Look it up if you have to! The resources include:Chemistry Unit 10--The Mole Concept Notes & Worksheets PacketChemistry Mole Quiz/PreactivityCounting by Weighing, ActivityMole Concept Quiz IMole Concept Quiz II, I have compiled all of the labs I use for my Chemistry I class into one document. If too much heat is applied, the anhydrous copper (II) sulfate (CuSO4), which has a grayish white color, decomposition starts at 250 degrees, while complete decomposition occurs around 600 degrees. Mass of evaporating dish 2. Copper suifate pentahydrate is used to determine the percent composition of water in a lab. then what do you do? The introduction to this, , students will experience the dehydration and re-hydration of, hydrated crystal, including doing the calculations involved. After comparing experimentally acquired ratios to the factual ratios for each substance, we determined that the ratios of magnesium sulfate was the closest one out of all four. Answer: _____ b) Calculate the number of moles of water in the hydrate sample that were driven off by heating? nH 2 O)? So the correct chemical formula is S r c l 2.2 waters for the next 1 37.2% water or 100 g of the compound gives us 32.7 g water Which will convert to moles water by dividing by its smaller mass, the remaining percentage is 62.8. nhi chung general chemistry chem 1411, hcc 11 november, 2017 post lab formula of hydrate and percentage of water of hydration introduction the purpose of this The ratios of other three substances were incongruous to each other. Then, the experimental ratio of water to magnesium sulfate being 6.63 to 1 with about 6% error strongly supports our hypothesis to a deeper level. We believe our hydrate was magnesium sulfate, because the unknown hydrate was more closely related in physical appearance to that of magnesium sulfate, compared to the the three other options. 1.) Hence the percentage composition of water in CuSO4.5H2O is 36.08 %. Step 3: Think about your result. It is appropriate for any college preparatory level high school chemistry class. What percentage of water was in the hydrate? iron ring While heating, be ready to adjust the height or Purpose: Determine the percent of water present in a hydrated copper (II) sulfate (CuSO 4 n H 2 O) and Epson Salts. An empirical formula of a chemical compound is the ratio of atoms in simplest whole-number terms of each present element in the compound. Students dehydrate copper (II) sulfate pentahydrate, crucible or evaporation dish and use their data to determine the % composition and the number of, molecules per formula unit of copper (II) sulfate. Balance Thus, at the end, we learned that there are countless numbers of applications of stoichiometry in chemistry. Record this figure as "Epsom salt, original (hydrated) mass" in Data Table 1. In order to determine the formula of the hydrate, [\(\text{Anhydrous Solid}\ce{*}x\ce{H2O}\)], the number of moles of water per mole of anhydrous solid (\(x\)) will be calculated by dividing the number of moles of water by the number of moles of the anhydrous solid (Equation \ref{6}). This, report requires students to directly apply their understanding of Empirical Formula and, procedure. This water can be driven off by heat to form the anhydrous (dehydrated) ionic compound, magnesium sulfate. I give you teacher set up instructions, has an introduction to help students understand why they are doing the, from copper (II) sulfate pentahydrate by heating and determine the empirical formula. Your LAB SETUP should be a sketch of the picture on the right. For your report explain what is happening at the molecular level when you add water. First, the assumption that the hydrate is associated with magnesium sulfate due to its white appearance is proven to be correct. This product contains 13 pages of chemistry multiple choice WITH ANSWERS on calculating the mass percent of an element, calculating the percent composition of a compound, determining a compounds empirical formula from percent data or mass data, determining the molecular formula of a compound and solving for the