Formula of a Hydrate Lab

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• Essay about Formula of a Hydrate Lab

  ...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 was determined. Salts appear to be dry, yet when heated, surprisingly large quantities of water are driven off, because water is loosely bonded to the hydrate. Procedure 1. Set the necessary lab equipment properly. 2. Weigh dry and clean crucible and its cover on the balance. Record. 3. Measure about 1 to 2 grams of the hydrate and record the weight using the weighing boat. 4. In moderate flame, heat the empty crucible with tilted lid for 3 to 5 minutes. Record what happens during the heating process. After recording, wait for crucible and lid to cool, and weigh, and record. 5. Repeat step 4 until the mass of the hydrate doesn’t change after each heating. If the mass changed 0.55 grams or less, stop heating the hydrate. This means all of the water has been driven off. 6. After recording all...

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• Essay on Formula of a Hydrate Lab

  ...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 white-colored copper sulfate anhydrous. Using the mass of the original sample of copper sulfate pentahydrate subtracted by the new mass of the copper sulfate anhydrous, the mass of water lost is obtained and used to find the empirical formula. The expectation for the empirical formula was CuSO4 * 5H2O. Procedure: 1. Set up ring and Bunsen burner 2. Weigh crucible 3. Weigh crucible and hydrate 4. Crush hydrate 5. Add hydrate to the crucible 6. Weigh crushed hydrate 7. Light Bunsen burner 8. Adjust ring stand and heat the hydrate until it turns white/gray 9. Cool then weigh the crucible Data: Mass of crucible 23.15 grams Mass of Crucible with crushed hydrate 29.62 grams Mass of crushed hydrate 6.47 grams Mass of crucible with crushed hydrate after heating 26.64...

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• Hydrate Lab Essay

  ...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 balance, Bunsen burner and hose, striker, ring stand, small iron ring, clay triangle, crucible and cover EQUIPMENT CHEMICALS Various hydrates Hazard Alert Avoid breathing dust or skin contact with hydrate. Clean up all spills immediately with a wet sponge or foam brush. INTRODUCTION If an opinion is said to not hold water it means that the point of view or statement put forward is illogical, inadequate, not sound or can be shown to be wrong. Hydrates are inorganic salts that hold water. They contain a specific number of strongly bonded water molecules as part of their crystal structure. Such water molecules are called water(s) of hydration, or water(s) of crystallization. The formula of a hydrate consists of the formula of the anhydrous (without water) compound followed by a dot, then the specific number of water...

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• Formula of a Hydrate Essay

  ... 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 driven off, usually by heat. Hydrated salts are characterized by the number of moles of water molecules per mole of salt. Sample Calculations: Mass of hydrate= 35.232g - 32.005g =3.227g Mass of anhydrous salt= 33.583g - 32.005g =1.581g Mass of water liberated= 35.232g – 33.586g =1.646g Mass of h2O in hydrate= 1.646g/3.227g X 100 = 51% % anhydrous salt in hydrate= 1.581g/3.227g X 100 = 49% Moles of anhydrous salt in 100g hydrate= 49% X 1mol/120.38= 0.407moles Moles of water in 100g of hydrate= 51% X 1mol/18.02= 2.83moles Moles of water per mole of anhydrous salt= 2.83moles/0.407moles= 6.95moles Average Moles of water per mole of anhydrous salt= 6.95mol / 6.91mol= 6.93mol Results: According to our results anhydrous salt magnesium has a formula hydrate of MgSO4 + 7H2O. The...

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• Hydrate Lab Report for Chemistry Lab Essay

  ...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. This ratio was then used to write the new and balanced equation of the dehydration process. The sample was then rehydrated to the original state and the percent of the hydrate recovered was calculated by using the mass of the rehydrated sample by the mass of the original hydrate and then multiplied by 100%. Data Presentation & Analysis Table 1: The data was collected from the lab experiment. Sample calculations are shown. Mass of beaker with sample 30.765g Mass of empty beaker 30.263g Mass of sample .502g Mass of beaker with sample after 1st heat 30.661g Mass of beaker with sample after 2nd heat 30.657g Heating mass difference .004g Mass of anhydrate .394g Mass of H2O .108g Molar mass of CuCl2 135.0g/mol Molar mass of H2O 18.0g/mol Moles of anhydrous sample 2.92x10-3 moles CuCl2 Moles of H2O released 6.00x10-3 moles of H2O Mass % of H2O 21.5% of H2O % Absolute...

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• Hydrate Lab Essay

  ...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, 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 being chemically bonded to the water molecules. This makes it anhydrous, because the hydrate can become an ionic solid and water due to the lack of chemical bonding. The purpose of this lab is to identify the number of moles of water in an ionic hydrate by heating the ionic hydrate to remove water. The process is to record the tare weight of a clean crucible. According to WiseGEEK, tare weight is the weight of an object (such as a jar, a cup, or, in this case, a crucible) when it is empty. You will add 2g of the copper sulfate hydrate crystals into the crucible, and then you weigh the crucible with the copper sulfate hydrate crystals and record the data. You...

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• Hydrate Lab Essay

  ...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 2d. The molar mass of 5H2O is 90.10 grams/mol 2e. The molar mass of the entire compound is 159.61 + 90.10 = 249.71 grams/mol 2f. The percent of water in the compound is mass of water/mass of compound = 36% Mass of crucible before heating | 40.00 grams | Mass of crucible + hydrate before heating | 41.38 grams | Mass of crucible + anhydrate after 1st heating | 41.08 grams | Mass of hydrate | 1.38 grams | Mass of anhydrate | 1.08 grams | Mass of water | .2 grams | Formula of anhydrous salt | Cu(SO4) – Copper Sulfate | Data Table Calculations 1. Mass of hydrate = 1.38 grams. Mass of anhydrous = 1.08 grams. Mass of water = .2 grams. 2. Ratio of anhydrous mass to hydrate mass is 5.4. 3. Moles of anhydrous salt: 1. 4. Moles of water are five moles. 5. Moles of water per mole of anhydrous salt was about 5.4/1 ratio but really is 5/1 6. Empirical...

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• Hydrate Lab Essay

  ...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 molecules bound to each formula unit. These salts are able to release water to become anhydrous, or the anhydrous compound can absorb water molecules into their ionic structures to become hydrated. (Crampton, 2014). The hydrated complex can easily become an anhydrous salt if the compound is heated causing the water to evaporate out of the compound. The mass of the water in the hydrate can be determined by subtracting the anhydrous complex from the hydrated complex. It is hypothesized that the chemical formula of a hydrate can be determined using the mass of the anhydrous salt compound and the mass of the evaporated water to identify the fixed mole ratio in which they exist. In this lab the chemical formula of hydrated magnesium sulphate is expressed as follows: MgSO4 xH2O APPENDIX Table 1: Mass calculations of hydrated and...

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