Part A: Spectroscopy 1. 0.05g of Iron(III) Nitrate in a 50-ml beaker. Add 17 mL of distilled water to the beaker and mix with a stir rod until the solid is completely dissolved. 2. Obtain another 50-mL beaker and add 0.05g of Chromium(III) Nitrate to the beaker.
The reaction that occurred with this step was displacement and metathesis in the form of gas formation. The balanced equation of this step looks as follows: CuSO4aq+Zns→Cus+ZnSO4(aq) Once this step was finished, the remaining copper was retrieved. First, to recover the copper HCl was added to remove all the zinc. When this happened, a yellow tint was observed in the liquid, as well as bubbling as the zinc was broken down. Once the copper dried out, it was weighed and came to a total of 240 mg.
After that, dissolve the sample in 2 mL of deionized water and shake the test tube for 1 to 1 ½ minutes to dissolve the solid. Place another dry test tube in a 50mL beaker and weigh it. Find a bottle of barium iodide and record the name and molar mass. Then, weight out either anhydrous barium iodide or barium iodide dehydrate into this test tube and dissolve is it in 2 mL of deionized water. Pour the contents of one of the test tubes into the other and a reaction should occur and you should see a white precipitate of barium sulfate form.
In another flask 50-mL of ice water was deposited with three-drop phenolphthalein. Using a volumetric pipet 50-mL of the 1-bromopropane was added into the empty flask in the bath. By the same method 50-mL of potassium hydroxide was delivered to the same flask while swirling the contents and remaining in the water bath. A 10-mL aliquot was immediately removed from the mixture and added to the ice water containing the phenolphthalein. When the pipet was half emptied into the ice water a timer was started.
Procedure 1. Begin to prepare an EDTA solution. Weigh out 3.62-3.64 g of NaH2EDTA and record exact mass. Add the weighed amount to a 250 ml volumetric funnel carefully using a funnel Wash the funnel with water to ensure all of the solid is delivered to the flask Add 100-200 ml of water and mix. Enough water should be added so that the flask is full to the 250 ml mark Tightly wrap the top of the flask with a Parafilm when finished 2.
LAB 6 ANALYSIS OF WATER IN PHOSPHATE Name: Lab Partners: None Date of Experiment: November 13, 12 Location: My House Course Number: CHE111C21 Abstract: In this experiment, we used a simple colorimeter and Beer’s Law to find the concentration of a tap water sample. A Beer’s law calibration curved was drawn showing the absorbance of varying concentrations of phosphate. Phosphate solutions will produce standard colors when mixed with ammonium molybdate and stannous chloride. The concentration of the unknown solution containing phosphate will be determined using the calibration curve. A voltmeter was used to measure the electrical resistance of different solutions.
The MgSo4 absorbed the last traces of water the ether solution. The solution was completely dry when it appeared crystal clear and MgSO4 floated in the liquid, when swirled. If solution is cloudy, more drops of MgSO4 were to be added until solution was completely dropped. 5) We decanted the solution from the solid MgSO4 into a 50 or 100 ml round bottom flask. 6) The ether was removed using the rotary evaporator.
h) A way to make hard water softer is to put an sodium nitrate and create a precipitate to mellow out the reaction. Another way of making it softer is by removing the calcium ions one way of doing that is by boiling the solution to take out some of the ions. Conclusion: Overall, we determined that sodium carbonate, Na2CO3, is the anion that can be used to precipitate the most metal cations. Also, we learned that the anion sodium chloride, NaCl, could be used to remove silver ions from solutions. The stuff that I found interesting was that how many colours you can get when you mix the cations and anions