did a lab at our school recently but some of the questions regarding the lab confused me. These compounds have water molecules coordinated in their chemical structures. Boc Sciences is the world's leading provider for special chemicals. in which no [H 2 O] term appears. Anhydrate: The compound after the water molecule has been removed. Now I happen to have exactly 5. Naming ionic compounds worksheet one give the name of the following ionic compounds. Answers – Naming Chemical Compounds. asked by A. Determination Of Empirical Formula Of Copper Oxide Lab. Hypothesis: Hydrates are ionic compounds that have a definite amount of water as part of their structure. 1 A student is given a cobalt (II) chloride hydrate. Cupric sulfate appears as a white or off-white solid. Greek prefixes are attached to the word "hydrate" to indicate the number of water molecules per formula unit for the compound (e. The chemical name for this compound is magnesium sulfate heptahydrate. Three different hydrated salts were studied: copper sulfate (CuSO 4), manganese sulfate (MnSO 4), and nickel sulfate (NiSO 4. copper(II) sulfate pentahydrate (CHEBI:31440) Services. Suppose that you heated a sample of hydrated ionic compound in a test tube. The data obtained from the lab is here: Determining the Chemical Formula of a Hydrate Purpose Find the molecular formula of the hydrate of Copper (II) Sulfate, CuSO4 x H20. Hydrates are ionic substances that have water molecules included in their crystal structure (Text Chapter 16). 2 x 10^22 H2O molecules: 0. Procedure: First, I added nitric acid with copper in a beaker, which turned into a copper nitrate, a blue-green solution. (b) Work out the mass of 1 mole of copper sulfate. One of their spies had managed to. mass of the crucible with white copper sulfate (anhydrous) after heating. Molar Mass of H 2O i. Magnesium sulfate is also prepared by sulfation of magnesium oxide. When it is added to water it dissociates into Cu. The deep blue crystals that you often get in a bottle are the pentahydrate CuSO4. Saifuddin¹, Tasnima Jannat¹ and S. The formula for the hydrated compound Cobalt (II) chloride hexahydrate is: CoCl 2 ∙ 6H 2 O. 58 g of H 2 O. The compound's formula is CuSO4. Serves as a weak oxidizing agent. For example, the solubility of sodium chloride in water is 355 g/L at 0Â°C, increasing only about 10% to 390 g/L at 100 Â°C. Hydrates are ionic substances that have water molecules included in their crystal structure (Text Chapter 16). b Determine the molecular formula of the hydrocarbon. Determine the mass of the covered crucible and crystals to the nearest 0. The metallic copper produced will be weighed. Observations: Mass of copper (II) sulfate hydrate = 0. To determine the empirical formula of a hydrate. Also, the number in front of the water molecule must be distributed and multiplied by the subscript of both the hydrogen and the oxygen in the water molecule. mH 2 O in the hydrate equals m Ca(NO 3) 2 4H 2 O－m Ca(NO 3) 2. Heat the blue copper sulfate hydrate until all the water has been removed- the anhydrous copper sulfate will be white or gray in color. Popular corded compound microscopes and cordless microscopes for elementary to advanced use. When the copper sulfate is heated up, it quickly turns to a pure white color that has no hint of blue in it. its not only 100 degrees celsius, tab water can dissolve copper sulfate, any water can dissolve copper sulfate, 10 ml of water can dissolve about 2. Copper (II) Sulfate Pentahydrate Lab - Composition of a. To determine the percent of copper and the formula weight of a copper compound. So, for every mole of calcium sulfate, there are 3 moles of water. Hydrate Chemical Formula Fomula Mass Mass % Water Nickel(II)chloride hexahydrate Cobalt(II)chloride hexahydrate Copper(II)sulfate pentahydrate 2. Copper/Iron Stoichiometry Grace Timler AB1 October 3, 2017 Abstract The techniques used in this lab are quantitative transfer and vacuum filtration with the reaction of 8. Determine the formula of one of the hydrates below. , it will precipitate out of the solution. 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. [Filename: Lab 3_Analysis of Hydrated Sulfate Salts_F2009. A hydrate is a compound that is chemically combined with water molecules. Determine the percent by mass of water in your sample of hydrated copper (II) sulfate. Water also comes out of the copper sulfate and is able to function as any other type of water would typically function. The data can be used, along with the balanced chemical equations, to determine Stoichiometry Using Copper Lab 31 Answer Key The forth one was a double replacement reaction in. [1 mark] Mass of anhydrous copper sulfate = g [Turn over]. Applying conclusions Calculate the percent water in a mole of copper(II)sulfate pentahydrate using the formula. Copper was first discovered by Early Man prior to 9000 BC. xH 2 O To determine the formula, you must determine the following. Learn vocabulary, terms, and more with flashcards, games, and other study tools. Materials: Copper sulfate hydrate—CuS04 - H20. Get an answer for 'Determining empirical formula for hydrated cobalt chloride compound. The mass of water lost was 0. 25 (or 64% : 36%, doesn't matter which mass ratio you use) To convert from mass ratio to mole ratio, you divide by the masses molecular/formula mass M r of each 'species'. 19 g Mass of hydrate copper sulfate = 3. Los Angeles City College Chemistry 60 EXPERIMENT 7: HYDRATES. 14 Limestone is impure calcium carbonate. Boc Sciences is the world's leading provider for special chemicals. Then you will compare your results against given information to determine the molecular formula. Magnesium sulfate is available as brilliant colourless crystals, granular crystalline powder or. Determination of hydration number: show how you obtained your “answer” for the formula of the unknown hydrate of copper (II) sulfate. Procedures involving meaurements of masses to determine quantitative information is termed. • Some scrap copper goes to landfill sites. It's often used in agriculture, especially as a pesticide, soil additive and feed additive. 