Copper Sulfate Lab Determining The Hydration Of A Compound Answers

This may help. Experiment 4: COMPOSITION OF A HYDRATE 55 Purpose: Copper(II) sulfate pentahydrate is an example of such a hydrate. It is bright. The percent of water in the original hydrate can easily be calculated: %H2O = X 100. Hypothesis: Hydrates are ionic compounds that have a definite amount of water as part of their structure. A desiccant is a hygroscopic substance that induces or sustains a state of dryness in its vicinity. (c) Calculate the maximum mass of water that could be collected when a sample of hydrated copper(II) sulfate of mass 2. No of moles of water evaporated = = 0. In order to calculate the mass percentage of water in it, we may assume that we have 1 mol of copper(II) sulfate pentahydrate. It is produced with one or seven molecules of water of hydration or in a dried form containing the equivalent of about 2 - 3 waters of hydration. _____moles of copper II sulfate : _____moles of water 2. 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. Copper(II) sulfate is an ionic compound with the chemical formula CuSO. Copper sulfate pentahydrate, CuSO 4. When ionic compounds are dissolved in water, the ions separate. Determine the percent by mass of water in your sample of hydrated copper (II) sulfate. 50 g is heated. 2O, copper (II) sulfate pentahydrate. 58g(CuSO4) Copper II Sulfate Anhydrate. These weighings will be used to calculate the moles of iron used and the moles of copper formed. Calculate an "average" percent, then compare to the theoretical percent mass. 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. Combine solutions and identify the reactions that form precipitates. 10 on page 454 to help you. Note that "x" indicates an unknown number of moles of water that you will have to determine in this lab. Problem #6: Determine the formula and name for the hydrate: 73. Materials: 1 Hot Plate 1 Wire Mesh 1 Small beaker 1 Glass Stirring Rod 1 Beaker Tong 1 Spatula Copper II Sulfate Hydrate (approx. Other Video Experiments: Calculating Formula Units of MgCl2. Name the following chemical compounds: 1) NaBr sodium bromide. Copper metal is noticeably forming on the bottom. 1551 - Tues. The Copper Lab demonstrates stoichiometry in chemistry. Calculate the molar mass of each part of the compound separately. The copper (II) sulphate in the experiment was heated twice in order to make the water of crystallization evaporate completely. Answers · 2. Copper sulfate is a bright blue, odourless crystalline solid which is soluble in water. What is "water of hydration " and how does it affect me (you)? 1. Upon completion of this lab, the student will be able to: 1) Describe the differences between an anhydrous and hydrate compound. 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. 2 which indicated that the mass of the water was 0. Your task is to determine the chemical formula of an unknown copper chloride hydrate by experiment. An anhydrous compound is one which has no water in its structure. The mass of the CuSO4 x 5H2O sample is 1. The compound may be available in a hydrated form or at a different concentration or purity. Answers the purpose of the lab. This can be done as follows. [Filename: Lab 3_Analysis of Hydrated Sulfate Salts_F2009. The % water of crystallisation in the crystals is 2. Show the image of Copper Sulfate. Causes hydroxylamine to ignite. (Hint: First determine GFM then use mole calculation) 5. Teacher Demo: Turning Iron into Copper. The Reactivity Series. In CuSO4 • 5H2O the bonding involves four water molecules coordinatively bound to the Cu 2+ ion in a square planar structure (Figure 5. We were trying to determine the mass of the hydrate, anhydrous salt, and water, as well as the empirical formulas for Copper (II) Sulfate (CuSO4). The copper (II) sulphate in the experiment was heated twice in order to make the water of crystallization evaporate completely. Name your compound by filling in the appropriate prefix: “copper(II) sulfate _____hydrate” 8. Chemical Reactions - ANSWERS 1. Q: A compound is isolated from the rind of lemons that is found to be 88. If e heating wi ol for two min ass in the d phere. I've tried with filtration and other method like reverse phase column chromatography, But still I didn't find. Turn off the burner. This lab used the idea of hydrates and molar mass to figure out the molecular formula of the hydrated cupric sulfate. , Ba(OH) 2 •8H 2 O = "barium hydroxide"). Hydrated water molecules are generally indicated in a formula as shown above for the case of the copper (II) sulfate, using a dot to separate the water molecules from the formula of the salt itself. The loss in mass of the compound after losing the water can be used to calculate the amount of water originally in the hydrated sample. The hydrate is Copper(II) Sulfate or CuSO4 After conducting the experiment I found the mass percentage of this compound is: 28. 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 amount of product that can be produced during a reaction, it is important to be able to calculate which reactant is the limiting reactant. How many grams of anhydrous copper (II) sulfate can we obtain from this amount? Show your work. Break up any large crystals before placing them in the crucible. You will not need more than 2. 10 on page 454 to help you. The molarity of KAl(SO4)2. 