml of 0.1 molar HCL is added, detailing the reaction between the acid and the base. The tutorial includes calculations of millimoles and pH, using the PKA value. It also discusses the analysis of a dry acid H2A with two PKAs and the concentration of species in a solution.

What is the primary purpose of a buffer solution?

• To neutralize all acids in a solution

• To maintain a stable pH in a solution

• To increase the acidity of a solution

• To increase the basicity of a solution

What happens to the pH of a buffer solution when a small amount of HCl is added?

• The pH increases significantly

• The pH decreases significantly

• The pH remains relatively stable

• The pH becomes neutral

Which component of the buffer reacts with HCl in the solution?

• NH3

• H3O+

• NH4+

• H2O

What is the result of the reaction between a weak base and a strong acid in a buffer solution?

• A reversible reaction

• A partial reaction

• A complete or quantitative reaction

• No reaction

How is the pH of a buffer solution calculated after the addition of an acid?

• Using the initial concentration of the base

• Using the initial concentration of the acid

• Using the Henderson-Hasselbalch equation

• Using the dilution factor

What does the pKa value indicate in a chemical solution?

• The strength of a base

• The temperature of the solution

• The concentration of the solution

• The strength of an acid

At a pH of 2.2, which species is predominant in a solution with pKa values of 3.6 and 4.5?

• H3O+

• A2-

• HA-

• H2A

What is the major species in a solution with a pH lower than its pKa1?

• The neutral form

• The protonated form

• The deprotonated form

• The ionic form

How do you determine the concentration of all species in a solution at a given pH?

• By diluting the solution

• By using the pKa values and the Henderson-Hasselbalch equation

• By measuring the temperature

• By adding more solvent

What is the concentration of H3O+ in a solution with a pH of 12?

• 0.1 M

• 1 M

• 10^-12 M

• 10^-2 M