Copper Sulfate Lab Determining The Hydration Of A Compound Answers

(b) The coordination sphere has a charge of 3. Kimberly Graziano & Hyunjae Kim. Copper has potent biocidal properties and is used to eliminate bacteria, viruses and parasites [L1828], [L1839]. Determination Of Water Crystalization Essay I. Anhydrate: The compound after the water molecule has been removed. 55 2Cl = 2(35. 35 g sample of Strontium nitrate, Sr(NO 3) 2 nH 2 O, is heated to a constant mass of 11. Copper oxide dissolves in acid, regenerating the copper (II) ion, which once again binds to water. After heating, the CuS04 that remains has a mass of 2. Hydrates are ionic substances that have water molecules included in their crystal structure (Text Chapter 16). The reddish tint of the cobalt(II) chloride solution results from the absorbance of light that is blue-green. Because we don't have a balance for measuring AMU because it is WAY TOO SMALL, we have to mass things in grams instead. Determining the Percent Composition and Formula of a Copper Chloride Hydrate Overview: The mass percents of Cu, Cl and H 2O in a compound are determined by separating and massing the three components. The first step in the determination of the percent copper in a copper-containing compound is to use a type of chemical reaction called a reduction to convert copper (II) ions (Cu2+) in a weighed sample of the compound of interest to metallic copper, by using a reducing agent, in this case magnesium metal. The lost mass is water, and the remaining mass is the anhydride. The % water of crystallisation in the crystals is 2. Why must the heated crucible be cooled to near room temperature before weighing? 3. Mass small beaker (empty) 2. 5H2O) sometimes have less water molecules attached to it (e. Heating blue crystals of copper sulfate pentahydrate above 100°C drives. Initially, before the reaction, the copper was in the copper compound, copper (II) oxide. Using the number of moles of copper II sulfate and moles of water, determine the smallest mole ratio. 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. 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. Both forms are incompatible with finely powdered metals. 14g of copper would be produced and if the iron was ferric iron, 1. We call such solids hydrates, and we call the bound water the water of hydration. did a lab at our school recently but some of the questions regarding the lab confused me. , it will precipitate out of the solution. Why is it important to scour the magnesium strip with steel wool at the start of the experiment? 2. Copper(II) sulfate, also known as copper sulphate, are the inorganic compounds with the chemical formula Cu SO 4 (H 2 O) x, where x can range from 0 to 5. (Alternative: Water has a gram formula mass of 18. 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. Answers · 2. (x)H2O at the end. 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. For example, Epsom salt (MgSO4·7H2O) is a heptahydrate of magnesium sulfate: within one mole of. Percent Water in a Hydrate PURPOSE To determine the percent water in a hydrate sample. calcium hydroxide + phosphoric acid Æ 10. Label three microscope slides, one with an H, one with and R and one with a C. Pre-lab questions: What two things make up hydrates? In order to determine the percent composition and the empirical formula of a hydrate, you must know how much water is in the hydrate. Rati os vary in different hydrates but are specific for any given hydrate. (The hydrate is CuSO4(nH2O; what is the value of n?) Calculate moles of anhydride by dividing G by the molar mass of CuSO4. For example, Epsom salt (MgSO4·7H2O) is a heptahydrate of magnesium sulfate: within one mole of. Based on your data, determine the molecular formula of CuSO4 • xH2O. Calculate the molar mass of each part of the compound separately. The water is chemically combined with the salt in a definite ratio. 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. CuSO4 is white, the pentahydrate crystal (CuSO4. Kimberly Graziano & Hyunjae Kim. Hypothesis: Hydrates are ionic compounds that have a definite amount of water as part of their structure. Answer: Na/Sodium 4) A teacher told a student that the amount of hydrated salt in lansfordite was 0. x H_2O has a molar mass of 250. Quantitative Data: Initial Mass of Copper: 2. 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 this lab you are going remove the water from copper sulfate hydrate by heating so you can experimentally determine its empirical formula: CuSO4( X H2O. For example, copper(II) sulfate appears as a blue solution in water. Copper sulfate as a hydrate is a blue solid; the anhydrous form is a dry white powder. xH 2O, where x is the number of molecules of water of crystallisation present. After the sulfuric acid was added to the beaker, the form of copper that resulted was copper ions with a 2+ charge. (e) By examining the ratio between these numbers, deduce the full formula for hydrated copper sulfate. In this investigation you will be given an unknown hydrate and asked to determine the percent of water in the compound. Ratios vary for different hydrates. Hydrate Lab. 5H2O may cause. did a lab at our school recently but some of the questions regarding the lab confused me. 