what will be the pH of a buffer prepared by mixing 600 ml of 0.1M sodium acetate solution and 40 ml of 0.2M acetic acid solution

Use the Henderson-Hasselbalch equation.

To determine the pH of the buffer solution, we need to use the Henderson-Hasselbalch equation, which is defined as:

pH = pKa + log([A-]/[HA])

Where:
pH is the unknown pH value of the buffer solution.
pKa is the dissociation constant of the weak acid.
[A-] is the concentration of the weak conjugate base (acetate ion) in the buffer solution.
[HA] is the concentration of the weak acid (acetic acid) in the buffer solution.

To apply this equation, we first need to find the pKa value of acetic acid. The pKa value of acetic acid is approximately 4.76.

Next, we need to determine the concentrations of acetate ([A-]) and acetic acid ([HA]) in the buffer solution. To find the concentration, we use the formula:

Concentration (C) = (Molarity x Volume) / Total Volume

For sodium acetate:
C[A-] = (0.1 M x 600 mL) / (600 mL + 40 mL)

For acetic acid:
C[HA] = (0.2 M x 40 mL) / (600 mL + 40 mL)

Now, we can substitute the values into the Henderson-Hasselbalch equation:

pH = 4.76 + log((C[A-]) / (C[HA]))

Calculate [A-] and [HA], and then substitute them into the equation to find the pH of the buffer solution.