Miracle Gro Gravimetric Analysis Essay

was generated from the reaction. After the fizzing stopped a liquid was leftover leading me to conclude the liquid leftover leading me to conclude the liquid leftover was the NaCl and H2O

Plantation fiction glorifies slavery and worships slave masters and tells of story of loyal slaves who would never betray their master. The Passing of Grandison is a critique of plantation fiction. Dick Owens, son of a wealthy slave master is in pursuit of Charity Lomax who told him “I’ll never love you Dick Owens, until you have done something. When that time comes, I’ll think about it.”. Dick sets a plan to take his servant Tom on his trip to the north. However, his father assures him that it is too dangerous to take Tom, for he is too smart. He instead offers Grandison, because the Colonel feels that he is trustworthy. Dick tried everything he could to get rid of Grandison while they were up north, and gave him ample

The purpose of this experiment was to identify given Unknown White Compound by conducting various test and learning how to use lab techniques. Tests that are used during this experiment were a flame test, ion test, pH test, and conductivity test. The results drawn from these tests confirmed the identity of the Unknown White Compound to be sodium acetate (NaC2H3O2) because there were no presence of ions and sodium has a strong persistent orange color. The compound then will be synthesized with the compounds Na2CO3 and HC2H3O2 to find percent yield. Weighed 1 gram of NaC2H3O2 and mixed it with ionized water. Boiled 12 mL of 1.0M Acetic Acid added into a beaker containing the sodium carbonate on a hot plate until all the liquid is evaporated

As had doing the baseline prior to changing the pH with a drastic qualitative and quantitative data change, seeing no color change and slope in the graph was concerning. However as multiple trials were completed and results were compared to other classmates, more confidence arose in the results as the numerous trials with similar results ensured validity. If there were things that could have been done differently, more precision and caution would have been taken whilst doing the lab; for example: re-reading the lab before beginning and taking time while measuring out solutions. The experiment had a few errors due to human error as well as random ones. For example, in one trial, distilled water was gathered through the hydrogen peroxide pipetter, creating a chance of error due to the cross-contamination of solutions. Additionally, in the initial attempt at the experiment, it was believed that cuvettes 2 and 3 needed to be put through the colorimeter before mixing together in the 4th cuvette, when in reality they did not need to be. A random error would be that there was a logger pro used the second day as there was no go link present as it had been the previous

In this experiment four samples from Susan’s Swamp were collected into four Mason jars and brought to Ivey. Then using a scale I measured 10 grams, 1 gram, and 0.1 grams of fertilizer and mixed it using a magnetic stirrer and stir bar into the Mason jars, with each jar containing one

In Station 1- reaction 2, Station 3- reaction 1, Station 4-reaction 1, Station 5 reaction 1, Station 6-reaction 1 and 2, and Station 7- 1 and 2 there was chemical reaction because all of those mixed ionic compounds created a precipitate. However some solutions did not become insoluble and produce precipitates such as: Station 1- BaCl2 (aq) + KNO3 (aq) , Station 2- KNO3(aq) + AgNO3(aq) and KNO3(aq) + CaSO4(aq), Station 3- Na2CO3(aq) + KNO3(aq) , Station 4- NaPO4(aq) + KNO3(aq), and Station 5- 2Na3PO4(aq) + KNO3(aq). The lab demonstrated the Solubility Rules when the equations that included Nitrates and Group 1 salts resulted in soluble compounds, and the ionic compounds that included Carbonates, Phosphates, Hydroxides,

The mixture began to turn greenish at the bottom of the tube. At the end of the experiment, the mixture and become completely

Research shows that NiCl2 is the green liquid. NiCl2 will not react with anything except with AgNO3 and Na2CO3, so the first step will be mixing all solutions with NiCl2 until those two chemicals are found.

After that, we take 0.80 g sodium carbonate and mix with 25 ml of distilled water to make a solution of sodium carbonate. The two solutions are mixed together in the 100 ml beaker, forming a milky white precipitate. The solution is

In the empirical data above the mean percentage of water in the iron salt crystal was 6.27%. The mean percentage of the potassium ion was determined to be 17.81%. For the iron ion the mean percentage was 12.20% and the average percent for oxalate was 57.20%. The total percentage of the mean adds up to 97.28%. The empirical formula using the means provided created the formula K2Fe(C2O4)3*2H2O. The total molar mass in this equations is 434.05 grams. The percent yield of iron salt using the actual yield of 8.71 grams with a theoretical yield of 17.8 grams is 49%.

Based on this chemical equation, four moles of hydrated copper sulfate reacted with six moles of ammonia to produce a precipitate of copper sulfate tribasic along with aqueous ammonium sulfate and liquid water. It was known that a chemical reaction was occurring when the ammonia was being added via the color change from light blue to dark blue. The precipitate formed from this solution was acquired via vacuum filtration, which involved the solution being separated from the precipitate via air pressure flowing out of the flask. The air pressure flowing out of the flask was caused by a faucet that was running water which was attached to a tube that was attached to the collection flask.

First source of error is observer subjectivity. The observations made on the qualitative results of the experiments are based entirely on observer’s ability to detect and interpret the results. A different observer may detect or interpret the same events differently. To avoid such errors, the observers should be briefed properly and in detail on the possible outcomes of the event so the record can have some uniformity between different observers, e.g., some guidance should be provided to determine what constitutes a small, medium and large piece of curd. Secondly, pH paper was used to determine the pH of the solution. The colors of the pH strip once dipped in the solution corresponded to the pH ranges usually in increments of 1. Thus using the pH paper did not give specific pH of the solution. In order to avoid such error pH meters can be used which provides its user with more accurate and exact pH

Phosphorous is found in lithospheres earth’s crust which is obtained within the rocks. The beginning of The Phosphorous Cycle commences by weathering of the rocks. Weathering is an action which is produced by one of the earth’s spheres, hydrosphere, which produces rain causing the outer layer of rocks to break down which then releases Phosphorous. After the phosphorous has separated from the earth’s crust, it travels to the ground causing it to be combined with lithosphere, soil. Phosphorous is absorbed by the earths sphere, biosphere such as plants through their roots acting as an extra source of food. Phosphorous is needed for plants as it helps plant growth. One of animal’s main food sources is plants meaning in order for the phosphorous cycle to continue animals need to consume the plants which contain phosphorous. After the animals have consumed the plants

It is observed that mean values of all the concentrations of cations viz., Ca2+, Mg2+, Na+ and K+ ions are exceeded the desirable standard limit. The order of abundance is Ca2+ > Mg2+ > Na+ > K+. Sewage and industrial wastes are the important sources of calcium and magnesium (Subrahmanyam and Yahadaiah 2001). The spatial distribution of dominated cation Ca2+ and Mg2+ are presented in Fig. 7 and Fig. 8 respectively. Bicarbonate represents the major form of alkaline, since it is formed in considerable amounts from the action of carbon dioxide upon basic materials in the soil (Sawyer et al

formation of a precipitate film could interfere with subsequent exams. Ferric nitrate, ferric sulphate and