Half-fill the dish with about 3.0 g of Epsom salts (magnesium sulfate hydrate). upon heating, the empirical formula of the hydrate can be determined. The formula for Epsom salts can be written as MgSO4•xH2O, where x indicates the number of moles of water per mole of magnesium sulfate. An example of a hydrate is magnesium sulfate. The formula mass of a hydrate always includes the mass of the water molecules that are an integral part of the formula. An empirical formula of a chemical compound is the ratio of atoms in simplest whole-number terms of each present element in the compound. An anhydrate is the substance that remains after the water from a hydrate has been removed through heating.. The process of removing water from a hydrate, usually through applied heat. Ratios vary in different hydrates but are specific for any given hydrate. Formula for Hydrate (salt) MgSO4 _____H2O. The formula mass of CuSO4• 5H2O is therefore 159.61 g/mol + 90.08 g/mol = 249.69 g/mol. See the answer . Question: Using the formula you obtained in 11, write a balanced equation for the dehydration of the MgSO4 hydrate you used in the experiment. Relevance. if 9.86g of epsom salt dissolved in 50ml of water reacts with excess BaCL2(aq) 9.30 g of the insoluble BaSO4 (s) is obtained after drying. For example, Glucose is C 6 H 12 O 6; it’s empirical formula is CH 2 O. Gently heat the dish and contents with the cover ajar for two minutes. Hydrates are compounds that contain water with a definite mass in the form of #H_2O# in their molecular formula. .056 = 7 .0083 .0083 =1 .0083 Formula: MgSO4 x 7H2O Conclusion: In the Formula of a Hydrate Lab, our hypothesis was correct. I need to find the X in CuSO4 multiplied (x) XH20 ( how many waters are there. They are known as “hydrated salts”, or simply, hydrates. Find the chemical formula and the name of the hydrate. In this investigation you will be given an unknown hydrate and asked to determine the percent of water in the compound. Percentage by mass of water of crystallisation in hydrated MgSO4.xH2O was: 3.0652g5.9804×100=51.25% The number of moles of water in the hydrated MgSO4.xH2O sample was: 3.0652g18g/mol=0.1703 moles Formula mass of anhydrous MgSO4 was Mg + S + O ×4, i.e. The salt may be magnesium sulfate (MgSO 4), sodium phosphate (Na 3 PO 4), calcium chloride (CaCl 2), or sodium carbonate (Na 2 CO 3). Keep in mind you are to complete two trials with the unknown magnesium sulfate hydrate. Objective/Goals: You will use techniques of quantitative analysis to determine the percent by mass of water in a solid and the formula for water of hydration (or hydrate). 7. Wiki User Answered . What is the formula of the hydrate? Determining a Mole Ratio: Hydrate Analysis Lab . 6 H2O iron (III) chloride hexahydrate. Assume the quantitative yield and determine the formula of the epsom salt MgSO4 8 xH20----->MgSO4 (aq) MgSO4(aq)+BaCl2(aq)------>MgCL2(aq)+BaS... determine the formula fo the MgSO4 hydrate… Magnesium sulfate hydrate: MgSO4.7H2O. MgSO4 x 1mol = .0083 mol MgSO4 120.4g. The formulas for these substances are MgSO 4 *7H 2 O and Na 2 CO 3 *10H 2 O. Magnesium sulfate heptahydrate. Determining the empirical formula of a hydrate Background Different elements can form chemical bonds to create compounds. Magnesium can be found in Group 2, also known as the Alkaline Earth metals in the periodic table. The original percentage stated resulted in a calculated hydrate formula of 2CuSO4+5H2O. View Copy of U5L14 Formula of a Hydrate Lab.docx from ENG 1B 101 at Texas Connections Academy @ Houston. Equipment/Materials: Crucible (without lid), clay triangle or wire triangle, iron ring, ring stand, lab burner (Bunsen or Fisher), crucible tongs, electronic balance, heat pad, approx. For example, sodium and chlorine combine to form sodium chloride, NaCl. Pre-lab questions: 1. Question: Epsom Salts Is A Hydrate Of Magnesium Sulfate, MgSO4 . Procedure: 1. Now it's time for data analysis. The symbol for Magnesium sulfate is MgSO4. QUESTIONS Calculations Table Mass of