i'm having a hard time for my chemistry project an my topic on titration and my topic is to determine the mass percentage of iron in steel wool and i can not get as much information on the steps to follows how to create the titration and equipment needed etc.
please can you help me out??
I could help a lot more if you put your question in order. It runs on and on, has no punctuation marks, I can't tell where a sentence starts or ends. But I get the general idea. You want to determine iron in a sample. Look in your text or on the web. The Zimmerman-Reinhart procedure works well. Steel wool will go into solution much easier than iron ore; therefore, you won't have trouble dissolving the sample. Here is one site but there are others.
http://www40.homepage.villanova.edu/michael.spritzer/1502Expt7.htm
hey thanks for the help. well exactly the
main point of my question was that I'm doing a experiment in titration and my topic is to determine the percentage of iron in steel wool but i couldn't get procedures on how to carry out the experiment.
But if you have other ways to help me please on the experiment.. I will glad to take it..
Thank-you very much
Of course, I'd be happy to help you with your chemistry project on determining the mass percentage of iron in steel wool through titration. Here are the steps and equipment you need:
Materials and Equipment:
1. Steel wool sample
2. Dilute hydrochloric acid (HCl)
3. Potassium permanganate (KMnO4)
4. Dilute sulfuric acid (H2SO4)
5. Sodium oxalate (Na2C2O4)
6. Burette
7. Pipette
8. Conical flask
9. Stopwatch or timer
10. White tile or background
Step-by-step Procedure:
1. Begin by preparing your steel wool sample. Take a small amount of steel wool and cut it into small pieces.
2. Weigh an accurately measured mass of the steel wool using a digital balance.
3. Transfer the weighed steel wool into a conical flask.
4. Add dilute hydrochloric acid (HCl) to the flask to dissolve the iron present in the steel wool. The reaction is as follows:
Fe(s) + 2HCl(aq) → FeCl2(aq) + H2(g)
5. Make sure the reaction is allowed to proceed completely. This may take a few hours, depending on the amount of iron present.
6. After the reaction is complete, prepare a standardized solution of potassium permanganate (KMnO4).
7. Fill the burette with the standardized KMnO4 solution.
8. Use a pipette to transfer a measured volume of the steel wool solution from the conical flask into a separate flask.
9. Add dilute sulfuric acid (H2SO4) to the flask containing the transferred solution. This helps to acidify the solution and prevent any interference by other substances.
10. Titrate the transferred solution with the KMnO4 solution until a permanent color change occurs. The color changes from violet (KMnO4) to colorless.
11. Record the initial and final burette readings to determine the volume of KMnO4 solution required for the titration.
Calculation of the mass percentage of iron in steel wool:
1. From the balanced equation, determine the stoichiometry between KMnO4 and iron:
5FeCl2(aq) + KMnO4(aq) + 8HCl(aq) → 5FeCl3(aq) + MnCl2(aq) + KCl(aq) + 4H2O(l)
2. Use the volume and molarity of KMnO4 solution required in the titration to determine the moles of KMnO4 used.
3. Since the stoichiometry between KMnO4 and iron is known, you can convert the moles of KMnO4 to moles of iron.
4. Use the known mass and molar mass of the steel wool sample to determine the mass of iron present.
5. Finally, calculate the mass percentage of iron in the steel wool by dividing the mass of iron by the initial mass of the steel wool sample and multiplying by 100.
Remember to carefully document your procedure, data, and calculations, and ensure that you follow appropriate safety precautions while working with chemicals. Good luck with your project!