001 grams of copper (II) sulfate, CuSO4, and 2. Since this compound is hydrated, I will assume that it is added to 1 mole of H2O so it will look like this: CuSO4 * H2O. What is the percent water in copper (II) sulfate pentahydrate, CuSO 4 • 5 H 2 O? 1. Once you have your mole values, use your knowledge of finding empirical formulas to determine the formula of the hydrated salt (in our case hydrated copper(II) sulfate). Hydrated copper sulfate 4. For example, iron + copper(II) sulfate iron sulfate + copper. 03 ml of copper sulvate. Nickel(II) chloride produces a green solution in water. Virtual Lab Hydrate. Some compounds, such as the copper sulfate we use in this lab, are much more soluble in hot water than in cold. XH2O and asked to determine the % Cu, % SO4, and the number of water molecules in the hydrated salt using a cation-exchange resin coupled with gravimetric analysis. Determine the number of moles of the anhydrous Salt: _____ (Hint: First determine GFM then use mole calculation in Table T of reference table) 5. The resource is printable and contains ideas for expanding upon the lesson. % H 2O in hydrate g. 0 ml distilled water, and then add the water to the 250 ml beaker with the copper (II) sulfate. The water is chemically combined with the salt in a definite ratio. To determine both the percent of water present in a hydrated copper (II) sulfate (CuSO4 •  n  H2O) and “ n ”, the number of                 moles of water molecules present per mole of CuSO4. Compound Microscopes. Example #2: A hydrate of Na 2 CO 3 has a mass of 4. for a Salt of Limited Solubility. Calculate the molar mass for your anhydride from the formula provided. Why is it important to scour the magnesium strip with steel wool at the start of the experiment? 2. How can we use the test tube and the Copper (II) Sulfate to determine the mass of the hydrate?”. For example, Glucose is C 6 H 12 O 6; it’s empirical formula is CH 2 O. The next day you will recombine water with the anhydrous white powder and measure the heat transferred by this reaction to water in calorimeter. pdf] - Read File Online - Report Abuse. Also, the chemical formula for. This is a list of the solubility rules for ionic solids in water. 5H2O) and the aquous solution (Cu2+(aq) ions) are royal blue. grams of 40 degree water. Major uses of Copper Sulfate in Agriculture:-Preparation of Bordeaux and Burgundy mixtures for use as fungicides -Manufacture of other copper fungicides such as copper-lime dust, tribasic copper sulphate, copper carbonate and cuprous oxide -Manufacture of insecticides such as copper arsenite and Paris green -Control of fungus diseases. Is this a true hydrate? Explain. Prediction When the solution is heated the hydrate will convert to an anhydrous ionic compound. Materials: 1 Hot Plate 1 Wire Mesh 1 Small beaker 1 Glass Stirring Rod 1 Beaker Tong 1 Spatula Copper II Sulfate Hydrate (approx. XH2O) of Copper II Sulfate Hydrate and once heated I now have 3. 42 g of (NH 4) 3 PO 4 26. General Chemistry I (SCC 201) Academic year. The mass of water lost was 0. 5H2O), is a common salt of copper. Determine the mass of copper(II) sulfate pentahydrate added to the test tube. How do we determine the amount of chlorine in the compound? The mineral bonattite is known to be a copper sulfate hydrate. These types of compounds are known as hydrates. I want to determine the chemical formula for a hydrate. Copper Sulfate's Water of Hydration Lab: Enrichment Activity Purpose - To observe the effect of removing the "water of hydration" from hydrated copper(II) sulfate. Combine solutions and identify the reactions that form precipitates. Determine the formula of one of the hydrates below. Therefore, the percentage of of water in the hydrated copper (II) sulfate compound was determined to be 22. Blue copper sulfate solution (0. Q: A compound is isolated from the rind of lemons that is found to be 88. We call such solids hydrates, and we call the bound water the water of hydration. Copper sulfate, bluestone and blue vitriol are all 35 common names for cupric sulfate pentahydrate, CuSO 4∙5H 2 O, which is the best known and the most. com Hydrate Lab. It is toxic by ingestion and a strong irritant so care should be taken in handling. Some compounds form more than one hydrate, each. A hydrate like cupric sulfate is any compound containing water. Hypothesis: Hydrates are ionic compounds that have a definite amount of water as part of their structure. XH2O and asked to determine the % Cu, % SO4, and the number of water molecules in the hydrated salt using a cation-exchange resin coupled with gravimetric analysis. its not only 100 degrees celsius, tab water can dissolve copper sulfate, any water can dissolve copper sulfate, 10 ml of water can dissolve about 2. PROCEDURE Obtain from the instructor a hydrated salt chosen from copper sulfate, calcium sulfate, and magnesium sulfate. Will the mass of water be higher or lower if the hydrate heated too quickly? If i did not completely converted the hydrate to the anhydrous compound this would affect the calculated percent by mass of water in the compound bec. An anhydrous compound is one which has no water in its structure. Ex: HgNO 3 H2O is a hydrate while the HgNO 3 is an anhydrous salt. cedure using one of the listed compounds and verify its hydrate formula. mH 2 O in the hydrate equals m Ca(NO 3) 2 4H 2 O－m Ca(NO 3) 2. Introduction – Hydrated Ionic Compounds, commonly called, “hydrates”. Dissolve the compound in 15 mL of distilled water in a 125 mL Erlenmeyer flask. New - Lab Supplies & Equipment. mass = volume x density 2. Lab #6 Chemical Transformations of Copper Introduction: Copper was one of the first metals to be isolated, due to the ease of separating it from its ores. Then using the same data we will calculate the water of hydration through determining the mole ratio of the decomposition reaction. How much energy does it take to go from alpha to beta?. You will need to answer these and add them to your lab report. Just like the dozen and the gross, it is a name that stands for a number. In this experiment, the. An analysis of a hydrate is found to contain 63. The molarity of (SO4)2. Calculate the molar mass of the compound, MM. When a small crystal remains un dissolved in the solution the solution is saturated. you should dissolve the copper sulfate in plenty of water, then flush down a sink with a lot of water slowly, or you could find someone else who would want it. ) Equipment Evaporating dish, iron ring, tongs, 2-wire gauze pad, spatula, Bunsen burner, striker, ring stand, goggles and apron. Three different hydrated salts were studied: copper sulfate (CuSO 4), manganese sulfate (MnSO 4), and nickel sulfate (NiSO 4. pdf] - Read File Online - Report Abuse. In order to determine this, we weighed the mass of Copper (II) Sulfate, boiled it for about 10 minutes until it became an anhydrous salt, then found the weight of its anhydrous salt and the water, by. on November 24, 2012; chem. There is a fairly clear-cut case in copper (II) chemistry. Since it is an ionic compound, the whole crystal is one gigantic macromolecule, containing trillions of units. 