Iodine Experiment

Submitted By Andrys10705
Words: 1634
Pages: 7


Table 1-Appearance of Zinc and Iodine:
Looks like small silver balls
Rubbing Alcohol
Looks like clear liquid
Zinc Granular
Looks like shredded pieces of silver
Zinc Powder
Looks like a gray fine powder
Zinc Mossy
Looks like small clumps of silver
Zinc Shot
Looks like small silver disks
Zinc Sheet
Looks like thin metal sheets
Zinc Rod
Looks like rods that are a dull gray color on the outside but a shiny silver on the inside where there are cuts
This table records the observations made about the physical appearance of all chemicals used in this experiment.

Tabulated Test Results and Calculations:

Part 1: Solubility Results

Table 2-Solubility of Iodine:
Liquid turned yellow but few pieces of crushed iodine still remained
Slightly Soluble
Liquid turned a dark red-brown color but few pieces of the iodine still remained
Slightly Soluble
Mineral Oil
Liquid turned a dark purple color and there were none to barely any pieces of iodine remaining
Potassium Iodide
Liquid appeared to be a black color with a red tint and there was no pieces of iodine left
Very Soluble
This table shows the results obtained when 2 pieces of solid iodine were added to 2 mL of solvent (water, alcohol, mineral oil, potassium iodide). It’s ability to dissolve was observed and recorded to be either ‘soluble, slightly soluble, or insoluble.’

Table 3-Solubility of Zinc:
Zinc remained at the bottom of the test tube with the water
3 moles of Hydrochloric Acid (HCL)
Zinc reacted with HCL and began to bubble
Slightly Soluble
This table shows the results obtained when a few pieces of granular zinc was added to 1 mL of the solvent (water and 3 moles of HCL). It’s ability to dissolve was observed and recorded to be either ‘soluble, slightly soluble, or insoluble.’

Part 2: Density of Zinc

Table 4-Volume of Zinc:
Mass of Zinc
Volume of Water
Volume of Water and Zinc
Volume of Zinc
This table calculated the volume of Zinc. In order to determine the volume of Zinc, the volume of water (in this case 16mL) is subtracted from the volume of water and zinc (third column).

Graph 1-Density of Zinc:

This graph plots the volume of zinc on the x-axis and the mass of zinc on the y-axis. The points on the graph indicate a straight-line relationship. This means that as the ‘cumulative displaced volume of water by zinc in mL’ increases, so will the ‘cumulative mass of zinc in grams’. The equation of the line is y= 6.5791x + 2.3937, making the slope of the graph 6.5791. The slope of the line will be equal to the density value of zinc. The actual density of zinc is 7.14 g/mL, according to The CRC Handbook of Chemistry and Physics. When 6.5791 is subtracted from 7.14 there is a 0.5609 difference between the accepted value and the experimental value (7.14-6.5791=0.5609).

Confidence Report:

The results obtained from this lab were mostly successful. When checking for solubility of Iodine within the given solvents (water, alcohol, mineral oil, potassium iodide) they were all somewhat soluble because they all had a change of color. This color indicated that some properties of the Iodine were able to dissolve into the solvents. Even though the solutions had a change in color, there were still some pieces of the iodine remaining at the bottom of the test tube (excepts for Potassium Iodide), which means while even though they were soluble, they weren’t able to completely dissolve. When testing for the solubility of zinc, our results differed than that of other groups. We found that zinc is insoluble in water but we also found that zinc was insoluble with HCL. When comparing the results from this experiment to the results of Menglu Ahu and Billey Huang, Zinc was supposed to react with HCL and begin to bubble. Below are Meglu and Billey’s results for the