Sarah Cunningham Lab Section:10206 Title: Separation Anxiety Objective The goal of this experiment was to use separation methods to make potassium nitrate compound the purest substance it can be. By the end of this experiment, certain separation techniques should be understood for the different sample types. Introduction It is essential for chemists to know how to separate mixtures when needed. This will come in handy when an element is toxic and cannot be mixed with other elements or compounds(Wood, 2023). It even came in handy back when gold miners needed to separate soil and water to find the gold(Libretexts, 2022). Different separation techniques allowed people to understand mass spectrometry, biomedical substances, and proteins. Techniques …show more content…
The experiment helped show the physical and chemical properties when they turned into one kind of matter. This experiment also made the students understand and execute vacuum filtrations and extractions. The chemistry behind separation techniques is crucial in order to isolate certain elements so they can’t be changed in the chemical reaction. One form of separating mixtures is evaporation. This technique separates solid substances that were dissolved in a liquid. Filtration is another technique used to separate substances in mixtures to find the purest form of the particles. This separation can filter out bacteria from water, making it safe to drink. (Libretexts, 2022). Sand, KNO3, CuSO4, and mineral oil were the different samples used to separate them back into their pure substances. Ethyl acetate's boiling point is 170.78 degrees F and mineral oil’s boiling point is 500 degrees …show more content…
Altering the temperature into a cooler state allowed all the KNO3 crystals to reappear again. When dissolving KNO3 and CuSO4 have negative ions are surrounded by water’s positive charges. This is because water is a polar solvent and allowed KNO3 and CuSO4 to separate in water(Wood, 2023). Finding the masses of all the substances was not 100% accurate. In ranking the smallest difference between original mass and recovered mass was the oil(17.941g), sand(3.990g), CuSO4(6.556g), and the KNO3(2.751g). Factors that contributed to error had been not fully transferring the mixtures from the flask to another container. Another source could have been human error from spillage of some of the components out of the flasks. These variables affected the accuracy and precision of the experiment. The purest sample of KNO3 crystals was not obtained because of these errors. To improve these fallacies, recrystallizing the KNO3 again would have helped get this compound to its purest element possible.
Introduction The purpose of this Lab was to identify the density of the unidentified object and determine what substance the unidentified object given by the teacher was. The density calculated in the experiment will stay the same because the density of the unidentified object will stay constant. The Independent Variable of this experiment was the calculated density and the unidentified object given. The Dependant Variable for this experiment was the density.
And this leads to the conclusion that this substance found in the mixture is indeed sodium. Alcohol was also another substance found in the mixture. Its noticeable as it was most likely was fraction 1 in the fractional distillation lab. Sharing a boiling point with alcohol, alcohol being 82 degrees celsius, and fraction 1 being 83 degrees celsius (which i extremely close). The substance, fraction 1, was also as flammable as alcohol is , when testing its flammibility.
Which totaled 93.00 grams then decreased 1.673 grams them the reaction took place. 2. The color of the copper carbonate hydrate as it was heated can help identify the product? The final color ended up being black which was CuO 3.
Lastly, the unknown compound was reacted with two different salts. For the first salt, 0.50 grams of KCl was mixed with 5 mL of water in one beaker while 0.5 grams of NaNO3 was mixed with 5 mL of water in a different beaker. Then, the NaNO3 solution was added to the KCl solution. To perform the reaction with the second salt, 0.50 grams of KCl was mixed with 5 mL of water and 1 mL of 1 M Ag(NO3)2 was added. After performing each reaction, the solution was observed to see if a reaction occurred and the pH value of the resulting solution was tested using a pH
Filtering, evaporating, centrifuging, and decanting something will only physically change it. Chromatography is used to separate different parts of a solution so that it can be identified. It can work because different substances have different attractions to things. Distillation can separate substances, such as salt water, as long as it has different boiling points. It can even be used to purify salt water but it is not cost efficient or energy efficient so it is not suitable for everyday use.
