The watch glass was removed with the beaker tongs. Using a rubber bulb and a stirring rod to stir the solution continuously, 15.00mL of .25M BaCl2 solution was added to the solution in the beaker. The watch glass is replaced and the solution is keep hot but not boiling for 15 minutes. The precipitate was allowed to settle. When the liquid above the precipitate was clear, the solution was tested for completeness of precipitation when a few drops of BaCl2 solution were added from a pipette.
10. Repeat the procedure for a second metal. Analysis: Our data | Trial #1 | Trial | Mass of zinc | 1.99g | 4.01g | Mass of water in Calorimeter | 45g | 45g | Temp. of water in Calorimeter | 20°C | 21°C | Temp. of boiling water | 100°C | 100°C | Peak temp.
Quality Control for Athenium Baking Soda Company Introduction In this experiment, we will be using thermal gravimetric analysis (experiment 4) and HCL titration (experiment 12) to determine the percentage of NaHCO3 (baking soda) in the sample given. We will also be using emission analysis for group IA and IIA salts (experiment 10) to determine the impurities present. The purpose of this experiment is to determine the purity of a sample of baking soda given us by the Athenium Baking Soda Company. We will First determine the percentage of baking soda and then determine whether it contains particulates of CaCl2, LiCl, of KCl for the purpose of seeing whether it is pure and useable or not (the quality of the baking soda). We are performing the experiment to gain our spots on the team of quality control for the Athenium Baking Soda Company.
To perform this experiment, we will utilize emission spectra, titrations, and thermal gravimetric analysis, using knowledge from Experiments 10, 4, Titrations of Na2CO3 and NAHCO3 by HCl (hydrochloric acid) will be performed to determine the concentration of HCl, as well as the number of moles of HCl present within the sample of baking soda. As a result, we will be able to determine the molar concentration of HCl by determining its equivalence point (the point on the graph where the exact amount of rectant needed to perform a reaction has been added) from graphical analysis. Na2CO3(aq.) + HCl(aq.) ==> NaHCO3(aq.)
Lab 4: Determination of Percent by Mass of the Composition in a Mixture by Gravimetric Analysis Introduction Thermal gravimetric analysis is used to determine the percent by mass is used to determine the percent by mass of a component in a mixture. When a mixture is heated to an appropriately high temperature, one component in the mixture decomposes to form a gaseous compound. The mass of this particular component is related to the mass of the gaseous compound. In this experiment, the percent by mass of sodium hydrogen carbonate (NaHCO3) and potassium chloride (KCl) in a mixture will be determined. Experimental First, we weighed 2 samples, each has 1 gram of NaHCO3-KCl mixture Second, we put the samples in 2 crucibles (A and B) and weighed them.
Measure approximately 1 g of Copper(II) Sulfate Hydrate into the crucible and crucible and lid. 4. Heat the crucible gently. 5. Stirring carefully and observe the color of the hydrate until it changes to a consistent white color, then the Copper(II) Sulfate is dehydrated.
Then take jug with room temperature water and pour out three cups into the pot. Before placing it on the stove and heating the water to repeat the experiment, the water temperature was taken to ensure that it was approximate to the room temperature. Literature Review: According to an article in The New York Times, the notion of a body of cold water will reach boiling point quickly as to an identical body of hot water under the same parameters is false (O'Connor, 2008). In this experiment it is not to prove what has already been done, rather to find if the rise of water bodies would be parallel. The notion is to calculate the slope of increase in water temperature given two different starting points, are they both identical.
Safety goggles and lab apron must be worn for the experiment. 2. Fill a 250 cm³ beaker about 2/3 full with water. Place the beaker of water on a hot plate or ring stand with the wire gauze. Begin heating the water to the boiling point 3.
Every few minutes, the lid of the crucible was lifted carefully with a tong to see if the magnesium had started to burn and also to left some air enter the crucible to make the experiment more efficient. 6. When the magnesium had completely reacted, the crucible was heated strongly without the lid on for few minutes. Then, the crucible was placed on gauze for it to cool down. 7.
2: First you measure the mass of the copper tacks and also try to get the mass of the water in the thermos as close to 0.1 kg since 1 dl of H20 = 0.1kg H20. 3: Using the test tube holder, sink the test tube with the copper in it into the 4: The electric kettle is now supposed to make the water boil and raise the temperature of the copper as close to 100ºC (T1cu) but it is not very likely that you will get exact 100ºC due to heat loss. This step will almost certainly take a couple of minutes. 4: Measure the temperature of the water in the thermos (T1w) and then add the tacks to the water in the thermos. 5: Now measure the temperature of the water (T2cu and T2w will have the same temperature).