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Compare And Contrast The Separation Of Copper Chloride And Sodium Chloride Mixture

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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 methanol was then evaporated from the copper (II) chloride and methanol solution leaving behind the copper (II) chloride. …show more content…

The solubility rate of copper (II) chloride in methanol is 53g/100ml whilst the solubility rate for sodium chloride is 65g/ml. Although there solubility rate is fairly close the difference is enough that when little amounts of methanol is added only the copper (II) chloride dissolves. A factor that affects the solubilty of metals is their molecular mass. Copper (II) has a molecular mass of 63.546 whilst sodium has a molecular mass of 22.989769 meaning copper has higher solubility rate than sodium, this is because as the molecular mass of a metal increases it becomes difficult for molecules to hold onto their solute particles and when those particles break away they can easily dissolve into the solvent. Therefore because coppers molecular mass is greater than sodiums it’s solute particles breakaway with less resistant meaning copper dissolves better. Hence in the sample only copper (II) chloride will dissolve leaving the sodium chloride behind once filtered through. The copper (II) chloride can then be obtained by evaporating the methanol; which has a boiling point of 65 degrees celsius whilst copper (II) chloride has a boiling point of 993 degrees celsius, thus allowing the methanol to be easily evaporated out of the solution eliminating concerns of the copper (II) chloride evaporating alongside the methanol. Purpose To investigate different methods of separating copper (II) chloride and sodium chloride in order to obtain the original masses of both substances. Hypothesis Copper (II) chloride and sodium chloride can successfully be separated from eahothe by using dissolution, filtration and evaporation Appartus 4g copper (II) chloride 4g sodium chloride 50ml

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To separate the Ramos mixture the group first first conducted the dissolve, filter, evaporate method, and prepared the lab for as well. Though for this lab the substance

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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.

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After placing the aluminum in said beaker, one should gather a stir stick and stir the solution in order to speed up the reaction. One should stir the solution until there are no visible silver pieces of aluminum left in the beaker of what was the copper (II) chloride solution. When there are no visible silver pieces of aluminum left in the beaker, this means that the reaction has occurred. After the reaction has occurred, one needs to separate the products, which are copper and aluminum chloride, from each other in order to see how much copper was able to be produced. Seeing as the products are a solid in the form of copper and a liquid in the form of aluminum chloride, the process of filtration can be used to separate them.

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Throughout the experiment, copper was altered a total of 5 times, but after the final chemical reaction, solid, elemental copper returned. Each time the solution changed color, a precipitate formed, or when gas appeared, indicated that a chemical reaction was occurring. For the first reaction, copper was added to nitric acid, forming the aqueous copper (II) nitrate (where the copper went), along with liquid water, and

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The values of mass percent lost by dehydration for each trial were found to be relatively consistent and accurate in comparison to the known value of the mass percent of water for copper sulfate (36.08%). This is expected because the values should be at the same fixed values across the samples, as they are all using the same sample of the hydrate copper sulfate. We can assume that if the experimental value was lower than the known value, there was still some water present in the salt that was not fully dehydrated. If the experimental value was higher than the known value, we can assume that heat was applied for too long of a duration, leading to decomposition of the copper sulfate samples. To get more accurate results with less variation, experimenters could exert extra effort to ensure that variables such as duration of heating and temperature of the flame remain exactly consistent across the trials.

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As the water was added to the heated sample, the solid copper chloride began to dissolve into a pretty blue-green solution, as a result of the compound breaking apart into individual Cu2+ and Cl- ions. When the water was first mixed with the copper chloride, it dissolved the solid pretty slowly, turning into a sort of mush at first. However, eventually, the water dissolved all of the solid copper chloride and the solution was homogenous. Since the compound just changed physical form, from solid to liquid, this change was purely physical. Just as in the first part of the experiment, the chemical character of the compound was not altered, so the compound did not experience a chemical change.

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