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. This reaction involves a color chang from blue to almost white. Note that "x" indicates an unknown number of moles of water that you will have to determine in this lab. The mass of this substance is measured. The mass of the compound was initially 4. It's for the pentahydrate, with 5 water molecules for each CuSO4 molecule. b Determine the molecular formula of the hydrocarbon. 5H2O while that of the anhydrous one is CuSO4. It is sometimes called blue copper for this reason. (c) When a piece of zinc metal is added to copper(II) sulfate solution there is an immediate reaction. 0 ml distilled water, and then add the water to the 250 ml beaker with the copper (II) sulfate. Causes hydroxylamine to ignite. com Hydrate Lab. When the crucible and lid have cooled, determine the mass to the nearest 0. In many cases, hydrates are coordination compounds. The steps you need to take in order to determine. Read and understand the entire lab. So the color comes from the hydration of Cu2+. Calculate the percentage by mass of water in the crystals. Hypothesis: Hydrates are ionic compounds that have a definite amount of water as part of their structure. In this lab you are going remove the water from copper sulfate hydrate by heating so you can experimentally determine its empirical formula: CuSO4( X H2O. 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. Hydrates occur quite commonly among chemical. 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. Based on your data, determine the molecular formula of CuSO4 • xH2O. 20 g sample of limestone is added to excess dilute hydrochloric acid and the gas collected; 258 cm3 of carbon dioxide were collected at a temperature of 27 oc and a pressure of 1. 4H2O)? I'm required to explain why the copper sulfate hydrate we used in a lab had 4 water molecules attached to it (CuSO4. Background: Hydrates are chemical compounds that contain water as part of their crystal structure. pdf] - Read File Online - Report Abuse. Allow the crucible to cool before measuring the mass. 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. What is a hydrate? 2. Predict what will happen to the crystal. 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. The purpose for this lab is to determine the empirical formula for an unknown hydrate, understand what an empirical formula represents and the relationship between and use of hydrated and anhydrous compounds. 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. The chemistry of copper. question_answer. They may shatter and form a powder as the water of hydration is driven off. The hydrated salt is vigorously reduced by hydroxylamine [Mellor 8:292(1946-1947)]. This lab activity combines in-class problem-solving with lab work. 58 g of H 2 O. 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. 4% water 71. 25 x 100 / 6. Because we don’t have a balance for measuring AMU because it is WAY TOO SMALL, we have to mass things in grams instead. 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. We have the compound microscope you are looking for! Copper (II) Sulfate, 5-Hydrate Download PDF. for a Salt of Limited Solubility. Compounds of copper. The compound's formula is CuSO 4. 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 test is a test to determine whether or not the carbohydrate contains a free aldehyde or ketone group (as indicated above). Determination Of Water Crystalization Essay I. Determining the Chemical Formula of Hydrated Copper (Ⅱ) Sulfate Using the Empirical Formula Introduction In this experiment, the molecular formula of hydrated Copper (Ⅱ) Sulfate will be determined. 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. (x)H2O at the end. Some compounds, such as the copper sulfate we use in this lab, are much more soluble in hot water than in cold. 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. (Alternative: Water has a gram formula mass of 18. Calculate the molar mass of the compound, MM. xH2O (where x is the number of hydrates) Assume 100 g sample. Lab- Hydrate Ratio of Epsom Salt Goggles must be worn! Overview: Epsom salt (aka magnesium sulfate) is a combination of MgSO 4 and H 2 O. (a) Work out the formula for copper sulfate. Copper(II) Reduction Glucose will react with a basic solution of copper(II) sulfate (called Benedict’s Reagent) to form the insoluble copper(I) oxide, which is red (although it may appear yellow at first). (c) When a piece of zinc metal is added to copper(II) sulfate solution there is an immediate reaction. The water of hydration, as the combined water is. The ratio of moles of water to moles of compound is a small whole number. , it will precipitate out of the solution. More often than not, x is a whole number, but keep in mind that there are some exceptions. Copper sulfate, bluestone and blue vitriol are all 35 common names for cupric sulfate pentahydrate, CuSO 4∙5H 2 O, which is the best known and the most. 4 Calculate the mass of anhydrous copper sulfate produced. 