001", then it could be used to calculate the mass of Ca(NO 3) 2 via reaction equation. (Whole number ratio between the salt and the hydrate that makes up this particular compound. When all the water has been evaporated from a hydrate it is known as an anhydrous compound. I Used the mass of the copper II sulfate hydrate and the mass of the copper II sulfate anhydrate to determine the mass of water. The reaction series includes single replacement, double replacement, synthesis, and decomposition reactions. (a) There are two Na + ions, so the coordination sphere has a negative two charge: [PtCl 6] 2−. We found that copper sulfate contained more water. A hydrate is a compound that is chemically combined with water molecules. The % water of crystallisation in the crystals is 2. , it will precipitate out of the solution. When heated above 100oC, hydrates lose their water molecules fairly easily since the. In the space below, write a balanced chemical formula to represent the reaction "solid copper (II) sulfate pentahydrate decomposes to produce anhydrous copper sulfate (another solid) and water vapor. Innovating Science's 5-hydrate lab-grade copper (II) sulfate comes in a 500g bottle. The mass of the hysrate used was 2. Splattered out the determined molecular formula would have less of copper ii sulfate and more water molecules because. The formula for the hydrated compound Cobalt (II) chloride hexahydrate is: CoCl 2 ∙ 6H 2 O. The amount of water consumed in the reaction is so minute (because K is very small). Determine the mass of the water that was lost by heating 5. 2) Determine moles of Na 2 CO 3 and water:. Water also comes out of the copper sulfate and is able to function as any other type of water would typically function. Molar Mass of H 2O i. This video demonstrates how to calculate the percent water in copper (II) sulfate pentahydrate by analysis of its chemical formula. pdf] - Read File Online - Report Abuse. [M r of CuSO 4. When it has dried. In many cases, hydrates are coordination compounds. 4H2O) while the literature states that copper sulfate typically has 5 water molecules. One example of a hydrate is copper (II) sulfate pentahydrate. • Copper ores are non-renewable. It is sometimes called blue copper for this reason. _____moles of copper II sulfate : _____moles of water 2. Chemical compounds that contain water molecules as a part of their crystalline. 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. Copper oxide dissolves in acid, regenerating the copper (II) ion, which once again binds to water. The loss in mass of the compound after losing the water can be used to calculate the amount of water originally in the hydrated sample. Purpose - To observe the effect of removing the "water of hydration" from hydrated copper(II) sulfate. Many crystalline compounds contain water as part of their structure. Examples of synthesis reactions include: · Synthesis of sodium chloride. A student heats 2. determine the formula and the name of the iron chloride produced. The percentage of water in the original hydrate can easily be calculated using the formula for percent composition found in Reference Table T. Infer the empirical formula of the hydrate from the formula of the anhydrous. 2 which indicated that the mass of the water was 0. This chemist knows what he's talking about. (e) By examining the ratio between these numbers, deduce the full formula for hydrated copper sulfate. Your task is to determine the chemical formula of an unknown copper chloride hydrate by experiment. Procedure. The data will be translated into a one significant figure answer. 145 g Water 1. Hand in your work before leaving class. (a) There are two Na + ions, so the coordination sphere has a negative two charge: [PtCl 6] 2−. Add about 20 drops of 0. In this week's lab you will determine the formula of a hydrated compound. Determine the percent by mass of water in your sample of hydrated copper (II) sulfate. In this lab you will calculate the percent composition of water in a hydrate and determine the empirical formula of the hydrate you are working with. The water in these compounds can be removed quantitatively by heating the compound with a bunsen burner. The water is chemically combined with the salt in a definite ratio. We will be heating the Copper (II) Sulfate in the test tubes. x H_2O has a molar mass of 250. The % water of crystallisation in the crystals is 2. A hydrate is a crystalline compound that contains a specific number of water molecules attached to an ionic formula unit. What is “water of hydration ” and how does it affect me (you)? 1. To name a coordination compound, no matter whether the complex ion is the cation or the anion, always name the cation before the anion. In part A of the lab, we will synthesis the coordination compound tetraamminecopper (II) sulfate monohydrate [Cu(NH 3) 4]SO 4•H 2O. 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. For example, copper(II) sulfate appears as a blue solution in water. If equation (1) is correct, the moles of copper should equal the moles of iron. mH 2 O in the hydrate equals m Ca(NO 3) 2 4H 2 O-m Ca(NO 3) 2. (b) Work out the mass of 1 mole of copper sulfate. Gains water readily. Part G — Oxidation-reduction and Single Displacement Reactions: Cu2+(aq) Cu(s) The blue copper ions in solution react with the magnesium atoms in the solid metal. Calculate the accepted. 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. The compound’s formula is CuSO4. 5H2O may cause. Calculate the percentage of water in your copper (II) sulfate crystal, then share your results with others in the lab. Copper sulfate pentahydrate is a blue compound that forms striking blue crystals and dissolves readily in water. The mass of the CuSO4 x 5H2O sample is 1. 58g(CuSO4) Copper II Sulfate Anhydrate. 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. 