Double Displacement Reaction Lab

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

The objective of this experiment will be to combine various substances, liquids and metals, and to observe their behavior when they are combined. The types of reactions observed shall determine the nature of these reactions: physical or chemical.

Steel wool was used since it is virtually pure iron. In this reaction single displacement had occurred.

There was an assortment of different changes indicating that chemical changes were taking place such as change in color or chemicals bubbling when combined with another chemical.

Single displacement reactions are reactions where one reactant replaces part of the other (Helmenstine, Thought Co, 2014). The elements with higher reactivity replaces the elements with lower activity, an example of this is the statue of liberty that is made from iron and coated with copper, the copper started reacting with air and a bluish green coating is formed. This coating reacts with the iron inside and a single replacement occurs and the outside copper is replaced back (Vista, 2017).

Chemical changes occurred in five out of the eight experiments completed in this lab. Although the main focus of experiment two was

1. What type of macroscopic evidence for chemical change did you observe during this experiment? Give at least three different examples.

b) Iron and Barium were present in unknown 3. Assigned unknown reacted with all 4 reactants and formed precipitate with 3 of them (Sodium carbonate, sodium hydroxide and Sulfuric acid). During the experiment it reacted very similarly to Iron (III) nitrate and Barium nitrate. For example, with it was tested against Ammonium Chloride, the color of the solution changed to a light green, very identically to Iron (III) nitrate and Ammonium Chloride. Besides, unknown 3 formed an orange brownish precipitate when it was tested with sodium carbonate. Iron (III) nitrate acted similarly. Moreover, unknown 3 reacted similar to Barium nitrate when it was tested against ammonium chloride and sulfuric acid. It did not form any precipitate with ammonium chloride but formed a very light white precipitate, which is identical to barium nitrate’s reaction against sulfuric acid. Therefore, the two present metal in unknown 3 are Iron and barium.

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 this lab there was a performance of a single replacement chemical reaction. The reactants of the reaction was solid iron metal, and copper (II) sulfate solution. This was a gravimetric lab and therefore it was crucial to begin by massing the reactants individually. The copper (II) sulfate was initially a solid. A procedure was conducted to dissolve the copper (II) solid by heating it in water to create the necessary solution. Once that was complete the following action was to react the solid iron and the copper (II) sulfate solution. The single replacement chemical reaction took place and there was a replacement of copper with iron. The products of the reaction was solid copper metal and an iron (II) sulfate solution. The solid copper was

Looking at the way a substance combining with another substances that can make a whole different reaction is very interesting. The main goal of this experiment is to observe some typical chemical reactions, identify some of the products, as well as summarize the chemical changes in terms of balanced chemical equations. This chemical reactions lab will require an apparatus, chemicals, procedure, and lab questions to help the performer of the experiment understand and comprehend the lab being performed. The lab is a way to see how the combining the different substances will create a slow, unique, and abstract reaction or it will reveal a quick and fast reaction by the combining of the different chemical substances we will be using throughout the lab.

Several of the chemicals were clear, including Sodium Hydroxide, Sodium Sulfate, Potassium Nitrate, Calcium Nitrate, Magnesium Nitrate, Sodium Chloride, and Sodium Phosphate. The other chemicals were all different colors, including blue and yellow. Potassium Ferricyanide was a dark yellow. Likewise, Iron (III) Nitrate was an orangey-yellow color. Lastly, Copper (II) Nitrate was a light blue. Throughout the lab, different reactions took place. Some products changed colors, formed precipitates, and one even produced gas. There was no reaction between Potassium Nitrate and any other reactants, including Potassium Ferricyanide, Sodium Phosphate, Sodium Sulfate, Sodium Hydroxide, Sodium Chloride, and Sodium Carbonate. These all remained clear, except for the Potassium Nitrate and Potassium Ferricyanide that has a natural yellow tint due to the color of the Potassium Ferricyanide. Magnesium Nitrate did not react with Potassium Ferricyanide, Sodium Phosphate, Sodium Sulfate, or Sodium Chloride. These all remained clear, and the Potassium Ferricyanide and Magnesium Nitrate remained a yellow tint. It did react with Sodium Hydroxide and Sodium Carbonate to form precipitates,

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

The purpose of this lab was to evaluate our skills of decanting a supernatant liquid without losing the solid and successful completion of a series of reactions. This was done through five chemical reactions involving copper. In this lab, elemental copper was put through five different chemical reactions in order to convert it into different compounds. By the end of the fifth reaction, the copper was back to its elemental state.