Copper Sulfate Lab Determining The Hydration Of A Compound Answers









Multiply mass (step 1) by mass % (step 2) and divide by. You obtained the mass percent of water in the copper sulfate hydrate. 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. 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. 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. Explain your prediction. 32 g Anhydrous copper sulfate 3. 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. 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 was first discovered by Early Man prior to 9000 BC. PRE-LAB (must be completed before the lab can be started in class) 1. Experiment*1,*Hydrates* 125* (Qualitative*observations* Place copper(II) sulfate hydrate (CuSO4·xH2O(s)), nickel(II)( sulfate hydrate (NiSO4·xH2O(s))( and( cobalt. CuSO 4 ∙5H 2 O is actually [Cu (H 2 O) 4 ]SO 4 ∙4H 2 O; four molecules of water of hydration are coordinated to the copper ion, whereas the fifth water molecule is linked to the sulfate ion, presumably by hydrogen bonding. It is widely used as an algaecide and fungicide. This would give you the % CuSO4. Which compound's solubility, that of copper (II) sulfate or of ammonia, varies. determine the number of moles of copper produced and the number of moles of iron used in the reaction. blue color makes it a good indicator for the presence of copper. 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. Calculate the percentage by mass of water in the crystals. These compounds often come in the form of a crystal which can then be heated in order to remove the water in the form of steam. The mass of this substance is measured. The change from hydrate to anhydrous salt is accompanied by a change in color:. The copper (II) sulphate in the experiment was heated twice in order to make the water of crystallization evaporate completely. 2) Determine the moles of each compound:. The water molecules remain as molecules, but they are loosely bonded into the hydrated crystalline structure in the 5:1 ratio. The occurrence of the reaction will be obvious since the blue cupric sulfate solution turns green due to the iron going into solution. When water is incorporated into the crystal lattice of a compound, a hydrated compound forms. If it heated too strongly, the colour of copper sulphate will turn to black. Ratios vary in different hydrates but are specific for any given hydrate. 81g (ii) mass of residue after heating: 5. Equipment Required: Glass test tube. But the solubility of many compounds is little affected by solvent temperature. 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. We will be heating the Copper (II) Sulfate in the test tubes. 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. This laboratory investigation explored the relationship between percent composition and molar ratios and how to use one to find the other. Pre-laboratory Assignment: Properties of Hydrates. The archaic name for copper(II) sulfate is blue vitriol. I think they are the same. Determination of hydration number: show how you obtained your "answer" for the formula of the unknown hydrate of copper (II) sulfate. Hypothesis: Hydrates are ionic compounds that have a definite amount of water as part of their structure. Determine the mass of solution by multiplying the volume of the solution by the density of the solution. The purpose of this lab was to determine and identify two unknown compounds using a flame that produced different colors. Pre-laboratory questions: A hydrate is a salt bonded hydrated copper sulfate. A seed crystal of the solute is dropped into the solution. Calculate the mass of water and multiply it by the number of moles indicated in the hydrate formula. 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. [Filename: Lab 3_Analysis of Hydrated Sulfate Salts_F2009. P r e -L a b : 1. 2O, copper (II) sulfate pentahydrate. In order to calculate the mass percentage of water in it, we may assume that we have 1 mol of copper(II) sulfate pentahydrate. The compound without the water molecule is called an anhydrate and the process is called dehydration. The atomic mass of Cu can be found on the. on November 24, 2012; Stats. web; books; video; audio; software; images; Toggle navigation. For example, if a sample of copper sulfate pentahydrate is heated, the bright blue crystals of the hydrate are converted to the white, powdery, anhydrous salt. The compound formula defines the formula unit, the simplest whole-number ratio of positive and negative ions giving an electrically neutral unit. Generally, water of hydration can be driven from hydrates by heating, leaving behind the anhydrous salt. Chemical Equations: label "Chemical Equations". question_answer. 5000 g of a copper(ii) sulfate hydrate with an unknown number of attached water molecules. Such compounds are referred to as hydrates. PURPOSE: 1. 030 mol, and that the amount of water lost on heating was 0. C For Chemistry delves into the chemistry of science experiments. When ionic compounds are dissolved in water, the ions separate. 03 ml of copper sulvate. asked by A. It is an unstable compound as oxo-acids are generally unstable and is more commonly found in the CuSO 4 state. The archaic name for copper(II) sulphate is “blue vitriol” or “bluestone”. It's often used in agriculture, especially as a pesticide, soil additive and feed additive. 