I was told to find the concentration of acetic acid in vinegar when only using baking soda and common lab equipment. Can someone tell me how
Thanks
I wonder how "common lab equipment" is defined. I wonder how accurately this is to be done.
Does that mean we can't use any other chemical?
I would prepare a 0.1M baking soda solution (NaHCO3) and fill a buret. Add phenolphthalein indicator, then add NaHCO3 from buret until the indicator turned. Calculate M acetic acid.
Well I asked about using phenolphthalein and my teacher said that it was not a good idea. But when I was looking online, I saw some experiments using the amount of gas produced to find the amount of acetic acid in a 20Ml of vinegar in g/ml
If you could tell me how this this done, that would be a massive help.
Also, I tried another way in which I reacted baking soda and vinegar, then put the products on a hot plate to evaporate the H2O so I was only left with the sodium acetate. After that, I calculated how much HCl I would need to react it and put in that amount of HCl so I now have a a solution of acetic acid and NaCl. the problem now is that I don't know how to isolate the acetic acid.
If you are able to tell me how they figured out the g/ml of acetic acid in vinegar by measuring the amount of gas produced of tell me how you can isolate the acetic acid from NaCl you would be a HUGE help.
Thanks
To find the concentration of acetic acid in vinegar using baking soda and common lab equipment, you can perform a simple acid-base titration. Here's a step-by-step guide on how to do it:
1. Start by obtaining the necessary equipment:
- Vinegar sample (the one you want to analyze)
- Baking soda (sodium bicarbonate)
- Distilled water
- Burette (or a graduated pipette)
- Beaker or Erlenmeyer flask
- pH indicator (phenolphthalein is commonly used)
- Balance (to weigh baking soda)
2. Prepare a standard sodium bicarbonate solution:
- Weigh a calculated amount of baking soda accurately (e.g., 0.5 grams).
- Dissolve the baking soda in a known volume of distilled water to make a solution (e.g., 500 mL). This will be your standard solution.
3. Perform the titration:
- Transfer a fixed volume of vinegar (e.g., 25 mL) into the beaker or Erlenmeyer flask.
- Add a few drops of the pH indicator, such as phenolphthalein, to the vinegar sample.
- Slowly titrate the vinegar with the standard sodium bicarbonate solution from the burette or using a graduated pipette. The sodium bicarbonate will react with the acetic acid in vinegar, forming carbon dioxide gas, water, and sodium acetate.
- Continue the titration until the endpoint is reached, which is typically when the color of the indicator changes. In the case of phenolphthalein, it will usually turn from colorless to pink when all the acetic acid is neutralized.
- Record the volume of the sodium bicarbonate solution required to reach the endpoint.
4. Calculate the concentration of acetic acid:
- Use the balanced chemical equation for the reaction between acetic acid (CH3COOH) and sodium bicarbonate (NaHCO3) to determine the mole ratio between the two substances.
- Calculate the moles of sodium bicarbonate used in the titration based on the volume and concentration of the standard solution.
- From the mole ratio, determine the moles of acetic acid present in the vinegar titrated.
- Finally, divide the moles of acetic acid obtained by the volume of vinegar used in the titration to calculate the concentration of acetic acid in the vinegar.
It's important to note that this is a simplified explanation, and actual experimental details may vary based on factors such as the specific equipment and reagents available.