9-19-13 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%. 2 M NaOH to the solution, and record your observations. Then the percentage composition will. magnesium sulfate). mass of anhydrous copper sulfate after heating. A mole (mol) is the amount of a substance that contains 6. Iron is higher up in the electrochemical series than copper so elemental iron can displace copper from a copper compound such as copper sulphate in solution. Determine the percent by mass of water in your sample of hydrated copper (II) sulfate. When you heat up these crystals to about 100C they start losing part of their water and a different comp. Notice that the 5:1 ratio is the maximum ratio of water molecules to copper(II) sulfate. Answer keys are provided separately. The last reaction will release the copper atoms as copper metal again. Now I happen to have exactly 5. Estimating enthalpies of solution from lattice enthalpies and hydration enthalpies The hydration enthalpies for calcium and chloride ions are given by the equations: The following cycle is for calcium chloride, and includes a lattice dissociation enthalpy of +2258 kJ mol -1. The Reactivity Series. Analyzing results Calculate the percent water in your sample. Your task is to determine the chemical formula of an unknown copper chloride hydrate by experiment. Aim: To determine the formula of the hydrate of copper (II) sulfate. The mass of this substance is measured. Determination Of Water Crystalization Essay I. It's for the pentahydrate, with 5 water molecules for each CuSO4 molecule. magnesium sulfate). 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 previous reaction that took place involved aqueous copper(ii) sulfate and solid zinc. 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. 3) P 2O 5 diphosphorus pentoxide. PURPOSE: To determine the percentage of water in a hydrate. (b) Work out the mass of 1 mole of copper sulfate. The amount of water consumed in the reaction is so minute (because K is very small). One simply needs to determine the number of moles of water per mole of anhydrous compound in the hydrate. Answers the purpose of the lab. 2) Ca(C 2H 3O 2) 2 calcium acetate. Hydrate Lab. I think they are the same. The calculated mass of water lost from the hydrated copper (II) sulfate compound was determined to be. 25 = 36% [ A r values: Cu=64, S=32, O=16, H=1 ] The mass ratio of CuSO 4 : H 2 O is 4. Percent Copper and Formula of a Copper Compound Sofia Economides Date Preformed: 3/19/2012 Date Submitted: 3/26/2012 Lab Partners: Anita Smith, Taylor Bell, Derek Bourgeois 1. What is Copper sulfate pentahydrate: Copper(II) sulfate pentahydrate (CuSO4. 145 g Water 1. Purpose In this experiment you will synthesize the coordination compound tetramminecopper (II) sulfate monohydrate [Cu(NH 3) 4]SO 4•H 2O. If the hydrate was not completely converted to the anhydrous compound, the mass of anhydrous Cu(II)SO4 would increase because it would not be pure anhydrous Cu(II)SO4, instead it would be CuSO4•5H2O, in other words you would be weighing the compound plus water. example, copper (II) sulfate pentahydrate can be converted to anhydrous copper (II) sulfate by heating: CuSO4 • 5H2O (sol) → CuSO4 (sol) + 5H2O (gas). BaCl 2 • x H 2 O , barium chloride x-hydrate CuSO 4 • x H 2 0, copper sulfate x-hydrate Procedure: 1) Record the mass of an empty, clean and dry evaporating dish. It can kill bacteria , algae, roots, plants , snails , and fungi. 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. 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. Copper is found naturally in many food sources including meats, vegetables, and grains. Also, the chemical formula for hydrated copper(II) sulfate (or copper sulfate pentahydrate) is CuSO4. The part of the iron nail that was in the copper sulphate solution was covered in a thin layer of copper, which is why it should have looked reddish in colour. Introduction - Hydrated Ionic Compounds, commonly called, "hydrates". An empirical formula of a chemical compound is the ratio of atoms in simplest whole-number terms of each present element in the compound. You will need to answer these and add them to your lab report. 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. Record the letter of your unknown hydrate on your data table. Molar Mass of CuSO 4 h. This A Reversible Reaction of Hydrated Copper (II) Sulfate Lab Resource is suitable for 6th - 12th Grade. Examples of synthesis reactions include: · Synthesis of sodium chloride. the percentage of the hydrate was 35%. This is a great lab to introduce or reinforce percent composition and empirical formulas. The process may be accompanied by physical change, such as color change. In this experiment, a known mass of hydrated copper (II) sulfate is heated to remove the water of crystallisation. Naming ionic compounds worksheet one give the name of the following ionic compounds. mass of beaker-165. Chemistry Chapter 6 DETERMINATION OF THE FORMULA OF COPPER (II) SULFATE Purpose To determine the number of moles of water in a mole of hydrated copper (II) sulfate is written as CuSO4•n H2O. Determine the con-ect formula and name of the hydrate. The name of the complex is sodium hexachloroplatinate (IV), and the coordination number is six. Pre-Lab, Hydrated salts A student was working in lab studying compounds known as HYDRATES. Crush the copper sulfate hydrate (blue compound) using a mortar and pestle. EXPERIMENT 7 Pre-Lab Assignment Determining the Empirical Formula of a Compound Name Date 1. Explanation: The formula of copper(II) sulfate pentahydrate is. Determine the percent by mass of water in your sample of hydrated copper (II) sulfate. They may shatter and form a powder as the water of hydration is driven off. yH2O, ZnSO4. Measure the. The aim of experiments was to determine the percentage of water in hydrated Ca(NO 3 ) 2. 