Understanding Of Basic Solubility Principles And Precipitation Reactions

In experiment A the results from the precipitation of CaC2O4 H2O from the salt mixture were obtained by weighing the items listed on Table 1 on a scale.

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

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

The purpose of this experiment is to study ionic reactions, to be able to write balanced equations, and to be able to write net ionic equations for precipitation reactions.

For the cation analysis, 0.566 g of an unknown compound was dissolved completely in 5mL of distilled water in a centrifuge tube, thus confirming this solution as a stock solution. A flame test was performed on the stock solution to give a general idea of what test was to e preformed on the stock solution deriving the information from our logic trees in part 1. The logic tree from part 1 and the flame test confirmed that we needed to conduct an ammonia test on the stock solution. To being the ammonia test, 15 M NH4OH was added drop wise (about 20 drops) to the stock and the color of the solution and the color of the solution was recorded. 10 more drops of 15 M NH4OH

We were given known aqueous solutions of following reagents:  BaCl2  Na2SO4  MgSO4  Na2CO3  CH3COONa 2. Following known solid hydrates were also given to us:  CuSO4  BaCl2  MgSO4  Na2CO3  Na2SO4  CH3COONa 3.

For the first part of this experiment, six dry test tubes were obtained and labeled accordingly to test the following halides: 2-chlorobutane, 2-bromobutane, 1-chlorobutane, 1-bromobutane, 2-chloro-2-methylpropane, and bromobenzene. To each of the six test tubes 2ml of 15% sodium iodide in acetone was added. 4 drops of the appropriate halide was added to the test tube labeled for that specific halide. After adding the halide, the test tube was then shaken to mix thoroughly. If a precipitate formed the time it took was recorded. Since none of the solutions formed a precipitate at room temperature after five minutes, the test tubes were placed inside of a hot bath at about 50°C. After one minute, the test tubes were taken out of the hot bath and allowed to cool. If any test tubes formed a precipitate, the time it took was recorded on a table.

Many ionic compounds can be separated from an aqueous solution in solid form using evaporation and centrifugation techniques. Evaporation results in separation by phase, as a liquid is vaporized, and centrifugation results in separation by weight. Evaporation was used to isolate the insoluble compound sodium sulfate as a solid. Centrifugation was used to isolate the soluble compounds silver chloride, barium sulfate, and zinc hydroxide as solids. To

Solubility Lab Report The purpose of this lab was to demonstrate the solubility of compounds created through reactions between certain dissolved substances. The solubility or insolubility of these compounds creates a visual demonstration of solubility rules. To obtain the data, the molar mass of each compound was calculated, and divided by 100 to determine the mass (in grams) needed. The compounds used in the lab include KNO3, Na2CO3, NH4Cl, NaOH, Pb(NO3)2, K2CrO4, AgNO3, CoCl2, Ba(NO3)2, CuSO4, and NaI. Filter paper was placed on a scale and tared, and the correct amount of salt was measured using a scoopula.

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

1. Start Virtual ChemLab and select Precipitation Reactions from the list of assignments. The lab will open in the Inorganic laboratory.

The cations in both the known and unknown samples were identified by using qualitative analysis, of which were determined to be acidic, basic, or neutral by using litmus paper. Acid-base reactions, oxidation-reduction reactions, and the formation of complex ions are often used in a systematic way for either separating ions or for determining the presence of specific ions. When white precipitate formed after adding hydroxide, aluminum ion was determined to be present in the solution. However, nickel was determined to test positive when the solution changed to a hot pink color after adding a few drops of dimethylglyoxime reagent and iron was present when the solution was a reddish brown color when sodium hydroxide was added to the mixture at the very beginning of the experiment. Qualitative analysis determines that ions will undergo specific chemical reactions with certain reagents to yield observable products to detect the presence of specific ions in an aqueous solution where precipitation reactions play a major role. The qualitative analysis of ions in a mixture must add reagents that exploit the more general properties of ions to separate major groups of ions, separate major groups into subgroups with reactions that will distinguish less general properties, and add reagents that will specifically confirm the presence of individual

Different techniques can be used to determine the solubility of a solution, such as filtration through paper cloth or evaporation by heat. In this experiment, the solubility was obtained through evaporation of the solvent by heat. Potassium sulfate and sodium chloride will used in solutions to test the solubilities at room temperature and approximately 40℃. Potassium sulfate will also be used in a solution to test the uncertainty of the experiment.

The purpose of this experiment is to identify some commonly occurring anions & to study some of the reactions used for their identification.

In conclusion to the first portion of the experiment, which included the continuous heating and cooling of a 1.5-gram sample of barium chloride dihydrate, the litmus paper tested indicated that there was no release of acidic vapors during the separating of the water and compound bonds. In other words, the chemical equation BaCl2 + 2H2O (s)  BaCl2 + 2H2O (g), labeled as 5.3 in the original lab report, is best used to describe the transition which took place during this portion of the lab.