Henderson Hasselbalch

How do you calculate the pH of a buffer solution using the Henderson-Hasselbalch equation?

• pKa + log([weak acid]/[conjugate base])

• pKa - log([conjugate base]/[weak acid])

• pKa + log([conjugate base]/[weak acid])

• pKa - log([weak acid]/[conjugate base])

In the Henderson-Hasselbalch equation, what does the log of a number less than one indicate?

• A negative value

• A positive value

• A neutral value

• An undefined value

What happens to the pH of a buffer solution when the concentration of the weak acid is greater than the concentration of the conjugate base?

• The pH becomes neutral

• The pH remains the same

• The pH decreases

• The pH increases

What can be inferred if the pH of a buffer solution is greater than the pKa of the weak acid?

• The solution is not a buffer

• The concentrations of the weak acid and conjugate base are equal

• The concentration of the conjugate base is greater than the weak acid

• The concentration of the weak acid is greater than the conjugate base

What is the significance of a particulate diagram in understanding buffer solutions?

• It shows the exact number of particles in the solution

• It helps visualize the relative concentrations of components

• It determines the pH of the solution directly

• It identifies the strong acids and bases present

How many grams of NaOH must be added so that the resulting pH is 5.50? (hint: use algebra starting from the Henderson-Hasselbalch Equation)

• 1.26

• 5.24

• 7.63

• 9.64

What is the Henderson-Hasselbalch equation used for?

• Calculating the pH of a strong acid solution

• Calculating the pH of a buffer solution

• Calculating the concentration of a solute in a solution

• Calculating the boiling point of a solution

• 4.74

• 7.00

• 3.00

• 5.00

A buffer is most effective when:

• The pH is equal to 7

• The concentrations of the acid and its conjugate base are equal

• The solution is diluted

• The solution is heated

• 9.26

• 8.74

• 10.74

• 7.00