9 g of water is given off. The calculated mass of water lost from the hydrated copper (II) sulfate compound was determined to be. A student heats 2. To determine the percentage of water in hydrated Copper (II) sulfate. The water of hydration, as the combined water is. It is produced with one or seven molecules of water of hydration or in a dried form containing the equivalent of about 2 - 3 waters of hydration. Copper sulfate pentahydrate is a blue compound that forms striking blue crystals and dissolves readily in water. P r e -L a b : 1. When the hydrate of copper sulfate is heated, the anhydrous form of copper sulfate is produced. A desiccant is a hygroscopic substance that induces or sustains a state of dryness in its vicinity. Answer: x=5 5) 11. a sample of the hydrous copper sulfate will be weighed then dissolved in water to separate the salt into the copper ions, sulfate ions and water molecules. The compound may be available in a hydrated form or at a different concentration or purity. It is toxic by ingestion and a strong irritant so care should be taken in handling. using these data, calculate the number of water molecules that is present in the formula of this hydrate (obviously before heating). 3g mass of beaker with bluestone-173. By dissolving the two salts and determining the enthalpy changes, we can work out the enthalpy change of hydration. Next a solution of barium chloride in water is added. EXPERIMENT 7 Pre-Lab Assignment Determining the Empirical Formula of a Compound Name Date 1. Introduction: The purpose of this lab is to determine the number of grams of copper that will be produced from an oxidation reduction reaction when you know the mass of Aluminum that reacted with a known amount of copper 2 sulfate pentahydrate and to compare this to the actual yield of copper. Calculate the mass of water and multiply it by the number of moles indicated in the hydrate formula. If blue copper ( II) sulfate is heated , an endothermic reaction occurs and the blue crystals lose their water. Materials: Copper sulfate hydrate—CuS04 - H20. the percentage of the hydrate was 35%. A certain hydrate is found to have the following percent composition by mass: 20. _____moles of copper II sulfate : _____moles of water 2. The compound’s formula is CuSO4. Background theory When certain ionic solids crystallize from aqueous solutions, they combine with water, which then becomes a part of the crystalline solid. Materials: Test-tube. Observing our nitrate, it has a white crystalline structure, representing that similar to table salt. Many crystalline compounds contain water as part of their structure. formula of this hydrate. XH2O) of Copper II Sulfate Hydrate and once heated I now have 3. The copper(II) sulfate pentahydrate molecule is what you have shown. Purpose: 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. All these concepts were learned in class, and this. The toxicity of copper sulfate depends on the copper content. A coordination compound typically contains a complex ion (with ligands bound to a central metal cation), counter ions, and, sometimes, waters of hydration. Which compound's solubility, that of copper (II) sulfate or of ammonia, varies. An example of a hydrate is magnesium sulfate. xH 2 O Determine "x", where x is a whole number. Analysis of Hydrated Sulfate Salts lab. You may wish, if time permits, to perform a second determination. In this experiment the hydrates of copper(II) sulfate, CuSO 4. Ratios vary in different hydrates but are specific for any given hydrate. 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. (The hydrate is CuSO4(nH2O; what is the value of n?) Calculate moles of anhydride by dividing G by the molar mass of CuSO4. 5 Copper is obtained from copper ores or by recycling copper. 69 x 10^19 CCl2F2 molecules: 1. 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. 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. 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. In this lab, we do not measure the amount of chlorine in the sample, We need the amount of chlorine to determine the formula of the compound. A hydrate is a compound that has one or more water molecules bound to each formula unit. 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. (water of hydration) as part of their structure. Add about 20 drops of 0. 2 x 10^22 H2O molecules: 0. We did a lab today in chem class and I need help solvng a problem. EXPERIMENT 7 Pre-Lab Assignment Determining the Empirical Formula of a Compound Name Date 1. Introduction: You will determine the percentage of water in a hydrate and the empirical formula of a hydrated salt. Your answer must also explain why the mass of copper sulfate hydrate decreases as it is heated. Kimberly Graziano & Hyunjae Kim. Why are there no referendums in the US? Do sorcerers' Subtle Spells require a skill check to be unseen? Customer Requests (Sometimes) Dr. Copper is an essential mineral that plays a key role in many physiological processes, including angiogenesis, skin generation and expression and stabilization of skin proteins. The salt exists as a series of 34 compounds that differ in the degree of hydration. How many moles Copper (II) Sulfate in 1 grams? The answer is 0. 