You prepared the buffer by adding about 0.2 g of each of the weak acid and its conjugate base to 25.0 mL of water. The goal was

Answer:

To achieve the desired outcome, 8.55 mL of NaOH is necessary.

Explanation:

Considering that:

the weak acid has a mass of 0.4 g

and a molecular weight of 234 g/mol

so, the number of moles of the weak acid is calculated as 0.4 g/234 g/mol = 0.00171 mole

To convert half of the weak acid (WA) to conjugate base (CB), we must add NaOH.

Thus, [WA]=[CB] 0.00171/2 = 8.55×10⁻⁴ mole of NaOH required

Further, knowing that the concentration of NaOH is 0.10 M

the volume needed to achieve this result can be calculated as follows:

=

= 8.55 mL of NaOH is necessary