Molar Mass Of Crystals Lab Report

While the solution dissolved, 50 mL of distilled water was added to a 150 mL beaker and heated on the hot plate. When the solution started to boil 2.65 grams of Na2SiO3*5H2O was added to the beaker with a stir bar and heated to a gentle boil. When both solutions began to boil, the sodium silicate solution was slowly added to the sodium aluminate. The solution was kept at 900C for 60 minutes and stirred with stir bar. After 60 minutes, the zeolite solution was cooled for 5 minutes and for the magnetized zeolite , 0.78 grams of FeCl3 and 0.39 grams of FeSO4*7H2O was added to the flask and stirred until the iron parts dissolved.

Calculate the percent yield of alum crystals for each trial. 4. Discuss the sources of error that affected the percent yield. 5. Write the balanced net ionic equations for the following reactions: a. 2 Al(s) + 2 KOH(aq) + 6 H2O(liq) → 2 KAl(OH)4(aq) + 3 H2(g) b. 2KAl(OH)4(aq) + H2SO4(aq) → 2 Al(OH)3(s) + 2 H2O(liq) + K2SO4(aq), Al(OH)4-(aq) + H+(aq) → Al(OH)3(s) + H2O(liq) c. 2Al(OH)3(s) + 3 H2SO4(aq) → Al2(SO4)3(aq) + 6 H2O(liq), Al(OH)3(s) + 3 H+(aq) → Al3+(aq) + 3 H2O(liq) d. Al2(SO4)3(aq) + K2SO4(aq) + 24 H2O(liq) → 2 KAl(SO4)2•12 H2O, K+(aq) + Al3+(aq) + 2 SO42-(aq) + 12 H2O(liq) → KAl(SO4)2•12

A third error was miscalculating the volume in each vial, which could have been prevented by making sure the beads accurately made up for any difference in volume between the

Kendrell Goodwin Formula of a hydrate Objective/hypothesis The objective of this lab is to calculate the number of moles of the anhydrous salt and the moles of water driven off. The purpose of this lab is to determine the formula of the hydrated salt. The outcome expected in this lab is that the Procedure Get a porcelain crucible and cleanse with soap then rinse with tap water. Follow up after rinsing with tap water, with rinsing with distilled water.

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

As seen in table 1, the theoretical yield was .712 g of C_17 H_19 NO_3. The % yield of this experiment was 7.51 % of C_17 H_19 NO_3. . This low yield can be explained from a poor recrystallization technique combined with potential contamination. Throughout the experiment, the mixture changed color from green, orange, to yellowish lime, and eventually clear.

Swikriti Dasgupta HL IB Chemistry Determination of the Relationship Between Concentration and Rxn in Voltaic Cell: Research Question: How does the concentration of CuSO4 affect the voltaic cell as measured by voltmeter? Variables: Table 1: Independent Variable for Determining the Relationship Between Concentration and Rxn in Voltaic Cell: Independent Variable How it will be changed CuSO4 CuSO4 solution was diluted to 50% using distilled water. Then the diluted CuSO4 was further diluted to prepare 20%, 40%, 60%, 80%, and 100% dilution.

The developed analytical procedure for molybdenum determination was used for ore

The substitution reaction was successful but not fully effective. 19. If the data was inconclusive, then comparing various compounds and the unknown based on physical characteristics would be the first step, titrations would also be a good method. 20. 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

The purpose of this experiment is to successfully grow a crystal. Materials: • Epsom Salt • Food Coloring • Beaker, Small bowl, or Jar Procedure: 1. Bring 1/2 cup of water to a boil. 2.

EXPERIMENTAL PROCEDURE 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. At the beginning of the lab the specimen was removed from the furnace using tongs and quenched in water. Then, the specimen was put into the oil at 190oC for 6 min.

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.

In this experiment, the amount of water lost in the 0.99 gram sample of hydrated salt was 0.35 grams, meaning that 35.4% of the salt’s mass was water. The unknown salt’s percent water is closest to that of Copper (II) Sulfate Pentahydrate, or CuSO4 ⋅ 5H2O. The percent error from the accepted percent water in CuSO4 ⋅ 5H2O is 1.67%, since the calculated value came out to be 0.6 less than the accepted value of 36.0%.This lab may have had some issues or sources of error, including the possibility of insufficient heating, meaning that some water may not have evaporated, that the scale was uncalibrated, or that the evaporating dish was still hot while being measured. This would have resulted in convection currents pushing up on the plate and making it seem lighter by lifting it up

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

One of the possible systematic error that may occur in this experiment is that the hydrated (II) ammonium sulfate is contaminated as the iron (II) salt was left uncovered. The iron (II) salt was prepared by the lab assistant and the salt was left at the table uncovered for students to scoop the desired amount of salt they want. The iron (II) salt might be contaminated by dust particles and even saliva. This would cause the standard iron (II) solution to have less iron (II) salt in it and this means that less potassium permanganate solution is needed to titrate the iron (II) solution. This is a systematic error because the iron (II) solution used throughout the experiment.