95 g Mass of anhydrous copper sulfate = 2. Then using the same data we will calculate the water of hydration through determining the mole ratio of the decomposition reaction. There were a total of 11 compounds, 9 were known and 2 were not. Copper sulfate is an inorganic compound that combines sulfur with copper. 4H2O)? I'm required to explain why the copper sulfate hydrate we used in a lab had 4 water molecules attached to it (CuSO4. Dissolve the compound in 15 mL of distilled water in a 125 mL Erlenmeyer flask. Chemistry Lab #4 Page 1 of 2. 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. Copper(II) sulfate, also known as copper sulphate, are the inorganic compounds with the chemical formula CuSO4 (H 2 O) x, where x can range from 0 to 5. Questions: 1. If we are given the formula of a hydrate, we can calculate the percentage water of hydration. Determine the formula of the hydrate and then write out the name of the hydrate. The resulting anhydrous compound weighs 3. Many ionic compounds naturally contain water as part of the crystal lattice structure. Should the Bunsen burner flame be kept heating one area of the crucible?. number of moles of copper produced. It is sometimes called blue copper for this reason. 5H2O) sometimes have less water molecules attached to it (e. Lab: Percent Composition of a Hydrate. 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. Gains water readily. All these concepts were learned in class, and this. Although this is an acceptable testing method, in some cases it is necessary to perform a comparative test by mixing a 3% and 5% dilution by weight solution. Analysis of Hydrated Sulfate Salts lab. From the amounts of the reactants, you will determine which reactant is the limiting reactant, and from this amount, calculate the theoretical yield of copper metal. Calculate moles of anhydride by dividing (C-G) by the molar mass of H2O. Why is it important to scour the magnesium strip with steel wool at the start of the experiment? 2. The water in these compounds can be removed quantitatively by heating the compound with a bunsen burner. The water is chemically combined with the salt in a definite ratio. Empirical Formulas and mol: The empirical formula is the simplest whole-number ratio of numbers of mols of atoms in one mol of a compound. The reddish tint of the cobalt(II) chloride solution results from the absorbance of light that is blue-green. EXPERIMENT 7 Pre-Lab Assignment Determining the Empirical Formula of a Compound Name Date 1. This may help. (At the end of this tutorial we have some examples to show you how coordination compounds are named. 03 ml of copper sulvate. 09 g of water. 42 g of (NH 4) 3 PO 4 26. In an imcomplete reaction of the excess zinc with the copper sulfate there will be excess ions that are left in the solution. Since it is available commercially, copper sulfate is usually purchased and not prepared in the laboratory. Record the letter of your unknown hydrate on your data table. pdf] - Read File Online - Report Abuse. Calculate the following about the copper sulfate pentahydrate: (a) Molecular weight of CuSO4*5H2O (b) Moles of CuSO4*5H2O: {convert 1(a) to moles} (c) Moles of Cu in the copper sulfate: 3. Analysis of Hydrated Sulfate Salts lab. For example, Epsom salt (MgSO4·7H2O) is a heptahydrate of magnesium sulfate: within one mole of. resistant surface on your lab table to cool. Copper Sulfate absorbs water easily, forming a weak bond between the copper sulfate and five water molecules. 5% copper by mass. Determine the mass of the covered crucible and crystals to the nearest 0. The ratio of moles of water to moles of compound is a small whole number. The water in these compounds can be removed quantitatively by heating the compound with a bunsen burner. The pentahydrate (CuSO 4 ·5H 2 O), the most commonly encountered salt, is bright blue. PURPOSE: 1. In Benedict's reaction, copper is reduced and the product forms a red precipitate. The metallic copper produced will be weighed. BaCl 2 • x H 2 O , barium chloride x-hydrate CuSO 4 • x H 2 0, copper sulfate x-hydrate Procedure: 1) Record the mass of an empty, clean and dry evaporating dish. Determine the percent by mass of water in your sample of hydrated copper (II) sulfate. _____moles of copper II sulfate : _____moles of water 2. Determination of Copper in Anhydrous Copper Sulphate Some chemical compounds especially inorganic salts, incorporate water into their crystallized structures. Be sure to include the number for the moles of water in the formula for the hydrate. Label three microscope slides, one with an H, one with and R and one with a C. calculate the enthalpy changes. 5H2O is a blue crystal at room temperature. But when copper sulfate is heated (as in a fire), these weak bonds are broken and the water evaporates. 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. Copper (II) Sulfate Pentahydrate. It was done in June, a few weeks before our final exams. CuSO4 5H2O Copper (II) sulfate pentahydrate. The MIL-STD-753 copper sulfate test provides the process for a 1. Calculate the percentage of water of hydration in calcium chloride dehydrate, CaCl2 ( 2H2O. 5H 2 O CuSO4 + 5H 2 O hydrated copper(II) sulfate Solid hydrated copper(II) sulfate is blue. 58g(CuSO4) Copper II Sulfate Anhydrate. Notice each formula has a "*" between the compound's formula and the number of water molecules that are coordinated in the structure. Calculate the. The water is chemically combined with the salt in a definite ratio. Displaying all worksheets related to - Determination Of Empirical Formula Of Copper Oxide Lab. This is the same as saying the composition Formula of Copper Sulfate Hydrate Experiment Duplicate (a) Mass of crucible or dish and hydrate g. Materials: Copper sulfate hydrate—CuS04 - H20. Your teacher will tell you which one to do. Measure the. EXPERIMENT 7 Pre-Lab Assignment Determining the Empirical Formula of a Compound Name Date 1. 