Lab Report: The Synthesis Of Alum

Question3: Experiment 3 The unknown acid sample was 1 • Monoprotic Acid Trails Initial NaOH solution (mL) final NaOH solution (mL) The volume of NaOH to titrate the acid (mL) Amount of Unknown Acid sample 1 (g) The moles of the Unknown Acid (mol) Molar mass of the Unknown Acid (g/mol) A 3.38 28.31 24.93 0.150 0.0026 57.69 B 0.18 29.32 29.14 0.175 0.0029

Materials 1. Clean and dry 250 mL beaker. 2. Determine the mass of 2 Alka-Seltzer® tablets. 3.

In order to begin this experiment, first one must find the balanced chemical equation for the reaction which occurs between the aluminum and copper (II) chloride. This balanced equation being 2Al(s)+3CuCl2 (aq)3Cu(s)+2AlCl3 (aq). After finding this equation, one must use the process of stoichiometry in order to find how many grams of aluminum are needed in order to produce 0.15 grams of copper. In this experiment, the purpose was to produce between 0.1 and 0.2 grams of copper, so one should attempt to produce 0.15 grams of copper seeing as it is the average of those two numbers. The first step in the stoichiometric process which one has to complete is finding how many grams of copper are in one mole of copper.

Observe the reaction and record how fast the Alka-Seltzer dissolves. 7. Place an Alka-Seltzer tablet into a second empty water bottle. 8. Pour 16 oz of room-temperature water into the bottle.

In order to find the amount of a product made during a double displacement reaction, the product has to be separated from the solution. From this number of moles of precipitate can be calculated. From there the number of moles of reactants can be calculated using the mole ratios of the particular reaction that occurred. As seen in Table 5 it is shown that by finding out the number of moles of the unknown, the molar mass of the unknown can be calculated. From the found mass of the unknown compound, the mound of the original ion can be found.

Lastly, the unknown compound was reacted with two different salts. For the first salt, 0.50 grams of KCl was mixed with 5 mL of water in one beaker while 0.5 grams of NaNO3 was mixed with 5 mL of water in a different beaker. Then, the NaNO3 solution was added to the KCl solution. To perform the reaction with the second salt, 0.50 grams of KCl was mixed with 5 mL of water and 1 mL of 1 M Ag(NO3)2 was added. After performing each reaction, the solution was observed to see if a reaction occurred and the pH value of the resulting solution was tested using a pH

The purpose of the lab was to discover the properties and the trends of the alkaline earth metals. In part A, the trend was as the atomic number increase in the alkaline earth metals the elements are more reactive. The alkaline earth metals each have two electrons in their outer shell and because all electrons want to become stable they are ready to give up the two electrons. When they are combined with water, the chemical reaction occurs differently based on each element.

To calculate the experimental mass the substance of each bag and the bag its self was measured using a balance. After gathering the mass subtract the mass of the empty bag to the mass of the unknown substance, in order to just have the mass of the substance. Afterward the mass of the unknown substance was divided by the number of moles recorded on the bag of the substance. The measurements are displayed on the table

Using the equation m = ΔTf/Kf , the molality of the unknown solution was found. Then, moles of unknown were calculated, which was used to calculate the average molar mass of unknown. Theory: After the experiment was completed, the data

I. Purpose: To experimentally determine the mass and the mole content of a measured sample. II. Materials: The materials used in this experiment a 50-mL beaker, 12 samples, a balance and paper towels. III.

The second step that you will need to do is to fill the boiled water up in an unblemished glass cup that reaches the exact amount of sixteen ounces. The third step that you will need to do is to get the recording of the water’s temperature. The fourth step you will need to do is to place two tablets of Alka-Seltzer in the water. The fifth and final step that you will need to do is to get either a stopwatch or a timer and calculate the specific amount of time it will take for these tablets of Alka-Seltzer to completely

The actual yield of the reaction was 4.411 grams of copper and was obtained through the experiment

The percent recovery of the copper was calculated using the equation, percent recovery = (the mass of the copper recovered after all the chemical reactions/the initial mass of the copper) x 100. The amount of copper that was recovered was 0.32 grams and the initial mass of the copper was 0.46 grams. Using the equation, (0.32 grams/0.46 grams) x 100 equaled 69.56%. The amount of copper recovered was slightly over two-thirds of the initial amount.

The final product weight for percent yield was only the solid E product, which missed one half of the final product produce. If both products were weight, the percent yield would have been larger that it was. Instead of 22.33%, it could have been 44.66%. To prove that both products were obtained, but only one of the two products was analyze, a TLC plate of the DCM layer, that contains both products, and of the final product, was obtain.

Once dissolved, fill the rest of the volumetric flask up to the line on the neck of the flask. Again mix the solution. Use four, 10mL volumetric flask, and label them from 1-4. Add approximately 2mL of copper sulfate pentahydrate into flask 1, 4mL to flask 2,