6% copper(II) sulfate This is how I find the number of hydrates in the solution: CuSO4. Copper (II) Sulfate Pentahydrate. Calculate the number of moles of anhydride from its molar mass and your mass of. EXPERIMENT 7 Pre-Lab Assignment Determining the Empirical Formula of a Compound Name Date 1. 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. The metallic copper produced will be weighed. This experiment is intended to introduce students to hydrated compounds. Show the image of Copper Sulfate. If too much heat is applied, the anhydrous copper (II) sulfate (CuSO4), which has a grayish white color, can be decomposed to copper (II) sulfide, a black colored compound. 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. Copper sulfate pentahydrate, CuSO 4. Allow the crucible to cool before measuring the mass. 5% copper by mass. The copper(II) sulfate pentahydrate molecule is what you have shown. 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. The reaction indicates the 1:1 ratio between the iron and the copper. Pre-Lab Question. 14 Limestone is impure calcium carbonate. How can removing water change the color of a substance? Lab partners remove the water of crystallization from hydrated copper (II) sulfate, record their observations, then rehydrate the solid. 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. PROCEDURE: 1. To find the percent of water by mass for any given hydrate, just follow these steps: Write out the formula for the hydrate. Background: Many crystalline compounds contain definite amounts of water that are trapped within their solid-crystalline structures. Percent of Water in a Hydrate. But when copper sulfate is heated (as in a fire), these weak bonds are broken and the water evaporates. Metal Displacement Reactions. Ratios vary in different hydrates but are specific for any given hydrate. Upon completion of this lab, the student will be able to: 1) Describe the differences between an anhydrous and hydrate compound. 1 A student is given a cobalt (II) chloride hydrate. Copper Sulfate absorbs water easily, forming a weak bond between the copper sulfate and five water molecules. Moles of CuSO 4 j. 2O means that 5 waters of hydration are part of the formula. Palladium crystal has 2 bond lengths, Alpha and Beta. The anhydrous form is a pale green or gray-white powder, whereas the pentahydrate, the most commonly encountered salt, is bright blue. 7) SO 2 sulfur dioxide. Digication ePortfolio :: General Chemistry (Alexander Antonopoulos) by Alexander P. It also can be used to prevent the growth of algae. These types of compounds are known as hydrates. A hydrate has a definite number of water molecules bound to each anhydrous salt unit. Determine the formula of the hydrate and then write out the name of the hydrate. The reaction is reversible. b) Calculate the number of moles of water present. Home Data and Calculations. Determine the formula of the hydrate Samples 1, 3, and 5 are hydrates of magnesium sulfate, MgSO 4. 9% Copper (II) Sulfate (CuSO 4); and 36. 545 g of hydrate is heated and 63. An anhydrate is the substance that remains after the water from a hydrate has been removed through heating. Our goal is to determine this value by comparing the moles of copper sulfate (anhydrate) to the moles of water. the "*" represents a weak chemical bond known as a hydration bond. I want to determine the chemical formula for a hydrate. For example, copper(II) sulfate appears as a blue solution in water. COPPER SULFATE PENTAHYDRATE can be dehydrated by heating. 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. Define a hydrate: compounds, typically crystalline that weakly attract water molecules and retain them within the crystalline structure. I wanted to separate copper sulfate from water. No, copper sulfate can't form on electrical wires. 5 Copper is obtained from copper ores or by recycling copper. For those of you who love covalent compounds youre in for a real treat. Hydrate Lab. 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. Molar Mass of CuSO 4 h. pdf] - Read File Online - Report Abuse. Cuso4 Hydrate Cuso4 Hydrate. Many crystalline compounds contain water as part of their structure. PROCEDURE: When copper (II) sulfate hydrate, a blue crystalline solid containing embedded water molecules (called a hydrate), is heated in air, it loses the water molecules and the blue solid is transformed to a white anhydrous (no water) crystal known as. Obtain about 3 g of copper(II) sulfate pentahydrate, CuSO4·5H2O using an analytical balance. The compound formula defines the formula unit, the simplest whole-number ratio of positive and negative ions giving an electrically neutral unit. The data will be translated into a one significant figure answer. Materials: 1 Hot Plate 1 Wire Mesh 1 Small beaker 1 Glass Stirring Rod 1 Beaker Tong 1 Spatula Copper II