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. magnesium sulfate). Digication ePortfolio :: General Chemistry (Alexander Antonopoulos) by Alexander P. new compound having altogether different properties and applications. (c) Calculate the number of moles of copper sulfate remaining after heating. Rati os vary in different hydrates but are specific for any given hydrate. Copper Sulfate's Water of Hydration Lab: Enrichment Activity I. Why are there no referendums in the US? Do sorcerers' Subtle Spells require a skill check to be unseen? Customer Requests (Sometimes) Dr. Memo from Hydrates u2018R Us Industries To: Use your answers to parts b and c to determine the formula of hydrate of nickel (II) chloride. The theoretical (actual) percent hydration (percent water) can be calculated from the formula of the hydrate by dividing the mass of water in one mole of the hydrate by the molar mass of the hydrate and multiplying by 100. Applying conclusions Calculate the percent water in a mole of copper(II)sulfate pentahydrate using the formula. The formula for copper(II) sulfate pentahydrate is written as: CuSO4. Remove the filter paper with the copper from the funnel and leave it to dry. Copper(II) sulfate is an example of a substance that dissolves in water. You will be performing a chemical reaction to see how copper and sulfur combine to form something new, copper sulfide. 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. It decomposes at 650°C to cupric oxide (CuO). The name of the anhydrous salt is followed by a prefix indicating the number of water molecules followed by the word hydrate. Observe the hydrated compound with a hand lens. Equipment Required: Glass test tube. Answers · 2. 7) SO 2 sulfur dioxide. Click "Resources" below for a PDF of the experiment. In many cases, hydrates are coordination compounds. 145 g Water 1. Hydrated copper sulphate is blue in color while anhydrous copper sulphate is white in color. For example, Glucose is C 6 H 12 O 6; it's empirical formula is CH 2 O. Aim: To determine the formula of the hydrate of copper (II) sulfate. Initially, before the reaction, the copper was in the copper compound, copper (II) oxide. Such compounds are referred to as hydrates. Also, the chemical formula for. The salt exists as a series of 34 compounds that differ in the degree of hydration. Copper Sulfate’s Water of Hydration Lab: Enrichment Activity I. 9 on page R54 at the back of your. Why is it important to scour the magnesium strip with steel wool at the start of the experiment? 2. What is Copper sulfate pentahydrate: Copper(II) sulfate pentahydrate (CuSO4. Copper compounds and minerals are often green or blue. Alcohols and phenols are formed when a hydrogen atom in a hydrocarbon, aliphatic and aromatic respectively, is replaced by –OH group. We were trying to determine the mass of the hydrate, anhydrous salt, and water, as well as the empirical formulas for Copper (II) Sulfate (CuSO4). Calculate the mass of hydrated iron (II) sulfate. 5H2O and multiply by 100. For example: hydrated copper sulfate (blue) ⇌ anhydrous copper sulfate (white) + water. 5H 2 O is 250] (3) mass of water = g (Total for Question 8 = 5 marks) hydrated copper(ll) sulfate ice water open tube. pdf] - Read File Online - Report Abuse. 19 g Mass of hydrate copper sulfate = 3. Finding the Hydration Number The hydration number can be conveniently found by heating the compound and measuring its mass loss. PURPOSE: To determine the percentage of water in a hydrate. Write hypotheses to the lab. (c) Mass of test tube with copper oxide (g): 18. (e) By examining the ratio between these numbers, deduce the full formula for hydrated copper sulfate. The reaction series includes single replacement, double replacement, synthesis, and decomposition reactions. 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. Its melting point is 110 ̊C (230 ̊F), density 2. 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. _____moles of copper II sulfate : _____moles of water 2. (Benedicts reagent contains sodium bicarbonate, sodium citrate and copper sulfate). Express your answer as a chemical equation. 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. Graphically determine both the percentage of water in an unknown hydrate of copper (II) sulfate (CuSO4∙xH2O), and the empirical formula of the hydrate If we plot the mass of the water versus the mass of the hydrate, we can use the slope of the line to find what?. “The hydrate” refers to the wh ole compound, the copper (II) sulfate. To determine the percent of copper and the formula weight of a copper compound. If your technique is perfect, you will. The water in these compounds can be removed quantitatively by heating the compound with a bunsen burner. To find the relative molecular mass of a hydrated copper sulfate, simply write out the formula for the compound first. 58g(CuSO4) Copper II Sulfate Anhydrate. To determine the percentage of water in hydrated Copper (II) sulfate. (a) Work out the formula for copper sulfate. Molar Mass of CuSO 4 h. 14g of copper would be produced and if the iron was ferric iron, 1. 0980g 1a) Calculate mass of H2O that was driven off. An excess of copper (II) sulfate solution (to make sure that all the iron is reacted) will be added to a known amount of iron. Cupric sulfate appears as a white or off-white solid. b) Melting Point Determination: Individual elements and compounds have unique melting points (ie: the temperature at which the compound passes from the solid to the liquid phase). 