The absorption spectrum is measured using a spectrophotometer and the data is graphed in Excel. The peak of the line is used to find Vmax of Fe2+. Vmax is used to find the moles of Fe2+ and ligand. The unknown n is a ratio of moles ligand divided by moles Fe2+. Results and Discussion For the first part of the experiment (Part A), five different 100 mL volumetric flasks were each filled with 1,2,3,4 and 5 mL of iron (II) solution.
(0.050) (0.1) = 0.0083 moles b. Pour 8.3 mL of the stock solution to get the amount needed. c. Measure out 8.3 mL in a graduated cylinder 8. Exercise 8: a. 41.8 mL are used b. 0.00079 moles EDTA4- c. 0.00079 moles ZnI2 d. 0.0517 grams of ZnI2 are in the sample e. 0.0517/0.237= 21.8% f. Error Is 6.34% Lab Report: Part 1: In this lab we used the following supplies: * Zinc Iodide * Na2H2EDTA(s) * Calmagite indicator solution * pH 10 buffer solution * 6M Acetic Acid * Unknown Zinc Compound The main purpose for this part of the lab was to determine the amount of zinc ion in a sample of ZnI2 by titration.
5 .For part III, Average was needed to be found after Find the Mass/A of each all 5 disk. To do that Add all the values in Table 3 and divide them by 5. 6 .For Part III, Percent difference between the average value and the slope of the derivative diameter graph was found by doing this: ((slope of the derivative vs. diameter graph- average)/slope of derivative vs. diameter graph)*100 =67.9% VII. Analysis Questions/Answers 1. The Slope in Part I represents π 2.
Part C: Density of Sodium Chloride (NaCl) Solution, a sample of NaCl was obtained and measured using a 100mL beaker and a 10mL pipet to determine the concentration of the solution. In order to obtain the appropriate result, a calibration graph and density measurement was used to determine the concentration of the sodium chloride solution. In conclusion, based on the water temperature of 21.8°C in part A’s graduated cylinder experiment obtained, it was determined that the average density was .0973g/mL with a percentage error of 2.5%. When graphed the measurement was equal to Y=0.988x. Part B: The graduated pipet’s average density at 22.3 °C was determined to be 0.9785g/mL with a percentage error of 1.89% shows the graduated pipet to be more accurate and precise.
5.04H: Gas Stoichiometry Lab Worksheet Name: _________________________ Data and Observations: Present all relevant data in a data table below. Include an observations section for any observations that you made during the lab. (5 points) Data Table| Mass of magnesium strip (grams)|0.0304g| Volume of gas collected (mL)|10ml| Barometric pressure (atm)|1.1| Room Temperature (°C)|21 | Vapor pressure of the water (torr)|18.7| Calculations: 1. Write the balanced equation for the reaction conducted in this lab, including appropriate phase symbols. (2 points) Mg(s) + 2 HCl(aq) → H2(g) + MgCl2(aq) 2.
A balance can measure mass, which is best, defined as the amount of matter in a sample. In order to measure an objects volume, the student will have to use water displacement for irregular metals and various formulas to find the volume of three-dimensional objects. The density, which is the ratio of the mass over the volume, can be used to identify a metal or element. There are multiple reasons as to why the student will perform this lab. First off is to test the student’s knowledge on using measurement tools accurately when measuring the mass and volume of the metals in this specific lab.
I added varying levels of substrate to the test tubes in each experiment. The amount of substrates were .5 grams, 1 gram, 2 grams, 4 grams, and 8 grams. The output of the experiment (the dependent variable) was the number of molecules of product formed per minute at (106). RESULTS Test Tube # | pH Level | Amount of Substrate | Number of Molecules of Product Formed per Minute (106) | Test Tube #1 | 3 | .5g | 19 | Test Tube #2 | 3 | 1.0g | 39 | Test Tube #3 | 3 | 2.0g | 82 | Test Tube #4 | 3 | 4.0g | 96 | Test Tube #5 | 3 | 8.0g | 96 | | | | | Test Tube #1 | 5 | .5g | 39 | Test Tube #2 | 5 | 1.0g | 81 | Test Tube #3 | 5 | 2.0g | 168 | Test Tube #4 | 5 | 4.0g | 198 | Test Tube #5 | 5 | 8.0g | 198 | | | | | Test Tube #1 | 7 | .5g | 72 | Test Tube #2 | 7 | 1.0g | 145 | Test Tube #3 | 7 | 2.0g | 300 | Test Tube #4 | 7 | 4.0g |
| | | An Activity Series 1/9/13 Makieya DunhamPartners: Jasmine Lewis and Danielle Anderson | | | Problem Statement: In this lab we determined the activity series for five metals and for three halogens. In the first part of the lab we used a microscale technique to rank the metals that reacted with the other metal nitrates from most reactive to least reactive. The metal that reacts with another metal nitrate, then the solid metal have reduced the other metal ion and is the more reactive metal of the two. In the second part of the lab we used the solvent extraction technique to derive an activity series for the halogens. Safety Precautions: When in the lab we wore goggles, an apron, and gloves the entire time.
Add hydrochloric acid to a test tube. Cut a piece of magnesium ribbon (couple of centimeters). Record the physical properties of both substances. 2. Write a hypothesis on what you think will happen when mixed.
Introduction This first laboratory experiment required the toss of a five separate pennies and determining how many of the five pennies would land with the heads facing up on the table. By using this method of tossing the coins, the class as a whole was able to compare their own data to other people’s data and see the different outcomes of each individual’s results. The data collected was a comparison of the average number of heads per toss versus the actual number heads that occurred. Though we all did our own experiments, the results of the class data in total was very similar to each of our own individual data. The experiment started out with each of us being grouped together to compare our individual results with those in our groups.