Sulfate Hydrate (approx. Add about 20 drops of 0. The hydrate of copper (II) sulfate in this experiment has the formula Cu(SO 4). Displaying all worksheets related to - Determination Of Empirical Formula Of Copper Oxide Lab. [3 marks] 1 2 3. The purpose of this experiment is to determine, through a series of various reactions, the concluding mass from a standard amount of copper, determining how copper is affected through different types of reactions, and how scientific laws hold during actual reactions. cedure using one of the listed compounds and verify its hydrate formula. Copper (II) Sulfate Pentahydrate Lab - Composition of a. 375 x 10^-22 g: A salt crystal has a mass of 0. The correct option is: A) The hydration of anhydrous copper salt is an exothermic reaction by -79. 18 copper wire evaporating dish 250 mL beaker (2) weighing paper concentrated HNO. One example of a hydrate is copper (II) sulfate pentahydrate. Zn + CuSO 4 ZnSO 4 + Cu When a piece of aluminium metal is added to copper(II) sulfate solution the initial reaction is very slow. Equipment Required: Glass test tube. To dispose of copper sulfate. Percent of Water in a Hydrate. Greek prefixes are attached to the word "hydrate" to indicate the number of water molecules per formula unit for the compound (e. It's often used in agriculture, especially as a pesticide, soil additive and feed additive. The salt exists as a series of 34 compounds that differ in the degree of hydration. Hand in your work before leaving class. Copper sulfate is an inorganic compound that combines sulfur with copper. 95 g Mass of anhydrous copper sulfate = 2. Moles of H 2O *same answer 1. 03 ml of copper sulvate. The crystals turn white and become anhydrous copper ( II) sulfate crystals again. The difference in mass between the total copper chloride hydrate and the sum of the reduced copper metal and water molecules corresponds to the mass of chloride in the sample. The Copper Lab demonstrates stoichiometry in chemistry. The use of. Molar Mass of CuSO 4 h. Purpose – To observe the effect of removing the “water of hydration” from hydrated copper(II) sulfate. 0153 grams of iron powder, Fe. Measure the mass of the empty crucible using the balance. Generally, water of hydration can be driven from hydrates by heating, leaving behind the anhydrous salt. The mass of the compound was initially 4. These chemistry experiments are not only fun, but very educational for all of those interested in scientific chemical reactions and properties. A hydrate is a compound which has a define number of water molecules chemically attached to the crystal. They may shatter and form a powder as the water of hydration is driven off. In this experiment, you will work first work with copper (II) sulfate pentahydrate and confirm that there are indeed five moles of water associated with each mole of copper (II) sulfate. (a) Work out the formula for copper sulfate. The metallic copper produced will be weighed. (b) Work out the mass of 1 mole of copper sulfate. It has an electronic configuration of [Ar] 4s 1 3d 10, but, perhaps surprisingly, its most common oxidation state is +2. The formula unit for the salt appears first, followed by the water formula. When water is incorporated into the crystal lattice of a compound, a hydrated compound forms. Analyzing results Calculate the percent water in your sample. The correct option is: A) The hydration of anhydrous copper salt is an exothermic reaction by -79. b Determine the molecular formula of the hydrocarbon. Apparatus and Chemicals 0. Formula: CuSO4 Elements: Copper, Hydrogen, Oxygen, Sulfur CAS Number: 7758-98-7. Step 2: Investigating mole quantity of water in an unknown hydrated compound. Should the Bunsen burner flame be kept heating one area of the crucible?. Introduction. 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. (c) When a piece of zinc metal is added to copper(II) sulfate solution there is an immediate reaction. Since this compound is hydrated, I will assume that it is added to 1 mole of H2O so it will look like this: CuSO4 * H2O. Show the image of Copper Sulfate. calcium hydroxide + phosphoric acid Æ 10. Lab 2 - Determination of the Empirical Formula of Magnesium Oxide Goal and Overview The quantitative stoichiometric relationships governing mass and amount will be studied using the combustion reaction of magnesium metal. water lost by the hydrate. 09 g of water. Calculating molar mass: What is the molar mass of this hydrated compound? 3. Experiment*1,*Hydrates* 125* (Qualitative*observations* Place copper(II) sulfate hydrate (CuSO4·xH2O(s)), nickel(II)( sulfate hydrate (NiSO4·xH2O(s))( and( cobalt. The water molecules are loosely. 7 x 10^25 O3 molecules: 3700 g: Calculate the mass (in grams) for: 9. The compound's formula is CuSO4. 5 hydrate for every mole of copper(II) sulfate(2:7 ratio). % of water = (mass of water lost /mass of the hydrate salt ) x 100. determine the formula and the name of the iron chloride produced. When the copper sulfate is heated up, it quickly turns to a pure white color that has no hint of blue in it. 