anhydrous magnesium sulfate Desiccants the percentage of the hydrate was 35%. As for sulfate, it is a polyatomic ion. Wet Lab Experiments ... {MgSO4*7H2O}\): magnesium sulfate heptahydrate). Determine the mass of the hydrate by subtracting entry #4 from entry #1 in the Data Table. A sample of copper (Il) sulfate hydrate has a mass of 3.97 g. After heating, the CuS04 that remains has a mass of 2.54 g. Determine the con-ect formula and name of the hydrate. The actual hydrate formula for the copper (II) sulfate compound was CuSO4+5H2O. MFCD00149785. Virtual Lab: Hydrates. The water is chemically combined with the salt in a definite ratio. Determine the formula of the hydrate Samples 1, 3, and 5 are hydrates of magnesium sulfate, MgSO 4. xH 2 O Samples 2 and 4 are hydrates of zinc sulfate, ZnSO 4. xH 2 O To determine the formula, you must determine the following # mols H 2 O # mols H 2 O x = _____; or y = _____ # mols MgSO 4 # mols ZnSO 4. 6. Allow the crucible and cover to cool on a piece of wire gauze. For example: The formula mass of CuSO4 is 159.61 g/mol and the total molar mass of 5 water molecules is 90.08 g/mol. However, not all compounds form in a 1:1 ratio of their constituent elements. Use the following data to find the formula of the hydrate BeO . A 5.018 gram sample of a certain hydrate of magnesium sulfate, MgSO 4 •xH 2 O, is heated until all the water is driven off. Rule 3. Organizing Conclusions Using your answers to Calculations items 2, 4, and 5, determine the mole ratio of MgS04 to H20 to the nearest whole number D, I L4AU,qd, 7. 3. They can also be … (Mg) stands for magnesium and (SO4) stands for sulfate. 6. Background: Hydrates are ionic compounds (salts) that have a definite amount of water (water of hydration) as part of their structure. Epsom salts is a hydrate of magnesium sulfate, MgSO 4. Top Answer. Examples are: magnesium sulfate heptahydrate (epsom salts) and sodium carbonate decahydrate (washing soda). 10034-99-8. magnesium sulphate heptahydrate. 24 + 32 + 16 ×4 = 120. The purpose of this experiment is to determine the empirical formula of a hydrate. What is the mass of the anhydrous salt? The mass of the sample after complete dehydration was 2.41 g. What is the mass of the water lost during heating? Find the formula and name of the hydrate. See Answer. Greek prefixes are attached to the word "hydrate" to indicate the number of water molecules per formula unit for the compound (e.g., Ba(OH) 2 •8H 2 O; 8 water molecules = "octahydrate"). The resulting anhydrous compound weighs 2.449 grams. When we heated the compounds, we got a formula of CuSO4 x 6H2O for the copper sulfate, and MgSO4 x 7H2O for the … 2. What is the formula of the hydrate? MgSO₄•7H₂O. 1 decade ago. You will actually be determining the mole ratios of the products through mass analysis. In addition, the mass percent of water lost by the hydrate can be calculated. 2013-03-23 19:06:35. In contrast, an anhydrate does not contain water, and has had all of its water removed. What is the formula for copper (II) sulfate? 2 H2O. Solution: 1) Determine mass of water driven off: 4.31 − 3.22 = 1.09 g of water. Favorite Answer. 2) Determine moles of Na 2 CO 3 and water: Magnesium has an atomic mass of 24.305, and an atomic number of 12. A 5.018 gram sample of a certain hydrate of magnesium sulfate,MgSO4•xH2O, is heated until all the water is driven off. 5 H2O copper (II) sulfate pentahydrate. What is the formula of the hydrate? Measure and record the exact mass in Data Table entry #1. 12H 2 O . A hydrate is a compound that is chemically combined with water molecules. 4 Answers. These compounds often come in the form of a crystal which can then be heated in order to remove the water in the form of steam. Magnesium sulfate (1:1) heptahydrate Therefore the formula is MgSO 4 . This problem has been solved! Epsom Salt, MgSO4 * xH20 is a water soluble MgSO4 hydrate. Mass of hydrate = 8.61 grams. 