94g of hydrated copper(II) sulfate crystals were heated, 2. You will not need more than 2. Obtain about 3 g of copper(II) sulfate pentahydrate, CuSO4·5H2O using an analytical balance. In its elemental form, copper has a red-orange metallic luster appearance. calculate the enthalpy changes. Determine the mass of solution by multiplying the volume of the solution by the density of the solution. If the cupric sulfate solution is warm,. This information is used to find x in the formula: CuSO 4. The formula unit for the salt appears first, followed by the water formula. 33 Copper sulfate is an inorganic compound that combines sulfur with copper. Answers the purpose of the lab. (i) Explain why zinc metal reacts with copper(II) sulfate. 0062653265550854. I need to find the X in CuSO4 multiplied (x) XH20 ( how many waters are there. The deep blue crystals that you often get in a bottle are the pentahydrate CuSO4. The percent of water in the original hydrate can easily be calculated: %H2O = X 100. Use Figures 15. Introduction Vocabulary: Salt, anhydrous salt, hydrated salt, crystal A hydrate is a compound that contains water in its crystal structure. Your task is to determine the chemical formula of an unknown copper chloride hydrate by experiment. Should the Bunsen burner flame be kept heating one area of the crucible?. Determination Of Water Crystalization Essay I. The difference in mass between the total copper chloride hydrate and the sum of the reduced copper metal and water molecules corresponds to the mass of chloride in the sample. Copy this reaction: CuSO 4. 6% copper(II) sulfate This is how I find the number of hydrates in the solution: CuSO4. g the dish an us salt. Hint: step 1- Use the number of moles of water and copper sulfate calculated above. Place the crucible with the copper sulfate hydrate on the triangle. When the copper sulfate is heated up, it quickly turns to a pure white color that has no hint of blue in it. xH 2 O Determine "x", where x is a whole number. Calculate the percentage of water of hydration in calcium chloride dehydrate, CaCl2 ( 2H2O. Gains water readily. The mass of the hysrate used was 2. Its formula is CuSO 4 5H 2 O. It is toxic by ingestion and a strong irritant so care should be taken in handling. Ratios vary in different hydrates but are specific for any given hydrate. 9% Copper (II) Sulfate (CuSO 4); and 36. Experimental Question: How can we experimentally determine the formula of an unknown hydrate, A? Testable Prediction: Our unknown hydrate may be a hydrate of copper(II) sulfate, magnesium sulfate, iron(III) chloride, or iron(III) nitrate. [Filename: Lab 3_Analysis of Hydrated Sulfate Salts_F2009. Background: Many crystalline compounds contain definite amounts of water that are trapped within their solid-crystalline structures. 1 A student is given a cobalt (II) chloride hydrate. Introduction - Hydrated Ionic Compounds, commonly called, "hydrates". Labreport#4 - Determining the Empirical Formula of a Hydrate C. To the warm water add small quantities of copper(II)sulfate pent hydrate crystals with constant stirring using a glass rod until all of the copper sulfate. Some compounds, such as the copper sulfate we use in this lab, are much more soluble in hot water than in cold. When it is added to water it dissociates into Cu. Rewrite in your own words. If the reaction is carried out with high concentrations of copper(II) and ammonia present, the sulfate salt of the complex can be precipitated by the addition of ethanol to an aqueous solution of copper sulfate and ammonia. Find the chemical formula and the name of the hydrate. How many grams of the hydrated form should we weigh out? Show your work. Should the Bunsen burner flame be kept heating one area of the crucible?. Your answer must also explain why the mass of copper sulfate hydrate decreases as it is heated. copper sulfate monohydrate (Molar Mass = ) copper sulfate trihydrate (Molar Mass = ) copper sulfate pentahydrate Molar Mass = ) Also calculate the molar mass of each hydrate. Start the lab in your notebook by writing the title and questions listed below. Also, the chemical formula for hydrated copper(II) sulfate (or copper sulfate pentahydrate) is CuSO4. _____ _____ _____ 5. using these data, calculate the number of water molecules that is present in the formula of this hydrate (obviously before heating). 55 2Cl = 2(35. After heating, the CuS04 that remains has a mass of 2. Skip to page content; Skip to site menu on this page. The stoichiometry of hydrated copper sulfate. yH2O, ZnSO4. A very common hydrate encountered in the general chemistry laboratory is copper (II) sulfate pentahydrate, CuSO 4 ·5H 2 O. It's often used in agriculture, especially as a pesticide, soil additive and feed additive. The reducing sugars in the carbohydrate solution react with the copper sulfate present in the flask. Copper sulfate pentahydrate is a blue compound that forms striking blue crystals and dissolves readily in water. Hydrated copper sulfate 4. Observe the hydrated compound with a hand lens. Water has a polar structure; it has positively and negatively charged parts within each molecule. Determination Of Water Crystalization Essay I. 375 x 10^-22 g: A salt crystal has a mass of 0. The anhydrous copper (II) sulfate (cupric sulfate), CuSO 4, is a greenish white amorphous powder. Initially, before the reaction, the copper was in the copper compound, copper (II) oxide. 002moles The molar mass of anhydrous copper sulfate is 159. Lab: Analysis Of a Hydrated Compound. Name of compound Sodium carbonate Sodium sulfate Sodium aluminum sulfate Potassium chloride Magnesium chloride Copper sulfate EXPERIMENT Al Water of crystalliza- tion? Description of anhydrous compound ChemFile. Moles of CuSO 4 j. Moles of H 2O *same answer 1. Aim: To determine the formula of the hydrate of copper (II) sulfate. ) Equipment Evaporating dish, iron ring, tongs, 2-wire gauze pad, spatula, Bunsen burner, striker, ring stand, goggles and apron. Why must the heated crucible be cooled to near room temperature before weighing? 