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. Pre-Lab Question. Purpose – To observe the effect of removing the “water of hydration” from hydrated copper(II) sulfate. 7g Would this be a ballanced equation for this reaction? CuSO4•5H2O+ heat= CuSO4+5H2O so would you do this %by mass=mass. In this week's lab you will determine the formula of a hydrated compound. Aim: To determine the formula of the hydrate of copper (II) sulfate. Its melting point is 110 ̊C (230 ̊F), density 2. The hydrated salt is vigorously reduced by hydroxylamine [Mellor 8:292(1946-1947)]. 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. Hydrated copper (II) sulfate has some water in the structure already. Kimberly Graziano & Hyunjae Kim. Determine the mass of the covered crucible and crystals to the nearest 0. 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. Hypothesis: Hydrates are ionic compounds that have a definite amount of water as part of their structure. Heat( the crucible over a( Bunsen. Determination Of Water Crystalization Essay I. Analysis of Hydrated Sulfate Salts lab. The ratio of moles of water to moles of compound is a small whole number. It is sometimes called blue copper for this reason. Specific Learning Objectives: By completing this exercise, the user will gain experience in how to make use of mass measurements before and after two chemical transformations to discern the empirical formula of a copper chloride hydrate, Cu x Cl y •zH 2 0. Place the crucible with the copper sulfate hydrate on the triangle. _____moles of copper II sulfate : _____moles of water 2. 58 g of H 2 O. Step 2: Investigating mole quantity of water in an unknown hydrated compound. Use solubility Table B. 03 = 5 So: there are 5 times more moles of water. Should the Bunsen burner flame be kept heating one area of the crucible?. Mass small beaker (empty) 2. Applying conclusions Calculate the percent water in a mole of copper(II)sulfate pentahydrate using the formula. 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. Causes hydroxylamine to ignite. Prerequisites: Some familiarity with the use of scientific. the percentage of the hydrate was 35%. Displaying all worksheets related to - Determination Of Empirical Formula Of Copper Oxide Lab. 4 2–, acts as a chelating bidentate ligand, donating 2 electron pairs from 2 oxygen atoms to the transition metal center, Fe3+ (Figure 2). You will need to answer these and add them to your lab report. This is written CuSO4. The barium ions will react with the sulfate ions to produce BaSO4 which is insoluble in water, i. This video tutorial will show you how to determine enthalpy change in the hydration of MgSO4 (anhydrous magnesium sulfate). To create the copper(II) sulfate solution, you will be adding about 3. My attempt to answer these questions: 1a) Since anhydrous copper sulfate has no water. An anhydrate is the substance that remains after the water from a hydrate has been removed through heating. 030 mol, and that the amount of water lost on heating was 0. Dissolve the compound in 15 mL of distilled water in a 125 mL Erlenmeyer flask. Graphically determine both the percentage of water in an unknown hydrate of copper (II) sulfate (CuSO4∙xH2O), and the empirical formula of the hydrate The actual formula of the hydrate is. Los Angeles City College Chemistry 60 EXPERIMENT 7: HYDRATES. For example… A 15. Using a spatula, add approximately 5 g of copper sulfate hydrate crystals to the crucible. You will be performing a chemical reaction to see how copper and sulfur combine to form something new, copper sulfide. [Filename: Lab 3_Analysis of Hydrated Sulfate Salts_F2009. Determine the percent by mass of water in your sample of hydrated copper (II) sulfate. Copper metal collects on the solid magnesium. Apparatus and Chemicals 0. 95 x 10^-2 g: Calculate the mass (in grams) of a single chitin molecule (C8H13O5N) 3. 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. The toxicity of copper sulfate depends on the copper content. The anhydrous copper (II) sulfate (cupric sulfate), CuSO 4, is a greenish white amorphous powder. Often used as a component in Benedict's and biuret reagents, this makes the chemical a perfect fit in any educational or research lab dealing with biochemistry or organic chemistry. COPPER SULFATE PENTAHYDRATE can be dehydrated by heating. , Ba(OH) 2 •8H 2 O; 8 water molecules. It is widely used as an algaecide and fungicide. Your task is to determine the chemical formula of an unknown copper chloride hydrate by experiment. CuSO4 5H2O Copper (II) sulfate pentahydrate. Some compounds, such as the copper sulfate we use in this lab, are much more soluble in hot water than in cold. Observing our nitrate, it has a white crystalline structure, representing that similar to table salt. The name of this compound is “copper sulfate pentahydrate”. Hydrate Lab. List of Hydrate Compounds, Common Compounds of Hydrate H2O$, Formula, Molecular Weight. Copy this reaction: CuSO 4. Greek prefixes are attached to the word "hydrate" to indicate the number of water molecules per formula unit for the compound (e. All these concepts were learned in class, and this. Copper compounds and minerals are often green or blue. In this experiment, a known mass of hydrated copper (II) sulfate is heated to remove the water of crystallisation. Use Figures 15. Many compounds possessing transition metal ions absorb visible