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Flame Test Lab Report

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The results from most of the experiment best fit with Potassium chloride, although not all the test fit with potassium chloride. For example, in “Part A” When the salt was put in the flame it made the flame turn violet. This supports the conclusion that the salt is potassium chloride because potassium chloride also makes a violet flame when burned. The flame test was the most conclusive test because all 8 of the possible salts that were given have very significant flame color. None of the other salts have a violet color flame when burned which goes to prove that the salt is potassium chloride. Another example is when the salts water attraction from there air was tested. When the salt was set out for 20 minutes the mass of the salt changed …show more content…

Which is the same as potassium chloride as potassium chlorides melting point is 770 degrees Celsius. “Part B” experiment was to figure out the water percentage of the unknown salt “579” and the results of this test after some calculations was that there was 0.024% of H2O inside of salt “579”. This percentage is very low and out of the 8 salts its closes to zero percent water. Potassium chlorides water percentage is zero which only helps prove the point that the salt “579” is potassium chloride. In “Part C” the density of the salt was calculated, and it turned out to be 1.73 g/mL and compared to the 8 known salts it could be potassium chloride which is 1.98 g/mL or calcium chloride dehydrate 1.85 g/mL. Considering the other 6 characteristics of calcium chloride dehydrate there is no way this is possible because its water percentage is 24.5% and salt “579” water percentage is 0.024%. The least reliable test result was “Part D” the heat of solution of salt “579” which was significantly different from potassium chlorides heat of solution. The heat solution of salt “579” was -2.44 kcal/mol and the heat solution of potassium chloride is 4.404

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Chemical compounds that are available to determine are CaCO3, CaCl2, Ca(NO3)2, mgCl2, MgSO4, KCl, HCl, HC2H3O2, KNO3, K2SO4, NaC2H3O2, Na2CO3, NaCl, Na2SO4, HNO3, H2SO4, HNO3, H2SO4, NH4Cl, (NH4)2SO4, K2CO3, 0.1 M AgNO3, 0.2 M BaCl, Mg(s), NaOH, and KOH. To start this experiment, start with the flame test by gathering a Bunsen burner and a Nichrome wire. Connect the Bunsen burner with a rubber tube to a laboratory gas. To prepare solutions for the flame test, weigh out 0.205 gram of Unknown Compound using an analytical balance and mixed it into a 140 mL beaker filled with 20 mL ionized water. Ensure that solid is completely dissolved using a stirring rod.

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The purpose of this lab was to be able to use physical characteristics to determine the identity of an unknown compound. The data from this experiment classified aluminum as metallic; ascorbic acid, paraffin, palmitic acid, sucrose, graphite, and water as molecular; sodium chloride as ionic. In order to determine this, 3 tests were conducted. The first test was to test the conductivity of each substance at room temperature. In this test, only graphite and aluminum conducted.

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Flame Tests of the Elements Lab 1. According to your observations, which metal ion is present in your unknown samples? Explain your rationale.

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a. Water boils to produce steam at 100 C (212 F) b. Water produces gas with sodium metal c. Water and oil separate when combined d. Water dissolves sugar 22. In the experiment, students put brine shrimp in water with different concentration of salt and counted the number. Which of the following changes to the experiment will increase confidence in the validity of the result? a. Count the number of dead brine shrimp instead of living brine shrimp b. Add more brine shrimp to the water with the highest salt concentration c.

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562 Words | 3 Pages

Objective: In this lab, students learned the different methods there is to separate substances from one another. They practiced the process of decantation, extraction, filtration, and sublimation. Introduction: Theory: Before being able to isolate the components in a mixture, the students should’ve become familiar with the physical properties of each of the substances. The students were given an unknown sample which has a combination of three different components.

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The dissolution of the salt could be reversed by evaporating the water as shown in part one of the experiment, just as evaporating the water could be reversed by adding water as demonstrated in part two of the

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Abstract In this experiment the separation of a copper (II) chloride and sodium chloride mixiture was attempted. The main aim was to separate the compounds from eachother while receiving as much of the original mass of both substances as possible - in perfect conditions the original mass will be received after seperation. Many techniques were considered but dissolution, filtration and evaporation proved to be easiest and most reliable in a school environment with school equipment. The copper (II) chloride and sodium chloride mixture was dissolved in a methanol solution and filtered out leaving the sodium chloride behind.

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The beaker was placed on the heating element on high heat and was left undisturbed until it began to boil. When the solution reached a rolling boil, the temperature of the water was tested and recorded utilising the same method as the first trial. Two more trials of the 0.5 M mixture were conducted. The experiment was repeated three times more with 11.688 grams of salt to create a 1 M mixture. The experiment was repeated three times more with 17.532 grams of salt to create a 1.5 M mixture.

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The purpose and significance of this experiment was to find the specific heat and figure out an identification of an unknown metal. The specific heat was calculated through a given formula. The unknown metal was found through descriptions that matched the unknown metal. The unknown elements would be one of the following: Al, Bi, Cd, Cu, Fe, Pb, Ni, Na, Sn, or Zn. First the specific heat of water was measured, then heat flow was measured using equations.

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Also, it is really stable - it has a 0 for the stability rating. It does not even react with water. Sodium chloride is not a huge safety or hazard issue, so it will not have much information

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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

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