Mount the buret on the ringstand and fill it above the zero mark with the prepared sodium hydroxide solution. Open the stopcock and allow the buret to drain until the liquid level is at zero. Make sure all the air bubbles are out of the tip of the buret. Read and record the intial buret reading to the 0.01mL. Place the 125mL flask containing the first KHP
By ways of decanting (using a class stirring rod to guide solution), pour the solution into the funnel until it is about half an inch from the top. The solution should be clear and colorless 8) Allow the flask to cool. While the flask and solution are cooling, wash the funnel and beaker with LOTS of tap water to remove all traces of KOH. Also throw away any carbon on the filter paper. 9) Once the solution is cool enough to touch, add 35mL of 3M H2SO4 (measured out in 50mL graduated cylinder) SLOWLY AND STIR CONSTANLY.
Once it started boiling the temperature was taken and it was 102 degrees Celsius. After the first results were recorded and beaker C was cleaned out and put away, beaker B (5 grams of salt) was placed onto the hot plate. As beaker b started boiling the temperature was recorded at 100.8 degrees Celsius. The results were then written, the beaker was cleaned out, and then put away. The
Based on the handbook, the color of the iodine should be violet black, which was one of the properties I observed. It is soluble in alcohol, mineral oil, and potassium iodide and insoluble in water. I obtained the same results although for some substances more iodine dissolved than others. This could have been because perhaps we used too big pieces of solid iodine. If there wasn’t enough solution to react with it then that would explain why we still had some left over that didn’t.
Add 3.0 mL of 1.0 M Copper (II) nitrate to the test tube. Add 5.0 mL of sodium hydroxide to the test tube; mix the reaction with a stirring rod. Feel the bottom of the tube and write down any changes you notice. Place test tube into the heated beaker and heat the tube until no changes are happening. Write down everything you notice.
Place a funnel on the top of the buret and slowly add 5g of dry alumina. When all of the alumina has been added, rinse the inside of the buret with additional petroleum ether to flush down any alumina that may be stuck to the sides. Add another 1-cm layer of dry clean sand on top of the alumina. Drain the solvent from the column until the solvent is at a level just above the top of the sand. The column is now ready for the addition of the mixture to be separated.
Next, obtain a 5 mL serological pipet and thoroughly rinse it with the buffer solution, then discard the buffer solution into the 250 mL beaker. Now, use the pipet to distribute 5 mL of the buffer solution into three 50 mL beakers. Be sure that the 50 mL beakers have been cleaned are dried prior to this. Next, locate the three pre filled burets in the lab room. Find the buret labeled 1.0M HCl and add exactly 1.00 mL of HCl to just one of the three 50 mL beakers with buffer solution already in them.
The average was 4.92 which is pretty close comparably to the standard. B. Why is it better to use white vinegar rather than dark vinegar for this titration? White vinegar is better to use due to the fact that it contains only acetic acid and water where other vinegars contain more chemicals. C. Write a balanced equation for the neutralization of acetic acid with NaOH.
Properties of Water Lab Part A. Observations: When Copper Chloride was mixed into water the Copper Chloride started as small crystals in the bottom and sides of the test tube, but once shaken they completely dissolved into the water. When Copper Chloride was dropped into the alcohol it seemed to clump together and sink to the bottom, when shaken lightly or even vigorously the crystals of Copper Chloride simply moved around but retreated back to the bottom of the test tube when left still, it did not mix at all. Questions: 1. When Copper Chloride is added to water and shaken vigorously the copper Chloride completely dissolves leaving a pale transparent blue solution. 2.
The last two cations should be separated with the observations of the additional NH4OH added. With that all the cations are separated, a confirmation test was given to all the cations. 20 drops of each cation solution were placed in new centrifuge tubes. A Bunsen burner was set up with a sharp blue cone that was inside of the flame, then a Nichrome loop was dipped into HCl then dipped into one of the cation