light when dissolved in water. The balanced chemical reaction : Types of reaction : Single-displacement reaction : It is a type of reaction in which a single element displaces another element in a compound. This lab requires the use of safety goggles … Always wear safety goggles and a lab apron to protect your eyes. This would give you the % CuSO4. An example would be something like washing soda, with its formula consisting of the following. How many grams of the hydrated form should we weigh out? Show your work. Hypothesis: Hydrates are ionic compounds that have a definite amount of water as part of their structure. Labreport#4 - Determining the Empirical Formula of a Hydrate C. 0980g 1a) Calculate mass of H2O that was driven off. You will need to answer these and add them to your lab report. Molar Mass of CuSO 4 h. Science Concept: Iron and copper elements exchange places with each other in a water solution. For example, if a sample of copper sulfate pentahydrate is heated, the bright blue crystals of the hydrate are converted to the white, powdery, anhydrous salt. new compound having altogether different properties and applications. 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. 5H2O) and the aquous solution (Cu2+(aq) ions) are royal. Displaying all worksheets related to - Determination Of Empirical Formula Of Copper Oxide Lab. 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. Determination of hydration number: show how you obtained your “answer” for the formula of the unknown hydrate of copper (II) sulfate. Write the chemical formula for copper(II) sulfate pentahydrate and determine its molar mass. Circle the letter next to each sentence that is true about hydrated compounds. Calculate the number of moles of anhydride from its molar mass and your mass of. Displaying all worksheets related to - Determination Of Empirical Formula Of Copper Oxide Lab. 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. Allow the crucible to cool before measuring the mass. Determine the solubility product constant (Ksp) for a sparingly soluble salt. With the m H 2 O and mCaCO 3, the percentage becomes able to worked out. 41 g Using these results, determine the mass of water in the sample of hydrated copper (II) sulfate and from this information calculate the empirical formula of the sample. To find the relative molecular mass of a hydrated copper sulfate, simply write out the formula for the compound first. Many hydrate salts can be transformed to the anhydrous (without water) compound by heat. xH2O (where x is the number of hydrates) Assume 100 g sample. Observe the hydrated compound with a hand lens. Answer keys are provided separately. 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. mass of beaker-165. Heating blue crystals of copper sulfate pentahydrate above 100°C drives. Copper Sulfate absorbs water easily, forming a weak bond between the copper sulfate and five water molecules. 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 molarity of (SO4)2. 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. In this lab, we will be working with a hydrate of Copper (II) sulfate. 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. Chemistry- Determining the Formula of a Hydrate Lab, Sept. An empirical formula of a chemical compound is the ratio of atoms in simplest whole-number terms of each present element in the compound. C For Chemistry delves into the chemistry of science experiments. It is toxic by ingestion and a strong irritant so care should be taken in handling. Reco hydrous salt MPOSITIO ust be worn a definite am e hydrate is a hydrate is nhydrous salt nt of water in nd the mass of water in th r x 100 ate (CuSO 4 ⋅ 5 sulfate is acc CuSO 4 + white of the. 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. In many cases, hydrates are coordination compounds. My attempt to answer these questions: 1a) Since anhydrous copper sulfate has no water. 6) K 3N potassium nitride. This is a class experiment suitable for students who. The change from hydrate to anhydrous salt is accompanied by a change in color:. 5H2O and multiply by 100. How do we determine the amount of chlorine in the compound? The mineral bonattite is known to be a copper sulfate hydrate. Many crystalline compounds contain water as part of their structure. Determine the percent by mass of water in your sample of hydrated copper (II) sulfate. 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. What are hydrates? If you're studying chemistry, you probably need to know what a hydrate is and the role it serves. (the hydrate is CuSO4(nH2O, what is the value of n?) 2. Answer keys are provided separately. 32 g Anhydrous copper sulfate 3. (Hint: First determine GFM then use mole calculation) 5. 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. This would give you the % CuSO4. The mass of CaCO 3 could be found by subtracting the mass of filter paper from "0. Using the reaction below determine the number of water molecules per mole of copper (II) sulfate hydrate: CuSO 4. water lost by the hydrate. Calculating molar mass: What is the molar mass of this hydrated compound? 3. Copper sulfate pentahydrate, expressed in chemical notation as CuSO4-5H2O, represents a "hydrate. The Lane-Eynon method is an example of a tritration method of determining the concentration of reducing sugars in a sample. When water is incorporated into the crystal lattice of a compound, a hydrated compound forms. b) Calculate the number of moles of water present. mass of anhydrous copper sulfate after heating. 