Molar Mass Of Crystals Lab Report

In this experiment, the percent yield was 90%. This number implies that there was little error in this experiment. However, this result could have been caused by certain external factors. Firstly, because the NaHCO3 compound was not stored in a sealed container, therefore dust particles could have changed the results, and making the product impure. Also, there are uncertainties associated with the instruments used in this experiment. This, if the products were measured slightly more than should be, this could have affected the concentrations of the solutions, and therefore causing a larger

The powder on the filter paper could've fell and this caused it to have a smaller percent purity, percent yield and also cause a lower absorbance and concentration of pure ASA. Another error would be not using a properly dried sample for the pure ASA in part C when making the crystals, this could have cause tye percent yield error. This would make a lower melting point. To prevent this from occurring next time there could be a dry sample that is completely dry and this would not alter the mass of the sample and this would make the solution have a more

The overall goal of this lab was to produce an unknown oxalate compound, find its percent composition, calculate its molecular formula, and determine the limiting reactant in its formation. A reaction between iron III chloride hexahydrate and potassium oxalate monohydrate produced 3.307g of potassium trioxalatoferrate (III) trihydrate with a 62.0 percent yield. A permanganate titration determined the average percent composition of oxalate was 53.3% with a 2.22% standard deviation. The percent composition revealed the compound’s empirical formula to be FeK3(C2O4)3•3H2O. Potassium oxalate proved to be the limiting reactant.

I would alter this experiment by doubling the recipe and keeping the crystal in the refrigerator for 2 days to get a larger, more defined crystal.

To get a better yield, redoing the experiment would require careful attention in the recrystallization steps: amount of solvent used, how hot solvent is, if the mixture cools to room temperature before placing it in an ice

once we did that we added HCl to the precipitate. Then we had to centrifuge the solution and put the supernate into two test tubes to test for ions and nickel. In the experiment, we tested positive for iron but then tested for nickel and didn’t get anything. The reason behind this was when we added .2M KSCN to our supernate and turned it a dark red color swiftly. after we added NH3 to the solution, a precipitate formed for nickel. we mixed everything together which formed an orange specks of precipitate formed. we tested calcium and in our unknown we did have calcium. precipitate formed when we added K2C2O and NH3 to the supernate. Then, we did flame test and we see a color changed to see if calcium appeared which it

The theoretically yield for this experiment, based off of the mass of aluminum pieces originally weighed out, was 19.0144 g, while our actual yield was 12.7222 g. This is a 66.91% yield. Ideally, of course is a 100% yield. Factors that may have caused this in our own experiment include, but may not be limited to: 1) There was barely any hydrogen gas being produced in the first step when we took it off the heat, but enough to infer that the reaction may not have been completely over, possibly affecting the amount of potassium aluminum hydroxide produced 2) Having to filter the reaction mixture in the first step more than once, because we neglected to turn on the vacuum the first time, we may have lost some of the mixture in the process. 3) In the last step, when the solution was put in the ice bath, it was up to us when we thought enough crystals had been formed as to when to filter the crystals. Perhaps waiting longer would have produced more

(1) If the crucibles were not put in the oven at the end of the experiment, there could be excess moisture trapped in the crucible. This contributes to the mass of the weighed crucible at the end of the experiment, meaning the mass would be higher than it would normally be. After calculations, it can be concluded that the moisture in the crucible shifts the data up, creating an artificially high concentration of Al3+. (2) Reading the volumetric pipet to 25.00mL is an incredibly crucial step in this experiment because it’s the only source of Al3+ that is added to the reaction. This step affects the end result when weighing the precipitate because in the reaction, the Al3+ is the limiting reagent and is in a 1:1 stoichiometric ratio with the precipitate product. If the pipet is read too low, then the result would be an artificially low concentration because the mass would be lower. If the pipet is read too high, then the result would be an artificially high concentration because the mass would be higher. (3) On Day 3, if we did not rewash the beaker with DI water after initially pouring the solution into the crucible to be filtered, it would affect the final results of the experiment. If the beaker was not washed, not all the solution/precipitate would end up in the crucible/filtration system, which would mean a possible low reading on the mass and concentration of Al3+ because some of the precipitate would remain on the beaker. The precipitate left on the beaker would not be accounted for in the calculations, and would result in a lower measured mass and

Claim: Electrons with higher energy will be positioned further away from the nucleus than electrons with lower energy.

The specimen Al 2024 which was consist of 3.8-4.9% Cu, 1.2-1.8% Mg, 0.3-0.9% Mn, and Fe, Cr, Zn, Ti in a little amount had been inserted into a furnace set at 500oC approximately 50 minutes for a solution treatment before the lab. Its height was 7 mm and width was 25 mm.

The chemical reactions can be found below in Table 2.8 The amount of copper metal extracted from the 0.9899 g sample of malachite was measured to be 0.5682g. The theoretical yield of copper metal was calculated to be 0.5690 g. The percent yield was calculated to be 0.135%. The sample calculations for theoretical yield and percent yield can be found after Table 3.

Based on the size of your error bars and standard deviations, identify the salt concentration that was the most precise.

This element has been known since ancient times and in general, is a shiny, grayish metal that rusts in damp air. This metal is non-toxic and plays a large role in all forms of life, especially human beings. As hemoglobin iron carries oxygen from the lungs to our cells, it keeps human’s alive. In fact, human bodies contain of about 4 grams of iron and need to intake a healthy dose of it daily (Royal Society of Chemistry, Iron). Without iron humans start to face severe health problems, including the development of anemia. Other then being an important aspect in humanity Fe, one of the three magnetic elements, the other two being cobalt and nickel, is also the fourth of Earth’s most abundant mineral, by mass (Royal Society of Chemistry, Iron). The source of this iron comes naturally from ores deep in the earth’s crust in sedimentary crusts, since iron oxidizes remarkably fast on the Earth’s surface. For commercial use, pure Iron can transform into steel or an alloy by adding other impurities and elements, making it an

Everyone in the room was using the same solutions so we ran out at the end so I did not have 40 ml to conduct my last experiment with the correct amount

Valenzuela et. al. (1995) [100] has proposed a hydrometallurgical procedure for the separation of molybdenum from Chilean molybdenite concentrate. The molybdenite concentrate was first leached with nitric acid originated from the reaction of NaNO3 and H2SO4, which provided a solid phase, composed of MoO3 and residual solution. Molybdenum was separated with alkylphosphonic acid PC-88A by solvent extraction method, from the leach liquor containing copper, rhenium and iron among other impurities. The extraction efficiency of molybdenum was about 96% at pH 0.8 with zero co-extraction of other metals. The loaded organic was stripped with ammonia aqueous solution. One extraction stage and two stripping stages were required for the enrichment of Mo