hi, i am trying to develop a lab where i find the solubility of Sodium acetate. I was wondering in i was in the right path.

We are given these three compounds:
Acetic acid aka vinegar
baking soda (sodium hydrogen carbonate)
0.100mol/l Naoh(aq)
0.100/l HCL(aq)

So we are not given Sodium acetate so we have to first titrate NAOH with Acetic Acid which produces the sodium acetate and water. here is the equation.

Naoh + CH3COOH = CH3COONa + H2O

So i am going titrate acid(CH3COOH) to base (Naoh). How do i measure solubility of Acetic Acid( CH3COONa ) from that? check when it forms a precipitate?

Are you having a problem with the posting?

To measure the solubility of Sodium acetate (CH3COONa) from the titration of acetic acid (CH3COOH) with sodium hydroxide (NaOH), you would not look for the formation of a precipitate. Instead, you can determine the solubility by measuring the volume of NaOH needed to neutralize the acetic acid.

Here's a step-by-step procedure to determine the solubility of Sodium acetate:

1. Prepare a standard solution of NaOH by diluting the provided 0.100 mol/L NaOH to a known concentration. This can be done by diluting a known volume of the concentrated solution with a known volume of water. Make sure you accurately measure and record the final concentration of the diluted NaOH solution.

2. Prepare a solution of acetic acid (CH3COOH) by diluting the provided vinegar. You may need to determine the concentration of acetic acid in the vinegar using a known method (such as titration) or by checking the label if it provides the concentration.

3. Set up a burette with the standardized NaOH solution.

4. Take a known volume (e.g., 25 mL) of the diluted acetic acid solution in a flask and add a suitable indicator to detect the endpoint of the titration. Phenolphthalein is commonly used for acid-base titrations.

5. Slowly add NaOH solution from the burette into the flask while continuously stirring. The NaOH will react with the acetic acid, producing Sodium acetate and water.

6. As you approach the endpoint of the titration, the indicator will change color. The endpoint is reached when a permanent color change is observed, indicating neutralization. Record the volume of NaOH required to reach the endpoint.

7. Repeat the titration several times to obtain consistent results.

8. From the volume of NaOH used in the titration, you can calculate the moles of acetic acid that reacted. Since the stoichiometry of the reaction is 1:1, this will be the same as the moles of Sodium acetate formed.

9. If you know the initial volume and concentration of acetic acid, you can calculate the concentration of Sodium acetate in the final solution. From that, you can determine the solubility (in mol/L) of Sodium acetate.

By following this procedure, you can find the solubility of Sodium acetate in the solution after the titration of acetic acid with NaOH. Keep in mind that other factors, such as temperature and the presence of other solutes, may affect the solubility.