286g, and this number is calculated to be 28. EXPERIMENT 7 Pre-Lab Assignment Determining the Empirical Formula of a Compound Name Date 1. Calculate the formula mass. It's also used in the manufacture of other copper compounds and in electroplating baths. 81g (ii) mass of residue after heating: 5. After heating, the CuS04 that remains has a mass of 2. Calculate the number of moles of anhydride from its molar mass and your mass of. It was done in June, a few weeks before our final exams. In this week's lab you will determine the formula of a hydrated compound. This video demonstrates how to calculate the percent water in copper (II) sulfate pentahydrate by analysis of its chemical formula. Hydrated copper sulfate 4. 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. The next day you will recombine water with the anhydrous white powder and measure the heat transferred by this reaction to water in calorimeter. After sulfuric acid was added to the beaker, copper was found as copper ions with a 2+ charge instead of the previous copper(ii) oxide form. If equation (1) is correct, the moles of copper should equal the moles of iron. Mass small beaker (empty) 2. Enthalpy and Entropy of Zinc with Copper Sulfate. 70g The mass of the dish and hydrate was 43. pdf] - Read File Online - Report Abuse. An anhydrous compound is one which has no water in its structure. xH 2 O Determine "x", where x is a whole number. 35 g sample of Strontium nitrate, Sr(NO 3) 2 nH 2 O, is heated to a constant mass of 11. • Copper ores are non-renewable. To create the copper(II) sulfate solution, you will be adding about 3. Compound Microscopes. Step 2: Investigating mole quantity of water in an unknown hydrated compound. Displaying all worksheets related to - Determination Of Empirical Formula Of Copper Oxide Lab. Chemical Database Copper sulfate Identifications. water lost by the hydrate. EXPERIMENT 7 Pre-Lab Assignment Determining the Empirical Formula of a Compound Name Date 1. After sulfuric acid was added to the beaker, copper was found as copper ions with a 2+ charge instead of the previous copper(ii) oxide form. apply Hess’s Law to find the overall enthalpy. 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. the green comes from copper ions resulting from various compounds formed by salts in the air. Many hydrate salts can be transformed to the anhydrous (without water) compound by heat. Many compounds possessing transition metal ions absorb visible light when dissolved in water. A hydrate is a compound that has one or more water molecules bound to each formula unit. Start studying Lab 15- Hydrate Analysis. Los Angeles City College Chemistry 60 EXPERIMENT 7: HYDRATES. Calculate the molarity (molar concentration) of the copper(II) sulfate solution. Place the crucible with the copper sulfate hydrate on the triangle. Using a spatula, add approximately 5 g of copper sulfate hydrate crystals to the crucible. 41 g Using these results, determine the mass of water in the sample of hydrated copper (II) sulfate and from this information calculate the empirical formula of the sample. 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. The use of. I need to find the X in CuSO4 multiplied (x) XH20 ( how many waters are there. EXPERIMENT 7 Pre-Lab Assignment Determining the Empirical Formula of a Compound Name Date 1. When the precipitated copper was washed, zinc ions were removed. 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. 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. When all the water has been. Name your compound by filling in the appropriate prefix: “copper(II) sulfate _____hydrate” 8. Finally write the correct name of the hydrate (using prefixes mono- di- tri- tetra- penta- hexa- or hepta-, as appropriate) and write a balanced chemical equation describing the decomposition of hydrated compound to form anhydrous compound. Copper sulfate pentahydrate is a blue compound that forms striking blue crystals and dissolves readily in water. 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. Click "Resources" below for a PDF of the experiment. The water is chemically combined with the salt in a definite ratio. The compound without the water molecule is called an anhydrate and the process is called dehydration. While the hydrate is heating, draw representations of. Mass small beaker (empty) 2. Why is it important to scour the magnesium strip with steel wool at the start of the experiment? 2. If the cupric sulfate solution is warm,. Introduction – Hydrated Ionic Compounds, commonly called, “hydrates”. 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. Displaying all worksheets related to - Determination Of Empirical Formula Of Copper Oxide Lab. Gains water readily. When copper (II) sulfate is obtained by crystallization from a water. 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. Hydrate Lab Report for Chemistry Lab. Answer to: A hydrate of copper (II) sulfate with formula CuSO_4. Many ionic compounds naturally contain water as part of the crystal lattice structure. 