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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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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5H2O 2) There are at least two reasons why heating to find percentage of water in hydrated crystals is not recommended for all hydrates. The first reason is that some hydrates have such a strong bond with the water that not all of it will be able to be removed. The second reason is that different hydrates have their own mass. Depending on the mass and type of hydrate‚ some of the molecule may be burned off from heating. This would lead to a false accusation that the mass loss was all from water
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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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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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The lab in which we conducted last Tuesday was an analysis of a hydrate and what happens to it when it is heated. A hydrate is a crystalline compound which water molecules are chemically bound to it. In the lab‚ we were to analyze the difference in grams of the hydrate and the anhydrate. An anhydrate is the crystalline compound without the water molecules bound to it. During our lab‚ we were to heat up the crucible‚ the crucible with hydrate‚ and the crucible with an anhydrous and write down each
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Formula of a Hydrate Lab Design: Problem: What is the chemical formula for a hydrated copper (II) sulphate compound? Controlled Variable: The mass of hydrated copper (II) sulphate. Responding Variable: The mass of dehydrated copper (II) sulphate‚ mass of H2O Materials: Ones on the handout + Hot plate. Procedure: 1. Mass 3.00g of hydrated copper (II) sulphate using electronic balance 2. Measure the mass of a thin‚ crucible dish using electronic balance 3. Gently pour hydrated
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Copper Chloride Lab Report Procedure Part A: 1. Pick up the container of copper chloride dehydrate‚ and observe material. Describe crystals in detail‚ and write down all of the observations. Part B: 1. Take a 100 ml beaker and fill ¼ of it with water. Use a spatula to add some copper chloride dehydrate to the beaker filled with water. Record the observations. Be sure to observe the water and the copper chloride dehydrate. 2. Stir the contents in the beaker with
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Abstract: Hydrates are compound with a constant composition. Concepts of Law of Definite Proportions (hydrates remain in constant proportions) and Law of Conservation of Mass (this idea is used to determine the mass of water in the compound and‚ subsequently‚ the formula of the compound) are expressed in this experiment. In this experiment‚ the goal was to find the formula of copper sulfate pentahydrate by heating a sample of the blue compound in order to evaporate the water and receive the
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