Double Replacement Reaction Lab Report

2. Write a statement to explain the molecular composition of the unknown solution based on the results obtained during testing with the Biuret solution and each sample solution.

To determine which ions are present in the two unknown solutions. This will be accomplished by mixing three known solutions with three testing solutions. You will use this information to determine which ions are present in the unknown solutions.

3. Carefully felt the sides of the test tube and observed the resulted chemical reaction for about 30 seconds.

Procedure: In this experiment, various chemicals were mixed together, to determine a reaction. Using two drops from chemical 1 and two drops of chemical two, unless otherwise stated, then recording the type of physical reaction or color changes that occurred.

The purpose of this particular lab was to experiment and identify the chemical and physical changes throughout the experiment.

8. The Tubes were observed for a final 5 minutes, noting any color changes in the solutions.

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

Conclusion – The main idea of this experiment is that if you have the reactants of a double replacement reaction that you should be able to find out several things. First, you can figure out the products from switching the positive ion with the other positive ion. Once you have found the products you can determine the phase of matter they are in from Table F and H. Finally, you can also determine whether the reaction went to completion or not. The observations and data above leads me to believe that our experiment is valid. We were very careful and observant of the directions that needed to be taken. Once source of error could have been that certain substances were placed in the wrong wells, causing your data to stray from the correct information. One way this experiment could be applied to a real life situation is he residue in the bottom of a glass in your bathroom. There is stuff dissolved in water, and any trace of water left in a glass will eventually evaporate and leave the residue.

The materials needed for this experiment included test tubes, a test tube holder, the unknown compound #202, 35mL beakers, gloves, safety goggles, ethanol (to clean equipment), stirrer (to mix solutions), the 15 possible compounds that are provided, pH strips, distilled water, wooden splints, spatula to get out unknown compound #202, waste bucket, Bunsen burner, graduated cylinder, 500mL beaker for the waste, plastic dishes to measure out compound and the scale.

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 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

The main purpose of this experiment was to show that single displacement reactions between metals according to their reactivity, with more reactive elements having the power to displace less reactive elements and take their place in a chemical compound (Beran, 2014). This was supported by the results of the experiment, where solid metals were combined with aqueous solutions that contained another element, and reactions only took place when the solid metal was more reactive than the other element in the compound. Only three attempted trials resulted in a failure to produce a reaction, namely the combinations of copper with hydrochloric acid, and copper with nickel sulfate. The outcomes of these trials are justifiably reasonable because copper is ranked lower in the

Well B1 was filled Wells B1 through B6 had each of its wells’ pH tested by a pH strip indicator. Well B1 was filled with hydrochloric acid and turned the pH strip a dark pink or red rose color, the pH was recorded at one. Well B2 was filled with acetic acid and turned the pH strip an orange color that had a pink hint to it, the pH was recorded at three. The fact that the names of these substances have the word acid in them, indicates that these two substances are acids. Well B3 was filled with the distilled water turned the pH strip an orange color with a darker ring of orange, almost red around it, the pH was recorded at four.

In the fourth reaction, 15 mL of 6.0 M sulfuric acid was added to the copper (II) oxide while stirring. The balanced equation for this reaction is as follows:

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.