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. So the color comes from the hydration of Cu2+. Copper is found naturally in many food sources including meats, vegetables, and grains. x H 2 O, and magnesium sulfate, MgSO 4. The calculated mass of water lost from the hydrated copper (II) sulfate compound was determined to be. So, for every mole of calcium sulfate, there are 3 moles of water. Rati os vary in different hydrates but are specific for any given hydrate. Copper is element number 29 in the periodic table. The name of the complex is sodium hexachloroplatinate (IV), and the coordination number is six. Chemistry- Determining the Formula of a Hydrate Lab, Sept. Determine the percent by mass of water in your sample of hydrated copper (II) sulfate. cedure using one of the listed compounds and verify its hydrate formula. Chemical Database Copper sulfate Identifications. If your technique is perfect, you will. Why must the heated crucible be cooled to near room temperature before weighing? 3. It has an electronic configuration of [Ar] 4s 1 3d 10, but, perhaps surprisingly, its most common oxidation state is +2. Analysis of Hydrated Sulfate Salts lab. Should the Bunsen burner flame be kept heating one area of the crucible?. When you finished this part of the lab empty the re-hydrated CuSO 4 ·5H 2 O into the beaker provided by your instructor for this purpose. Copper sulfate is generally a blue color. To calculate the percent composition, we took the. Describe what happens on the DATA SHEET. The reaction produced copper(II) sulfate and water. An example of a hydrate is magnesium sulfate. Notice that the 5:1 ratio is the maximum ratio of water molecules to copper(II) sulfate. 81g (ii) mass of residue after heating: 5. The hydrate of copper (II) sulfate in this experiment has the formula Cu(SO 4). 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. 95 g Mass of anhydrous copper sulfate = 2. Using the reaction below determine the number of water molecules per mole of copper (II) sulfate hydrate: CuSO 4. Obtain about 3 g of copper(II) sulfate pentahydrate, CuSO4·5H2O using an analytical balance. A sulfate salt of copper. 70g The mass of the dish and hydrate was 43. 2 x 10^22 H2O molecules: 0. “The hydrate” refers to the wh ole compound, the copper (II) sulfate. Initially, before the reaction, the copper was in the copper compound, copper (II) oxide. Start studying Lab 15- Hydrate Analysis. Hydrated copper sulfate 4. 1551 - Tues. Calculate the number of moles of copper(II) sulfate that will be in the solution. 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. But when copper sulfate is heated (as in a fire), these weak bonds are broken and the water evaporates. 03 ml of copper sulvate. What is "water of hydration " and how does it affect me (you)? 1. This salt exists as a series of compounds that differ in their degree of hydration. An ionic hydrate is an ionic compound that has water molecules trapped within its crystal lattice (Refer to your textbook for more information). Molar Mass of CuSO 4 h. Determine formulas for simple ionic compounds In ordinary chemical reactions, the nucleus of each atom (and thus the identity of the element) remains unchanged. 16, 2008 The lab report will be due on Thursday, Sept. Crush the copper sulfate hydrate (blue compound) using a mortar and pestle. 1534g Mass of anyhydrous copper (II) sulfate = 0. Hydrate Chemical Formula Fomula Mass Mass % Water Nickel(II)chloride hexahydrate Cobalt(II)chloride hexahydrate Copper(II)sulfate pentahydrate 2. This number is then converted to an amount of grams that can be measured in a laboratory. You may wish, if time permits, to perform a second determination. When a hydrate Is heated, the crystal structure of the compound will change. Older names for this compound include blue vitriol, bluestone, vitriol of copper, and Roman vitriol. Then answer the following questions. 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. 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. Then using the same data we will calculate the water of hydration through determining the mole ratio of the decomposition reaction. Hydrated copper sulfate 4. Moles of H 2O *same answer 1. In this experiment, a known mass of hydrated copper (II) sulfate is heated to remove the water of crystallisation. Chemistry Lab Report-Determining the Empirical Formula of a compound. Calculate the molar mass of each part of the compound separately. I don't know how to do this. The copper(II) sulfate pentahydrate molecule is what you have shown. Goal: To determine the empirical formula of a copper chloride compound. It's for the pentahydrate, with 5 water molecules for each CuSO4 molecule. 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. 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. Determination of the amount of water of crystallisation in hydrated sodium carbonate Theory 2 Hydrated sodium carbonate has the formula Na 2CO 3. The mass of the recovered copper is 1. The mass of each component (Cu, Cl, H 2 O) is converted to moles, whereby the law of multiple proportions allows the use of a ratio to determine the empirical formula of. A desiccant is a hygroscopic substance that induces or sustains a state of dryness in its vicinity. Two forces determine the extent to which the solution will occur:. Purpose In this experiment you will synthesize the coordination compound tetramminecopper (II) sulfate monohydrate [Cu(NH 3) 4]SO 4•H 2O. CuSO4 can be used as herbicide, fungicide and pesticide. The “hydrate” or the CuSO 4·5H 2O, when heated turns into an anhydrous salt with this formula: CuSO 4 when the water is given off as an invisible gas to the air. 