How Does Tin Chloride Mixture

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 Vitamin C turned to a red/orange color with no physical/chemical reaction. For the salt the solution turned to an orange color with no physical/chemical reaction. With the Alka-Seltzer, the solution turned to a brown color with no reaction as well. Last but not least, the Baking soda turned to an orange/brown color with no reaction.

chloride solutions, which resulted in a variety of colored flames. The color with which each cation

In a chemistry stockroom, a vial of an Unknown White Compound was found. In order to properly dispose of the substance, the substance has to be identified .The possible compounds has been limited to one of 15 different compounds. Also, approximately 5 grams of the Unknown White Compound (UWC) were available for testing. In order to determine the properties of the compound, a series of tests was conducted. These tests included a ph test, a conductivity test, a flame test, a sulfate test, a halide test, an ammonium test, a solubility test, and a carbonate test. Using the results of these experiments, it was hypothesized that the UWC is potassium chloride. To further confirm the hypothesis, a synthesis of potassium chloride was conducted.

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.

Eleven mystery test tubes labeled from K-1 to K-11 contained: 6M H2SO4, 6M NH3, 6M HCl, 6M NaOH, 1M NaCl, 1M Fe(NO3)3, 1M NiSO4, 1M AgNO3, 1M KSCN, 1M Ba(NO3)2, 1M Cu(NO3)2 respectively. The contents of the test tubes were determined by chemical experiments. Solution K-1 contained NiSO4 because when solution K-9, ammonia which was identified by its pungent odor, was added, an inky dark blue color was made. Iron (Fe (NO3)3) was determined to be in test tube K-2. KSCN was found in test tube K-11 since Fe (NO3)3 and KSCN makes a bloody color when mixed together. Flame tests were conducted in which K-8

This reaction is going in the reverse direction. This shows Le Chatelier’s Principle as it explains that when a system at equilibrium is subjected to a change that upsets the equilibrium, the system will neutralize the disturbance to restore equilibrium to the system. The reaction is moving in the reverse direction as when HCl is added to the solution, there becomes an excess amount of products because more molecules are being added. When the concentration of the products was increased, there were a greater number of effective collisions between the molecules in the products. This then increased the rate of the reverse reaction. Due to the excess amount of products, the system shifted in the reverse direction in order to decrease the products. By moving in the reverse direction, the system was able to produce more reactants to reduce the products. This brought the system back to

The purpose of this experiment is to distinguish the relationships between reactants and products, in addition to expanding on concepts such as single displacement reactions, mole ratio values, moles to mass, theoretical yields, limiting reactants, excess, stoichiometric relationships and percentage errors.

The Chemical Baggies Lab demonstrated to students how certain chemicals cause diverse chemical or physical changes depending on what substances were mixed together in a designed controlled experiment. During the process of this experiment, almost identical observations were made about different combinations of chemicals that had at least one substance in common. For example, the frequent observation that was made throughout the experiment was that heat was felt. Even though there were distinct chemical combinations, there was one substance that generated a certain observation or characteristic, such as a mixture has to comprise of the phenol red for there to be a color change, which was learned from this lab. Also, calcium chloride

Unknown 2: Silver ; Unknown 2 Forms precipitate with HCl, then confirms by turning black with NaOH. It remains clear when tested with NaOH after silver removal indicating that iron is not present. No reaction takes place during the reaction with SCN and HCl further indicating that iron is not present. Potassium ferrocyanide does not form a blue precipitate indicating that zinc is not present. Therefore unknown two only contains silver.

During the flame testing of one compound, a bit of the sample was dropped into the flame, which contaminated it for the remaining compounds that were to be flame tested. When the flame colours we observed were compared with actual colours of compounds, which showed that many of the colours we recorded were inaccurate. This occurred due to the contamination of the flame. In addition, many times the same spatula was used, which also led to the incorrect flame colours, since instead of one metal ion, there was a trace of

Experimental approach: In the first reaction, copper metal turnings oxidize when put in contact with nitric acid and become copper nitrate.

The main objective of this experiment is to carry out qualitative analysis to identify metal cations in unknown solution 1.

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

UV-VIS spectrophotometry is one of the most widely-used methods for determining and identifying many inorganic species. During this experiment, this spectrophotometry was used to determine the equilibrium constant, Keq, of the Fe3+(aq)+SCN-(aq)↔ FeSCN2+(aq) reaction. By determining the amount of light absorbed, the concentration of the colored FeSCN2+ solution was also quantitatively determined. From that data, the concentrations of the reagents at equilibrium may also be determined. This experiment should thus provide a Keq value without computing for the concentration of each of the species in the reaction. This