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. (d) Calculate the number of moles of water lost. In many cases, hydrates are coordination compounds. (Benedicts reagent contains sodium bicarbonate, sodium citrate and copper sulfate). Why is it important to scour the magnesium strip with steel wool at the start of the experiment? 2. of Moles Empirical Formula = CuN 2 O 6 [actually Cu(NO 3) 2] 100 g compound contains 63. The difference in mass is due to the water lost by the hydrate. Copper was first discovered by Early Man prior to 9000 BC. Dissolve the compound in 15 mL of distilled water in a 125 mL Erlenmeyer flask. It is believed that the process was known (metallurgy) as early as 4500 BC. But the solubility of many compounds is little affected by solvent temperature. The mass of water lost was 0. A hydrate is a compound that has one or more water molecules bound to each formula unit. Greek prefixes are attached to the word "hydrate" to indicate the number of water molecules per formula unit for the compound (e. Why must the heated crucible be cooled to near room temperature before weighing? 3. (b) A sample of solid hydrated copper(II) sulfate is heated gently in a test-tube. example, copper (II) sulfate pentahydrate can be converted to anhydrous copper (II) sulfate by heating: CuSO4 • 5H2O (sol) → CuSO4 (sol) + 5H2O (gas). It is toxic by ingestion and a strong irritant so care should be taken in handling. If you have taken a lab course in chemistry, you have very likely admired the deep blue color of copper sulfate crystals, CuSO 4 ·5H 2 O. Determine the number of moles of water per mole of hydrated copper (II) sulfate. 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. Also, the chemical formula for. You will need to answer these and add them to your lab report. blue color makes it a good indicator for the presence of copper. We have the compound microscope you are looking for! Copper (II) Sulfate, 5-Hydrate Download PDF. We can calculate the heat of hydration. Use solubility Table B. 15 g mol − 1. Laboratory Analysis of a hydrated salt. Why are there no referendums in the US? Do sorcerers' Subtle Spells require a skill check to be unseen? Customer Requests (Sometimes) Dr. Introduction – Hydrated Ionic Compounds, commonly called, “hydrates”. 1 A student is given a cobalt (II) chloride hydrate. 1 Answer Ernest Z. Copper sulfate pentahydrate is a blue compound that forms striking blue crystals and dissolves readily in water. 14g of copper would be produced and if the iron was ferric iron, 1. Biuret test is a general test for compounds (proteins and peptides) having two or more peptide (CO-NH) bonds. Introduction: Hydrates are ionic compounds (salts) that have a definite amount of water as part of their structure. Calculate the percentage of water of hydration in calcium chloride dehydrate, CaCl2 ( 2H2O. Start studying Lab 15- Hydrate Analysis. The stoichiometry of hydrated copper sulfate. When the copper sulfate is heated up, it quickly turns to a pure white color that has no hint of blue in it. Equipment Required: Glass test tube. In this experiment, as was mentioned, a hydrate of copper sulfate will be studied (C uSO4 5H2O). 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. b) Describe the crystalline structure of the hydrate in your Active Safety goggles and a lab apron must be worn at all times in a chemistry lab. Determine concentration in percent by mass of the solute in solution. after heating the hydrate, you have 3. After the sulfuric acid was added to the beaker, the form of copper that resulted was copper ions with a 2+ charge. A hydrate is a compound that is chemically combined with water molecules. More often than not, x is a whole number, but keep in mind that there are some exceptions. Aluminum & Copper(II) Sulfate Redox Lab 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. hydrate bonds are much weaker than the ionic bonds between the salt ions. A solution is prepared by dissolving 50. LAB: Copper Sulfate Crystals Preparation Last Name: _____, First_____ Date_____ Compounds that form crystals are ionic. Start studying Lab 15- Hydrate Analysis. Other Video Experiments: Calculating Formula Units of MgCl2. (b) The coordination sphere has a charge of 3. With the m H 2 O and mCaCO 3, the percentage becomes able to worked out. Then the percentage composition will. Also, this is im-portant now: five molecules of water are “loosely” bonded to that ionic compound. This laboratory investigation explored the relationship between percent composition and molar ratios and how to use one to find the other. We call such solids hydrates, and we call the bound water the water of hydration. Analysis of Hydrated Sulfate Salts lab. 