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. 15 g mol − 1. 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. From this data we determined the empirical formula for the 2 compounds. 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. 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. 1551 - Tues. Background: Hydrates are chemical compounds that contain water as part of their crystal structure. 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. It is bright. These classes of compounds find wide applications in industry as well as in day-to-day life. If the PDF does not display below, you may also download it here. Experiment 4: COMPOSITION OF A HYDRATE 55 Purpose: Copper(II) sulfate pentahydrate is an example of such a hydrate. The compound's formula is CuSO 4. Calculate the mass of water driven off. Copper (II) Sulfate Hydrate Compound Formula Lab Hello, so in my general chemistry class for Uni we had a lab where we had a Copper 2 Sulfate Hydrate compound, then we used a brunsen burner to remove all of the water, and we were able to figure out that mass of the H2O and the CuSO4. For example, the solubility of sodium chloride in water is 355 g/L at 0°C, increasing only about 10% to 390 g/L at 100 °C. determine the formula and the name of the iron chloride produced. What is the percent water in copper (II) sulfate pentahydrate, CuSO 4 • 5 H 2 O? 1. 1534g Mass of anyhydrous copper (II) sulfate = 0. The change from hydrate to anhydrous salt is accompanied by a change in color:. 25 g of hydrated copper sulphate, CuSO 4!xH. 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. To create the copper(II) sulfate solution, you will be adding about 3. LAB 10 WATER OF HYDRATION. They may shatter and form a powder as the water of hydration is driven off. A HYDRATE is a compound that contains water in its. If we are given the formula of a hydrate, we can calculate the percentage water of hydration. For those of you who love covalent compounds youre in for a real treat. 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. 03 ml of copper sulvate. XH2O) of Copper II Sulfate Hydrate and once heated I now have 3. But when copper sulfate is heated (as in a fire), these weak bonds are broken and the water evaporates. Blue copper ( II ) sulfate crystals will also turn white in the presence of concentrated sulfuric. Principle: When biuret is treated with dilute copper sulfate in alkaline medium, a purple colored compound is formed. Copper sulfate is generally a blue color. We did a lab today in chem class and I need help solvng a problem. In this week's lab you will determine the formula of a hydrated compound. Copper sulfate pentahydrate is a blue compound that forms striking blue crystals and dissolves readily in water. Students are provided with CuSO4. 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. 5H2O) sometimes have less water molecules attached to it (e. This information was then used to determine the empirical formula of the hydrate , defined as a compound formed by the addition of water to another molecule. Calculate the mass percentage of water in the hydrate. This banner text can have markup. 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. It's often used in agriculture, especially as a pesticide, soil additive and feed additive. pdf] - Read File Online - Report Abuse. Should the Bunsen burner flame be kept heating one area of the crucible?. Google docs does not seem to be working for everyone so I will accept labs via e-mail. In many cases, hydrates are coordination compounds. 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. Formula: CuSO4 Elements: Copper, Hydrogen, Oxygen, Sulfur CAS Number: 7758-98-7. accurately determining the mass of the hydrate and the mass of the anhydrous salt. xH 2 O Determine "x", where x is a whole number. For example… A 15. Determination of hydration number: show how you obtained your "answer" for the formula of the unknown hydrate of copper (II) sulfate. XH2O) of Copper II Sulfate Hydrate and once heated I now have 3. There are therefore 6. You will not need more than 2. Determine the mass of copper(II) sulfate pentahydrate added to the test tube. copper sulfate monohydrate (Molar Mass = ) copper sulfate trihydrate (Molar Mass = ) copper sulfate pentahydrate Molar Mass = ) Also calculate the molar mass of each hydrate. I need to find the X in CuSO4 multiplied (x) XH20 ( how many waters are there. These types of compounds are known as hydrates. 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. CuSO4 can be used as herbicide, fungicide and pesticide. 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 oxide dissolves in acid, regenerating the copper (II) ion, which once again binds to water. Copy this reaction: CuSO 4. An example of a hydrate is magnesium sulfate. 