Sketch the titration curve for the tirtation of (0.10M) HCl vs 25.0mL (0.50M) NaOH
To sketch the titration curve for the titration of HCl with NaOH, we need to understand the reaction that takes place. In this case, HCl (hydrochloric acid) reacts with NaOH (sodium hydroxide) to form water (H2O) and NaCl (sodium chloride) according to the balanced chemical equation:
HCl + NaOH -> H2O + NaCl
The titration curve represents the change in pH of the solution as NaOH is slowly added to HCl. To understand how the pH changes during titration, we need to consider the stoichiometry of the reaction and the dissociation of HCl.
1. Before the titration starts:
- The initial pH of HCl is low since it is a strong acid.
- Both the HCl and NaOH solutions have different concentrations, so we need to calculate the moles of HCl and NaOH present.
2. Initial stage:
- At the beginning of the titration, before any NaOH is added, the pH remains low due to the presence of excess HCl.
3. During titration:
- As NaOH is added to the HCl solution, it reacts according to the balanced chemical equation.
- The pH starts to rise gradually since NaOH is a strong base and reacts with the acidic HCl.
- Initially, the pH changes slowly because the added NaOH reacts with the excess HCl until it is completely neutralized.
- Once all the HCl is neutralized, the pH rapidly increases since any additional NaOH will now contribute to increasing the pH.
4. Equivalence point:
- The equivalence point is reached when stoichiometrically equal amounts of HCl and NaOH react with each other.
- At this point, all the HCl is completely neutralized, and the pH should be near neutral (pH 7).
- The volume of NaOH required to reach the equivalence point can be calculated using the equation: Moles of HCl = Moles of NaOH.
5. After the equivalence point:
- Any additional NaOH added after the equivalence point will cause the pH to increase significantly since the solution becomes basic due to excess NaOH.
To accurately sketch the titration curve, you would need to plot the pH on the y-axis and the volume of NaOH added on the x-axis. The pH gradually increases until it reaches the equivalence point, where it sharply increases and becomes relatively constant beyond that point.
Note: This explanation is based on the assumption that the reaction is taking place in water and there are no other factors influencing the titration curve.