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. Procedures involving meaurements of masses to determine quantitative information is termed. We can calculate the heat of hydration. When copper (II) sulfate hydrate, a blue crystalline solid containing embedded water molecules (called a hydrate), is heated in air, it loses the water molecules and the blue solid is transformed to a white anhydrous (no water) crystal known as copper (II) sulfate. We obtained the percentages through experimental procedures of reacting Ca(NO 3) 2 with Na 2CO 3 , filtrating and drying CaCO 3. 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. Ratios vary in different hydrates but are specific for any given hydrate. Then the percentage composition will. You obtained the mass percent of water in the copper sulfate hydrate. For example, iron + copper(II) sulfate iron sulfate + copper. Its blue crystals look and feel dry, but each mole of the anhydrous salt is actually bonded to five moles of water. asked by A. In my grade 11 chemistry class, we performed a lab in which we added 1. The anhydrous form is a pale green or gray-white powder, whereas the pentahydrate, the most commonly encountered salt, is bright blue. In many cases, hydrates are coordination compounds. Background theory When certain ionic solids crystallize from aqueous solutions, they combine with water, which then becomes a part of the crystalline solid. Pre-laboratory Assignment: Properties of Hydrates. data, determine the empirical formula for the hydrate. Your task is to determine the chemical formula of an unknown copper chloride hydrate by experiment. The difference in mass is due to the water lost by thehydrate. Using the number of moles of copper II sulfate and moles of water, I need help determining the smallest whole number ratio. Hypothesis: Hydrates are ionic compounds that have a definite amount of water as part of their structure. 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. Add the Cupric Sulfate Hydrate to the evaporating dish till 2. Copper(I) sulfate, also known as cuprous sulfate and dicopper sulfate, is the chemical compound with the chemical formula Cu 2 SO 4 and a molar mass of 223. For example: hydrated copper sulfate (blue) ⇌ anhydrous copper sulfate (white) + water. In this experiment, as was mentioned, a hydrate of copper sulfate will be studied (C uSO4 5H2O). on November 24, 2012; Stats. The water is chemically combined with the salt in a definite ratio. The lost mass is water, and the remaining mass is the anhydride. Use solubility Table B. The copper ions are floating in the solution along with water and sulfate ions. 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. Solution of copper(II) sulfate is often. EXPERIMENT 7 Pre-Lab Assignment Determining the Empirical Formula of a Compound Name Date 1. A very common hydrate encountered in the general chemistry laboratory is copper (II) sulfate pentahydrate, CuSO 4 ·5H 2 O. Lab: Analysis Of a Hydrated Compound. 14 Limestone is impure calcium carbonate. Hydrate Chemical Formula Fomula Mass Mass % Water Nickel(II)chloride hexahydrate Cobalt(II)chloride hexahydrate Copper(II)sulfate pentahydrate 2. Prediction When the solution is heated the hydrate will convert to an anhydrous ionic compound. Copper (II) Sulfate Pentahydrate Lab - Composition of a. 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. Calculate moles of anhydride by dividing (C-G) by the molar mass of H2O. 100 Ml beaker 250 Ml beaker graduated cylinder stirring rod wash bottle w/de-ionized water forceps. Traditionally, this lab has used copper sulfate pentahydrate as the hydrate. 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. Lab 1 - Determining Hydrate Formulas This is the reason my 4 variables to determine the hydrate formula was the total mass of the hydrated Zinc(II) Sulfate (ZnSO4) salt in the crucible with the lid, the mass of the Zinc(II) Sulfate (ZnSO4) salt in the crucible with the lid after the fourth time it has been. To determine the percent of copper and the formula weight of a copper compound. Should the Bunsen burner flame be kept heating one area of the crucible?. The atomic mass of Cu can be found on the. blue color makes it a good indicator for the presence of copper. They may shatter and form a powder as the water of hydration is driven off. To find the relative molecular mass of a hydrated copper sulfate, simply write out the formula for the compound first. This is written CuSO4. No of moles of = = 0. The salt exists as a series of 34 compounds that differ in the degree of hydration. To dispose of copper sulfate. In this experiment, the. 95 g Mass of anhydrous copper sulfate = 2. Calculating molar mass: What is the molar mass of this hydrated compound? 3. Name of compound Sodium carbonate Sodium sulfate Sodium aluminum sulfate Potassium chloride Magnesium chloride Copper sulfate EXPERIMENT Al Water of crystalliza- tion? Description of anhydrous compound ChemFile. The mass of the compound was initially 4. pdf] - Read File Online - Report Abuse. Reaction 2 : Mix Potassium Iodide and Lead (II) Nitrate. 