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. determine the number of moles of copper produced and the number of moles of iron used in the reaction. The “·5” does NOT mean times five (×5). This is a class experiment suitable for students who. Many crystalline compounds contain water as part of their structure. 032 2O = 2(16. Memo from Hydrates u2018R Us Industries To: Use your answers to parts b and c to determine the formula of hydrate of nickel (II) chloride. 100 Ml beaker 250 Ml beaker graduated cylinder stirring rod wash bottle w/de-ionized water forceps. Three different hydrated salts were studied: copper sulfate (CuSO 4), manganese sulfate (MnSO 4), and nickel sulfate (NiSO 4. 03 ml of copper sulvate. 5 H 2 O is:. The mass of the compound was initially 4. A student trying to determine if a white solid is a true hydrate heats the sample and finds that there is evolution of water, that the residue obtained is soluble in water and that the solution is colorless. Calculate moles of anhydride by dividing (C-G) by the molar mass of H2O. #N#Support and supervise as students: collect data according to the worksheet. This salt exists as a series of compounds that differ in their degree of hydration. Copper Sulfate’s Water of Hydration Lab: Enrichment Activity I. mass of anhydrous copper sulfate after heating. Why is it important to scour the magnesium strip with steel wool at the start of the experiment? 2. 94g of hydrated copper(II) sulfate crystals were heated, 2. Then the percentage composition will. In this experiment, the. Answer: x=5 5) 11. Why is it important to scour the magnesium strip with steel wool at the start of the experiment? 2. , it will precipitate out of the solution. Google docs does not seem to be working for everyone so I will accept labs via e-mail. 5 H 2 O is:. Determine the number of moles of water per mole of hydrated copper (II) sulfate. The theoretical (actual) percent hydration (percent water) can be calculated from the formula of the hydrate by dividing the mass of water in one mole of the hydrate by the molar mass of the hydrate and multiplying by 100. The lab work has two objectives: first, confirm the formula of a hydrate with known formula and second, find the formula of a hydrate in which the salt formula is known but not the molar amount of water. For instance, several chemists might get different answers when measuring a piece of rope or rubber band if they do not know what the tension is supposed to be. When the precipitated copper was washed, zinc ions were removed. 2) Determine the moles of each compound:. So, for every mole of calcium sulfate, there are 3 moles of water. pdf] - Read File Online - Report Abuse. No of moles of water evaporated = = 0. We have seen this reaction before in the copper. Calculate moles of anhydride by dividing (C-G) by the molar mass of H2O. new compound having altogether different properties and applications. [1 mark] Mass of anhydrous copper sulfate = g [Turn over]. 81g (ii) mass of residue after heating: 5. PURPOSE: To determine the percentage of water in a hydrate. 5 hydrate for every mole of copper(II) sulfate(2:7 ratio). 32 g Anhydrous copper sulfate 3. 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. A hydrate has a definite number of water molecules bound to each anhydrous salt unit. After heating, the mass was 3. 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. mass of anhydrous copper sulfate after heating. Turn off the burner. Is this a true hydrate? Explain. 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. 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. 10 on page 454 to help you. 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. Explanation: The formula of copper(II) sulfate pentahydrate is. From the amounts of the reactants, you will determine which reactant is the limiting reactant, and from this amount, calculate the theoretical yield of copper metal. To determine the percentage of water in hydrated Copper (II) sulfate. 030 mol, and that the amount of water lost on heating was 0. 4 Calculate the mass of anhydrous copper sulfate produced. When you heat up these crystals to about 100C they start losing part of their water and a different comp. Its melting point is 110 ̊C (230 ̊F), density 2. Heat can be used to dehydrate a hydrated salt causing the H 2 O molecules to. Chemical Equations: label "Chemical Equations". Calculate the following for the oxygen:. 1 Answer Ernest Z. Determination of the formula of a hydrate of copper(II) sulfate Computer Simulation. Why must the heated crucible be cooled to near room temperature before weighing? 3. Solubility is a result of an interaction between polar water molecules and the ions that make up a crystal. Determining the Chemical Formula of a Copper Chloride Hydrate. Why is it important to scour the magnesium strip with steel wool at the start of the experiment? 2. Introduction. When the hydrate of copper sulfate is heated, the anhydrous form of copper sulfate is produced. Other Video Experiments: Calculating Formula Units of MgCl2. The mass of the CuSO4 x 5H2O sample is 1. Turn off the burner. It is believed that the process was known (metallurgy) as early as 4500 BC. A compound that is hydrated simply means that it has H2O combined with it. Rati os vary in different hydrates but are specific for any given hydrate. _____ _____ _____ 5. calculate the precent by mass of water in a sample of hydrated copper (II) sulfate. 