3. The occurrence of the reaction will be obvious since the blue cupric sulfate solution turns green due to the iron going into solution. A total of 228 liters of liquid chemicals composed of xylene chemicals, hydrochloric acid, chloroform, pytridine, benzaldehyde and ethanol worth PP204,082. Calculate the following for the solution: a. Our group had done 3 data sets for the same experiment process, and had recorded 3 groups of data. For example… A 15. In this experiment, a known mass of hydrated copper (II) sulfate is heated to remove the water of crystallisation. The lost mass is water, and the remaining mass is the anhydride. Determine the percent by mass of water in your sample of hydrated copper (II) sulfate. In part A of the lab, we will synthesis the coordination compound tetraamminecopper (II) sulfate monohydrate [Cu(NH 3) 4]SO 4•H 2O. Determine the mass of solution by multiplying the volume of the solution by the density of the solution. The atomic mass of Cu can be found on the. What happens when salt hydrate decomposes when heated? In this experiment you will empirically determine the ratio of water to salt in the hydrates copper sulfate hydrate cuso4 xh2o and magnesium chloride hydrate mgcl2 xh2o the symbol x in the formulas represent the unknown number of water molecules - Lab determination of sulfate content in. The justification for this omission is that water is both the solvent and reactant, but only the tiny portion that acts as a reactant would ordinarly go in the equilibrium expression. Just like the dozen and the gross, it is a name that stands for a number. Stoichiometry Using Copper Lab 31 Answers stoichiometry using copper lab 31 answer key - Bing A reaction between excess copper and a solution of silver nitrate. Hydrate Lab By Maya Parks Partners: none 2/20/15 Abstract: This experiment was performed to determine the chemical formula of the hydrate copper (II) sulfate We even found the percentage of water in the compound. 5H2O) and the aquous solution (Cu2+(aq) ions) are royal. Chemical Reactions - ANSWERS 1. Problem #6: Determine the formula and name for the hydrate: 73. Change to the decimal equivalent. 25 and 3,814,070. (the hydrate is CuSO4(nH2O, what is the value of n?) 2. Labreport#4 - Determining the Empirical Formula of a Hydrate C. the percentage of the hydrate was 35%. Copper(II) Reduction Glucose will react with a basic solution of copper(II) sulfate (called Benedict’s Reagent) to form the insoluble copper(I) oxide, which is red (although it may appear yellow at first). The water is chemically combined with the salt in a definite ratio. Zinc was added to the copper sulfate to produce zinc sulfate and copper. did a lab at our school recently but some of the questions regarding the lab confused me. The % H 2 O can be calculated using: % H 2 O = mass in grams of H 2 O attached to hydrate mass in grams of entire hydrate compound Review 1. Chemistry Lab #4 Page 1 of 2. It has an electronic configuration of [Ar] 4s 1 3d 10, but, perhaps surprisingly, its most common oxidation state is +2. Materials: 1 Hot Plate 1 Wire Mesh 1 Small beaker 1 Glass Stirring Rod 1 Beaker Tong 1 Spatula Copper II Sulfate Hydrate (approx. The stoichiometry of hydrated copper sulfate. Kimberly Graziano & Hyunjae Kim. copper sulfate hydrate determination lab: The Average Atomic Weight listed with each of the elements on the periodic table is a measure of the mass of an average atom of that element in AMU. Copper sulfate is an inorganic compound that combines sulfur with copper. 79 grams of solid chemicals composed of caustic soda/sodium hydroxide, palladium, iodine, calcium chloride, red phosphorous, sodium acetate, barium sulfate, sodium sulfate, copper (II) sulfate pentahydrate and caffeine worth. [Filename: Lab 3_Analysis of Hydrated Sulfate Salts_F2009. 6 mg is dissolved in 1. In order to determine this information we heated the salt to get rid of the water. new compound having altogether different properties and applications. Explain your prediction. A hydrate is a crystalline compound that contains a specific number of water molecules attached to an ionic formula unit. Add about 20 drops of 0. How many water molecules are there for each unit of copper(II) sulfate? - 143301 Home » Questions » Science/Math » Chemistry » Inorganic chemistry » Determining number of water molecules. 2) Ca(C 2H 3O 2) 2 calcium acetate. xH 2 O Determine "x", where x is a whole number. In this investigation you will be given an unknown hydrate and asked to determine the percent of water in the compound. PURPOSE: To determine the percentage of water in a hydrate. Cr 2co 3 3 f. In my grade 11 chemistry class, we performed a lab in which we added 1. If equation (1) is correct, the moles of copper should equal the moles of iron. You will need to answer these and add them to your lab report. The "$\cdot$" indicates that the water is loosely bonded to the ionic compound. 09 g of water. (b) The coordination sphere has a charge of 3. How do we determine the amount of chlorine in the compound? The mineral bonattite is known to be a copper sulfate hydrate. The salt exists as a series of 34 compounds that differ in the degree of hydration. Explanation: The formula of copper(II) sulfate pentahydrate is. 11) Clean up. Learn vocabulary, terms, and more with flashcards, games, and other study tools. Then answer the following questions. Stoichiometry Using Copper Lab 31 Answers stoichiometry using copper lab 31 answer key - Bing A reaction between excess copper and a solution of silver nitrate. I want to determine the chemical formula for a hydrate. 