Determining the Chemical Formula of a Hydrate Chemistry 11 3/5/2013 Purpose: To determine the percent by mass of water in a hydrate of copper (II) sulfate hydrate. Hypothesis: I hypothesize that when the solution is heated the hydrate will convert to an anhydrous ionic compound. Then the percentage composition will be determined by weighing the mass of the white crystals. Materials: 400ml beaker‚ hot plate‚ tongs‚ scoopula‚ electronic balance‚ glass rod‚ hot pad‚ and 4g of hydrated
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Arumugam Gold 3 Calculating the Formula of a Hydrate through Experimentation Purpose The purpose of this lab is to determine the formula of a given hydrate through collecting and calculating experimental data. Data Mass (g) of crucible 29.9g Mass (g) of crucible with hydrate 32.35g Mass (g) of crucible and anhydrous salt 31.39g Questions and Calculations 1. What was the mass of the original hydrate? 2.45g of hydrate Calculations: Mass of crucible with hydrate (32.35g) - Mass of crucible (29
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Title: Formula of a Hydrate. Objective: Determining the percentage of water and the chemical formula of a hydrate. Background: Water has a polar structure and it has positively and negatively charged parts within each molecule. This gives it a strong attraction toward ions. The ions in some salts attract and form strong bonds with water molecules. These salts‚ when they have absorbed water‚ are called hydrates. Anhydrous salts are salts that can form hydrates but which have had all the water
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[ print page ]03.09 Molar Mass of Compounds: Determining the Formula of a Hydrate—Text Version When hydrates are heated‚ the water of hydration evaporates and is released as vapor. The remaining solid is known as the anhydrous salt‚ which is the compound same compound without the water molecules trapped inside. Title:The title of the lab should be at the top of the lab report. Purpose: In one or two complete sentences‚ state the purpose of this laboratory investigation. Materials: List
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electrons. Ionic solids are salts (such as NaCl) that are held together by a strong force of attraction between ions of opposite charge. Molecules are the smallest physical units of an element or a (chemical) compound. Ionic solids are also known as salts because salts are ionic compounds 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
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Formula of a Hydrate Lab Wednesday October 29‚ 2014 Chemistry Honors Purpose This lab was done to determine the percentage of water in a hydrate‚ which was CuSO4 ?H20. Not only the percentage of water can be found‚ the moles of water can be found per one mole of anhydrous salt. An anhydrous salt is a hydrate that lost its water. Using various lab equipment such as burners‚ crucible‚ and balance‚ and techniques such as the mass-to-mole ratio and mass to percentage‚ the percentage of water in a hydrate
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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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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
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Determining Percent of Water Crystallization and the Chemical Formula of a Hydrate Aim: To determine the percent water of crystallization and the chemical formula of a hydrate Materials * 400 ML beaker * Glass rod * 3 to 5 grams of hydrated copper (II) sulfate CuSO4 (crushed) * Bunsen burner * Spatula * Heating pad * Clamp and stand * Electronic balance Procedures Refer to Lab sheet Observations 1. The powder seems to be very bright and shiny before any heating 2.
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Determining the Number of Water Molecules in a Hydrate Results Mass of empty beaker 55.11 g Mass of beaker with hydrated copper (II) sulfate 58.13 g Mass of hydrated copper (II) sulfate 3.02 g Mass of beaker with dehydrated copper (II) sulfate (last weighing) 57.22 g Mass of dehydrated copper (II) sulfate 2.18 g Mass of dehydrated copper (II) sulfate (2nd weighing) 2.11 g Questions 1. Calculate the value of “n”. Show your work. Include an example of ALL calculations involving
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