Determination of Cobalt Oxalate Hydtrate Introduction The objective of this lab is for students to determine the percentage of cobalt oxalate hydrate using the gravimetric analysis. They will also do a redox titration to determine the percentage of oxalate in the compound. After the percentages are calculated‚ you will determine the percent water by the difference of Oxalate and Cobalt from %100. Procedure Determination of Cobalt 1. Weigh 0.3 g of solid cobalt oxalate hydrate (from lab 8) on a balance
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Composition of Cobalt Oxalate Hydrate Experiment 12 Robbie Kinsey Partner: Debnil Chowdhury Chem. 1312-D TA’s: Russell Dondero & Sylvester Mosley February 9‚ 2000 Purpose The purpose of this lab was to determine the percent cobalt and oxalate by mass‚ and with that information‚ the empirical formula for cobalt oxalate hydrate‚ using the general formula Coa(C2O4)b.cH2O. Procedure The powdered cobalt oxalate hydrate was weighed
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The purpose of the lab is to identify the compound based on a constant composition by performing a serious of tests. The hydrate is solid crystals compound and appears to be dry: since an ionic compound (salt) is crystallized from an aqueous solution (water)‚ by heating the hydrate the water is released from ionic structure; therefore it is possible to measure the weight of the ionic compound and calculate its ratio to the liquid in the hydrate. The goal of the lab is to establish the identity
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Unit 6 Lab Report 1. Objective: To find the percent composition of water in an unknown hydrate. 2. Materials: Goggles‚ apron‚ evaporating dish‚ hot plate‚ and stirring rod 3. Procedure: get the mass of a evaporating dish‚ put a sample of the hydrate onto the evaporating dish and mass the dish with hydrate. Put the dish with hydrate on the hot plate on high heat. Break up any clumps that form during the heating process. Observe any color
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9-19-13 Dehydrating and Rehydrating a Hydrate Introduction The mass percent of water was determined using the mass of water and dividing it by the total mass of the hydrate and then multiplying that answer by 100%. The number of moles of water in a hydrate was determined by taking the mass of the water released and dividing it by the molar mass of water. The number of moles of water and the number of moles of the hydrate was used to calculate the ratio of moles of water to moles of the sample
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that are formed from a reaction between an acid and a base. Hydrates are inorganic salts which contain specific numbers of water molecules. Not all hydrates contain simple formulas. According to Formula of a Hydrate‚ to be anhydrous is to be without water‚ or to have all water removed. Some hydrates can become anhydrous by heating them‚ meaning hydrates can be separated into salts and water after heating. An ionic hydrate is a hydrate with water molecules attached to a crystal lattice instead of
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A The % Composition and Empirical Formula of a Hydrate: It Doesn’t Hold Water‚ Or Does It? 1. To determine the percent water in an unknown hydrate. 2. To calculate water(s) of crystallization for an unknown hydrate. 3. To determine the formula of an unknown hydrate. OBJECTIVES SKILLS Proper use of the following equipment: Dial-O-Gram balance (Laboratory Technique I)‚ electronic balance (Laboratory Technique II) and Bunsen burner (Laboratory Technique III). Dial-O-Gram balance‚ electronic
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What is the Identity of this Hydrate? Date Performed: May 30‚ 12 Date Submitted: June 6‚ 2012 Name: 2968 Instructor: Reid A hydrate was given to our group and the identity of the hydrate was unknown. The lab workers were told to determine the identity of the unknown hydrate. The identity of the hydrate could be determined by calculating the hydrate’s percent of water. So the lab workers set out to determine the water percent of the unknown hydrate. The percent of any compound or element
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DETERMINATION OF THE CHEMICAL FORMULA FOR A HYDRATE USING MOLE RATIO OF WATER MASS AND MAGNESIUM SULPHATE INTRODUCTION Ionic (salt) compounds are able to hold loose bonds with water molecules. A hydrate is a compound that incorporates water molecules into its crystalline lattice structure (McGraw-Hill Ryerson‚ 2014). Identifying a compound as hydrated or anhydrous is important as the mass of the compound increases if it contains water molecules. In nature‚ hydrates exist with a fixed ratio of water
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Pre Lab 1a. Hydrated compound: ionic compound which contain water molecules inside their crystal lattice. The water is not chemically bonded to the crystal in any way and can be extracted by heating the compound. 1b. Anhydrous compound: a compound without water. 2a. The dot means that there are water molecules present in the crystal lattice in a specific ratio. 2b. For every mole of copper sulfate‚ there are five moles of water. 2c. The molar mass of copper (II) sulfate is 159.61 grams/mol
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