Lillian Zhang AP Chemistry 3rd Period Formula of an Unknown Hydrate The purpose of the Formula of an Unknown Hydrate lab is to determine the weight percentage of H2O hydrated to an unknown salt and the empirical formula for the hydrated salt. To do this‚ a massed amount of the hydrate is heated over either a hot plate or Bunsen burner. This causes the water to be removed‚ leaving the anhydrous salt behind in the dish. The mass of the anhydrous salt‚ now with the absence of water‚ is less than
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Introduction: An empirical formula of a chemical compound is the ratio of atoms in simplest wholenumber terms of each present element in the compound. For example‚ Glucose is C H O ; it’s empirical formula is CH O. 6 12 6 2 A hydrate is a compound that is chemically combined with water molecules. In contrast‚ an anhydrate does not contain water‚ and has had all of its water removed. Purpose: The purpose of this experiment is to identify the unknown hydrate‚ selected by your teacher
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3/4/14 Determining The Formula of a Complex Ion Luqman Khan Contents: Aim………………………………………………………………………………………………………………….……2 Results……………………………………………………………………………………….………………………2-6 - Raw Data………………………….………….……………………………………………………..…..2 - Qualitative Analysis………………………………………………………………………………….2 - Data Processing……………………………..……………………………………………………..3-5 - Graphical Results……………………………..…………………………………………….…….5-6 Conclusion…………………………………………………………………………………………………………6-7 Evaluation……………………………………………………………………………………………………………
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learned before on how to determine the empirical formula of a compound based on the test and also chemical analysis on it. Hence this experiment is mainly goes around with how to determine the empirical formula of Magnesium Oxide following various tight procedures in order to get the knowledge and apply it onto another compounds. We are investigating the empirical formula of Magnesium Oxide in this experiment. RESEARCH QUESTION: How empirical formula of Magnesium Oxide is obtained by heating Magnesium
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Chemistry Practical Report: Topic: Determining the Empirical Formula of Magnesium Oxide Patrick Doan 11 CHEM 11 26/9/08 Table of contents 1.0 Aim 1 2.0 Theory 2-3 3.0 Materials 4 4.0 Method 4 5.0 Results 4 - 5.1 Qualitative Observations 4 - 5.2 Example Calculations for each Calculated Value 5-7 -5.21 Experimental Values and Associated Errors 5-7 - 5.3 Accumulated Raw Data 8 - 5.4 Mean Experimental
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Hydrates Analysis NAME:_____________________________________ PERIOD:_________ Prelab 1. A 6.00g sample of calcium sulfate hydrate (CaSO4.x H2O) is heated until all the water is driven off. The anhydrous compound has a mass of 4.77 g. Calculate the value of x in the formula. 2. For the data in problem number 1 above‚ what is the mass percent water in the hydrate? 3. Calculate the number of grams of water that could be obtained by heating 2.00 g
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EXPERIMENT NUMBER 8 PERCENTAGE OF WATER IN A HYDRATE Objectives 1. To determine the percentage of water in barium chloride dihydrate. 2. To determine the percentage of water in an unknown hydrate salt. 3. To calculate the water of crystallization for the unknown hydrate salt. Discussion A hydrate salt is composed of anions (negative ions) and cations (positive ions) which are surrounded by and weakly bonded water molecules. Each hydrate salt has a fixed number of water molecules
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proportion in relation to the mass of the crystalline structure. This water that is trapped inside the hydrated solid structure is called water of crystallization or water of hydration. A salt with associated water of crystallization is known as a hydrate. The formula of a hydrated salt is written as the number of moles of water present in one mole of crystalline structure. Deliquescent materials are substances that absorb water from the atmosphere and eventually become hydrated. These materials‚ usually
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purpose of this lab was to study the composition of hydrates. Hydrates are ionic compounds that are chemical compositions made of water and salt. A main objective was to remove water from the hydrate by heating‚ and determine the amount of water that was in the hydrate. After doing this‚ one had to predict the empirical formula for hydrated copper sulfate. In doing this lab‚ one was able to see the gradual change in the composition of a hydrate into an anhydrous salt. The lab was carried out with
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Define and describe ionic and covalent bonds. An ionic bond is a type of chemical bond formed through an electrostatic attraction between two oppositely charged ions. A covalent bond is the chemical bond that involves the sharing of pairs of electrons between atoms. A compound is made when two or more atoms form a chemical bond‚ linking them together. The two types of bonds are ionic bonds and covalent bonds. In an ionic bond‚ the atoms are bound together by the attraction between oppositely charged
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