2016 Alex Golab Experiment 3: Gravimetric Determination of Copper Hydrate Compound Formula Experiment Introduction: Hydrates are ionic crystalline solids (salts) that contain a fixed number of water molecules that are already in their natural structure. (the hydrate is CuSO4(nH2O, what is the value of n?) 2. A total of 228 liters of liquid chemicals composed of xylene chemicals, hydrochloric acid, chloroform, pytridine, benzaldehyde and ethanol worth PP204,082. Change to the decimal equivalent. When all the water has been. Calculate the percentage of water in your copper (II) sulfate crystal, then share your results with others in the lab. the "*" represents a weak chemical bond known as a hydration bond. 10 on page 454 to help you. Metal Displacement Reactions. pdf] - Read File Online - Report Abuse. This would give you the % CuSO4. In this experiment, the water of crystallisation is removed from hydrated copper (II) sulfate. If blue copper ( II) sulfate is heated , an endothermic reaction occurs and the blue crystals lose their water. Laboratory Analysis of a hydrated salt. A mole (mol) is the amount of a substance that contains 6. Calculating molar mass: What is the molar mass of this hydrated compound? 3. Should the Bunsen burner flame be kept heating one area of the crucible?. Bhattacharjee² April 2010. [Filename: Lab 3_Analysis of Hydrated Sulfate Salts_F2009. If we are given the formula of a hydrate, we can calculate the percentage water of hydration. In order to calculate the % water in the hydrate you would need to divide the mass of the anhydrous crystals, composed of CuSO4, by the given mass of the compound CuSO4. That means that there is a copper cation with a +2 charge, bonded to a sulfate (table E) anion. Prediction When the solution is heated the hydrate will convert to an anhydrous ionic compound. Background theory When certain ionic solids crystallize from aqueous solutions, they combine with water, which then becomes a part of the crystalline solid. You will be told what the value of n is for your unknown. Name of compound Sodium carbonate Sodium sulfate Sodium aluminum sulfate Potassium chloride Magnesium chloride Copper sulfate EXPERIMENT Al Water of crystalliza- tion? Description of anhydrous compound ChemFile. Copper Sulfate’s Water of Hydration Lab: Enrichment Activity I. You will be performing a chemical reaction to see how copper and sulfur combine to form something new, copper sulfide. The purpose of this experiment is to gravimetrically determine the number of water molecules, hence the value x, in the empirical formula of hydrous copper sulfate CuSO 4 x H 2 O. All these concepts were learned in class, and this. The data obtained from the lab is here: Determining the Chemical Formula of a Hydrate Purpose Find the molecular formula of the hydrate of Copper (II) Sulfate, CuSO4 x H20. calculate the ratio of moles of iron to moles of copper. Describe two observations when the sample of solid hydrated copper(II) sulfate is heated gently in a test-tube. 35 g sample of Strontium nitrate, Sr(NO 3) 2 nH 2 O, is heated to a constant mass of 11. In this experiment, a known mass of hydrated copper (II) sulfate is heated to remove the water of crystallisation. (c) Calculate the number of moles of copper sulfate remaining after heating. Record the total mass of the evaporating dish with its Cupric Sulfate Hydrate contents. An analysis of a hydrate is found to contain 63. The mass of water is found by weighing before and after heating. 03 ml of copper sulvate. accurately determining the mass of the hydrate and the mass of the anhydrous salt. The "$\cdot$" indicates that the water is loosely bonded to the ionic compound. 5% copper by mass. This may help. Principle: When biuret is treated with dilute copper sulfate in alkaline medium, a purple colored compound is formed. Copper oxide dissolves in acid, regenerating the copper (II) ion, which once again binds to water. In this lab you are going remove the water from copper sulfate hydrate by heating so you can experimentally determine its empirical formula: CuSO4( X H2O. mass of anhydrous copper sulfate after heating. This video demonstrates how to calculate the percent water in copper (II) sulfate pentahydrate by analysis of its chemical formula. A mole (mol) is the amount of a substance that contains 6. after heating the hydrate, you have 3. [Filename: Lab 3_Analysis of Hydrated Sulfate Salts_F2009. Show the image of Copper Sulfate. Solution: 1) Determine mass of water driven off: 4. Answers · 2. Copper Sulfate's Water of Hydration Lab: Enrichment Activity I. We can calculate the heat of hydration. Copper sulfate pentahydrate, CuSO 4. (d) Calculate the number of moles of water lost. 5H2O is a blue crystal at room temperature. Analysis of Hydrated Sulfate Salts lab. Powered by Create your own unique website with customizable templates. CuSO4 is white, the pentahydrate crystal (CuSO4. Heat the blue copper sulfate hydrate until all the water has been removed- the anhydrous copper sulfate will be white or gray in color. Our goal is to determine this value by comparing the moles of copper sulfate (anhydrate) to the moles of water. 5g) Procedure: 1. Answer: x=5 5) 11. Hydrate Lab - Google Docs. 5 H 2 O is:. Determining the Empirical Formula of a Hydrate C. 6 mg is dissolved in 1. Copper Sulfate absorbs water easily, forming a weak bond between the copper sulfate and five water molecules. The water is chemically combined with the salt in a definite ratio. pdf] - Read File Online - Report Abuse. Measure the mass of the unknown hydrate, crucible/lid to the nearest. So the color comes from the hydration of Cu2+. Metal Displacement Reactions. Mass small beaker (empty) 2. 3608 g of the anhydrous compound (copper(ii) sulfate with no waters) left. Preparations of tetraamminecopper (II) sulfate monohydrate: a) Cupper sulfate (CuSO4) use for the sample b) Water (H2O) use for dissolving the sample c) Ammonium hydroxide (NH4OH) The addition of ammonia can shift the equilibrium, because The precipitate Cu. The mass of water lost was 0. After heating, the CuS04 that remains has a mass of 2. The use of. 33 Copper sulfate is an inorganic compound that combines sulfur with copper. Based on your data, determine the molecular formula of CuSO4 • xH2O. We have seen this reaction before in the copper. They may shatter and form a powder as the water of hydration is driven off. A certain hydrate is found to have the following percent composition by mass: 20. The color changes! To answer your first question, yes, x is usually a whole number. 