4) Write the formulas for the following compounds: a) barium chloride dihydrate BaCl2 . When we heated the hydrated salts, the hydrates evaporated and we were able to find the formula of the salts. We want to determine the formula for a hydrate of iron (III) chloride, FeCl 3 nH 2 O. ?H 2 O. Name: _ Chemistry A - U5L14 Formula of a Hydrate Lab Read and complete the lab… Shows how to determine the number of moles of water in a hydrates compound. The mass of the hysrate used was 2.00g. Properties of Hydrates. Hydrates are inorganic salts which contain a specific number of water molecules loosly attached. Here we are in the lab after dehydrating some iron (III) chloride salts. The mass of water lost was 0.70g. Copper sulfate hydrate: CuSO4.5H2O. After heating, the mass of the anhydrous compound is found to be 3.22 g. Determine the formula of the hydrate and then write out the name of the hydrate. The formula of a hydrate is represented in a special manner. Epsom salts is a hydrated ionic compound with the following formula: (MgSO4)•(xH2O) A sample of Epsom salts with a mass of 4.93 g was heated to drive off the water of hydration. The class average for the percentage of water in the hydrated copper (II) sulfate compound was 28.79%. Answer Save. Mass of water = 3.60 grams. The … In this part of the lab you will repeat the same procedure performed for the salt of known formula with a salt for which you do not know the hydrate formula. Lab 2: Determine the Percentage of Water in a Hydrate: The goal of this experiment is to learn how to properly calculate the ratio of salt to water, in a hydrated salt, and to calculate the percentage of water (by mass) within a hydrated salt. Record this result in Data Table entry #5. Lv 7. b) CuSO4 . Epsom salts, a strong laxative used in veterinary medicine, is a hydrate, which means that a certain number of water molecules are included in the solid structure. The mass of the sample after complete dehydration was 2.41 g. -Find the number of waters of hydration (x) in Epsom salts. Its formula is MgSO 4 7H 2O, indicating that seven moles of water are combined with one mole of magnesium sulfate in the crystalline form. A certain hydrate is found to have the following percent composition by mass: 20.3% Cu, 8.95% Si, 36.3% F and 34.5% H2O. Example #2: A hydrate of Na 2 CO 3 has a mass of 4.31 g before heating. When 5.00 g of FeC13 xH20 are heated, 2.00 g of H20 are driven off. Heat both the crucible and cover for about 2-3 minutes to ensure that any water that is adsorbed to the walls of the crucible or cover is driven off. We did a lab today in chem class and I need help solvng a problem. PROCEDURE. 3) Name the following compounds: a) FeCl3. Answer … To determine the number of moles of anhydrous salt and of H 2 O: 1 mol MgSO 4 # mols … skipper. Add a Comment. What is the mass of copper (II) sulfate? b) magnesium sulfate heptahydrate 0 0 1 0 0 0 0. Digication ePortfolio :: General Chemistry (Alexander Antonopoulos) by Alexander P. Antonopoulos at Salve Regina University. Anhydrous sodium sulfate can absorb water vapor and be converted to the decahydrate. Epsom salts is a hydrated ionic compound with the following formula: MgSO4⋅xH2O A sample of Epsom salts with a mass of 4.93 g was heated to drive off the water of hydration. Lab - Determining the Chemical Formula of a Hydrate Some ionic compounds form crystalline structures that trap water molecules within the crystalline framework. Le Chatelier’s principle predicts that an addition of heat to an endothermic reaction (heat is a “reactant”) will shift the reaction to the right (product side). Wash and dry a porcelain crucible and lid. Their formulas are written in two parts – the anhydrous salt, followed by some number of water molecules called the water of hydration. The resulting anhydrous compound weighs 2.449 grams. Organizing Conclusions Use your answer to Calculations item 6 to write the formula for the magnesium sulfate hydrate. In the chemical formula NaCl, there is a 1:1 ratio of sodium ions:chloride ions. It is generally possible to remove the water of hydration by heating the hydrate.