Nt1310 Unit 9 Final Lab Report

Put approximately 9-10(g) copper ore into beaker. Use spatula to break up any large pieces. Next add 17ml H2SO4 (aq) (hydro sulfuric acid) to the beaker. Began mixing until all or most traces of blue dissipate; or the copper ore will no longer dissolve (should appear as a milky liquid). Next use pipette to and remove solution and divide solution into 2 individual test tubes then Place test tubes into centrifuge and run centrifuge for 1 minute. Remove from centrifuge machine Fill a cuvette with the clear solution from the test tube making sure not to disturb the sediment at the bottom. Note the solution should bluish in tint Final place the cuvette in the colorimeter. Then record data and calculate in results section.

Scientists use an instrument called a spectrometer to quantitatively determine the amount of light absorbed by a solution. The primary inner parts of a typical spectrometer are described below. The spectrometer has a light source that emits white light containing a vast mixture of different wavelengths of electromagnetic radiation. The wavelength of interest is then selected using a monochromator (“mono” meaning one and “chromate” meaning color) and an additional exit slit. The separation of white light into different colors (wavelengths) is known as diffraction. The selected light then reaches the sample and depending on how the light interacts with the chemical compound of interest, some of the light is absorbed and some passes straight through. By comparing the amount of light entering the sample (P0) with the amount of light reaching the detector (P), the spectrometer is able to tell how much light is absorbed by the sample.

When you use a spectrophotometer you should not set the wavelength of light to be the same color of the solution. This is because if you set the wavelength to be the same color of the solution then no light will be absorbed. The reason why no light will be absorbed is because the color you see is the wavelength of light that is being reflected so you must set the wavelength to be the complementary color. The wavelength of light that was chosen for the lab was 450nm which coincides with a very dark blue color. The reason why choosing a dark blue makes the most sense for this experiment is because the color of the FeSCN2+ ion was blood red.

To begin the experiment, start by grabbing five cuvettes and labeling them one through five. After they have been labeled, add 2 mL of water to cuvette one, and 1mL of water to cuvette two through five. Then add 1mL of Catechol in cuvettes two through five. Because of the time considerations, test two cuvettes at a time. To do this, add 5 drops of Parahydroxybenzoic acid to cuvette two and 10 drops to cuvette three. Afterwards add 5 drops of Catechol Oxidase to cuvettes one through three. Blank out the spectrophotometer with cuvette one containing the water (H20). Then test the absorbency of cuvette two and three checking them every two minutes for twenty minutes, record your results. After those cuvettes have been tested, cuvette four and five need to be tested. Begin this by adding 15 drops of parahydroxybenzoic acid to cuvette four and 15 drops to cuvette five. Add in 5 drops of Catechol to cuvette four and five. Blank out the spectrophotometer again with cuvette one. Proceed to test cuvette four and five by checking the absorbance every 2 minutes for 20 minutes, record your

The purpose of this lab was for the student to get involved with his or hers new lab kit as well as being able to know, identify and use each other tools provided in the kit. Another key learning aspect of this lab is to teach the student how to measure properly the many units in the SI system. I will be using laboratory dilutions, measurements, and weights to then calculate using algebraic formula.

To begin, measure the mass of a dry empty 10-mL volumetric flask and stopper. This will be recorded to 3 decimal places. Once the first task is accomplished proceed by pouring 10 mL of DI water to the calibration mark on the volumetric flask and measure its mass which can then be discharged for this step. Next, transfer 100 mL of ethanol into a dry 150 mL beaker and through the use of a disposable pipet transfer ethanol from the beaker into the 10 mL volumetric flask until the calibration mark has been reached. Now place the stopper and measure the volumetric flask's mass.

Incorporation of assay controls included setting up a spectrophotomer and running the chart recorder with a full-scale deflection before the start of the assay. The set recorder had a corresponding value of 1 for the change in the absorbance. Therefore, prior testing was done to observe whether a change occurred in the readings. This helped to indicate that the results were valid, as they could have been affected by a fault during the setting up of the spectrophotometer. On the other hand this was considered as one of the controls for the experiment. Nevertheless, a new cuvette had to be used for each assay.

The Absorption Spectra With the spectrometer calibrated, pre-rinse and fill a new cuvette with solution B. Take observation of the absorption spectrum graph that is generated and take note of the λmax, where the absorbance is at its maximum point. Remember, to save this data on the spectrometer before moving

Of Exp #5: In this experiment we will learn about the spectroscope and how it works. To learn the concept of quantitative measurements, to construct a spectroscope and, to use it for taking quantitative measurements.

Place the vial in the Spectrophotometer with the arrow facing towards you 8. Have the temperature probe in the vial 9. Record the absorbance at variance temperature as the temperature cools 10. Repeat steps 1-9 at 542 nm using the Rhodamine B and 1-Propanol

concentration, record the absorbance readings at a fixed wavelength, and plot the absorbance vs. concentration data. The wavelength of 520 nm was selected for experiment Part

The purpose of this lab was to observe how light is altered as it goes through a solution containing a visible dye. In doing so, we will understand the relationship between absorbance, concentration and light path length. We first created different concentrations of blue stock solutions through dilution. We made 4 dilutions, which gives us 5 solutions in total. Each diluted cup (A-D) had 20 g of stock solution to start with and then 10, 30, 30, 46 g of distilled water was added respectively.

3.) Measure the mass of the first substance (0.25g) on the balance scale accurately. Once measured add the substance into the boiling tube containing 20ml of water and make sure the thermometer is still in the boiling

In this lab the concentration of allura red will be found. The vernier colorimeter will be used for this lab. Stock solution of a known concentration will be made, the absorption of each will be measured, when absorbance vs. concentration is plotted it should result in linear plot, which is called a calibration plot. The plot comes from the beer-lambert law, which is A=Kc. Measuring the concentration of allura red can be found by measuring the absorption of light through the solution. Cuvettes will be used in this lab to find concentration each solution; they will be placed in the cuvette then put into colorimeter to find absorption. Once that is complete data pairs will be examined by making a graph of absorbance vs. concentration with a

4. Prepare a vacuum filtration apparatus using a buchner funnel. Obtain one filter paper for each one of your samples, weigh them and record their mass in your notebook (label them with a pencil to be able to differentiate them later).