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?

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.So i am going titrate acid(CH3COOH) to base (Naoh). here is the equation.

Naoh + CH3COOH = CH3COONa + H2O

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.So i am going titrate acid(CH3COOH) to base (Naoh). here is the equation.
Naoh + CH3COOH = CH3COONa + H2O

Three incomplete posts. All the same. What is your question?

To determine the solubility of sodium acetate (CH3COONa), titration may not be the best method because sodium acetate is a highly soluble salt. However, you can still follow a different approach to obtain an estimate of its solubility. Here's how you can do it:

1. Start by preparing a saturated solution of sodium acetate. This can be done by adding excess sodium acetate to a known volume of water. Continuously stir the solution until no more solid sodium acetate dissolves. This indicates that the solution is saturated.

2. Once the saturated solution is prepared, filter it to remove any undissolved particles. You will be left with a clear solution containing sodium acetate ions.

3. Take a small portion of the solution and place it aside in a separate container. This will serve as your "test tube."

4. Now, slowly heat the remaining saturated solution in a separate beaker or flask. As the temperature increases, the solubility of sodium acetate will also increase. Continue heating until no more sodium acetate can dissolve in the solution, and a precipitate starts to form. This is the point at which the solubility of sodium acetate is exceeded.

5. As soon as the precipitate forms, immediately stop heating and allow the solution to cool down slowly. This will allow the excess sodium acetate to crystallize out of the solution.

6. Observe the test tube containing the small portion of the original solution. If you see any additional precipitate forming in the test tube as the solution cools, it indicates that the solubility of sodium acetate has been exceeded.

7. Measure the mass of the precipitate formed in the test tube (if any) and calculate its solubility using the mass of sodium acetate used to prepare the saturated solution.

Keep in mind that this method provides an estimate of the solubility of sodium acetate and may not be as accurate as other commonly used techniques. Nonetheless, it can give you a rough idea of the solubility under the given conditions.