Abstract This paper describes the methods used in the identification, investigation of properties, and synthesis of an unknown compound. The compound was identified as calcium nitrate by a variety of tests. When the compound was received, it was already known to be one of twelve possible ionic compounds. The flame test identified the presence of the calcium anion in the compound. The compound tested positive for the nitrate cation using the iron sulfate test. At this point it was hypothesized that the compound was calcium nitrate. Reactivity tests and quantitative analysis comparing the unknown compound with calcium nitrate supported this hypothesis. Synthesis reactions were then carried out and analyzed. Introduction The primary goal of this laboratory project was to identify an unknown compound and determine its chemical and physical properties. First the appearance, odor, solubility, and conductivity of the compound were observed and measured so that they could be compared to those of known compounds. Then the cation present in the compound was identified using the flame test. The identity of the anion present in the compound was deduced through a series of chemical tests (Cooper, 2009). At this point the identity of the unknown compound was hypothesized to be calcium nitrate. In order to test this hypothesis, both the unknown compound and known compound were reacted with five different compounds and the results of those reactions were compared. It was important to compare the known and unknown compounds quantitatively as well to ensure that they were indeed the same compound. This was accomplished by reacting them both with a third compound which would produce an insoluble salt that could be filte... ... middle of paper ... ... for various anions. Reactivity reactions and quantitative analysis comparing the unknown compound and calcium nitrate verified this hypothesis. Calcium nitrate was most safely and effectively synthesized by combining solutions of calcium chloride and lead nitrate. The MSDS data showed that the compound is a strong oxidizer but is not very toxic. Besides following standard laboratory safety measures, care should also be taken to ensure the compound is not exposed to heat, shock, or incompatible materials as listed on the MSDS that may cause fire or explosion. References 1. Tro, N. Chemistry: A Molecular Approach, Pearson, Upper Saddle River, NJ, 2009. 2. Cooper, M. M., Cooperative Chemistry Laboratory Manual, McGraw-Hill: New York, NY, 2009, p. 60. 3. Author unknown, Calcium Nitrate MSDS, (http://www.hvchemical.com/msds/cani/htm) 01 Mar 2009.
The purpose for this experiment was to determine why it was not possible to obtain a high percent yield when Calcium Nitrate Ca(〖NO_3)〗_2 with a concentration of 0.101 M was mixed with Potassium Iodate KIO_3 with concentration of 0.100 M at varying volumes yielding Calcium Iodate precipitate and Potassium Nitrate. Filtration was used to filter the precipitates of the solutions. The percent yield for solution 1 was 87.7%, and the percent yield for solution 2 was 70.8%. It was not possible to obtain a high percent yield because Calcium Iodate is not completely soluble and some of the precipitates might have been rinsed back to the filtrates when ethanol was used to remove water molecules in the precipitate.
The purpose of the Unknown White Compound Lab was to identify the unknown compound by performing several experiments. Conducting a solubility test, flame test, pH paper test, ion test, pH probe test, conductivity probe test, and synthesizing the compound will accurately identified the unknown compound. In order to narrow down the possible compounds, the solubility test was used to determine that the compound was soluble in water. Next, the flame test was used to compare the unknown compound to other known compounds such as potassium chloride, sodium chloride, and calcium carbonate. The flame test concluded that the cation in the unknown compound was potassium. Following, pH paper was used to determine the compound to be neutral and slightly
Furthermore, you will compare their reactions with water, universal indicator, vinegar and iodine solution to discover what the mystery powder is. Purpose: To identify the mystery powder based on its physical and
Felder, M. Richard, Elementary Principles of Chemical Processes, 3rd ed.; Wiley: New Jersey, 2000; p 631.
We have to emphasize the importance of memorizing certain names and formulas and some prefixes and suffixes that are used in building a system of nomenclature. From there on, it is a matter of applying the system to different names and formulas you meet. The summary all the ideas that will be presented in this essay help you to learn the nomenclature system.
The purpose of the experiment was to determine the solubility of calcium sulfate. In Part A with the resin, The number of moles in the original CaSO4 sample was determined to be 3.69 x 10-4 moles, and the molarity of calcium in the saturated CaSO4 solution was determined to be 0.0148 M. The molarity of calcium in the saturated CaSO4 solution is equal to the solubility of CaSO4, so the solubility of CaSO4 was determined to be 0.0148 M at 18.9 °C. In Part B with the titration using EDTA, the moles of calcium in the original saturated calcium sulfate solution was determined to be 3.87 x 10-4 moles in Trial 1 and 3.74 x 10-4 moles in Trial 2, so the molarities of calcium in the saturated solution were determined to be 0.0155 M in Trial 1 and 0.0150
Ionic liquids (ILs) are liquids composed entirely of ions. Molten salt is the term normally reserved for those systems that are liquid at high temperatures, for example NaCl (table salt is a liquid at ≈ 800 0C). Room-temperature ILs are liquid below 100˚C, have received considerable attention as substitutes for volatile organic solvents. Due to their remarkable properties, such as negligible vapour pressure, large liquidous range, high thermal stability, good ionic conductivity, high electrochemical stability, they are considered favourable medium candidates for chemical syntheses. ILs are usually categorized into four types based on their cation segment: 1) alkylammonium-, 2) dialkylimidazolium-, 3) phosphonium- and 4) N-alkylpyridiniumbased ILs (Figure 1). Ionic liquids are generally composed of a bulky organic cation, such 1-butyl-3 methylimidazolium and typically an inorganic anion such as a halide. Below are the chemical structures of some common cations and anions used to make ILs.
