Buffer Solutions and pH Changes

This video tutorial explains the reactions and calculations involved in adding a strong base, such as sodium hydroxide, to a buffer solution. It covers the reaction mechanism, the use of change tables, and the calculation of pH in buffer solutions. The tutorial also includes practice problems and explores base buffer solutions using the Henderson-Hasselbalch equation.

What is the main purpose of adding sodium hydroxide to a buffer solution in this experiment?

• To neutralize the buffer solution

• To increase the acidity of the solution

• To demonstrate the reaction with acetic acid

• To decrease the volume of the solution

Which ions are considered spectators in the reaction between sodium hydroxide and acetic acid?

• Sodium ions

• Hydrogen ions

• Hydroxide ions

• Acetate ions

What is the net result of the reaction between sodium hydroxide and acetic acid?

• Formation of sodium acetate and water

• No reaction occurs

• Formation of acetic acid and sodium hydroxide

• Formation of hydrogen gas

Why is a change table used in the calculation of pH after adding a strong base?

• To determine the initial concentration of reactants

• To identify the limiting reactant and calculate changes

• To calculate the volume of the solution

• To measure the temperature change

What happens to the pH of a buffer solution when a strong base is added?

• The pH becomes neutral

• The pH decreases significantly

• The pH remains constant

• The pH increases slightly

What is the effect of adding a large amount of strong acid to a buffer solution?

• The buffer solution loses its buffering capacity

• The buffer solution remains unchanged

• The buffer solution becomes more basic

• The buffer solution becomes more acidic

When a strong acid is added to a buffer, which component dictates the pH?

• The conjugate base

• The strong acid

• The water formed

• The weak acid

How is the pKa of a weak base calculated from its Kb?

• By adding Kb to Kw

• By dividing Kw by Kb

• By taking the negative log of Kb

• By multiplying Kb with Kw

What equation is used to calculate the pH of a base buffer solution?

• Henderson-Hasselbalch equation

• Arrhenius equation

• Boyle's law

• Avogadro's law

Why is the pH of a base buffer solution expected to be higher?

• Because it contains a strong acid

• Because it contains a weak acid

• Because it contains a weak base

• Because it contains a strong base