Identification of an Unknown Compound using Quantitative and Qualitative Analysis Lauren Tremaglio Chemistry 1011 Lab, Section 16 Instructor: Steven Belina October 3, 2014 Our signatures indicate that this document represents the work completed by our group this semester. Experimental Design and Discussion of Results The objective of this experiment was to identify an unknown compound through quantitative and qualitative analysis. In order to find the identity of the unknown compound, an initial qualitative test for solubility was performed. To begin, the solubility of the unknown compound in water was tested. If the compound is soluble in water, it can be inferred that it is either a polar covalent or ionic compound. …show more content…
In order to find the amount of a product made during a double displacement reaction, the product has to be separated from the solution. From this number of moles of precipitate can be calculated. From there the number of moles of reactants can be calculated using the mole ratios of the particular reaction that occurred. As seen in Table 5 it is shown that by finding out the number of moles of the unknown, the molar mass of the unknown can be calculated. From the found mass of the unknown compound, the mound of the original ion can be found. In all trials, some of the precipitate was lost through the filter. Therefor all values are most likely less than the actual values due to …show more content…
Most ionic compounds are soluble in water because waters partially dipole is attracted to anions and its partially negative dipole is attracted to cations. This can be further investigated by testing the compounds solubility in acetone. Ionic compounds are generally not soluble in acetone, while polar and nonpolar compounds are. One spatula tip of the compound was added to 50mL of acetone. Because acetone is a non-polar solvent and ionic compounds will not dissolve in it. The quantitative solubility of the unknown compound was determined to be 29/100ml. The known solubility of sodium sulfate is 28.11g/100mL water. Using the found solubility to compare to the known solubility of sodium sulfate. This solution created in the solubility test, the conductivity of the unknown compound was tested using an Ohmmeter to measure the resistance of the solution. Resistance is the measure of a substances ability to conduct
• ionic compounds can only conduct electricity if their ions are free to move. Ionic compounds only conduct when they are melted or dissolved in water and they do not do not conduct electricity when they are solid. Sodium chloride– it is soluble in water, it has high boiling and melting point, it does not conduct in its solid state, except when it dissolves in water or melted then it will conduct electricity.
This knowledge allowed for a balanced chemical equation for the titration to be created: H2X+2NaOH2H2O+Na2X. At the start of the experiment there was an amount of acid, of which the
Some of the factors are thermometer was calibrated to determine its precision. The actual melting points of water, phenylacetic acid, o-anisic acid, and benzilic acid to their observed melting points were determined by calibrated thermometer. Then the solubility tests were run in order to determine the appropriate solvent for the unknown solute (Table 1). After determination of a solute, a vacuum filtration technique was used to determine the pure form of compound. The melting point of the purified sample was determined and compared to the melting points of other known compounds.
The aim of this experiment was to prepare a buffer for an unknown amino acid with the goal of identifying the unknown amino acid. The objective was to use the Henderson Hasselbalch equation to determine the buffer capacity, and to use the pKa values and molecular weight, to identify the unknown amino acid through acid-base titrations. Titration was done on the unknown amino acid with a strong acid and base while titration was done on NaCl, which acted as a blank for identifying the unknown amino acid and was used to find the true titration curve of the amino acid. The pka values were found to be 1.95 and 8.88, and the molecular weight 133.98 g/mol. Moles extrapolated from the titration curve were used to find the molecular weight of the unknown amino acid, along with the pkas and the pI. This information when compared to the literature values of Gly, L-ala, L-ser, and L-asp (of which the unknown was one of) led to the conclusion that the identification of unknown C was likely to be L-Aspartic Acid.
In part 1, the 5 fuels, commercial biodiesel, methyl linoleate, 2-Butanol, Methanol, and Ethanol, were divided among five groups. Each group prepared 6 petri dishes; each dish fitted with a layer of filter paper, 30 seeds, and then another layer of filter paper on top. In preparation for the biodiesel methyl linoleate, 2.25 mL of the biodiesel along with 17.75 mL of water were used to make 20 mL of 10% biodiesel. This amount was split in half 4 times using a graduated cylinder and the appropriate amount of deionized water were added to make 10 mL each of 10%, 5%, 2.5%, 1.25%, and .63% of biodiesel solution. These were poured into the 5 appropriately labeled petri dish; the control dish got 10 mL of DI water.
Pages 96-98 in Chemistry 110 Lab Manual. Wilfrid Laurier University, ON, Canada. Abstract: The purpose of this experiment was to determine the level of purity by using the values for melting point and absorbance and chemically synthesizing aspirin by using phosphoric acid as a catalyst.
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Introduction: In this lab, of water in a hydrate, or a substance whose crystalline structure is bound to water molecules by weak bonds, is determined by heating up a small sample of it. By heating, the water of hydration, or bound water, is removed, leaving only what is called an anhydrous compound. Based on the percent water in the hydrate, it can be classified as one of three types: BaCl2O ⋅ 2H20, with a percent water of about 14.57%, CuSO4
8.1.2 Determination of solubility The solubility data for OXB as observed in 0.1 N HCl, pH 4.5 Acetate buffer, pH 6.8 Phosphate buffer and Purified water is presented in Table 25. OXB exhibited a pH independent solubility phenomenon in all pH conditions and various aqueous buffers. Table 25: Solubility data of OXB BCS solubility (pH solubility) profile of OXB Sr.
Lysergic acid diethylamide is a natural substance synthesized from the parasitic rye fungus, Claviceps purpurea2. Albert Hofmann, a natural products chemist at the Sandoz AG Pharmaceutical Company, synthesized it in 1938 while experimenting with pharmaceutical uses for ergot2,4. He intended for this series known as LSD-25 to be used as a circulatory and respiratory stimulant. However, after minimal testing LSD-25 aroused no special interest in the pharmacologists and physicians. Testing was then discontinued and not worked with until his curiosity struck him 5 years later.
The aim of this experiment was to create Butyl Ethanoate by the process of reflux esterification using 1-Butanol (, 16mL) and Ethanoic Acid (17.4M, 10mL) as raw materials. A catalyst sulphuric acid (18.0M, 2.0mL) was used to offer an alternate reaction pathway and forcing the equilibrium to shift to the right as it is a dehydrating agent result in a greater yield of ester. All reactants were heated under reflux for a total time of 45 minutes, boiling chips were added into the pear shaped flask to encourage even boiling and prevents the occurrence of superheating.
The Partition Coefficient (Kp) Excretion of Benzoic acid and its conjugate Base from Two Immiscible Phases Abstract: The partition coefficient is the ratio of concentrations of compounds in the two phases of a mixture of two immiscible solvents at equilibrium. The purpose of this experiment is to determine the partition coefficient of benzoic acid first in water with methylene chloride, and then in sodium bicarbonate solution with methylene chloride. The partition coefficient result for Part A (water with methylene chloride) was 3, while the result I got for Part B (methylene chloride with sodium bicarbonate solution) was 0.55. Both results correlate to the ideal values which were greater than 1 for part A, and less than 1 for part B.
They are only soluble in polar solvents, like water. This is due to the ions inside the lattice becoming surrounded by water molecules which easily bond to the ions. This means there is a decrease in the attraction that the ions have, resulting in the ionic structure breaking down. When in a solid state, they are unable to conduct electricity.
Bombay: Varghees Publication House, 1990; 171-196. [9]Venkatesh S, Y, Rao V, Anderson B. D, Intrinsic solubility estimation and pH-solubility behavior of cosalane (NSC 658586), an extremely hydrophobic diproticacid, Pharmaceutical Research, 1996; 13(10),