Determining The Precipitation Reaction Between Two Double-Exchange Reactions

The experiment is to observe a variety of chemical reactions and to identify patterns in

In Experiment B the limiting reactant was determined to be CaCl2 when two drops of the test reagent 0.5 M CaCl2 was added to the supernatant liquid in test tube 1, and a precipitate formed. Since there was a reaction, there was C2O42- in excess and Ca2+ is the limiting reactant in the original salt mixture present in test tube 1 . This was further confirmed when two drops of the test reagent .05M K2C2O4 was added to the supernatant liquid in test tube 2. There was no precipitate because Ca2+ was not present since it was the limiting reactant and instead C2O42- was in excess.

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.

to the unknown solution in order to completely precipitate the cations in part A. 2 A compound

In reference to the analysis of anions, Table 1 shows that a precipitate was formed when our unknown was combined with HNO3 and AgNO3, thus indicating the presence of a chloride ion. Because our unknown did not form a precipitate due to HCl and BaCl2, separate, effervesce, or smell, we concluded that neither sulfate, nitrate, carbonate nor

Introduction – A double replacement reaction is a chemical reaction between two compounds where the positive ion of one compound is exchanged with the positive ion of another compound. If you have the reactants of two reaction solution that you can determine the products. All you need to do is pair the positive parts of the compounds with the other compounds negative part. Once you find the products you can determine their phase of matter by using Table H. You can also use Table F to determine the solubility guidelines for aqueous solutions. If the product falls under soluble or exceptions to insoluble it is in the aqueous stare. If the product falls under

Experimental Method: A filtration apparatus was set up. Solid iron(III) chloride hexahydrate was dissolved in water. In a separate container, sodium acetate trihydrate (NaC2H3O2 x 3 H2O) was also dissolved in water. Sodium acetate trihydrate was then added to iron(III) chloride. 2, 4-pentanedione (C5H8O2) was dissolved in methanol; it was then added to the iron(III) chloride/sodium acetate solution. The product of this mixture was filtered, and the precipitate

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

There were five main purposes of the maalox lab that we wanted to accomplish. This included producing two precipitates, classifying reactions, providing visual evidence on a chemical change, using pH indicators to identify bases and acids, and describing what happens during neutralization. In the lab, there were two reactions that occurred. The reaction happened when there were reactants that combined to create end products. In the first reaction, the reactants used were alum and ammonia. The products that formed were aluminum hydroxide, potassium ammonium sulfate, and ammonium sulfate. In the second reaction, the reactants were magnesium sulfate and ammonia. The products that formed from the magnesium sulfate and ammonia were ammonium sulfate and magnesium hydroxide. Overall, we were able to accomplish the five main goals of the lab and were able to identify the reactants and products in each of the reactions.

In part 1, the precipitate that forms is a aluminum hydroxide and in part 2 it is magnesium hydroxide. A precipitate is an insoluble solid that emerges from a liquid solution. When the emergence of the insoluble solid from solution happens, it is called precipitation. The property change in the reactants of the lab are when the water, alum, ammonia, react and create the aluminum hydroxide. When the precipitate is formed, it is an endothermic reaction because the change in the product, aluminum hydroxide, decreases in temperature. This is a chemical reaction because different elements rearrange themselves to form a new substance and while they do so, they either absorb heat or give it

During the Law of Conservation of mass Lab I mixed various solutions and observed their chemical and physical change. The chemical change that occurs is the result of a new substance in all three experiments the Acid base Neutralization, Formation of a precipitate and the Formation of a gas. During the lad I learned that when you mix white vinegar with sodium hydroxide the result is a dark pink substance, when lead acetate and potassium iodide it forms a precipitate and water with alka seltzer results in the evaporation of the substance. While doing this lab I was surprised that the precipitate would be powdery and yellow because I thought that it would still be a liquid not powdery.

Ameera Inshanally Chemistry 113.1 7/14/14 Experiment #3: Precipitation Reactions Lab Partner: Steve Introduction Many reactions occur with a resulting precipitate and some do not, according to the solubility rules. Some compound are soluble under certain conditions and others are not. The formation of a solid when two compounds react is called precipitation, resulting in precipitate. This lab helps one to better understand how precipitate is formed and under what conditions.

The following lab report will discuss an experiment conducted to study the methods in which water can be tested for different metals and anions. This lab report will discuss the methods and results of the second half of the experiment. In the first half, various solutions (each containing either a particular metal or anion) were reacted with a series of substances and the observations were recorded. These observations were then used to develop a separation and identification scheme to test for each particular metal or anion when given a solution of unknown composition. This experiment demonstrates a practical use of precipitate reactions.

To start the experiment, a 150 mL beaker was weighed. By using the tare function, 6.619 g of nickel sulfate was added to 150 mL beaker. The substance was in the shape of crystals and had a teal green color. Then, 15 mL of deionized water was added to the beaker containing the nickel sulfate hexahydrate. The beaker was then set atop a hot plate and heated on setting four while constantly being stirred until the solid had dissolved. After the heating had occurred, the color of the liquid in the beaker was a light green color. The 150 mL beaker was taken off of the hot plate and set on a ring stand base to cool slightly. Next, on the same scale as before, 4.425 g of potassium sulfate was added to a 200 mL beaker. Then 50 mL of deionized water was added to the 200 beaker. It was heated at setting four on the hot plate and stirred until dissolved. Then warm nickel sulfate (150 mL beaker) was poured into the solution of hot potassium sulfate (200 mL beaker) and mixed

When two different ionic compounds are combined, it is possible for a precipitate to form. A precipitate is an insoluble solid that emerges from a liquid solution. The process in which the insoluble solid is formed is known as precipitation. For a precipitate to form, it should be part of the insoluble substance found in Figure 1.1.