Hydrate Lab The purpose of this lab is to analyze the percent water in a crystalline hydrate and to indentify the hydrate from a list of possible unknowns. The solid hydrate will be heated to remove the water, and the percent can be found by measuring the mass of the solid before and after heating. The hydrate will be indentified by comparing the percent water in the hydrate with the percent water calculated for the possible unknown. Before the lab there are pre-lab questions: 1. Describe the three general safety rules for working with a Bunsen burner.
From your three trials, calculate the average volume of Na2S2O3 needed for the titration of 25.00mL of diluted bleach. 3. Use the average volume and the molarity of Na2S2O3 to determine the molarity of the diluted bleach. (Find moles of Na2S2O3, convert to moles of NaClO, and divide by volume of dilute bleach that was titrated in each trial to get M). 4.
Conclusion:The purpose of this lab is to prepare and purify a fuel, ethanol C2H5OH. We learned to do so by the process of fermentation, and distillation. Over the course of 2-3 weeks, we collected and analyzed the data for this lab. On day 1, we prepared our sugar-yeast solution which contained warm water, sugar, and yeast. With the help of the water, the yeast was then the reactant, then which was activated.
Separation of the components of Extra-Strength Excedrin I: Acid-Base extraction Introduction The purpose of this experiment is to analyze the purity of Extra-Strength Excedrin® by utilizing thin-layer chromatography and determine the percent recoveries of its components. Three active ingredients will be extracted and collected from two tablets of Extra-Strength Excedrin® by utilizing acid-base extraction method. Three active ingredients of Extra-Strength Excedrin® are acetylsalicylic acid(aspirin), acetaminophen and caffeine, and their structures are: In addition, there is a binding material, which binds other three components together. These compounds can be separated by acid-base extraction because of their different acidities. A binding material can be separated by dissolving the tablet in ether since three active ingredients are soluble.
Use a calorimeter to measure the temperature change in each of three reactions. Calculate the heat of reaction, ∆H, for the three reactions. Use the results to confirm Hess’s law. Ev al Figure 1 ua tio Na+(aq) + OH–(aq) + H+(aq) ) + Cl–(aq) → H2O(l) + Na+(aq) + Cl–(aq) ∆H3 = ? n (3) Solutions of aqueous sodium hydroxide and hydrochloric acid react to form water and aqueous sodium chloride.
Determine the percent yield of this reaction, showing all steps of your calculation. (3 points) heoretical yield of H2 gas: (1.156 x 10^-3 moles)(1 mole H2/ 1 mole Mg) = 1.156 x 10^-3 moles Theoretical mass: (1.156 x 10^-3 moles)(2.02 g/mole) = 2.335 x 10^-3 g Using ideal gas law: P = (1.1 atm)(760 torr / 1 atm) - 19.8 torr = 816.2 torr V = 0.026 L T = 295 K Solve for n: n = PV/(RT) n = (816.2 torr)(0.026
For that we must put the temperature we found and put it into 1.01(x) + 4.43. 1.01 multiplied by 31.8 plus 4.43 equals 36.59 degrees Celsius. Now that all of our values are ready to be analyzed we can narrow down what the unknown substance is. I started with boiling point there was only 2 substance had a boiling point close to the boiling point that we found pentane and ethyl ether. Next the freezing point which didn’t eliminate either of them.
93 g/mol? Not we get to use it! Yay! 93 g/mol / 31.06 g/mol = 3 (this is the multiplier) Multiply that whole number through the subscripts of the empirical formula. 3 x (C H5 N) = C3H15N3 Hydrated compounds Solving process: 1st- the difference between the initial mass and that of the dry sample is the mass of water that was driven off.
After extraction was performed on the tablet it was then ran through an HPLC test. After performing HPLC and using the line equation three concentrations were found as well as the three main ingredients. The three main ingredients were caffeine, aspirin, and acetaminophen. The final concentrations were 0.02 mg/mL, 0.06 mg/mL, and 0.21 mg/mL. It