In this experiment, solid calcium nitrate, solid diammonium hydrogen phosphate, and aqueous ammonia are used to form calcium hydroxyapatite.
Solid A was identified to be sodium chloride, solid B was identified to be sucrose, and Solid C was identified to be corn starch. Within the Information Chart – Mystery White Solid Lab there are results that distinguishes itself from the other 4 experimental results within each test. Such as: the high conductivity and high melting point of sodium chloride, and the iodine reaction of corn starch. Solid A is an ionic compound due to its high melting point and high electrical conductivity (7), within the Information Chart – Mystery White Solid Lab there is only one ionic compound which is sodium chloride, with the test results of Solid A, it can be concluded that is a sodium chloride. Solid B was identified as sucrose due to its low electrical
The final product was p-methoxybenzoic acid and its identity was confirmed by melting point range of 183.6 – 184.8 oC, which closely corresponds to a standard of 185 oC. (Lehman). Since the melting point range is small, it confirms the purity of the product. Since the objective of the experiment was to determine the structure of the major component
Identifying Five Unknown Chemicals I was given 5 unknown samples, which are sodium chloride, sodium thiosulfate, calcium carbonate, sodium bicarbonate and sodium nitrate and these samples are all white and solid. However, I don’t know which substance is which sample and I was only given some information about the physical and chemical properties of these substances. In order to identify the 5 unknown samples, knowing which sample is which substance, I have to carry out this experiment, finding out the chemical and physical properties of these samples. How can we identify five unknown chemical samples that seem to look the same?
A white, powdery appearing precipitate of either BaCO3 or CaCO3 formed in the bottom of the test tube, and the precipitate was washed and the liquid was discarded. Acetic acid was added to the precipitate and was mixed until all of the precipitate dissolved, and then DI water was added. After the solution was no longer cloudy, NH4OH and K2CrO4 were added to the clear liquid and mixed thoroughly and centrifuged. Potassium chromate was added in step 12 because barium reacts with the chromate ion to form a yellow barium chromate solid.2 The resulting dark orange liquid was decanted into a test tube labeled “step 14.” The solid precipitate was analyzed for the presence of barium by dissolving it in HCl, decanting the resulting liquid, and adding H2SO4 to that liquid. No precipitate formed, so the solution was then tested for the presence of calcium. A false positive (the finding of a result that is not accurate) may have occurred if the solution was still cloudy when NH4OH and K2CrO4 were added. The cloudiness of the liquid indicated that the precipitate which could have been BaCO3 or CaCO3 did not fully dissolve, so it could have lead to the presence of a white precipitate in step 13 that did not contain barium. (**Unfortunately, while cleaning up from the previous steps, we discarded the “step 14” test tube, so we watched another group that had calcium in
Not only is calcium usable in the lactic form found in dairy products, but in forms such as calcium citrate and calcium carbonate (Calcium Supplement Guidelines). These two sources are the most common types of calcium found as supplements, and are usually in the form of a pill. Calcium citrate contains by mass 21 percent calcium, while calcium carbonate contains by mass 40 percent calcium. Calcium Carbonate can be found naturally in sources such as bone-meal, oyster shell, and dolomite, but these are all capable of containing toxins such as lead or mercury and should be avoided (Got Calcium?). Even when being careful to avoid such sources it is still important to check for a United States Pharmacopeia symbol to ensure purity of the source. When used to a source such as milk this may seem like extra work but it prevents toxins and other unnecessary ingredients from being accidentally ingested.
The purpose of this lab to find if some certain compounds are made up of ionic or covalent bonds and to determine the properties of these compounds. This lab relates to the things we have been learning in class because compounds are part of our everyday life, so it’s nice to know some of the characteristics about it. In this lab we poured a small amount of the sample to a piece of labeled filter paper. To test the hardness, we separated a small amount of the sample and tried to crush it with the spatula. Next, we tested the conductivity of the sample by pouring each beaker with 30 mL of water. Then, Replace a paper clips on the edge of the beaker and if they were secure and partially under water. We then connected the wires to a battery and
The actual, theoretical, and percent yield of sodium chloride was found. Sodium Carbonate was mixed with hydrochloric acid and the liquid was boiled until there was nothing left. The result was the production of salt, or sodium chloride.