Chem 2 Lab Report PDF

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Mini-Report: Galvanized Nails

Name: Gabriel Ting Partner’s Name: Daisy Butzer

PRE-LAB 1.

2. An abundance of hydrogen gas; the flame test would be a small orange flame. In the presence of oxygen gas, the flame will cause combustion In the presence of carbon dioxide, the flame will get put out. 3. Ting, Gabriel Lab Section 1415:05 1/27/2019 Title: 6M HCL causes Galvanized Nails to lose Mass over a Period of Time Introduction: Each nail is believed to have a coating of zinc on the outside of it. The zinc is used to prevent the nails from getting rust easier. The zinc coating protects the galvanized nail for the safety of people using the nail and it should last longer in the long term because of this coating. It is believed that the nails that will follow the industry standard which is found out by the chemical reactions to relieve the coating on the nail when a galvanized nail is put into a solution of hydrochloric acid. (Burgstahler, Albert 1992) Hydrochloric acid is being used to remove the zinc coating off the galvanized nail which will cause the nail to lose mass. The HCL will also cause the nail to lose its protective quality and be more able to get rust on the nail. The experiment we are doing will see how much zinc coating is put on the nail and how protective the zinc is onto dangerous Ph levels. Methods: First off you would want to obtain 5 nails and measure the length of each nail with a ruler in mm. You also need to measure the diameter using a caliper in mm. Take the nails to a electronic mass measurer and measure the mass of each nail. Make a table with the following; length of nail, start/stop time of the reaction, initial/final mass of the nail, and any observations that were seen during the experiment and record all the data collected. You will want to put each nail into a small test tube and mark them to not get them confused later with numbers. Put the five test tubes into a test tube rack to hold all the test tubes. Obtain 6M Hydrochloric acid in a small beaker. Pour the Hydrochloric acid into the small test tube for one of the nails just enough to cover the nail. Record any observations that take place and have a timer out for five minutes to measure how much time it takes for the nail to be soaked in the acid. After the five minutes are up pour the contents into a waste beaker and take forceps and remove the nail from the waste beaker. Remeasure the nail for the mass and record down the mass. Do this for the four other nails but use the same waste beaker. After all, five nails are done obtain 75ml of 2M NaOH and add 20 mL of the base into the waste solution. Record the observations seen. Using a Ph test make the solution until it is 8-9 Ph by adding more NaOH into the waste solution. Do not exceed a Ph of 9 though for it is very dangerous. Clean up all the equipment used by putting

the waste chemicals in the appropriate containers and rinsing out all the beakers and test tube used. Results: Length Mass Initial (g) Mass Final (g) Diameter Start Time Stop Time Observation s

Trial 1 38 mm 1.187

Trial 2 38mm 1.164

Trial 3 39mm 1.207

Trial 4 39mm 1.178

Trial 5 39mm 1.184

Average 38.6mm 1.184

1.125

1.076

1.101

1.092

1.091

1.097

3.1mm 3.1mm 3.1mm 3.1mm 3.1mm 3.1mm 0 0 0 0 0 0 5 mins 5 mins 5 mins 5 mins 5 mins 5 mins The solutions when mixed with the HCL were fizzing and producing a lot of bubbles. The color changed into a clear champagne color and left gray rust powder into the solution.

The average mass of zinc lost was calculated out to be 0.087 g. The average mass of zinc per inch is 0.479 Grams per inch^2. The standard deviation of the sample is -0.0022 grams. Discussion and Conclusion: The hypothesis was supported by the results and data from the experiment. The nails lost mass when it was put into the Hydrochloric acid solution. The zinc layer was complete dissolved in the HCL after a period of being in the solution for 5 minutes. It is very similar to the experiments done by the students of the University of Oklahoma found on a source by John C. Salzsieder in 1995. His goal of the experiment was to analysis the amount of zinc that was dissolved in the solution of the galvanized nails when mixed with hydrochloric acid. (Salzsieder, 1995) There was also another study published by the university of north Colorado with a similar process on how the acid would dissolve the nail. They inverted the reaction of the gas and collected how much gas was released by the acid and the nail to show the rate of corrosion of the nail. (Burgstahler) When adding the base NaOH to the waste solution the solution turned into a white precipitate. The solution became a more yellowish color and the PH rose until it hit between Ph 8 and 9.

Literature Cited: 1. Standard Deviation Formulas. Math Is Fun https://www.mathsisfun.com/data/standard-deviation-formulas.html (Accessed Jan 27, 2019) 2. Rusting Rates of Iron Nails www.csun.edu/~ml727939/coursework/695/rusting rates of iron nails/rusting rates of iron nails.htm (Accessed Jan 27, 2019) 3. Gravimetric-gasometric determination of zinc on galvanized nails Albert W. Burgstahler J. Chem. Educ., 1992, 69 (7), p 575 DOI: 10.1021/ed069p575 Publication Date: July 1992 4. Statistical Analysis Experiment for the Freshman Chemistry Lab, John C. Salzsieder, J. Chem. Educ., 1995, 72 (7), p 623 DOI: 10.1021/ed072p623 Publication Date: July 1995

5. Gravimetric-Gasometric Determination of Zinc on Galvanized Nails, Albert W. Burgstahler University of Northern Colorado...