19 g Mass of hydrate copper sulfate = 3. The hydrate being used in this experiment is copper (II) sulfate “x”hydrate. Copper(II) sulfate, also known as copper sulphate, are the inorganic compounds with the chemical formula Cu SO 4 (H 2 O) x, where x can range from 0 to 5. (d) Calculate the number of moles of water lost. accurately determining the mass of the hydrate and the mass of the anhydrous salt. Observations: Mass of copper (II) sulfate hydrate = 0. Analyzing results Calculate the percent water in your sample. Find the formula and name of the hydrate. The toxicity of copper sulfate depends on the copper content. 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. It is an unstable compound as oxo-acids are generally unstable and is more commonly found in the CuSO 4 state. Add the Cupric Sulfate Hydrate to the evaporating dish till 2. 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. Purpose – To observe the effect of removing the “water of hydration” from hydrated copper(II) sulfate. Home Data and Calculations. The compound formula defines the formula unit, the simplest whole-number ratio of positive and negative ions giving an electrically neutral unit. Materials: 1 Hot Plate 1 Wire Mesh 1 Small beaker 1 Glass Stirring Rod 1 Beaker Tong 1 Spatula Copper II Sulfate Hydrate (approx. 14 Limestone is impure calcium carbonate. The correct option is: A) The hydration of anhydrous copper salt is an exothermic reaction by -79. We systematically heated and cooled the copper sulfate three times. Use experimental data to calculate the number of moles of water released by a. 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. You will be performing a chemical reaction to see how copper and sulfur combine to form something new, copper sulfide. 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. It is believed that the process was known (metallurgy) as early as 4500 BC. 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. Introduction Vocabulary: Salt, anhydrous salt, hydrated salt, crystal A hydrate is a compound that contains water in its crystal structure. 00g of copper (II) sulphate which was dissolved in water. Many crystalline compounds contain water as part of their structure. The % H 2 O can be calculated using: % H 2 O = mass in grams of H 2 O attached to hydrate mass in grams of entire hydrate compound Review 1. 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. c) Calculate the number of moles of CuSO4 present. 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. Summarizes observations clearly. If the cupric sulfate solution is warm,. Suppose that you heated a sample of hydrated ionic compound in a test tube. PROCEDURE: 1. 58g(CuSO4) Copper II Sulfate Anhydrate. Copper oxide dissolves in acid, regenerating the copper (II) ion, which once again binds to water. Calculate the weight percent sulfur in the sample given the following data: Mass Final constant mass of crucible Mass of vial with solid unknown sample Mass of vial after sample removal Mass of crucible + BaSO4 after first heating Mass of crucible BaSO4 after second heating Mass of crucible BaSO4 after third heating 10. The ratio of moles of water to moles of compound is a small whole number. 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. The hydrate of copper sulfate in this experiment has the formula CuS0 4 •. Write hypotheses to the lab. Copper/Iron Stoichiometry Grace Timler AB1 October 3, 2017 Abstract The techniques used in this lab are quantitative transfer and vacuum filtration with the reaction of 8. Copper sulfate is a bright blue, odourless crystalline solid which is soluble in water. Crystals of copper sulfate pentahydrate always contain five molecules of water for each copper and sulfate ion pair. Determination of hydration number: show how you obtained your "answer" for the formula of the unknown hydrate of copper (II) sulfate. How can removing water change the color of a substance? Lab partners remove the water of crystallization from hydrated copper (II) sulfate, record their observations, then rehydrate the solid. xH2O (where x is the number of hydrates) Assume 100 g sample. My attempt to answer these questions: 1a) Since anhydrous copper sulfate has no water. The ionic compound (without the waters of hydration) is named first by using the rules for naming ionic compounds (e. This video demonstrates how to calculate the percent water in copper (II) sulfate pentahydrate by analysis of its chemical formula. c) Calculate the number of moles of CuSO4 present. The salt exists as a series of 34 compounds that differ in the degree of hydration. Determine the number of moles of the anhydrous Salt: _____ (Hint: First determine GFM then use mole calculation in Table T of reference table) 5. Study the effect on the aqueous solubility equilibrium of this salt in the presence of an additional amount of one of the ions that it contains (in this case, the effect of added Ca2+). The amount of water driven off can be determined. What are hydrates? If you're studying chemistry, you probably need to know what a hydrate is and the role it serves. [Filename: Lab 3_Analysis of Hydrated Sulfate Salts_F2009. pdf] - Read File Online - Report Abuse. 02 × 10 23 representative particles of that substance. 