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.
Explain your answer. Water itself is an example of a homogeneous mixture. It often contains dissolved minerals and gases, but these are dissolved throughout the water. Is isopropyl alcohol (rubbing alcohol) a heterogeneous or homogenous mixture? Explain your answer.
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
Do this before it cools or water will travel backwards into your tube and contaminate your solid product. I 1 Collecting a liquid product: If you loosely wrap a damp paper towel around the upper-outer section of the boiling tube away from the flame, you might be able to condense a gaseous produCt into its liquid ·state. In addition to this you should cut a large piece of qualitative filter paper in half and then fold it and theri curl it inside the boiling tube near the rubber stopper. If a liquid forms, the finer paper will help absorb it and prevent it from falling back onto the solid being heated. Make sure the rubber stopper is securely in place since gas can easily leak out.
Find the molarity is essential to numerous amounts of future procedures such as equivalent weigh. The titration of hydrochloric acid was also completed for practice of titrating and basic understanding of the characteristics of the strong acid. In all three titration experiments an indicator was used to illustrate the
Simple and Fractional Distillation of a Binary Mixture Introduction/Background – This experiment dealt with a 1:1 ratio of a stock mixture of cyclohexane and toluene. The aim of the experiment was to separate these two chemicals through the use of simple and fractional distillation. The separation of the two chemicals was possible because of the theory behind distillation. If there are two solvents, A and B, with two different boiling points, then they can be separated by evaporation and condensation. Knowing the different boiling points of the two liquids was useful in this experiment so that the sand bath could be heated to different temperatures to evaporate the two solvents.
Discussion & Conclusion In this experiment we learned how to synthesize the cyclohexene by dehydration of cyclohexanol. We procedure the first step where we have to mix the components. Then we heat the R.B.F with a fractionating column, distilled water. Then we obtained the layers, and we transferred the organic layer to a small, dry Erlenmeyer flask. We added anhydrous Sodium Sulfate as a drying agent.
Physical changes were indicated when a substance only reacted once. The powders indicated is the following: Powder A was chemical, Powder B was Chemical,Powder C was physical and powder D was chemical. These results were proven by the physical and chemical changes each of the powders were exhibited. These experiments essentially demonstrated the changes and reactivity of the powders. Taking a Step
Halides Lab: Background information: Halide ions are reactive and useful. Salts are positively charged ions (metals) combined with any negative ions (nonmetal), and when placed in a solution (water) it separates into the cations and anions that made it up. The Purpose of this lab is to find out how the Halides react with the indicators, and to determine the identity of the two unknown solutions (A and B). Color of solutions prior to experiment: NaF | NaCI | KBr | KI | Unknown A | Unknown B | clear | clear | clear | clear | clear | clear | Color of indicator prior to experiment: 5% Bleach (NaOCI) | 0.2 M Na2S2O3 | 0.1 M AgNO3 | 0.5 M Ca(NO3)2 | clear | clear | clear | clear | Halide solutions | NaF | NaCI | KBr | KI | unknown A | unknown B | Test 1: Ca(NO3)2 | Cloudy White (Nothing) | Clear | Nothing | light yellow (Nothing) | Nothing | Nothing | Test 2, Part A: AgNO3 | clear (Nothing) | Milky White | Gold (Cloudy yellow) | milky green (Cloudy yellow) | turned white, film developed on top layer | Milky | Test 2, Part B: add Na2S2O3 to test tube from part A | Dark Orange/brown | Clear | Dark Gold(precipitate yellow then clear) | milky green (no change) | white precipitation, settled on bottom | Milky | Test 3: NaOCI (Bleach) | Clear (Nothing) | Nothing | Nothing | Orange (Clear) | Nothing | Orange | Unknown A is identified as NaCI (Sodium Chloride), because in test#1 the solution turned a cloudy white color when Ca(NO3)2 (Calcium nitrate) was added. In the first part of test#2, when AgNO3 (Silver nitrate) is added, the solution turned white, with a thin layer of film developing on the surface.
The chemical method uses selective separation. By knowing the quantity of each component in a mixture gives one the ability to readily duplicate mixture at will. Therefore the procedure will need dutiful analyzing and documentation. Procedure: The mixing of the three components SiO2 (s), NaCl (s) and CaCO3 (s ) with water produced a white milky substance which was then filtered leaving SiO2 (s), and