number of water molecules in a hydrate. Many of the "classic" chemistry experiments are included with, few that I've tweaked over the years.Labs-Thickness of Aluminum FoilDensity CubesDensity of PenniesConservation of MassMixture SeparationIdentifying Elements, Compounds, and MixturesDimensional Analy, Chemistry Lab Bundle 1: 31 Labs, 17 Inquiry, Quiz, Key, PPT, PDF/Word, (450PAGES) CHEMISTRY MULTIPLE CHOICE Grade 11 Chemistry all units WITH ANSWERS, Chemistry Curriculum Full Year Guided Notes Bundle. Use the information to answer the questions. First, the assumption that the hydrate is associated with magnesium sulfate due to its white appearance is proven to be correct. crucible & cover Calculate the Average % of Water in the Hydrate Samples. However, as we dehydrated the hydrate and discovered that a hydrate is made of some anhydrate and water with a certain ratio, we soon realized what a hydrate actually was. Use the dropper to add a very little water to the anhydrous copper (II) sulfate. Heat the contents again for a short time (3 minutes). 2. , as the hydrate appeared to be white due to the colorless magnesium.Thus, this knowledge of specific colors of ions led us to confidently conclude that the anhydrate was undoubtedly magnesium sulfate. The focus of this lesson is defining, look! \[x = \frac{n_{\ce{H2O}}}{n_{\text{Anhydrous Solid}}} \label{6}\], DO NOT perform any lab work outside of the stated lab hours. Once we know how much water is needed for each magnesium sulfate, we can then name the substance in MgSO 4 x H 2 O, where x represents the ratio. What is bound to the copper (II) ion in copper sulfate? After obtaining the data from the video and filling out your data table, you will then perform the necessary calculations to determine the mass, video shows the heating of an unknown hydrated sample. The number of water moles can also be known by repeating the same procedure, but with the molar mass of water instead. at a slight angle with its cover slightly ajar. Mass of water. Be specific. Second, the results are great! First, it is so easy to set upnot much prep at all. Since copper (II) sulfate is usually a bright blue due to Cu. 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Determing the Mass, Moles and Number of Particles. The error being only 5.58%, the overall ratio of water to magnesium sulfate was somewhat accurate. + lose uoa. Setup the ring stand with iron ring and ring. 3. What experimental evidence would you have to indicate you inadvertently, Determine the mass percent of each element present in. The water in a hydrate is bound loosely, and so is relatively easily removed by heating. crucible and contents and record the result in trial 1 of the observation table. Predict how experimental factors will impact the accuracy and precision of results. From the masses of the water and anhydrous solid and the molar mass of the anhydrous solid (the formula of the anhydrous solid will be provided), the number of moles of . As 6.63:1 is relatively close to 7:1, the expected ratio for this substance, we can thus conclude that the unknown hydrate is magnesium sulfate heptahydrate, MgSO. Write the formula of the one you chose. 9H2O), 1.48g CuSO4x 1 mol CuSO4/ 159.61g mol-1CuSO4 = 0.009273 mol CuSO4, 1.47g H2O x 1 mol H2O / 18.02g mol-1H2O = 0.08158 mol H2O, number of moles H2O / number of moles CuSO4, = 0.08158 mol / 0.009273 mol = 8.80 mol H2O / 1 mol CuSO4 (3 significant figures), 1.48g MgSO4x 1 mol MgSO4/ 120.36g mol-1MgSO4= 0.01230 mol MgSO4, number of moles H2O / number of moles MgSO4, = 0.08158 mol / 0.01230 mol = 6.63 mol H2O / 1 mol MgSO4, 1.48g FeCl3x 1 mol FeCl3/ 162.20g mol-1FeCl3= 0.009125 mol FeCl3, number of moles H2O / number of moles FeCl3, = 0.08158 mol / 0.009125 mol = 8.94 mol H2O / 1 mol FeCl3, 1.48g Fe(NO3)3 x 1 mol Fe(NO3)3/ 241.86g mol-1Fe(NO3)3= 0.006120 mol Fe(NO3)3, number of moles H2O / number of moles Fe(NO3)3, = 0.08158 mol / 0.006120 mol = 13.3 mol H2O / 1 mol Fe(NO3)3. Answer1) A hydrate is a solid ionic compound that contains specific number of water molecules in its crystal structure.