Hypothesis:
The exposure of air would not affect the amount of iron(II) ions as there is a protective layer which is mainly used to protect the tablet from moisture and bacteria. It could be oxidized from oxygen within air, which could cause a loss in Fe(II) ions as it gets oxidized, but it would not affect the loss greatly due to the protective layer.
Introduction
Iron tablets have been mainly used to help people with a deficiency iron within their blood as it can restore missing iron needed. Iron tablets tend to contain the compound Iron(II) sulfate which will oxidize to Iron(III) sulfate if left alone in air. However, iron tablets act as a form of medicine and doctors would always say to never leave medication anywhere wet, dirty, or left to be exposed outside the
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Take 5 tablets and place them in a conical flask with 50 cm3 of
1 mol dm-3 of sulfuric acid and place a stopper to cover block the top. Mix the solutions around by shacking it to try to get the tablets to dissolve faster.
Note: This is a slow process due to the protective layer around the tablet which prevents the tablet from being soluble in water so it takes a while to break it down. It should take at least a day, but after a day shake the contents again to try to get all the substance to react.
3. Using a filter funnel and filter paper inside, filter the acidic iron sulfate solution into a 100 cm3 volumetric flask and use a distilled water bottle to force any of the remaining solution out of the residue.
Note: When leaving pouring the solution into the filter paper, take a bit of caution as the residue is quite thick and the solution will drip down slowly and if poured too fast it could overflow and spill.
4. Add sulfuric acid until it reaches the mark, and place the cap on and shake it a bit, to mix everything together.
Note: Make sure everything is fully mixed and careful when pouring the sulfuric acid in to fill the mark. Use a pipette to get it in drop by drop so be safe and
Use a stopwatch or timer to determine the amount of time it takes for the tablet to completely stop fizzing out or until it completely stops dissolving.
Iron is naturally iron oxide and purified iron rapidly returns to a similar state when exposed to air and water. This whole process can be seen below in figure 3 – ‘The corrosion
Place a clean, dry 125 mL Erlenmeyer flask on balance, and slowly dispense liquid bleach until there is about .5 g. Record the mass of bleach, and add 25 mL of de-ionized water and about 2 g of KI. Swirl contents until the KI dissolves. Then add 3 drops of 1 M H2SO4, mix, and let stand for 1 or 2 minutes.
After the rinses, close the stopcock and fill the buret up to the 0.00mL line with NaOH. Quickly, open the stopcock to fill the tip of the buret and then close the stopcock. Record the initial volume of the NaOH to the nearest 0.01mL.
Switch to a solution of 1 part water to 1 part ammonia or 1 part water to 1 part hydrogen peroxide....
It is primarily excreted unchanged in the urine and has half life of 10 to 31 hours.
Note to environmentalists: The sulfuric acid was completely neutralized and properly discarded. Credits I would like to thank all the people who helped me with this project. I would especially like to thank my mother, for letting my go through an abundance of Baking Soda, Vinegar, and many of our other household items. I would like to thank my Father for helping me understand the science of this project, and my whole family for helping me do well. I'd also like to give credit to the following Brands of substances I used: Arm & Hammer Drano Revco Aspirin Mylanta Seaway And any other products I may have used along the way.
Iron is called a trace mineral, but its effects are mighty. We need it to produce hemoglobin, the oxygen carrier in red blood cells that brings oxygen to the rest of the body. Iron is also needed to produce myoglobin, the oxygen reservoir in the muscle cells.
Use glassware as directed by your instructor. Place a test tube placed inside a beaker with ice water to collect the product from the apparatus. Obtain the 10mL round bottom flask from the apparatus. Obtain two graduated cylinders of 10mL. On one graduated cylinder measure 4mL (85% H3PO4) of Phosphoric Acid and pour into the 10mL round bottom flask. On the other graduated cylinder measure 3mL of Cyclohexanol and pour into the flask as well. With a pipet add 5 drops of Sulfuric Acid (H2SO4) into the flask. Attach the round bottom flask to the distillation apparatus. Place thermometer with rubber stopper on the apparatus to obtain the temperature Start with the water flow through the condenser. Turn on and heat the reaction until the product starts to distill. Distill and collect until thermometer temperature rises to 85˚C. Once there is no more product to collect obtain the test tube of product. Two layers should be formed, top layer of cyclohexane and bottom layer with water. Obtain a pipette and remove the bottom layer (water) if any. Add 10% (5mL) of Sodium Bicarbonate (NaHCO3) to nuclearize any acid in the solution. Mix well and remove once again the bottom layer of water with pipette. Add 5mL of water and mix well to wash the top layer. After the two layers form again, remove entirely the bottom layer of water and add a few pellets of Calcium Chloride. Obtain a 50mL or 100mL beaker and weigh.
9. Get your stopwatch ready and drop the Alka-Seltzer tablet at the same time you started the timer. 10. When it finishes dissolving (you can see through the water and there is no more fizzing.) stop the timer and record the results. 11.
For this experiment we have to use physical methods to separate the reaction mixture from the liquid. The physical methods that were used are filtration and evaporation. Filtration is the separation of a solid from a liquid by passing the liquid through a porous material, such as filter paper. Evaporation is when you place the residue and the damp filter paper into a drying oven to draw moisture from it by heating it and leaving only the dry solid portion behind (Lab Guide pg. 33.).
Once the mixture had been completely dissolved, the solution was transferred to a separatory funnel. The solution was then extracted twice using 5.0 mL of 1 M
Pure iron has a hardness that ranges from 4 to 5. It is soft and ductile. Iron can be easily magnetized at ordinary temperatures and at 790°C the magnetic property disappears. Pure iron melts at about 1535°C, boils at 2750°C, and has a specific gravity of 7.86. Chemically, iron is an active metal. When exposed to humid air, iron forms a reddish-brown, flaky, decay known as rust.
2nd step heat the mixture: Make sure the agarose dissolves. Wait until it boils and when you are going to transfer the mixture, wear gloves to avoid getting burnt. Transfer the mixture into a removable gel tray.
I left the HCl alone, for the 1.5M solution I put 75 cm3 of HCl and 25