Lead Iodide Essay

solutions using qualitative analysis techniques. 1 Silver (Ag + ) and lead (Pb 2+ ) created a solution of

One of the most important skills to have in the chemistry lab is the understanding of how chemicals will react. Knowing for example, how a chemical will react with a metal, is an excellent way of determining the amount of a particular metal in a deposit. This knowledge was used in this lab to determine the amount of copper in an unknown sample mixture. It is also known that the determination of the percent concentration of a certain solution, will directly effect the percent transmission and absorption of a solution, dependent upon its dilution. By first testing known concentrations of a solution, and plotting this information graphically, a line is formed

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.

This lab revolves around precipitate it reactions. The precipitate reactions happen when it had cations (positive atoms) and anions (negative atoms) in aqueous solutions combined to form an insoluble ionic solid, which is called a participate. In order for these reactions to occur they must be Aqueous and this can be determined by using solubility rules. Predicting these reactions a sign test to find out which ions are present in a solution. Double displacement reactions are the kinds used in this lab. This means that the compound will switch partners and form a bond with a different part. The reaction occurs in Aquarious solution and one of the products that is formed is in soluble.

Seven test tubes were labeled numerically with 2 mL of VO3- and H2SO42- added to each tube. A small pea size portion of solid Na2SO3 was added to the first test tube. Then, 20 drops of distilled water were added to the second test tube. In the third test tube, 20 drops of (.2 M) NaBr were added. Then, to drops of (.2 M) NaNO2 were added into the fourth test tube. A small portion of Fe(NH4)2(SO4)2 * 6H2O was added into the fifth test tube. The sixth test tube had 20 drops of (.2 M) H2Cr2O4 added, where the seventh test tube was the control tube with no additional chemicals added. All the test tubes were left to react for 3 minutes and then heated in a heated bath for approximately 20 minutes.

The purpose of this experiment was to learn how single replacement reactions occur when tested and how to identify one. The first test, zinc and copper (II) sulfate, produced copper. The chemical reaction also had a chemical change, which was a color change. A similar reaction occurred when tested with magnesium and copper (II) sulfate and copper and silver nitrate. This occurred because zinc, magnesium, and copper are more active than the elements in the ionic compound.

The Spec 20 was turned on and set the wavelength for maximum absorbance for copper(II) solutions, 600 nm, 30 minutes prior to the start of the experiment. 12 test tubes were cleaned thoroughly and a tape label was added to the top identifying which solution would be placed within and then they were set in a test tube rack to dry. The amount of solid copper(II) sulfate pentahydrate (CuSO4 H2O ) needed to create 20.0 mL of 0.5 molarity solution was calculated, using the equation for molarity the molar mass, as 2.50g. The CuSO4 H2O and a 100 mL beaker were carried to the instrument room. Small amounts of solid CuSO4 H2O were placed onto a paper towel which was gently tapped over the beaker until exactly 2.50g was reached. Approximately 5

The many different aqueous solutions involved were potassium nitrate, zinc nitrate, potassium ferricyanide, sodium phosphate, sodium hydroxide, magnesium nitrate, copper (II) nitrate, sodium chloride, iron (III) nitrate, calcium nitrate, sodium sulfate, and sodium carbonate. These different reactants were combined to test whether or not a precipitate, color change, or both would occur in that in that those reactions. The purpose of this lab was to demonstrate what a double replacement reaction as well as a precipitate

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

When one looks back at the procedure of the experiment, trials 1, 2, 3, 4, 5, and 6 all use 6 M HCl for their reactions, and if this were to be substituted for 6 M HNO3, then these reactions would have still taken place, except in trial 2 because copper is less reactive than hydrogen in all cases, but their final observations may yield different colored solids and solutions (Beran,

There are numerous ways of isolating and purifying a substance, and an investigation of the differences of each procedure were performed. In two different procedures, lead nitrate and potassium iodide were used to isolate and purify pure solid lead iodide, and the differences in the limiting reactant and solid lead iodide was observed. The amount of solid lead iodide was calculated by the measuring the mass of which the solid lead iodide was created in before and after the purification of solid lead iodide.

Iodine is one of the most critical elements necessary for normal functioning of the human physiology. The significance of iodine to the thyroid gland is already well established but its role as a potential anti-carcinogenic agent has been realized only in the recent past. At the molecular level iodine can be a potential anti-inflammatory agent as well as an antioxidant and is known to facilitate apoptosis1. These properties make iodine an ideal candidate to serve as a viable anti-cancer agent. A correlation between iodine and cancer was first reported by a study carried out by Stocks in 1924. The study highlighted that there is a high incidence of cancer in the geographical regions with high rates of goiter2. This observation

This experiment was designed on the basis of previously obtained knowledge of metals and their reactivity with acids. It is known that when metals

At the end of the experiment when the lid was removed, it was found out that the blue colour of the copper (II) sulphate solution has faded away. It was turned to pale grey and there were some precipitates present. It was the zinc powder that was in excess to ensure that the copper (II) sulphate solution could react fully with the zinc powder.