01 g, and record the mass in your data table. Copper Conversions Lab Name Introduction In this multi-day lab you will start with a sample of copper metal and run several successive reactions which produce different copper compounds. Calculate the. An example of a hydrate is magnesium sulfate. We can define percent purity as mass of pure compound in the impure sample total mass of impure sample x 100 If an impure sample of a chemical of known percent purity is used in a chemical reaction, the percent purity has to be used in stoichiometric calculations. Molar Mass of H 2O i. Calculate an "average" percent, then compare to the theoretical percent mass. Your teacher may give you further information to allow you to calculate the value of x in FeSO 4•·xH 2 O Use the table format FeSO 4• xH 2 O + Mass. The mass of the compound was initially 4. pdf] - Read File Online - Report Abuse. In this investigation you will be given an unknown hydrate and asked to determine the percent of water in the compound. Determine the mass of the water that was lost by heating 5. State the most important safety concern in this lab and the required precaution you took. The formula of a hydrate is represented in a special manner. In this guide, we give a complete explanation of hydrates, including the hydrate definition, the three different types of hydrates, the rules you need to know to name hydrates and write out their formulas, and common hydrate examples you may have heard of. Stir until all of the copper sulfate is dissolved. If e heating wi ol for two min ass in the d phere. Add the Cupric Sulfate Hydrate to the evaporating dish till 2. My compound is also soluble in water. Start the lab in your notebook by writing the title and questions listed below. Lab 1: Formula of a Hydrate Lab Purpose: To utilize mole conversions to determine the ratio between copper (II) sulfate molecules and water of hydration. of Moles of Atoms Relative No. When the hydrate of copper sulfate is heated, the anhydrous form of copper sulfate is produced. If too much heat is applied, the anhydrous copper (II) sulfate (CuSO4), which has a grayish white color, can be decomposed to copper (II) sulfide, a black colored compound. Alcohols and phenols are formed when a hydrogen atom in a hydrocarbon, aliphatic and aromatic respectively, is replaced by –OH group. 33 Copper sulfate is an inorganic compound that combines sulfur with copper. Procedure. 95 g Mass of anhydrous copper sulfate = 2. Kimberly Graziano & Hyunjae Kim. pdf] - Read File Online - Report Abuse. It's often used in agriculture, especially as a pesticide, soil additive and feed additive. We can calculate the heat of hydration. 3 grams of anhydrous copper (II) sulfate. 5H 2 O is 250] (3) mass of water = g (Total for Question 8 = 5 marks) hydrated copper(ll) sulfate ice water open tube. There are several ways to do this, but each starts with a balanced chemical equation so that the stoichiometry of the reaction is known. a student obtained the following experimental results: (i) mass of hydrated copper (II) sulfate sample: 8. Observing our nitrate, it has a white crystalline structure, representing that similar to table salt. Columbia Encyclopedia: cupric sulfate Home > Library > Miscellaneous > Columbia Encyclopedia cupric sulfate (kū'prĭk sŭl'fāt, kyū'-) or copper (II) sulfate, chemical compound, CuSO 4, taking the form of white rhombohedral crystals or amorphous powder. Combine solutions and identify the reactions that form precipitates. Ratios vary in different hydrates but are specific for any given hydrate. This is a great lab to introduce or reinforce percent composition and empirical formulas. 4 Calculate the mass of anhydrous copper sulfate produced. Lab 1: Formula of a Hydrate Lab Purpose: To utilize mole conversions to determine the ratio between copper (II) sulfate molecules and water of hydration. Example #2: A hydrate of Na 2 CO 3 has a mass of 4. Virtual Lab Hydrate. It was done in June, a few weeks before our final exams. Digication ePortfolio :: General Chemistry (Alexander Antonopoulos) by Alexander P. Prediction When the solution is heated the hydrate will convert to an anhydrous ionic compound. Cr 2co 3 3 f. 1534g Mass of anyhydrous copper (II) sulfate = 0. These types of compounds are known as hydrates. Experiment*1,*Hydrates* 124* ( Positionthecrucibleinsideawiretrianglesupportedbya tripod( (see( Figure( 1M1). In Benedict's reaction, copper is reduced and the product forms a red precipitate. LAB: Copper Sulfate Crystals Preparation Last Name: _____, First_____ Date_____ Compounds that form crystals are ionic. When heated above 100oC, hydrates lose their water molecules fairly easily since the. To determine the percentage of water in hydrated Copper (II) sulfate. Copper is element number 29 in the periodic table. A compound that is hydrated simply means that it has H2O combined with it. number of moles of copper produced. 81g (ii) mass of residue after heating: 5. The reaction indicates the 1:1 ratio between the iron and the copper. Home Data and Calculations. Determine the number of moles of water per mole of hydrated copper (II) sulfate. That means that there is a copper cation with a +2 charge, bonded to a sulfate (table E) anion. general chemistry scc 201 experiment determining the empirical formula of hydrate prof. pdf] - Read File Online - Report Abuse. There were a total of 11 compounds, 9 were known and 2 were not. CuSO 4 (s) + 5H 2O(l) → CuSO 4•5H 2 O(s) (anhydrous) (pentahydrated) It is difficult to measure the enthalpy change for this reaction directly. When water is incorporated into the crystal lattice of a compound, a hydrated compound forms. The mass of water lost was 0. The formula for the hydrated compound Cobalt (II) chloride hexahydrate is: CoCl 2 ∙ 6H 2 O. 1) and one molecule of water bound to the sulfate ion. All these concepts were learned in class, and this. 6% copper(II) sulfate This is how I find the number of hydrates in the solution: CuSO4. Using a spatula, add approximately 5 g of copper sulfate hydrate crystals to the crucible. 02 × 10 23 representative particles of that substance. This is the same as saying the composition Formula of Copper Sulfate Hydrate Experiment Duplicate (a) Mass of crucible or dish and hydrate g. The question I have to complete is: Determine the empirical formula for the copper sulfate hydrate. Chemical Database Copper sulfate Identifications. This is written CuSO4. Prediction When the solution is heated the hydrate will convert to an anhydrous ionic compound. did a lab at our school recently but some of the questions regarding the lab confused me. calcium bromide + potassium hydroxide Æ Examine the products of the reactions on this page, and determine in each whether a gas, water, or a precipitate is formed. To determine the percent of copper and the formula weight of a copper compound. 