Copper Sulfate Lab Report

Potential error could result in when quantitatively transferring in any step and spillinng or not transferring all of any given solution. When diluting each flask has a different level for where its specific volume is, so overfilling the flask is possible when not being focused on. The condition of each penny can impact the results by if some copper was chipped off, or if anything attached to the pennies could impact test results. All of these could result in a different than desired copper percentage. It is important that the absorbance of each penny be within the range of absorbance the calibration curve has. This is because the curve created for this lab was made with 0.00 – 10.00mL of Cu^(2+)stock solution when using those values idealy this curve should therefore be 0-100% copper percentage. If values were found outside of this calibration curve then there would be problems with either calculations or a different curve would be needed to properly record

In this task the concentration of an unknown sample of copper sulphate using colorimetry was used to find the concentration. In this investigation copper sulphate was used which is CuSO4.5H20 as a formula. To make a standard solution which was 1M, the same clean equipment was used to make up the standard solution as used to make sodium carbonate. However there was one difference and that was that the hot distilled water was used to dissolve the copper sulphate crystals. There had to be enough hot water in order to dissolve the crystals into the beaker and then add cold distilled water to cool the solution.

The purpose of the experiment is to cycle solid copper through a series of five reactions. At different stages of the cycle, copper was present in different forms. First reaction involves reaction between the copper and nitric acid, and copper changed from elemental state to an aqueous. The second reaction converted the aqueous Cu2+ into the solid copper (2) hydroxide. In the third reaction Cu(OH)2 decomposed into copper 2 oxide and water when heated. When solid CuO reacted with sulfuric acid, the copper returned to solution as an ion (Cu2+). The cycle of reactions was completed with the reaction where elemental copper was regenerated by Zn and Cu

Washing of the copper is necessary in this experiment to separate the iron from the copper and make sure the iron is not counted in the mass of the copper.

The purpose of this lab was to determine the limiting reactant in a reaction between copper sulfate and iron. Using the reaction between copper sulfate and iron, the reaction was observed to see the reaction and transformation of matter. The copper sulfate was placed into a beaker, as the excess reactant, then iron filings added until the heated solution was completely reacted. This reaction created an excess of leftover. The law of conservation of mass can be observed in this reaction, and using the data found, the percent yield calculated.

Before the synthesis of the Copper Iodine Compound, the identities provided (CuNO3)2 and Nal weighed 1.65 g and 4.7 g, respectively. After being weighed, the (CuNO3)2 exhibited a blue color, while the Nal, through observation, was a white color. However, when both identities were combined, the product turned into a brown and red rocky material. Once 20 mL of deionized water was added, the product quickly turned pale pink paste. After the solution was repeatedly washed with a total of an additional 100 mL of deionized water, the product was powdery and pink with small grains, and was left to air-dry. Once the product was air dried, it was observed to be a pale pink color, while the filter paper was stiff as the product was hard and dry. Therefore, the solid was scraped off onto a recrystallizing dish. However, the mass of an empty recrystallizing dish needed to be recorded in order to compare how much of the synthesized copper iodide was obtained. Within this case, the empty recrystallizing dish used weighed 32.01 g, the product on the empty dish weighed 1.03 g, having a total weight of 33.04 g.

XIV. Record your observations of the dried, cooled copper metal and weigh the recovered copper.

Refer to the reaction of iron nails with a copper solution assignment in Module 3, Section assignment 3.4 Part F of the Chemistry 11 course.

Purpose: The purpose of this experiment was to observe the many physical and chemical properties of copper as it undergoes a series of chemical reactions. Throughout this process, one would also need to acknowledge that even though the law of conservation of matter/mass suggests that one should expect to recover the same amount of copper as one started with, inevitable sources of error alter the results and produce different outcomes. The possible sources of error that led to a gain or loss in copper are demonstrated in the calculation of percent yield (percent yield= (actual yield/theoretical yield) x 100.

The lab performed required the use of quantitative and analytical analysis along with limiting reagent analysis. The reaction of Copper (II) Sulfate, CuSO4, mass of 7.0015g with 2.0095g Fe or iron powder produced a solid precipitate of copper while the solution remained the blue color. Through this the appropriate reaction had to be determined out of the two possibilities. Through the use of a vacuum filtration system the mass of Cu was found to be 2.1726g which meant that through limiting reagent analysis Fe was determined to be the limiting reagent and the chemical reaction was determined to be as following:-

The objective of this experiment is to find out if I can slow down or speed up the reaction between copper sulfate and an iron nail. This experiment is significant because it is a test of what I will do with a francium and water reaction. The reaction between copper sulfate and iron is a single displacement reaction where the iron eventually replaces the copper and creates iron sulfate. Iron is able to displace copper in this reaction because it is more active. In the reaction iron can either solid or aqueous but copper sulfate must be aqueous to facilitate the reaction.

The experiment was composed of a series of five successive reactions that utilize five complementary reagents to produce four different copper compounds before reverting it back to its original form. The first chemical reaction that was completed was an oxidation-reduction reaction between copper (Cu) and nitric acid (HNO3), where copper was the reducing agent, the substance that loses electrons for reduction to occur in another substance, and nitric acid was the oxidizing agent, the substance that gains electrons the donated electrons so that reduction can occur in another substance. During this reaction copper was oxidized from an oxidation state of 0 to an oxidation state of +2, which resulted nitric acid becoming reduced. In addition, this

In Part C copper seemed to be the least reactive with the nitrate solutions of all of the metals that were tested. On the other hand, magnesium seemed to be very reactive, as it did have a reaction with each of the nitrate solutions. In Part B it seemed as though iron had the most violent reaction with hydrochloric acid. Magnesium is combined with both copper sulphate (CuSO4) and copper nitrate (Cu(NO3)2). The reactions with both solutions show some similarities such as producing particles.

When the zinc was added to the copper (II) sulfate solution, the solution started to bubble. As the solution was stirred, it turned a cloudy blue. Small flecks of a brown solid were visible. As the solution became colorless, the brown solid settled to the bottom of the beaker. The solid formed was copper in its elemental state. The color faded from the solution as the copper ions slowly formed into solid copper. The copper was poured into a funnel with filter paper and washed three times with 25 mL

And copper (II) ions were reduced to copper because it gained electrons and its oxidation number changed from +2 in copper (II) ions to 0 in copper.