Cucl3 Synthesis Lab

An error that could have been present during the lab includes not letting the zinc react completely with the chloride ions by removing the penny too early from the solution. For instance, the percent error of this lab was 45.6%, which was determined by the subtraction of the theoretical percent of Cu 2.5% and the experimental percent of Cu 3.64% and dividing by the theoretical percent of Cu 2.5%. This experiment showed how reactants react with one another in a solution to drive a chemical reaction and the products that result from the

While the solution dissolved, 50 mL of distilled water was added to a 150 mL beaker and heated on the hot plate. When the solution started to boil 2.65 grams of Na2SiO3*5H2O was added to the beaker with a stir bar and heated to a gentle boil. When both solutions began to boil, the sodium silicate solution was slowly added to the sodium aluminate. The solution was kept at 900C for 60 minutes and stirred with stir bar. After 60 minutes, the zeolite solution was cooled for 5 minutes and for the magnetized zeolite , 0.78 grams of FeCl3 and 0.39 grams of FeSO4*7H2O was added to the flask and stirred until the iron parts dissolved.

A spectroscopy curve was produced of the acid and the absorbance of the unknown mineral could be obtained in order to find what that unknown copper is. Through these methods there is not preferred method when it comes to finding the percentage of an unknown substance, but which is more effective in accurately depicting what that unknown substance is. Standard deviation plays a major part in this experiment to help balance out and find the mean of the unknown substance to help constitute what it is. Through this the difference between smelting and roasting is that one produces a metal from its ore and the other drices off the carbon to obtain an

If it was NaCl there would have been no precipitate formed during this final

The products were aluminum chloride and copper. A change in properties demonstrates that a chemical reaction occurred. One property that changed was the colors. Initially the aluminum foil was a shiny silver, and the copper chloride was a green-blue liquid. After we placed the aluminum into the copper chloride solution, the liquid clouded up a lot and turned to a light grayish hue.

The purpose of the lab was to discover the properties and the trends of the alkaline earth metals. In part A, the trend was as the atomic number increase in the alkaline earth metals the elements are more reactive. The alkaline earth metals each have two electrons in their outer shell and because all electrons want to become stable they are ready to give up the two electrons. When they are combined with water, the chemical reaction occurs differently based on each element.

Exercise 1 1. Suppose a household product label says it contains sodium hydrogen carbonate (sodium bicarbonate). Using your results from Data Table 1 as a guide, how would you test this material for the presence of sodium bicarbonate? B BoldI ItalicsU Underline Bulleted list Numbered list Superscript Subscript33 Words

When we placed the aluminum foil in copper chloride, a chemical reaction occurred. Before the reaction took place we had aluminum foil and copper chloride as our reactants. After the reaction happened, the products were aluminum chloride and copper. After the foil was placed in the copper chloride, the color of the aluminum foil had changed from a shiny silver, to a deep red. Also, the color of the copper chloride changed from a light blue to a murky green.

The powder on the filter paper could've fell and this caused it to have a smaller percent purity, percent yield and also cause a lower absorbance and concentration of pure ASA. Another error would be not using a properly dried sample for the pure ASA in part C when making the crystals, this could have cause tye percent yield error. This would make a lower melting point. To prevent this from occurring next time there could be a dry sample that is completely dry and this would not alter the mass of the sample and this would make the solution have a more

As seen in table 1, the theoretical yield was .712 g of C_17 H_19 NO_3. The % yield of this experiment was 7.51 % of C_17 H_19 NO_3. . This low yield can be explained from a poor recrystallization technique combined with potential contamination. Throughout the experiment, the mixture changed color from green, orange, to yellowish lime, and eventually clear.

- ​A hydrate is a salt that contains water as a part of its crystal structure. The hydrate used in this lab was Copper (ll) Sulfate Pentahydrate. To heat the hydrate in this lab a crucible is needed. A crucible is a heat resistant container used to heat things to high temperatures. In this lab a mole was used to determine the measurements of all substances.

Copper Cycle Lab Report Ameerah Alajmi Abstract: A specific amount of Copper will undergo several chemical reactions and then recovered as a solid copper. A and percent recovery will be calculated and sources of loss or gain will be determined. The percent recovery for this experiment was 20.46%.

The percent recovery of the copper was calculated using the equation, percent recovery = (the mass of the copper recovered after all the chemical reactions/the initial mass of the copper) x 100. The amount of copper that was recovered was 0.32 grams and the initial mass of the copper was 0.46 grams. Using the equation, (0.32 grams/0.46 grams) x 100 equaled 69.56%. The amount of copper recovered was slightly over two-thirds of the initial amount.

If only one reactant is increased, then the chemical reaction will only produce a certain amount of products after the limiting reagent is used up, and in this experiment, the most mass the reaction could produce was 0.4 grams. Although we kept adding calcium chloride, not adding sodium hydroxide in the same proportions will not yield more product, which is the main goal in conducting this lab. We should have seen a plateau at 0.4 grams to show that the limiting reagent inhibited further Ca(OH)2 production, but we made several mistakes in our experiment, which made the data unusable to conclude. Once again, the data is polluted, so these number are not accurate, but it is the data our group has to work with. The theoretical yield should have been more than the actual yield, and the percentages should have been less than 100.

The solution with the pigments was spotted 15 times on both region A and region B and then allowed to dry. When the plate was dry it was placed into the tank for at least 20