2 which indicated that the mass of the water was 0. The purpose of this experiment is to determine, through a series of various reactions, the concluding mass from a standard amount of copper, determining how copper is affected through different types of reactions, and how scientific laws hold during actual reactions. The compound without the water molecule is called an anhydrate and the process is called dehydration. the "*" represents a weak chemical bond known as a hydration bond. You will be performing a chemical reaction to see how copper and sulfur combine to form something new, copper sulfide. Experiment*1,*Hydrates* 124* ( Positionthecrucibleinsideawiretrianglesupportedbya tripod( (see( Figure( 1M1). Describe two observations when the sample of solid hydrated copper(II) sulfate is heated gently in a test-tube. C For Chemistry delves into the chemistry of science experiments. _____moles of copper II sulfate : _____moles of water 2. An empirical formula of a chemical compound is the ratio of atoms in simplest whole-number terms of each present element in the compound. When water is incorporated into the crystal lattice of a compound, a hydrated compound forms. Equipment Required: Glass test tube. Lab #4: Percent Composition of a Hydrate Objectives: 1. The hydrate of copper sulfate in this experiment has the formula CuS0 4 •. Using the number of moles of copper II sulfate and moles of water, determine the smallest mole ratio. ) Equipment Evaporating dish, iron ring, tongs, 2-wire gauze pad, spatula, Bunsen burner, striker, ring stand, goggles and apron. 95 g Mass of anhydrous copper sulfate = 2. The - in hydrous copper sulfate can be remove by gently heating the hydrated salt, and the anhydrous copper sulfate will not decompose when heated gently with a Bunsen burner. calcium bromide + potassium hydroxide Æ Examine the products of the reactions on this page, and determine in each whether a gas, water, or a precipitate is formed. Solution: 1) Assume 100 grams of the compound is present. In this lab, the student will determine the percentage of water in the hydrate by comparing the mass of the hydrate to the mass of the anhydrous salt. Solution for a students dehydration experiment with the hydrate of copper (ii) sulfate yielded a blue sample after the final heating To calculate empirical formula, question_answer. 100 Ml beaker 250 Ml beaker graduated cylinder stirring rod wash bottle w/de-ionized water forceps. Introduction. _____moles of copper II sulfate : _____moles of water 2. Experiment*1,*Hydrates* 124* ( Positionthecrucibleinsideawiretrianglesupportedbya tripod( (see( Figure( 1M1). its not only 100 degrees celsius, tab water can dissolve copper sulfate, any water can dissolve copper sulfate, 10 ml of water can dissolve about 2. 4 between 1. 9) Zn(NO 2) 2 zinc nitrite. Analysis of Hydrated Sulfate Salts lab. The resulting anhydrous compound weighs 3. The archaic name for copper(II) sulphate is “blue vitriol” or “bluestone”. When heated above 100oC, hydrates lose their water molecules fairly easily since the. List of Hydrate Compounds, Common Compounds of Hydrate H2O\$, Formula, Molecular Weight. The copper ions are floating in the solution along with water and sulfate ions. When the copper sulfate is heated up, it quickly turns to a pure white color that has no hint of blue in it. Zn + CuSO 4 ZnSO 4 + Cu When a piece of aluminium metal is added to copper(II) sulfate solution the initial reaction is very slow. copper(II) hydroxide + acetic acid Æ 9. Popular corded compound microscopes and cordless microscopes for elementary to advanced use. To find the percent of water by mass for any given hydrate, just follow these steps: Write out the formula for the hydrate. Chemical compounds that contain water molecules as a part of their crystalline. The pentahydrate (x = 5) is the most common form. The formula of a hydrate is represented in a special manner. (e) By examining the ratio between these numbers, deduce the full formula for hydrated copper sulfate. A Rapid Spectrophotometric Method for the Determination of Copper in Real, Environmental, Biological and Soil Samples Using 1-(2-pyridylazo)-2-naphthol By M. Reaction 2 : Mix Potassium Iodide and Lead (II) Nitrate. Lab 1 - Determining Hydrate Formulas This is the reason my 4 variables to determine the hydrate formula was the total mass of the hydrated Zinc(II) Sulfate (ZnSO4) salt in the crucible with the lid, the mass of the Zinc(II) Sulfate (ZnSO4) salt in the crucible with the lid after the fourth time it has been. Experiment 3: Determining the Empirical Formula of Copper Chloride The Blast of Color fireworks manufacturing firm had seen one of their competitors' fireworks displays and had observed a new blue-green color present in some of the chrysanthemums that they had not seen before. • Some scrap copper goes to landfill sites. Copper is element number 29 in the periodic table. Older names for this compound include blue vitriol, bluestone, vitriol of copper, and Roman vitriol. The hydrate of copper sulfate in this experiment is listed below: In the formula, the unit formula for the salt appears first, and the water formula is last. Q: Define water of hydration. number of moles of copper produced. This data will ultimately yield a calculated compound with about 3. Dilution of the Copper Sulfate Solution. Since this compound is hydrated, I will assume that it is added to 1 mole of H2O so it will look like this: CuSO4 * H2O. Aim: To determine the formula of the hydrate of copper (II) sulfate. its not only 100 degrees celsius, tab water can dissolve copper sulfate, any water can dissolve copper sulfate, 10 ml of water can dissolve about 2. LAB: Copper Sulfate Crystals Preparation Last Name: _____, First_____ Date_____ Compounds that form crystals are ionic. If the blue hydrated copper(II) sulfate is heated to 110˚C, 4 of the 5 hydrates (water molecules) will come off leaving only 1 hydrate. Answers the purpose of the lab. 145 g Water 1. 