An empirical formula of a chemical compound is the ratio of atoms in simplest whole-number terms of each present element in the compound. For example, Glucose is C 6 H 12 O 6; it’s empirical formula is CH 2 O. Drawing conclusions Using your answers from items 3 and 4, determine the empirical formula for the copper sulfate hydrate. Observing our nitrate, it has a white crystalline structure, representing that similar to table salt. 6. The formula of the hydrate shows the ratio of the moles of anhydrous salt to the moles of water; in the above case, that ratio is 1:5. Lab – Formula of a Hydrate - Help with calculations Magnesium sulfate ( MgSO 4) is a molecule that loves to hold on to water (hydrophilic). 8. A sample of blue vitriol (cupric sulfate hydrate) is heated. Testable Prediction: Our unknown hydrate may be a hydrate of copper(II) sulfate, magnesium sulfate, iron(III) chloride, or iron(III) nitrate. Record this result in Data Table entry #5. What is the formula of this hydrate? O. In this experiment, you will be given a sample of hydrate. 0.391 g Li 2SiF 6, 0.0903 g H 2O ? You will determine the mass of the water driven off by heating, as well … Water of hydration MgSO 4 • 7H 2 O. Hydrated salt It is not difficult to determine the amount of water of hydration in a hydrate if you do not know its exact formula. What is the formula of the hydrate? Texas A&M University, Texarkana. Solution: 1) Determine mass of water driven off: 4.31 minus 3.22 = 1.09 g of water 2) Determine moles of Na2CO3 and water: Hydrate Lab. Virtual Lab Hydrate.docx. Kimberly Graziano & Hyunjae Kim. Analyzing results Calculate the percent water in your sample. 5. Purpose. CH 2Cl 12.0 g + 2(1.0 g) + 35.5 g = 49.5 g 247.5 / 49.5 = 5 CH 2Cl x 5 = C 5H 10Cl 5 3. Problem #2: A hydrate of Na2CO3 has a mass of 4.31 g before heating. Experimental Question: How can we experimentally determine the formula of an unknown hydrate, A? What are the name and the formula of the hydrate? Answers 1) a) 40.51% H 2 O b) 43.83% H 2 O c) 28.9% H 2 O The resulting anhydrous compound weighs 3.120 grams. What is the molecular formula of the molecule that has an empirical formula of CH 2Cl and a molar mass of 247.5 g/mol? Determine the mass of the hydrate by subtracting entry #4 from entry #3 in the Data Table. A 4.175 gram sample of a certain hydrate of copper (II) sulfate, CuSO 4 •xH 2 O, is heated until all the water is driven off. If the mass of the hydrate was 8.881 g, what are the formula and name of the hydrated compound? A hydrate is a compound that is … PURPOSE: To determine the percentage of water in a hydrate. After heating, the mass of the anhydrous compound is found to be 3.22 g. Determine the formula of the hydrate and then write out the name of the hydrate. 7. Practice questions will ask you about hydrates vs. anyhdrates, how to solve for hydrate formulas, and the meaning of n in a hydrate formula. 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