INTRODUCTION Gravimetric analysis is a quantitative technique of chemical substance by weight. In this analysis, the element to be determined is isolated into a pure form that can be converting into a weighable compound. The technique has the following advantage: It is accurate, less expensive and possible errors can be checked easily through completeness precipitation test. There four different specific gravimetric method that can be used for separation of elements which are: electro method, volatilization method, particulate method and precipitation method. (JEFFERY et al. 1989). The electro-gravimetry method is based on the reduction of metal on a pre-weight electrode and the amount of the analyte is calculated from the weight gained by …show more content…
After the addition of 32%HCl the sample was filtered under gravity and the filtrate was kept for analysis. Precipitation …show more content…
While stirring the solution pH was adjusted to pH~1 using 2M HCl. The solution was heated to almost/ near boiling point (50°c) and an amount of 15ml warm (0.05M) BaCl2 was added drop wisely into the solution with constant stirring. After the addition of warm BaCl2, the precipitation was allowed to settle. Test for complete precipitation was done by adding few drops of warm BaCl2 to the solution. The solution was allowed to digest for about 40 min in warm water. After the digestion period, the supernatant was tested for complete precipitation by adding few drops of warm BaCl2 until no precipitation was formed. Filtration step The solution was filtered using a weighed Millipore filter paper and the precipitate was washed twice with deionised water. The precipitate containing BaSO4 and filter paper were dried and weighed. Calculations Mass of BaSO4 (g) = Precipitate + filter paper mass (g) – Tared filter paper mass (g) Mass of SO4 (g) = Mass of BaSO4 (g) * Molecular weight of SO4 (96.06 g/mol) / Molecular weight of BaSO4 (233.43 g/mol) SO4 concentration of sample (g/L) = Mass of SO4 (g) / Volume of original sample (25 mL / 1000)
Next, we determined the mass of the penny by placing it on a balance. The mass of the penny was 2.47 grams. Afterwards, we placed the penny in a beaker filled with 20 mL of 6 M HCl. In the end we put the beaker in the fume hood and allowed it to sit overnight. During day two of the penny lab, we removed the penny skin from the beaker using tweezers.
For this lab, zeolite and magnetized zeolite were synthesized and compared with charcoal to find out with would be the most effective in the sequestering of Procion Red dye. Finding the concentration and absorbance of each zeolite, magnetized zeolite, and charcoal, along with a calibration curve, the best adsorbent is determined. Charcoal was the overall best sequestration of the Procion Red dye, since the adsorbent was highest compared to the others. Introduction Pollution has increased in the environment over the years, so the purpose of this experiment is to find the best adsorbent of chemicals to reduce the pollution.
Cadet Eric Wiggins Date: 18 September 2014 Course Name: Chem 100 Instructor: Captain Zuniga Section: M3A Identification of a Copper Mineral Intro Minerals are elements or compounds that are created in the Earth by geological processes. The method of isolating metals in a compound mineral is normally conducted through two processes.
After copper ions were filtered, approximately 15mL of .5 M was added to the filtrate, which made the mixture acidic. Then, 20 mL was added into the filtrate to raise the pH of the mixture.
In addition, for calculating the mass of the pennies and the unknown substance, zero the balance and place it in the weigh boat to receive the data. Lastly, to calculate the density of the substances, use the formula D=MV, in which dividing the mass by the volume allows to do so. In order to be certain of the data that is collected, running multiple trials could help be accurate. A method to get an average value of the density can be expressed by the formula D1+D22. This formula basically allows one to add the data of all the trials and divide it by the number of trials that was performed.
The resin that had stuck to the sides of the burette was washed down by pipetting extra pH 3 citrate buffer along the sides. The column was tapped to ensure that the settled resin formed a level surface. After all of the resin settled, the buffer was drained into a waster beaker until the level of the buffer reached the top surface of the resin. For the remainder of the experiment, the top surface of the resin was not allowed to dry
The molar mass and pKa value was found by using LoggerPro to make a titration curve. Applying the first derviative to the titration curve allows the extrapolation of the equvillance volume, which in turn is used to calculate the
In this test, primary halides precipitate the fastest while secondary halides need to be heated in order for a reaction to occur. Comparison of the rates of precipitation of the obtained product to standard 1° and 2° bromide solutions will show whether the product is a primary or secondary
I. Purpose: To experimentally determine the mass and the mole content of a measured sample. II. Materials: The materials used in this experiment a 50-mL beaker, 12 samples, a balance and paper towels. III.
All things considered, the results proved that the unknown substance or element was barium since the calculated density was 3.9 g/mL. To expand upon, the density was calculated by measuring the mass of the metal and using the displacement method to determine the volume of the metal. Also, the best method of disposing the storm water would be to contact a Wastewater Treatment Plant (WWTP) so that they could put it through a purification process, making all that water reusable. Meanwhile, the percent of recovery was calculated by the formula Percent Recovery=observed valuetrue value *100%. Furthermore, according to the pie chart created in the data analysis, the sample given contained of the percent by mass for metal to be 5.2%, salt was 3.3%, wood was 3.1%, plastic was 4.5%, rock was 12.5%, sand was 11.8%, and water was 59.6%. Also, the formula used to calculate the percent error was Percent Error=observed value-true valuetrue
The mixture was then distilled. When the temperature was reached to about 59℃, half vial of distillate (1V) and 1 mL of the liquid residue (1L) were collected. For 61.0℃, the distillation was then continued. Samples (2V, 2L) were taken at about 61.0℃.
The Copper Cycle is a well-know experiment that is used to demonstrate the Law of Conservation of Mass. According to this law, mass is conserved during chemical reactions. In other words, the mass of copper in the reactants is supposed to equal the mass of copper in the products.1 The Copper Cycle is a series of 5 reactions over which the mass of copper is ideally conserved. These reactions are various types of reactions, which highlights that mass is conserved in all kinds of chemical reactions. However, due to experimental errors, some percent of copper is usually not recovered in the last step.
Immediately 10 μL of double distilled water was added with a micropipette; this way our concentration of the treatment was the intended concentration.
The developing solution was poured into a tank and was tightly covered with a glass lid, and the tank was allowed to be saturated to ensure that the solution was equilibrated in the gas phase. Silica plate for TLC analysis: A horizontal line was drawn with a pencil on the plate and it was about 1 cm above the bottom of the plate. The horizontal line was drawn faintly so as to avoid damaging the silica gel on the plate. On the horizontal line, two marks were made and one was named A and the other B. These marks were made towards the centre of the plate at a distance apart because when spots are made at the edge of a plate, the result would be an improper travel of the samples as the solvent advances on the plate.
Buffer solutions of pH 4 and 7 6. Graduated cylinder - 100 mL 7. Volumetric flask with stopper - 250 mL 8. Two 100-mL beakers 9. Two 50-mL Burettes 10.