Mass Of Salt And Hydrated Salt

2. The second source of error in the lab is when opening the lid of the crucible which allowed smoke of magnesium oxide to escape. During the lab, we removed the lid a couple of times to allow oxygen to enter the crucible so the magnesium reacts with the air to form magnesium oxide. However, the smoke could have easily escaped from the crucible because of the strong force of heat from the laboratory burner. This could have affected the lab results by decreasing the final mass when some of the product have escaped.

In experiment A the results from the precipitation of CaC2O4 H2O from the salt mixture were obtained by weighing the items listed on Table 1 on a scale.

Materials:Magnesium stripCrucibleCrucible coverClay triangleIron ringRetort standTongsBalanceBunsen burnerProcedure:1.obtained a strip of magnesium between 30-40 cm long2.coiled magnesium strip into a tight roll3.measured the mass of the crucible and cover4.Added the magnesium strip to the crucible and measured the

The purpose of this experiment was to determine the percent by mass in a hydrated salt, as well as to learn to handle laboratory apparatus without touching it. The hydrated salt, calcium carbonate, was heated with high temperature to release water molecules. Gravimetric analysis was used in this experiment to determine the percent by mass of water in a hydrated salt. The hypothesis of this experiment was accepted on the basis that the percent by mass of volatile water in the hydrated salt would be fewer than 30%. The percent by mass was determined by the mass of water loss devised by the mass of hydrated salt multiplied by total capacity

The mass percent of water was determined using the mass of water and dividing it by the total mass of the hydrate and then multiplying that answer by 100%. The number of moles of water in a hydrate was determined by taking the mass of the water released and dividing it by the molar mass of water. The number of moles of water and the number of moles of the hydrate was used to calculate the ratio of moles of water to moles of the sample. This ratio was then used to write the new and balanced equation of the dehydration process. The sample was then rehydrated to the original state and the percent of the hydrate recovered was calculated by using the mass of the rehydrated sample by

Experiment 2 focused on finding the enthalpy of solution of magnesium chloride. Testing the enthalpy of solution started with measuring out 10 mL of deionized water in a graduated cylinder for three separate trials, each trial having a different mass of magnesium chloride. The water was then poured into a well of a Styrofoam calorimeter then the initial temperature of water was taken using a temperature probe and the LoggerPro programming. A measured amount of magnesium chloride was placed in the same well as the water in the calorimeter,

Then we took 8.35mL of salt water and put it in the evaporating dish which we placed over a Bunsen burner until all the water was dried out. The mass of the evaporating dish with the solid was 83.39g which means the mass of the sodium chloride was 0.622g. Next we took the mass and divided it by the volume of the solution which was 8.35mL and got 0.074 as the original concentration. To the get molarity of the salt solution we had to divide the concentration by the mass of the sodium chloride and then multiply by 1000mL to get 1.3M of salt solution. Final thing we had to do was determine the number ions present in 8.35mL so we took 1.3 moles of NaCl and divided it by 1000mL then multiplied by 8.5mL to get 0.01105 number of Na ions and Cl. The data was as I expected for part A because I followed step by step instructions on how to convert from grams to moles and moles to number of molecules and for part B my answer of 1.3 molarity of salt solution matched with key provided on LoudCloud.

Record the mass of the sodium chloride in the data table. If it is too small to read, click on the

The mass of salt (.26 grams) was then divided by the total mass of mixture (3 grams) and then multiplied by 100 to get 8.7% salt. The mass of sand was determined by subtracting the 100mL beaker with filter paper and sand (54.57 grams) by the the empty 100mL beaker with filter paper weighing 52.74 grams, to get 1.83 grams of sand. The mass percent of sand was determined by dividing the 1.83 grams of sand by the mass of mixture (3 grams) and multiplying by 100 to get 61%

The initial magnesium had a mass of 0.06 g while the final compound had a mass of 0.08 g. Magnesium oxide had been formed, and no magnesium should have been lost over the process due to magnesium being unable to form gases or liquids with any of the elements it had been exposed to.

The goal of this experiment was to determine the empirical formula for a hydrate of magnesium sulfate and water. The technique that was used was measure the mass of the hydrate and then apply heat to evaporate the water. Then determine the mass of water that was in the hydrate and the mass of the remaining magnesium sulfate. The equation for the hydrate is determined by calculating the mole to mole ratio of the water and the anhydrous. The resulting formula will be formated as: MgSO4*_H2O

Subsequently, two porcelain crucibles were used, weighed, and heated for about 10 minutes and then placed into a desiccator to cool. The two empty porcelain crucibles were first heated because the heat would vaporize any impurities that were originally on the crucible. The first crucible weighed 11.9047 g and the second crucible weighed 12.3735 g. Once the mass of the two crucibles

Firstly, after removed from the Bunsen burner, the crucible was not given time to cool down before being weighed. Weighing a hot crucible can affect the accuracy of measurements by making the crucible appear to weigh heavier, causing the results to be overstated. Secondly, as state in the paragraph above, both samples did not weigh exactly 2g. In trial 1, the sample weighed slightly less than 2g but in trial 2 the sample weighed slightly more than 2g. Consequently, the net weight for the solid in trial 1 was understated and the net weight for the solid in trial 2 was slightly

The chart below shows the % change in mass after being in their concentrated solutions:

After that, it is crucial to convert the mass to volume. The water density at a temperature will aid this process. The compliance of the Volume Occupied by 1.000g of Water Weigh in Air table is deemed necessary throughout the comparison.