Fescn2 + By Observing Colour And Concentration Lab Report

The initial concentrations of the reactants in Table 1—that is, [Fe3+] and [SCN–] prior to any reaction—can be found by a dilution calculation based on the values from Table 2 found in the procedure. Once the reaction reaches equilibrium, we assume that the reaction has shifted forward by an amount, x. Notice from Table 1 that the value of x is simply equal to the equilibrium concentration of FeSCN2+(aq), or that x = [FeSCN2+] at equilibrium. The equilibrium value of [FeSCN2+] is determined spectroscopically using Beer’s Law. Its initial value in the table is zero because no FeSCN2+(aq) is added to the initial solution. Finally, the equilibrium concentrations of the reactants, Fe3+(aq) and SCN–(aq), are found by subtracting the equilibrium concentration of FeSCN2+(aq) from the initial concentrations of Fe3+(aq) and SCN–(aq), as shown in the table above. Once all the equilibrium values are

You want to investigate a new wave of vitamin water is pH neutral. Results are: Three of the five samples turn a murky

If the equilibrium lies to the right, the solution is basic and will be yellow. The first solution turns pink because the HCl is a strong acid and methyl orange is pink in acidic solutions. The equilibriums shift to the left side showing an increase in the amount of acid in the solution that is why the color changes to pink. The concentration of the solution then turns yellow because NaOH is a base and turns yellow in a basic solution. The equilibrium is shifted to the right when the NaOH is added.

In reference to the analysis of anions, Table 1 shows that a precipitate was formed when our unknown was combined with HNO3 and AgNO3, thus indicating the presence of a chloride ion. Because our unknown did not form a precipitate due to HCl and BaCl2, separate, effervesce, or smell, we concluded that neither sulfate, nitrate, carbonate nor

To conclude, the data we have collected from both experiments suggests that Le Chatelier’s principles are applicable and correct. When different substances were added to different solutions, the equilibrium shifted appropriately in order to gain a balance. The shifting of equilibrium resulted in different color changes in different mixtures. In part 2 of the experiment we the aforementioned changes were more easily spotted. We saw the relationship between forward and reverse reactions. When NaOH was added to tube #8 we saw that the color changed from orange into yellow, in order to gain balance but when we added HCl back, the color again changed to orange. Which clearly proved Le Chatelier’s

An experiment was done to determine the concentration of Allura Red in a commercially available beverage, Gatorade. This was done by using the colorimeter, the absorbance of five Allura Red solutions were measured. The graph obtained demonstrated a linear relationship and the equation obtained yielded a concentration of 1.9910-6M.

2) Adding OH⁻ would react with the Fe³⁺ in the system to form a precipitate Fe(OH)₃. This would decrease the [Fe³⁺] in the system. Equilibrium will shift left to counteract the change and the solution becomes lighter yellow in colour.

This reaction is going in the reverse direction. This shows Le Chatelier’s Principle as it explains that when a system at equilibrium is subjected to a change that upsets the equilibrium, the system will neutralize the disturbance to restore equilibrium to the system. The reaction is moving in the reverse direction as when HCl is added to the solution, there becomes an excess amount of products because more molecules are being added. When the concentration of the products was increased, there were a greater number of effective collisions between the molecules in the products. This then increased the rate of the reverse reaction. Due to the excess amount of products, the system shifted in the reverse direction in order to decrease the products. By moving in the reverse direction, the system was able to produce more reactants to reduce the products. This brought the system back to

This document is not meant to be a substitute for a formal laboratory report. The Lab Report Assistant is simply a summary of the experiment’s questions, diagrams if needed, and data tables that should be addressed in a formal lab report. The intent is to facilitate students’ writing of lab reports by providing this information in an editable file which can be sent to an instructor.

In this experiment, I saw that the product of Tin (ll) Chloride mixed with Potassium Dichromate is different from the product that resulted from Tin (lV) Chloride when mixed with the same reactant that was used with Tin (II) Chloride, Potassium Dichromate. They both resulted with different colours and smell. Tin (II) Chloride resulted with a light green colour, whereas Tin (IV) Chloride resulted with bright yellow colour. Similarly, Iron (llI) Chloride had a different product when mixed with Sodium Hydroxide, Ammonium Chloride added with Aqueous Ammonia, and Potassium Ferrocyanide compared to the product of Iron (ll) Sulfate, when mixed with the same reactants that was used to react with Iron (III) Chloride. And also same for Copper (ll) Thiocyanate

Depending on how much filtrate was collected and how well it filtered could have been a factor in the difference between the measured iron value and the RDI iron value. Another factor that could have had an impact on the difference between measure and RDI iron value is when we measured 5mL of 2.0 M of HCl into the test tubes 1 through 5, we also measured 5mL of stock solution in test tube 5. What could have had a factor in our results for measured iron value is how accurately we measured 5mL of test tube 5 mixture into test tube 4 of the 250.0 ppm mixture, and how accurately we measure 5mL of test tube 4 mixture to place into test tube 3 and so on. Depending on how accurate we poured 5mL of 500.0 ppm sample into test tube 4, 5mL of 250.0 ppm sample into test tube 3, 5mL of 125.0 ppm sample into test tube 2 and how well we shook up the mixture could of affected our results of our measured iron value and made a difference in comparison between the RDI iron value.

In this experiment, many errors came up. With that being said, errors relating to the spectrophotometer was the main cause of wrong readings and improper data. In addition to mechanical error, human error like mixing the wrong chemicals together could have drastically altered the results and data. Conclusion: The spectrophotometry was key in finding the value for the equilibrium for FeSCN2+, Fe3+, and SCN-.

In this experiment, a saturated calcium sulfate was already made and ready to use. 25.00 mL of this solution was then mixed with 10 mL of an ammonia buffer and 1 drop of

Step 1 and 2 was repeated by using distilled water by replacing the test solution.

3. Will the intensity of the color of the dye with a mordant changed after the: