GCC CHM 090 GCC, 2006 1 of 2 Names: _____ Lab Exercise: Percent Water in a Hydrate Introduction: A hydrate is a crystalline solid that traps water as part of its crystal structure. Your LAB SETUP should be a sketch of the picture on the right. Calculate the percent by mass of water by dividing the mass of H 2 O in 1 mole of the hydrate by the molar mass of the hydrate and multiplying by 100%. Mass of water. Copper suifate pentahydrate is used to determine the percent composition of water in a lab. From this lab, we are able to conclude that our prediction was strongly supported in both terms. (process and specific method used here). Chemistry: Lab - Formula of a Hydrate . Calculate the percent water in the hydrate sample, using Equation 2, percent water, % = (mass of water lost, g/mass of hydrate heated, g) (100%), determine the mass of a hydrated salt sample and the mass of the residue after heating the sample; from these masses you will calculate the mass of water lost during heating and the percent water in the hydrate, crucible and cover, crucible tongs, Bunsen burner, ring stand and support ring, pipe-stem triangle, ceramic-centered wire gauze, microspatula, balance, preparing and weighing crucible; heating and weighing unknown hydrate. 5 waters of hydration. Equation 2 (percent water in a hydrate) What errors would this cause in the calculation of the percent of water in the hydrate? This hydrate was previously mentioned in class to be magnesium sulfate heptahydrate. Mass of dish + hydrate 3. You will find that most students will obtain the expected results pretty much dead on, and the students love the very low, error and using simple steps of 1-4 find empirical formula for copper(II) sulfate crystals. Water is a very polar molecule which tends to be attracted to . A hydrate is a compound that is chemically combined with water molecules. What is a hydrate? Initial Data: Balance The, requires bunsen burners, rings, ring stands, crucibles, crucible tongs, and balances. Cross), Civilization and its Discontents (Sigmund Freud), Chemistry: The Central Science (Theodore E. Brown; H. Eugene H LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward), Principles of Environmental Science (William P. Cunningham; Mary Ann Cunningham), Campbell Biology (Jane B. Reece; Lisa A. Urry; Michael L. Cain; Steven A. Wasserman; Peter V. Minorsky), Topics for Exam 4 - Summary General Chemistry, Laboratory techniques option one report (1) Nicholas Mc Quagge, and magnesium sulfate, also known as Epsom salt. Number the aluminum dishes 1, 2, and 3 according to Figure 2. Setup the ring stand with iron ring and ring. If we had either heated the beaker with a strong flame from the beginning or increased the amount of time of heating, the number of moles of water during calculation could have been larger. The water is present in a definite and consistent ratio. Purpose: Determine the percent of water present in a hydrated copper (II) sulfate (CuSO 4 n H 2 O) and Epson Salts. The change, mass observed allows them to calculate the amount of, COMPOSITION EMPIRICAL FORMULA Multiple Choice Grade 11 Chemistry (13 PG), This product contains 13 pages of chemistry multiple choice WITH ANSWERS on calculating the mass, data or mass data, determining the molecular formula of, 12 font, times new roman, without text boxes and condensed into the least amount of space possible. 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. From the data the students can determine the experimental percentage of, composition and empirical formulas. It is appropriate for any college preparatory level high school chemistry class. What percentage of water is found in CuSOp5H20? Determine the number of moles of water, x, per mole of anhydrous salt and write the chemical formula of the hydrate sample. for the imperialist) and position the flame under the crucible so that the inside blue Examine the formula for the hydrate: CuSO, The actual mass percent of water in the hydrated copper (II) sulfate compound should have been, In the experiment involving hydrated copper sulfate, overheating causes a. connected to the rest of the formula with a raised dot, formula for copper (II) sulfate pentahydrate, how do we remove the waters of hydration from a compound? Determine the percent water of hydration in a hydrate sample. If not, repeat the heating/cooling/weighing process until two successive weighing have the same mass. Heat the compound gently Note the release of any steam from the beaker. Light the burner with a flame that is approximately 3 to 4 cm high (1 to 2 inches Finally, this is for balancing the chemical equation of the decomposition of a hydrate. Once the beaker is cool, measure the mass of the beaker, the anhydrous salt and the glass rod. You'll get a detailed solution from a subject matter expert that helps you learn core concepts. then what do you do? copper (II) sulfate hydrate Such compounds ar, compounds that have a specific amount of wat, writing the formula of a hydrate, a dot connects t, that of water and is viewed as an addition sign i, lose all or part of their water of hydration when e, this dehydration is accompanied by a colour chang, Give Me Liberty! The moles of water and inorganic salt in Epson salt were separately calculated and. CuSO5HO (s, blue)heatCuSO (s, white)+5HO (g) 3 steps to determining percent water in unknown hydrate. Honors Chemistry Worksheet - Hydrates ANSWER KEY. This Chemistry experiment illustrates the Law of Definite Proportions and reinforces the concept of Composition Stoichiometry. Each type of hydrate traps water in its own unique way, but heating a hydrate will release the The focus of this lesson is defining, look! Some sources of deviation of the data may include: a. 9. The accepted values for the percent of water in the following hydrates are as follows: BaCl, 2 H,0 - 14.8%, ZnSO, 7H,0 - 43.9% MgSO, 7H,0 - 51.2%, MgCl, 6 H,O=53.2% Fe(NO), 9 H,0 = 40.1% Based on your calculations above, which of the hydrates listed was your unknown? 1.7: Experiment 6 - Hydration of Salt is shared under a not declared license and was authored, remixed, and/or curated by LibreTexts. based on the chemical formula. Use a flathead screwdriver or a key to open the Sterno can's lid. Why Do Organism Look Like the Way They Do. Mass of anhydrous salt Calculations - Remember to show all of your work. 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