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?

The equation is

NaOH + CH3COOH ==> CH3COONa + H2O

Now, what is your question?

soorry i was writing the equation but computer went weird on me. So i titrate acid ( ch3cooh) to base ( naoh) and get sodium acetate ch3coohna but how do i measure solubility of sodium acetate? do i wait just until a precipitate forms at equilibrium(saturation)?

You need to let us know more about the procedure. Titration alone will not tell you the solubility. If you are using an indicator to show the end point of the titration, then molarity of NaOH*volume NaOH will be the mols CH3COONa formed and you can find the grams CH3COONa from that. But whether that dissolves or not depends upon the amount of water in the titration vessel.

Yes, you are on the right track! To determine the solubility of Sodium acetate, you can start by conducting a titration between Acetic acid (vinegar) and Sodium hydroxide (NaOH). The reaction between acetic acid and sodium hydroxide will produce sodium acetate and water.

Here is the balanced equation for this reaction:
CH3COOH (acetic acid) + NaOH (sodium hydroxide) → CH3COONa (sodium acetate) + H2O

To perform the titration, follow these steps:

1. Prepare a standard solution of NaOH by measuring out 0.100 mol/L NaOH solution. This will serve as the titrant.
2. Add a measured quantity (let's say, 'x' mL) of acetic acid (vinegar) into a flask. Use an indicator, such as phenolphthalein, to track the endpoint of the reaction.
3. Start adding the NaOH solution slowly into the flask with the acetic acid, while stirring continuously.
4. The NaOH solution will react with acetic acid until the endpoint is reached. The endpoint is when the indicator changes color, indicating that all the acetic acid has reacted with the NaOH.
5. Record the volume of NaOH solution, 'y' mL, that was required to reach the endpoint.

Now, using the volume of NaOH solution required to neutralize the acetic acid, you can calculate the concentration of sodium acetate that was formed:

Moles of NaOH used = concentration of NaOH (mol/L) × volume of NaOH (L)
Moles of NaOH used = 0.100 mol/L × y mL × 0.001 L/mL

Since the balanced equation tells us the stoichiometry between acetic acid and sodium acetate, we know that the moles of NaOH used are equal to the moles of sodium acetate formed.

Therefore, the concentration of sodium acetate (solubility) in the final solution is given by:

Concentration of sodium acetate = Moles of NaOH used / Volume of acetic acid (L)
Concentration of sodium acetate = (0.100 mol/L × y mL × 0.001 L/mL) / (x mL × 0.001 L/mL)

By calculating the concentration of sodium acetate, you can determine its solubility in the solution.