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. Crush the copper sulfate hydrate (blue compound) using a mortar and pestle. (x)H2O at the end. 100 Ml beaker 250 Ml beaker graduated cylinder stirring rod wash bottle w/de-ionized water forceps. Multiply mass (step 1) by mass % (step 2) and divide by. The formula of the hydrate copper(II) sulfate. Should the Bunsen burner flame be kept heating one area of the crucible?. Observing our nitrate, it has a white crystalline structure, representing that similar to table salt. Rati os vary in different hydrates but are specific for any given hydrate. New - Lab Supplies & Equipment. The steps you need to take in order to determine. Balanced equation : CuSO4 + Zn ---> ZnSO4 + Cu(s). [M r of CuSO 4. The water is chemically combined with the salt in a definite ratio. EXPERIMENT 7 Pre-Lab Assignment Determining the Empirical Formula of a Compound Name Date 1. Notice that the 5:1 ratio is the maximum ratio of water molecules to copper(II) sulfate. This video tutorial will show you how to determine enthalpy change in the hydration of MgSO4 (anhydrous magnesium sulfate). One common example is Epsom salt, MgSO 4 ∙7H 2 O. Just like the dozen and the gross, it is a name that stands for a number. It can kill bacteria , algae, roots, plants , snails , and fungi. State the most important safety concern in this lab and the required precaution you took. Copper(II) sulfate is a metal sulfate compound having copper(2+) as the metal ion. The stoichiometry of hydrated copper sulfate. 15 g mol − 1. 145 g Water 1. It can kill bacteria , algae, roots, plants , snails , and fungi. The formula for copper(II) sulfate pentahydrate is written as: CuSO4. 5H2O is toxic. Should the Bunsen burner flame be kept heating one area of the crucible?. Using a spatula, add approximately 5 g of copper sulfate hydrate crystals to the crucible. Initially, before the reaction, the copper was in the copper compound, copper (II) oxide. This information is used to find x in the formula: CuSO 4. Calculate the mass of water driven off. Magnesium sulfate is also prepared by sulfation of magnesium oxide. 95 g Mass of anhydrous copper sulfate = 2. The anhydrous form is a pale green or gray-white powder, whereas the pentahydrate, the most commonly encountered salt, is bright blue. We did a lab today in chem class and I need help solvng a problem. Using the reaction below determine the number of water molecules per mole of copper (II) sulfate hydrate: CuSO 4. The barium ions will react with the sulfate ions to produce BaSO4 which is insoluble in water, i. How many formula units of copper (II) sulfate pentahydrate are in just 3. Q: A compound is isolated from the rind of lemons that is found to be 88. 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. 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. Chemical compounds that contain water molecules as a part of their crystalline. For those of you who love covalent compounds youre in for a real treat. The resulting anhydrous compound weighs 3. 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. To find the percent of water of a hydrate. Step 2: Investigating mole quantity of water in an unknown hydrated compound. Observations of Products : Copper is in solid state and zinc sulfate in aqueous state. 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. Two forces determine the extent to which the solution will occur:. How many grams of the hydrated form should we weigh out? Show your work. Calculate the mass of water driven off. 6% dilution by weight solution. (Whole number ratio between the salt and the hydrate that makes up this particular compound. the copper sulfate, using a dot to separate the water molecules from the formula of the salt itself. Calculate an "average" percent, then compare to the theoretical percent mass. In this experiment, the water of crystallisation is removed from hydrated copper (II) sulfate. Hydrates occur quite commonly among chemical. This is the same as saying the composition Formula of Copper Sulfate Hydrate Experiment Duplicate (a) Mass of crucible or dish and hydrate g. In this experiment you analyze a hydrate to determine the percent of water present within it. Equipment Required: Glass test tube. The “·5” does NOT mean times five (×5). PHASE SYMBOLS MANDATORY IN ALL BALANCED EQUATIONS A Na 2CO 3(AQ) + CuSO 4 A Sodium carbonate + Copper (II) sulfate → Copper Six Lab Questions ANSWERS 1. The chemical equation of this reaction is:. Materials: Copper sulfate hydrate—CuS04 - H20. 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. Many hydrate salts can be transformed to the anhydrous (without water) compound by heat. containing a different number of moles of water of hydration. 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. When all the water has been evaporated from a hydrate it is known as an anhydrous compound. LAB % COMPOSITION OF A HYDRATE. The mass of this substance is measured. x H_2O has a molar mass of 250. What is Copper sulfate pentahydrate: Copper(II) sulfate pentahydrate (CuSO4. 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. b) Calculate the number of moles of water present. The blue color fades as the copper ions end up in the solid. This mass loss is usually due to the hydration water molecules being driven off. 7) SO 2 sulfur dioxide. 03 ml of copper sulvate. [Filename: Lab 3_Analysis of Hydrated Sulfate Salts_F2009. 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. 0062653265550854. substances, especially among ionic substances. For example, copper(II) sulfate appears as a blue solution in water. Add about 20 drops of 0. Obtain your unknown hydrate. It is widely used as an algaecide and fungicide. (Alternative: Water has a gram formula mass of 18. Copper sulfate is generally a blue color. The way we name a hydrated ionic compound is by using the same prefixes as used for binary covalent compounds. 