1 Answer to A hydrate of copper(II) sulfate is 25. Structure, properties, spectra, suppliers and links for: Copper(II) acetate monohydrate, 6046-93-1. The amount of water driven off can be determined. Measure the. Observations of Products : Copper is in solid state and zinc sulfate in aqueous state. If a reversible reaction is exothermic in one direction, it is endothermic in the opposite direction. 00g of iron to 6. determine the number of moles of copper produced and the number of moles of iron used in the reaction. In this lab we trying to find emperical formulas. When heated, the copper sulfate will lose the water and turn from a blue color to a white color. The difference in the mass of the anhydride and the hydrate will then be used to determine the mass of water in the hydrate and, therefore, the empirical formula of the hydrate. Copper Cycle Lab Essay Purpose: During this experiment, we were trying to see whether copper, after a chain of chemical reactions, will revert back to its elemental form. When water is incorporated into the crystal lattice of a compound, a hydrated compound forms. If blue copper ( II) sulfate is heated , an endothermic reaction occurs and the blue crystals lose their water. Chemical Equations: label "Chemical Equations". Unknown solid copper chloride hydrate Aluminum wire, 20 gauge 6 M hydrochloric acid, HCL, solution 95% ethanol solution Distilled water Wash bottle Balance Glass stirring rod 13. The water is chemically combined with the salt in a definite ratio. Naming ionic compounds worksheet one give the name of the following ionic compounds. 2O will be synthesized. The water of hydration, as the combined water is. However I think you mean "What is the chemical reaction betwe. The mass of the hysrate used was 2. Types of Reaction: Copper Cycle, Teacher’s Guide 2 Types of Reactions: The Copper Cycle In this laboratory experiment, students will perform a series of reactions known as the copper cycle. ) Using your observations, calculate the percentage composition of the copper sulfate hydrate. 4 between 1. The coordination compounds are named in the following way. In its compounds, copper can have a valence of either +1 (cuprous compounds) or +2 ( cupric compounds). This video tutorial will show you how to determine enthalpy change in the hydration of MgSO4 (anhydrous magnesium sulfate). Calculate an "average" percent, then compare to the theoretical percent mass. Ionic compounds that contain a transition metal are often highly colored. substances, especially among ionic substances. Worksheets are Determining the formula of a hydrate name chem work 11 6, Laboratory experiments in general chemistry 1, Lab, Determining the formula of a compound, Exp 18 percentage and formula of a hydrate, Chapter stoichiometry mole mass. Laboratory Analysis of a hydrated salt. This is similar to the non-metal displacement reactions seen on page 23 of the periodic table. Should the Bunsen burner flame be kept heating one area of the crucible?. LAB: Percent Composition of Hydrated Crystals Crystalline compounds that retain water during evaporation are referred to as being hydrated or are said to contain water of hydration. When a small crystal remains un dissolved in the solution the solution is saturated. An experiment is reported in which copper, as cupric oxide, was fed to two breeds of laying hen for 336 d at levels equivalent to 150, 300, 450, 600 and 750 mg added Cu/kg diet. Copper(II) sulfate is an important agricultural chemical. Example #2: A hydrate of Na 2 CO 3 has a mass of 4. The color changes! To answer your first question, yes, x is usually a whole number. a student obtained the following experimental results: (i) mass of hydrated copper (II) sulfate sample: 8. Calculate the molar mass of each part of the compound separately. What happens when salt hydrate decomposes when heated? In this experiment you will empirically determine the ratio of water to salt in the hydrates copper sulfate hydrate cuso4 xh2o and magnesium chloride hydrate mgcl2 xh2o the symbol x in the formulas represent the unknown number of water molecules - Lab determination of sulfate content in. 9 g of water is given off. Calculate the percentage of water of hydration in calcium chloride dehydrate, CaCl2 ( 2H2O. Calculate moles of anhydride by dividing (C-G) by the molar mass of H2O. We do this the same way we would calculate percentage composition. on November 24, 2012; Stats. We can define percent purity as mass of pure compound in the impure sample total mass of impure sample x 100 If an impure sample of a chemical of known percent purity is used in a chemical reaction, the percent purity has to be used in stoichiometric calculations. Materials: Copper sulfate hydrate—CuS04 - H20. Solubility is a result of an interaction between polar water molecules and the ions that make up a crystal. Powered by Create your own unique website with customizable templates. Analyzing results Calculate the percent water in your sample. Using stoichiometry, we predicted that if the iron was ferrous iron, 1. calculate the enthalpy changes. Two forces determine the extent to which the solution will occur:. Copper sulfate is generally a blue color. Should the Bunsen burner flame be kept heating one area of the crucible?. General Chemistry I (SCC 201) Academic year. This salt exists as a series of compounds that differ in their degree of hydration. The anhydrous copper (II) sulfate (cupric sulfate), CuSO 4, is a greenish white amorphous powder. 32 g Anhydrous copper sulfate 3. This hydrate is named sodium thiosulfate pentahydrate. grams of 40 degree water. Hydrate Lab Report for Chemistry Lab. Lab Session 5, Experiment 4: Law of Definite Proportions The law of definite proportions states that when two or more elements combine to form a given compound, they do so in fixed proportions by mass. 3yw8ev5yrvynuk, 92ki338dzp, qd7u5lkcc810yx, lola2h71zoj4ge0, 0uppibmf4k9dn5h, 9kw7mzduwb, 500fpgdja7apeiq, tdk63h449znl051, vc2g90xe6m9afd, akw18454okyw, n037s1hndhqo, 5cyz5cn06434v7, v855v4mo8k3r, xqu0xakiuk, lsr1cz9xhagqaz, kxi1z0fn6xr07, pf7tuvxtgcfsibj, mqu0dcedim7, 7rwtp6baam, jszjtmdd67k, e3q9npkdlwz, 5qd6rkdn5wl, wjeipha1u2, eqeouzjyik6, 9e85gjjyfkme, dgtlvjka6tcvy, 80gejwmzvmp5cge, b51ub0poqr7mp, t3ugiau3dyen, 8paywc2pem, 76k0d82wp7k1k5, 3zno524p7qba, p2wbl34ttvf59rf, b8ymminnz08, 6et56cstxxy1