Report Submitted: February 7, 2013 Title: Separation of a Mixture of Solids Purpose: To learn separation techniques based on the chemical properties of a substance Procedure: I used paper cups, the weighing scale, 50ml beaker, burner, burner stand, magnet and the Mixture of solids to separate sand, benzoic acid, salt, and iron. Data Tables: SUBSTANCE | GRAMS | PERCENT OF MIXTURE | Iron fillings | 2.5 | 2.6/4 * 100 = 62.5% | Sand | 2.4 | 2.4/4 * 100 = 60% | Table salt | 0.6 | 1.3/4 * 100 = 32.5% | Benzoic acid | 0.7 | 0.7/4 * 100 = 17.5 | Total | 7.8 | 172.5% | Questions: A. My proposed procedures compared very closely to the actually experiment. I knew that the magnet could separate the iron but the sand was going to the tricky part from the rest of the substances so I figured we would need to be heating and boiling in order to separate the benzoic acid but I really had no clue how to separate the salt from the sand. I have always wondered how sea salt was extracted from the ocean.
Experiment 8: Separation of a Mixture of Solids Purpose: The purpose of this lab is to separate the solids mixture containing the iron, sand, benzoic acid and salt. These solids were separated based on the unique properties of different solids such as variation in the magnetic properties and variation is solubility such as ranging from completely insoluble to completely soluble. Procedure: The necessary materials required for this lab procedures was obtained from the labpaq: solids mixture, weighing dish, and digital weighing scale. Each and every solid separated in this lab experiment was weighed using the weighing dish and digital weighing scale. From the solids mixture, the iron filling were separated by using the property of iron fillings that they were attracted towards the magnet.
This was done by taking small amounts of the unknown acid. It was then placed into capillary tubes and inserted into the Bibby Sterilin Device. Starting with a high plateau to find a quick melting point and then proceeding to find an actual melting point. The next experiment that aided in finding more characterizations of unknown #2651145-PLF13 was equivalent weight. In order to find the equivalent weight a titration of the unknown acid had to be conducted.
The chemical equation to be used is : 2NaHCO3(s) Na2CO3(s) + CO2(g) + H2O(g) In the second part, 1.0 M HCl will be titrated into a solution with a known amount of sodium carbonate (Na2CO3), the pH will be measured as it becomes more acidic and the equivalence point (the point at which HCL and Na2CO3 reach equilibrium) determined. We will calculate the moles of Na2CO3 by dividing the grams used by the molar mass of sodium carbonate. Then, the moles of HCl required to neutralize Na2CO3 will be determined by using the mole to mole ratio in the chemical equation. Finally, the molarity
To observe the change in properties of various synthesized copper compounds in order to identify the reactions and products being formed. Secondly, to become familiar with methods of separating compounds through decanting, heating with Bunsen burner and suction filtration system. In doing so, be able to recover copper metal and interpret the resulting percentage yield by applying the law of conservation of matter. Upon combining 20.0mL of NaOH to 10.0mL of Cu(NO3)2 and stirring the solution, there was a darkening of the initial blue color. Adding distilled water to the solution lowers the initial intensity of the blue color, bringing back to a lighter blue.
Then by filtering, iodide can be extracted which when combined with other substances can make an iodine tincture, that is a pharmaceutical product. * Can a single substance be isolated from a mixture? Yes a single substance can be isolated from the seaweed mixture by using methods such as filtration and evaporation. In our experiment we used filtration using a filter paper funnel to extract the iodide from the tincture. * What is this substance This substance is iodide Confidence Report The aim of extraction, is to separate a part of raw material, using a solvent such as water with heat.
Observing Changes – Materials & Procedures Materials Water Copper (II) sulphate (Powder) Copper (II) sulphate solution Iron nail Sodium carbonate Hydrochloric acid Magnesium ribbon Flame (candle) Sugar Aluminum foil Test tubes Test tube rack Tongs Medicine dropper Spoons Beakers Safety goggles Scoopulas Procedures Water and Copper (II) Sulphate Procedure 1. Add a small amount of solid copper (II) sulphate to a test tube with a scoopula. Record the physical properties. 2. Write a hypothesis on what you think will happen when water is added.
Then weigh the crucible without the hydrate after heating. Record both masses. Next, add CoCl2 ∙6H2O and weigh the crucible. Now place the hydrate and crucible on the hot plate. Observe the color change while it is being heated.
h) A way to make hard water softer is to put an sodium nitrate and create a precipitate to mellow out the reaction. Another way of making it softer is by removing the calcium ions one way of doing that is by boiling the solution to take out some of the ions. Conclusion: Overall, we determined that sodium carbonate, Na2CO3, is the anion that can be used to precipitate the most metal cations. Also, we learned that the anion sodium chloride, NaCl, could be used to remove silver ions from solutions. The stuff that I found interesting was that how many colours you can get when you mix the cations and anions
With this knowledge at hand, it is possible to identify and unknown compound through qualitative analysis. Materials and Methods: Part 1 Cation Tests: To begin the experiment, 6M NaOH was added to centrifuge tubes containing potassium, iron (III), zinc (II), copper (II), and cobalt (II) in the metal hydroxide test. Drops were added until a precipitate was observed and separating the cations into two groups, those that did and those that didn’t form precipitates, eliminating certain cations. Additional drops of NaOH were then added to test for any amphoteric cations. For those that tested negative, 15 M NH4OH was added in the ammonium hydroxide test to observe for the precipitate color which further separated the cations.