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. 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. This chemist knows what he's talking about. Magnesium is reacted with oxygen from the air in a crucible, and the masses before and after the oxidation are measured. To determine the percent of copper and the formula weight of a copper compound. Digication ePortfolio :: General Chemistry (Alexander Antonopoulos) by Alexander P. You may wish, if time permits, to perform a second determination. This lab used the idea of hydrates and molar mass to figure out the molecular formula of the hydrated cupric sulfate. There are therefore 6. Fishing (2009) points out that pentahydrate (CuSO4· 5H2O) is bright blue due to the water of hydration and when heated, the blue copper sulphate can be dehydrated to a grey-white power called anhydrous salt. Chemical Equations: label "Chemical Equations". This will be accomplished by adding concentrated ammonia (NH 3) to copper (II) sulfate pentahydrate which will displace the water molecules bound in the original copper complex, and a dramatic color change occurs. 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. Crystals of copper sulfate pentahydrate always contain five molecules of water for each copper and sulfate ion pair. 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. 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. Similarly, MgSO 4 ∙7H 2 O is actually [Mg (H 2 O) 6 ]SO 4 ∙4H 2. 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. Copper sulfate as a hydrate is a blue solid; the anhydrous form is a dry white powder. In this experiment you analyze a hydrate to determine the percent of water present within it. CuSO 4 (s) + 5H 2O(l) CuSO 4. One of their spies had managed to. The compound formula defines the formula unit, the simplest whole-number ratio of positive and negative ions giving an electrically neutral unit. 00 g of the hydrate. 1) and one molecule of water bound to the sulfate ion. Mass of water = 0. This is the same as saying the composition Formula of Copper Sulfate Hydrate Experiment Duplicate (a) Mass of crucible or dish and hydrate g. a student obtained the following experimental results: (i) mass of hydrated copper (II) sulfate sample: 8. Mass small beaker (empty) 2. Determine the percent by mass of water in your sample of hydrated copper (II) sulfate. For ionic compounds: Compound formula is the same as the empirical formula. Ratios vary in different hydrates but are specific for any given hydrate. This would give you the % CuSO4. 00 g of H20 are driven off. These types of compounds are known as hydrates. 100 Ml beaker 250 Ml beaker graduated cylinder stirring rod wash bottle w/de-ionized water forceps. Introduction: Ionic compounds often separate from water solution with molecules of water incorporated into the solid. 00 g of FeC13 xH20 are heated, 2. 2) Determine the moles of each compound:. 7) SO 2 sulfur dioxide. 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) sulfate. determine the number of moles of copper produced and the number of moles of iron used in the reaction. 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. Our goal is to determine this value by comparing the moles of copper sulfate (anhydrate) to the moles of water. Antonopoulos at Salve Regina University. xH 2 O To determine the formula, you must determine the following. Combine solutions and identify the reactions that form precipitates. 5H2O while that of the anhydrous one is CuSO4. Then answer the following questions. CuSO4 5H2O Copper (II) sulfate pentahydrate. Answers the purpose of the lab. COPPER SULFATE PENTAHYDRATE can be dehydrated by heating. Analysis of Hydrated Sulfate Salts lab. Read and understand the entire lab. The hydrate of copper sulfate in this experiment has the formula CuS0 4 •. The enthalpy change for the following reaction cannot be measured directly. 14g of copper would be produced and if the iron was ferric iron, 1. Place the crucible with the copper sulfate hydrate on the triangle. When heated, the copper sulfate will lose the water and turn from a blue color to a white color. Determine the formula of the hydrate and then write out the name of the hydrate. PROCEDURE Obtain from the instructor a hydrated salt chosen from copper sulfate, calcium sulfate, and magnesium sulfate. 58 g of H 2 O. A Copper-Sulfate-Based Inorganic Chemistry Laboratory for First tion of an ore containing copper sulfate and insoluble basic cop- per sulfates, (ii) determination of the number of water molecules in hydrated copper sulfate, and. % H 2O in hydrate g. The percent of water in the original hydrate can be calculated easily: % H 2O = Mass of water x 100 Mass of hydrate In this experiment, a hydrate of copper (II) sulfate (CuSO 4 ⋅ 5H. In its elemental form, copper has a red-orange metallic luster appearance. Determination of the amount of water of crystallisation in hydrated sodium carbonate Theory 2 Hydrated sodium carbonate has the formula Na 2CO 3. Introduction – Hydrated Ionic Compounds, commonly called, “hydrates”. % comp = (mass of part/mass of whole) 2. Introduction a. It's often used in agriculture, especially as a pesticide, soil additive and feed additive. You will heat the blue hydrate to find the empirical formula.
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