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. Suppose that you heated a sample of hydrated ionic compound in a test tube. on November 24, 2012; Stats. 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. Moles of H 2O *same answer 1. 1) and one molecule of water bound to the sulfate ion. Should the Bunsen burner flame be kept heating one area of the crucible?. Objective: To determine the %-ammonia and %-copper in the amine-copper sulfate coordination compound, [Cu(NH3)x]SO4 * y H2O, synthesized in a previous lab period and from this deduce a value for the number of coordinated ammonia molecules x and the number of waters of hydration, y, in the molecular formula. Dissolve the compound in 15 mL of distilled water in a 125 mL Erlenmeyer flask. It can be made by the action of sulfuric acid on a variety of copper(II) compounds, for example copper(II) oxide; this oxide can be generated with the addition of hydrogen peroxide to the acid. Drying agents (also called desiccants) come in various forms and have found widespread use in the foods, pharmaceuticals, packing, electronics and many manufacturing industries. (Benedicts reagent contains sodium bicarbonate, sodium citrate and copper sulfate). the green comes from copper ions resulting from various compounds formed by salts in the air. Explanation: The formula of copper(II) sulfate pentahydrate is. xH2O, MgSO4. 4g while that mass of copper (II) sulfate was 1. 71g of copper would be produced. Explain your prediction. Why is it important to scour the magnesium strip with steel wool at the start of the experiment? 2. Introduction - Hydrated Ionic Compounds, commonly called, "hydrates". When the hydrate of copper sulfate is heated, the anhydrous form of copper sulfate is produced. Hypothesis: Hydrates are ionic compounds that have a definite amount of water as part of their structure. asked by A. Multiply mass (step 1) by mass % (step 2) and divide by. 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. In this lab you will calculate the percent composition of water in a hydrate and determine the empirical formula of the hydrate you are working with. Using the mass of the copper II sulfate hydrate and the mass of the copper II sulfate anhydrate, determine the mass of water lost from the hydrate. Analysis of Hydrated Sulfate Salts lab. In this experiment, a hydrate of copper sulfate will be studied (CuSO4. Students dehydrate copper (II) sulfate pentahydrate in a crucible or evaporation dish and use their data to determine the % composition and the number of water molecules per formula unit of copper (II). Copper was first discovered by Early Man prior to 9000 BC. Copper Sulfate's Water of Hydration Lab: Enrichment Activity I. 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. We were trying to determine the empirical formula for copper sulfate and magnesium sulfate. Your answer must also explain why the mass of copper sulfate hydrate decreases as it is heated. 2 M NaOH to the solution, and record your observations. 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. 31 g before heating. 11) Clean up. 03 ml of copper sulvate. I Used the mass of the copper II sulfate hydrate and the mass of the copper II sulfate anhydrate to determine the mass of water. CuSO4 can be used as herbicide, fungicide and pesticide. The chloride mass was determined by difference. The water of hydration, as the combined water is. Your answer must also explain why the mass of copper sulfate hydrate decreases as it is heated. 5H2O while that of the anhydrous one is CuSO4. 2 which indicated that the mass of the water was 0. Hydrate- Data logger experiment INTRODUCTION If white anhydrous copper (II) sulfate powder is left in the atmosphere it slowly absorbs water vapour giving the blue pentahydrated solid. The theoretical (actual) percent hydration (percent water) can be calculated from the formula of the hydrate by dividing the mass of water in one mole of the hydrate by the molar mass of the hydrate and multiplying by 100. When heated, the copper sulfate will lose the water and turn from a blue color to a white color. The copper(II) sulfate pentahydrate molecule is what you have shown. From the amounts of the reactants, you will determine which reactant is the limiting reactant, and from this amount, calculate the theoretical yield of copper metal. Use the dropper to add a very little water to the anhydrous copper (II) sulfate. PURPOSE: To determine the percentage of water in a hydrate. If a reversible reaction is exothermic in one direction, it is endothermic in the opposite direction. This can be done as follows. Write the chemical formula for copper(II) sulfate pentahydrate and determine its molar mass. Displaying all worksheets related to - Determination Of Empirical Formula Of Copper Oxide Lab. Memo from Hydrates u2018R Us Industries To: Use your answers to parts b and c to determine the formula of hydrate of nickel (II) chloride. 2 x 10^22 H2O molecules: 0. 6) K 3N potassium nitride. When heated, the copper sulfate will lose the water and turn from a blue color to a white color. Lab: Analysis Of a Hydrated Compound. I don't know how to do this. in which no [H 2 O] term appears. after heating the hydrate, you have 3. For the lab, stoichiometry was used to predict the amount of copper that would be left over. It is represented by the general equation: A + X à A X where A and X can be elements or compounds and A X is a compound. Hydrated copper sulphate is blue in color while anhydrous copper sulphate is white in color. Name the following chemical compounds: 1) NaBr sodium bromide.

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