Title: Separation of a Mixture of Solids Purpose: To learn about separating solids and how this happens. By separating the solids one will be able to tell the difference between a mixture and a pure substance. Procedure: Four main steps. Separating the iron from the mixture with a magnet. Separate the sand by boiling water and pouring the water off, then move on to separating the Benzoic acid using filter paper.
The R-squared value shows us the correlation between the two variables in each graph that we were comparing. A consistent, precise R-squared value would be ideally 1. In all three cases, only one of our methods gave us this result: Titration. So given our results titration was the most precise method. But, our Ideal Gas Law method was more precise than crystallization from the previous week due to our newly found R-squared value of 0.8909.
The reason I believe they were the most effective am because they both caused the inks to spread out the furthest amount. While vegetable oil, and alcohol did not do all that much. (5 points) Score 3. Which solvent caused the ink from the dots to move the most? Which solvent caused the ink from the dots to move the least?
The hypothesized result was that the furthest distance would be the most effective, and absorbance would decrease as the light became closer. The results supported the hypothesis and showed that the three distances all yielded a relatively similar and that all the absorbances were in fact lower than the control group. The results also showed that as the light was moved further away from the chloroplasts the DPIP was reduced faster, producing a lower absorbance. Effect of Light Wavelength In this experiment different colors of light were tested in order to see which caused the photosynthetic process to be the most efficient. Discs made of spinach leaves were deoxygenated and placed in beakers with different wavelengths of light in order to measure which wavelength produced the most oxygen the fastest.
Graphically, it would appear that Styrofoam is the best calorimeter because it remains steady throughout the trial, but this does not connect with the calculated calorimeter constants. Based on the calculations, the next best insulator after cloth towels is aluminum foil, and then paper towels. On the contrary, it would make more sense if Styrofoam was the next best insulator after the cloth towels based of the graphs. Conclusion: In conclusion, the purpose of the experiment was to determine which of several common substances are the best thermal insulating materials. From the data collected, it is observed that the best cup calorimeter out of all the given materials is ceramic.
the alkali due to the use of caustic soda or soda ash and hydrogen peroxide, wetting agents and other auxiliaries would remain in the core of the fiber processed even after 2 or 3 washes. These residual chemicals like alkali's and peroxide are detrimental to the production of uniform flawless fabric production. The core residual alkali would lead to immature hydrolisation of the reactive dyes and results in streaky and uneven dyeing. | The residual peroxide present in the fiber will oxidize the reactive dyes' chromophore that contain the metal ions and lead to tonal variation and sometimes uneven dyeing. In some cases the chrmophore itself is getting destroyed into a colorless product and lead to pale or white patchy dyeing.
The third test will utilize thin layer chromatography to evaluate the purity of the aspirin as well as testing for the presence of leftover salicylic acid or other by products of the reactions. Experimental: Week 1: For the synthesis of the aspirin, 250 mL of water was boiled. 1.5 g. of salicylic acid were poured on a test tube. Then, 3.5 mL of acetic anhydride and four drops of 85% phosphoric acid were added. A cotton ball was placed to prevent vapor escape.
Identify that your Excedrin is a mixture of organic molecules using thin layer chromatography (TLC), melting point (mp) and Proton Nuclear Magnetic Resonance Spectroscopy (1H-NMR). 2. Determine the solubility of the components of Excedrin in various solvents. 3. Separate the components of your poisoned Excedrin using solubility characteristics and extractions.
Acid Base Titration Purpose: The purpose is to calculate the molarity of a NaOH solution by titrating the base with 5mL of standard HCl solution in each trial. By adding the base with unknown molarity to the acid with 0.10M the molarity of NaOH can be calculated. The base, NaOH, helps bring the pH of the acid, HCl, closer to seven, which neutralizes it. When using the buret the amount of NaOH used is able to be determined. Then by writing a balanced chemical equation and using the titration formula, Nb+Ma+Va=Na+MbVb , the molarity is able to be determined.
We are looking to find wether the reaction is exothermic or endothermic. Experiment 2: the aim for this experiment is to record the pH level of a sodium hydroxide and hydrochloric acid reaction. Then record it into the graph, it should resemble the standard neutralization curve, as shown under the introduction. Materials: what you will need for both experiments: Experiment 1: ➢ 20g baking soda ➢ 20g citric acid ➢ 2 cm strip of magnesium ➢ 50 ml of 5M HCl acid ➢ 50 ml measuring cylinder ➢