The separation of the ink for us was very little because we did not have enough time to let the solvent travel completely. The choice of our solvents could be connected to the separation process by having some solvents been able to better separate a substance than others because they have similar polarity. The molecules interacted with the mobile phase, because they got pulled up the chromatography paper using the solute. .
In order to separate KNO3 and CuSO4, which are both soluble in water, recrystallization was used. The reason the two components can be separated through recrystallization is because of the temperature dependence of solubility, KNO3 is much more soluble in hot water and insoluble in cold water while CuSO4 is only slightly more soluble in hot water. When the filtrate was heated the solution was saturated with KNO3 but when the system was cooled, the KNO3 became insoluble and pure crystals reformed while CuSO4 stayed dissolved in the
(1) The purpose of the separation lab procedure was to help my group members and I successfully formulate our own plan before completing the experiment, handling multiple materials and substances, etc. It acted as a step-by-step plan that guided us throughout the experiment and ensured that we were well prepared ahead of time (ie. knowing what kind of materials were necessary and gathering the correct measurements of each substance); this made the experiment day much less hectic for all of us. It made reaching our goals (achieving > 85% recovery for each substance) more realistic and convenient. (2)We predicted that we would be able to easily separate each substance from the mixture through the use of our designed procedure. By using a bar magnet, we predicted that all the iron (and only the iron) would attract and quickly maneuver its way through the beaker and into the
Abstract In this experiment the separation of a copper (II) chloride and sodium chloride mixiture was attempted. The main aim was to separate the compounds from eachother while receiving as much of the original mass of both substances as possible - in perfect conditions the original mass will be received after seperation. Many techniques were considered but dissolution, filtration and evaporation proved to be easiest and most reliable in a school environment with school equipment. The copper (II) chloride and sodium chloride mixture was dissolved in a methanol solution and filtered out leaving the sodium chloride behind.
The first experiment involved in this four-week project was the extraction and
All things considered, the results proved that the unknown substance or element was barium since the calculated density was 3.9 g/mL. To expand upon, the density was calculated by measuring the mass of the metal and using the displacement method to determine the volume of the metal. Also, the best method of disposing the storm water would be to contact a Wastewater Treatment Plant (WWTP) so that they could put it through a purification process, making all that water reusable. Meanwhile, the percent of recovery was calculated by the formula Percent Recovery=observed valuetrue value *100%. Furthermore, according to the pie chart created in the data analysis, the sample given contained of the percent by mass for metal to be 5.2%, salt was 3.3%, wood was 3.1%, plastic was 4.5%, rock was 12.5%, sand was 11.8%, and water was 59.6%. Also, the formula used to calculate the percent error was Percent Error=observed value-true valuetrue
+ -.0005g of KNO3 dissolved in 20 + -0.5 mL. A 10 mL graduated cylinder was used to accurately measure. The pH of potassium nitrate was recorded and the probe was removed and
Intro: Separation and purification of an unknown/complex compound can be done by using techniques such as liquid-liquid extraction, solid-liquid extraction, recrystallization, melting point, and thin layer chromatography. In this experiment, these techniques were used to separate excedrin’s components containing caffeine, excedrin, and acetaminophen, Each component has its own chemical properties and characteristics such as polarity, reactivity, and solubility. Knowing how to separate and purify compounds from each other is an important skill within in a lab setting. A few techniques for first initially separating compounds apart are liquid-liquid extraction and solid liquid extraction. Liquid-Liquid extraction involves using a seperatory funnel and release on varying solubities and different solids in immiscible solvents.
In general, the process of chromatography is about a mixture of various components enter the chromatographic process and different components are flushed in different rates through the system. The mixture migrates at different rates over adsorptive materials during the separation. In short, the principle of chromatographic separation describes
This was possible because the mixture of potassium oxalate and iron (III) chloride is not soluble in water. This product created a precipitate, which resulted in a green crystallized product. The crystal precipitate was then isolated from the rest of the liquid substance and dried to determine the percent composition to determine the formula. The second day of the coordination compound synthesis lab consisted of performing titrations and then determining the mass of oxalate (ox) (2). An ion-exchange technique was then used to find the amount of potassium and iron (III) in the compound.