On the axis below, draw the titration curve for the titration of CH3COOH (a weak acid) with NaOH (a strong base). In the titration, the equivalence point occurs when 40 mL of NaOH has been added. Make sure to label your x- and y-axis and put numbers on your grid. Make sure your diagram starts at a reasonable pH and ends at a reasonable pH. Label the equivalence point at the correct pH and volume of NaOH.
To draw the titration curve for the titration of CH3COOH (acetic acid) with NaOH (sodium hydroxide), we need to understand the pH changes that occur during this chemical reaction. Here is how you can plot the titration curve:
1. Label the x-axis as the volume of NaOH (in mL) added and the y-axis as the pH.
2. Determine the initial pH of acetic acid (CH3COOH) before any NaOH is added. Since CH3COOH is a weak acid, its initial pH will be less than 7 but greater than 0. Let's assume it is approximately 2.5.
3. Start by plotting this initial pH on the graph at zero volume of NaOH added (0 mL).
4. At the beginning of the titration, the pH will be influenced by the excess acetic acid. As the NaOH is added, it will react with the acetic acid to form sodium acetate and water.
5. Determine the volume of NaOH (in mL) at which the equivalence point is reached. In this case, it is given as 40 mL of NaOH.
6. At the equivalence point, the moles of NaOH added will be stoichiometrically equal to the moles of acetic acid. This means that the acetic acid will be completely neutralized, resulting in a solution of only sodium acetate. At this point, the pH will be closer to neutral, around 7.
7. Plot the equivalence point on the graph by marking 40 mL on the x-axis and the corresponding pH value.
8. Before reaching the equivalence point, the pH will gradually increase as more NaOH is added. After the equivalence point, the pH change will be less significant.
9. Continue the curve until you reach a reasonable pH, which is often around 12 for the titration of a weak acid with a strong base.
10. Connect the plotted points smoothly to create the titration curve.
Remember, the shape of the titration curve will depend on the dissociation constant (Ka) of acetic acid and the concentration of both the acid and base solutions. These values were not provided in the question, so the exact curve would require further calculations. However, the general trend described above will give you a reasonable approximation of the titration curve for this specific case.