Experimental Question: How can we experimentally determine the formula of an unknown hydrate, A? A residue of 3.60 g of remains from the heating of a 4.76 gram sample of a hydrated calcium chloride. 9. Complete the folowing and submit your answers as a word document in Canvas. The formal name of this hydrate is “magnesium sulfate heptahydrate”. Problem #2: A hydrate of Na2CO3 has a mass of 4.31 g before heating. 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. On a macroscopic, practical level, the parts will be moles. Determine the mass of the hydrate by subtracting entry #4 from entry #3 in the Data Table. The residue masses 2.48 g. Answers 1) a) 40.51% H 2 O b) 43.83% H 2 O c) 28.9% H 2 O Record this result in Data Table entry #5. Virtual Lab Hydrate.docx. 5. Purpose. If the mass of the hydrate was 8.881 g, what are the formula and name of the hydrated compound? 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. Gently heat ... U5L14 Formula of a Hydrate Answer Recording Sheet (2).docx. Texas A&M University, Texarkana. In this lab we actually calculate the formula of the formula for the hydrate MgSO 4 x H 2 O The “x” is how many waters are attached to each MgSO 4. O. 0.391 g Li 2SiF 6, 0.0903 g H 2O ? Kimberly Graziano & Hyunjae Kim. A hydrate is a compound that is … An empirical formula of a chemical compound is the ratio of atoms in simplest whole-number terms of each present element in the compound. Testable Prediction: Our unknown hydrate may be a hydrate of copper(II) sulfate, magnesium sulfate, iron(III) chloride, or iron(III) nitrate. The resulting anhydrous compound weighs 3.120 grams. 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: What are the name and the formula of the hydrate? In this experiment, you will be given a sample of hydrate. Hydrate Lab. 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. 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. 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? For example, Glucose is C 6 H 12 O 6; it’s empirical formula is CH 2 O. 2. 8. What is the formula of this hydrate? 6. A sample of blue vitriol (cupric sulfate hydrate) is heated. Analyzing results Calculate the percent water in your sample. You will determine the mass of the water driven off by heating, as well … 8. Lab – Formula of a Hydrate - Help with calculations Magnesium sulfate ( MgSO 4) is a molecule that loves to hold on to water (hydrophilic). Applying conclusions Calculate the percent water in a mole of copper(II)sulfate pentahydrate using the formula. Practice questions will ask you about hydrates vs. anyhdrates, how to solve for hydrate formulas, and the meaning of n in a hydrate formula. Drawing conclusions Using your answers from items 3 and 4, determine the empirical formula for the copper sulfate hydrate. 7. formula units and molecules. PURPOSE: To determine the percentage of water in a hydrate. Observing our nitrate, it has a white crystalline structure, representing that similar to table salt. 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? CHEM 1311. Determine the formula for the hydrate from the given information: a. 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