Qualitative Analysis : The Chemical Compounds

To determine which ions are present in the two unknown solutions. This will be accomplished by mixing three known solutions with three testing solutions. You will use this information to determine which ions are present in the unknown solutions.

Experiment 55 consists of devising a separation and purification scheme for a three component mixture. The overall objective is to isolate in pure form two of the three compounds. This was done using extraction, solubility, crystallization and vacuum filtration. The experiment was carried out two times, both of which were successful.

Ionic compounds are soluble in water to a certain point depending on the compound. The level of solubility changes among different compounds. Some ionic compounds can completely dissolve in water and appear to be a homogeneous mixture. Although, some ionic compounds dissolve very little, and could be considered insoluble, since it does not dissolve fully. Depending on the compound, the level of solubility can be high or low. However, ionic compounds could dissolve to a certain degree. If the solution appears to be a heterogeneous mixture, many may assume through visual representation that it may be insoluble. As stated previously, the smallest amount of solubility should be considered. To confirm whether or not the substance is soluble, observe the efficiency when conducting electricity. Due to practical reasons, the slightest solubility could be considered insoluble by people.

For example, silver nitrate formed a white precipitate when it was tested with ammonium chloride. In contrast, unknown 3 did not formed any precipitate with ammonium chloride. Ammonium chloride change the color of unknown 3 to a light green while the solution of silver nitrate and ammonium chloride was cloudy white solution. Likewise, the metal in unknown 3 could have been Calcium neither. Data and observation shows that calcium nitrate whether formed a white precipitate or did not react at all while unknown 3 formed an orange precipitate. Therefore, silver and calcium are not the two metal present in unknown

the ions of SO42-, CO32-, Cl-, and I-,identify them separately, and use the observation to identify the unknown.

When the bag of Unknown substance A was measured, its mass was determined to be 6.49 g, and the amount of moles given was 0.111 mol. Using our experimental method, we determined the molar mass of Sodium chloride was 58.44g/mol. When the mass of Unknown substance A (6.49 g) was divided by the molar mass of Sodium chloride (58.44 g/mol), the answer was 0.111, which was the exact amount of moles given for Unknown substance A. Thus, it was determined that Unknown A was Sodium chloride. The process was repeated and the conclusion of our data is as

A topic of great importance to all scientists is the identification of compounds, which is relevant in all aspects of their work in some way shape or form. Weather it may be determining what is causing sickness or what is polluting the air, it is very prevalent in the science world. In project 2, identification of cations and anions was preformed through a series of confirmation and elimination tests that ultimately led to identifying an unknown ionic compound made of cations and anions.

the  solution was recorded.  The  first test  performed was  an  Anion Elimination Test,  the Silver  Nitrate

The objective is to determine the presence of a cation and anion by a chemical reaction through determining the presence of the cations and anions in an unknown salt.

The eluting solvent passed down the column by the gravity and an equilibrium was established between the solute absorbed by the absorbent (silica gel in this experiment) and the eluting solving flowing down. Since the components in the sample had different polarity and they interacted with the stationary phase and the mobile phase differently, the components would be carried by the solvent to a different extent and a separation of the components could be achieved.

In this lab, a lab group will do multiple tests on water for contrasting ions. Tests confirming the absence or presence of the ion. The lab group will be dealing with five distinct solutions. A control sample, tap water sample, ocean water sample, and a distilled water sample. The group will also use a reference solution. A reference solution is a solution with a firm vigorous existence of the ion being tested. So, It is like an example of what the precipitate should look like when the ion is existent and visible in the water sample. The solution may or may not contain an ion. Compare the results with the performance of the reference sample. Finally, if an ion is present, a chemical reaction will happen, making either a precipitate or a solution

This experiment will help students to get familiar with Ion Exchange Chromatography (IEC) which is used mostly to separate unknown mixture of metal ions. Anion and cation are known as two types of IEC. This column chromatography contains two phase such as stationary phase and mobile phase. In this experiment, stationary phase usually is made of organic resin or polymers because these are insoluble in water and barely inert. AG 1-X8 resin is used in this experiment because of their strongly basic anion exchanger. 3M HCl is used as mobile phase in this column chromatography. Cobalt (II) and Copper(II) bounds to different number of Cl- ligands, so they have different affinity to the resin.

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

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

Qualitative analysis is the use of experimental processes to identify the chemical parts of a substance. The knowledge of the meaning of soluble and insoluble is key to completing this experiment correctly and accurately. Soluble means that a compound readily dissolves in water and insoluble means that compounds do not dissolve in water. A precipitate is formed when two soluble compounds combine to form an insoluble compound. All nitrate solutions are soluble; therefore, the known solution was formed by dissolving nitrate salts of all the cations in the experiment in De-Ionized water. A centrifuge was used in each step of the experiment to spin