Repeat the procedure in Exercise \(67,\) but for the titration of 25.0 \(\mathrm{mL}\) of 0.100 \(\mathrm{M} \mathrm{HNO}_{3}\) with 0.100 $\mathrm{M} \mathrm{NaOH} .$

In this titration, a strong acid (HNO3) is reacted with a strong base (NaOH). The reaction that occurs during titration is as follows: \[ \mathrm{HNO_3} + \mathrm{NaOH} \rightarrow \mathrm{NaNO_3} + \mathrm{H_2O} \]

Before starting the titration, we need to find the initial moles of HNO3 and NaOH. We can use the given volumes and concentrations for this calculation. Moles of HNO3 = Concentration × Volume Moles of HNO3 = 0.100 M × 25.0 mL × (1 L/1000 mL) = 0.00250 mol

During the titration, the strong base (NaOH) is slowly added to the strong acid (HNO3). The moles of HNO3 and NaOH will react in a 1:1 ratio according to the balanced chemical equation. To find the equivalence point, which is when the moles of acid and base are equal, we need to calculate the volume of NaOH required for this to happen. Since both the acid and base have the same concentration (0.100 M), the volume of NaOH required for the equivalence point will be the same as the volume of HNO3, which is 25.0 mL.

The pH of the solution will change as the titration progresses. We can break down the titration process into three main stages: before the equivalence point, at the equivalence point, and after the equivalence point. 1. Before the equivalence point: At this stage, the unreacted HNO3 will contribute to the pH of the solution. Since HNO3 is a strong acid, it dissociates completely in water. \[ \mathrm{[H^+]} = \mathrm{concentration\:of\:HNO_3} \] Using the pH formula, where pH = -log([H+]), we can calculate the pH of the solution. 2. At the equivalence point: The moles of HNO3 and NaOH are equal at this point, meaning all the HNO3 has been neutralized. The solution consists of NaNO3 and H2O. Since NaNO3 is a neutral salt and does not contribute to the pH, the pH at the equivalence point will be 7. 3. After the equivalence point: At this stage, there is an excess of NaOH, which determines the pH of the solution. We can calculate the moles of remaining NaOH and use the formula pH = 14 - pOH to find the final pH. To calculate pOH, use the formula pOH = -log([OH−]), where [OH−] is the concentration of the hydroxide ion in the solution.

Once we have calculated the pH at different stages of titration, we can plot a titration curve, which shows the changes in pH as the titration progresses. The curve will have a steep rise in pH around the equivalence point and gradually level off before and after the equivalence point, indicating the changes in pH as the strong acid (HNO3) is neutralized by the strong base (NaOH).