Correlation Between Zinc And Copper Solutions

Repeat each concentration of sodium chloride solution 5 times to achieve a more accurate average. This is important because it can help me to detect any anomalies in my data caused by mistakes or errors. Identifying these mistakes can help to strengthen my investigation and reduce the amount of anomalous results.

This experiment is based on determining the chemical formula for a hydrated compound containing copper, chloride, and water molecules in the crystal structure of the solid compound, using law of definite proportion. The general formula of the compound is CuxCly•zH2O, and aim is to determine chemical formula of this compound.

After 15 minutes, the iron strip was corroded (its color was reddish brown), and the color of the solution slightly changed to green.

The objective of this lab was to use prior knowledge about the Law of Conservation of Matter and of different types of chemical reactions in order to evaluate if aluminum disappears during the reaction and copper appears. The reaction that occurred between Copper (II) Chloride and aluminum was a single replacement reaction. Clear signs that a chemical reaction took place include heat release/temperature change, color change, and formation of a precipitate. When a single element, in this instance aluminum, replaces another element in a compound, copper, a single replacement reaction occurs. A basic formula for these reactions is AB + C → AC + B.

After this, the solution was poured into a volumetric flask just about to the 1dm3 line and then it was left there to cool to the same temperature as the room before filling precisely to the 1dm3 line with distilled water. The molar mass of CuSO4.5H20 was 249.5 so that means 249.5g of copper sulphate was needed to dissolve, in order to make a standard solution, into 1dm3of distilled water. Following this, a linear dilution of the CuSO4.5H2O was made in order to be used to make a calibration curve after using the colorimeter to write down the absorbance of each sample. A linear dilution is diluted with distilled water in order for it to make the concentration weaker and weaker. For this investigation, the dilutions made ranged from 0.01 to 0.1 M/l . It was essential to only make up 10cm3

The first step that needed to be done in this experiment was adding hydrochloric acid (HCl)

Yes, because the solution seen was still blue meaning that not all the copper chloride was extracted from the beaker.

The Cu Later lab experiment is designed to allow you to practice lab skills in implementing and performing a series of reactions. Specifically, four types of chemical reactions will occur: oxidation/reduction; double replacement; single replacement; and decomposition. You will begin with a known amount of copper metal, which, after progressing through several steps, is reproduced. In this experiment you will observe and record the various changes such as heat, color changes, and production that occur. This procedure is used to observe some chemical reactions of copper and its compounds while also performing the lab appropriately as to retain the copper as much as

Heavy precipitate emerged immediately and solution turned white in color; solution then became opaque and turned light, bright blue in color.

-If the copper metal is submerged in the silver nitrate solution then in reaction, a pure, solid (Ag) silver product is created with an excess of (Cu (NO3)2) copper (II) aqueous liquid because a single displacement reaction occurs where the balance equation is then

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.

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.

Distilled water was used to dilute the solutions used in the cells, a hot plate was used to increase the temperature, sand paper to sand the metals, filter paper to act as the salt bridge, thermometer, and a voltmeter to measure the voltage. For part 1 of the experiment a total of 6 beakers are needed to hold the solutions to conduct the first test. For each metal two beakers are filled with 30mL of the .1M of solution for that metal using the graduated cylinder. Each metal solution is then paired with another metal solution such as Zinc with Copper and Zinc with Iron. Use the filter paper and soak it in the KNO3 solution to create a salt bridge, repeat this three times for each pair of metal solutions. Proceed to sand the metals then place them into their respective solutions and use a voltmeter to measure the voltage. Make sure to place the right clamps on the anode and cathode you will know if it is wrong because the voltage will be negative. Repeat this step for each of the pair of solutions then proceed onto part 2. In part 2 of the experiment zinc and copper solutions were used. Take two 50mL beakers and fill one with 30mL of zinc solution and the other with 30mL of the copper solution and connect them with filter paper that was soaked in KNO3. Sand the metal pieces for copper and zinc then place them in their respective solutions then proceeding to connect the voltmeter to

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

0.5% of copper sulphate solution was added by drop at a time and and the test tube was shaked continuously.