09 g of water. Chemistry Lab Report-Determining the Empirical Formula of a compound. The mass of water is found by weighing before and after heating. Find the formula and name of the hydrate. 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's often used in agriculture, especially as a pesticide, soil additive and feed additive. The goal of this experiment was to determine the product of copper (II) sulfate with iron. We were trying to determine the empirical formula for copper sulfate and magnesium sulfate. 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. A seed crystal of the solute is dropped into the solution. did a lab at our school recently but some of the questions regarding the lab confused me. asked by A. Percent Water in a Hydrate PURPOSE To determine the percent water in a hydrate sample. 5H2O) sometimes have less water molecules attached to it (e. Analysis of Hydrated Sulfate Salts lab. 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. A desiccant is a hygroscopic substance that induces or sustains a state of dryness in its vicinity. For example, Epsom salt (MgSO4·7H2O) is a heptahydrate of magnesium sulfate: within one mole of. 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. I wanted to separate copper sulfate from water. These classes of compounds find wide applications in industry as well as in day-to-day life. Measure out between 1 and 4 grams of copper sulfate hydrate that you have crushed into the crucible. List of Hydrate Compounds, Common Compounds of Hydrate H2O$, Formula, Molecular Weight. 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. 2 – 4 g of blue copper sulfate hydrate. number of moles of copper produced. Hydrated copper (II) sulfate has some water in the structure already. How do we determine the amount of chlorine in the compound? The mineral bonattite is known to be a copper sulfate hydrate. Calculate the following for the oxygen:. the green comes from copper ions resulting from various compounds formed by salts in the air. The water is chemically combined with the salt in a definite ratio. (water of hydration) as part of their structure. It contains a copper(2+). You will then determine its absorbance curve and compare it to other copper complexes. P r e -L a b : 1. If solid zinc is left unreacted in the solution the final weight of the copper would be artificially high, as the only thing in the evaporating should be the copper. 5 g of hydrated copper sulfate in a test tube. Procedure. When copper (II) sulfate is obtained by crystallization from a water. (c) Calculate the number of moles of copper sulfate remaining after heating. PURPOSE: To determine the percentage of water in 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. 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. 95 g Mass of anhydrous copper sulfate = 2. So that's my mystery molecule there, and we're able to measure the composition of the mystery molecule by mass. 9g mass of dehydrated bluestone-170. Pre-Lab Question. Materials: Copper sulfate hydrate—CuS04 - H20. Copper (II) sulphate has a considerable number of compounds, which have different degrees of hydration. The molarity of (SO4)2. Ex: HgNO 3 H2O is a hydrate while the HgNO 3 is an anhydrous salt. Popular corded compound microscopes and cordless microscopes for elementary to advanced use. 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. accurately determining the mass of the hydrate and the mass of the anhydrous salt. Note the amount of water being evaporated from the compound as it is being heated. These weighings will be used to calculate the moles of iron used and the moles of copper formed. The magnesium ions are colorless. Analysis of Hydrated Sulfate Salts lab. My attempt to answer these questions: 1a) Since anhydrous copper sulfate has no water. The anhydrous form is a pale green or gray-white powder, whereas the pentahydrate, the most commonly encountered salt, is bright blue. University. a) Measure the mass of the unknown hydrate, crucible/lid to the nearest 0. Ratios vary in different hydrates but are specific for any given hydrate. The formula for the hydrated compound Cobalt (II) chloride hexahydrate is: CoCl 2 ∙ 6H 2 O. Define a hydrate: compounds, typically crystalline that weakly attract water molecules and retain them within the crystalline structure. 0 ml distilled water, and then add the water to the 250 ml beaker with the copper (II) sulfate. The name of the anhydrous salt is followed by a prefix indicating the number of water molecules followed by the word hydrate. 5H2O and multiply by 100. 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. Notice that the 5:1 ratio is the maximum ratio of water molecules to copper(II) sulfate. A hydrate is a compound that has one or more water molecules bound to each formula unit. How much energy does it take to go from alpha to beta?. Observations of Products : Copper is in solid state and zinc sulfate in aqueous state. Determination Of Water Crystalization Essay I. Its blue crystals look and feel dry, but each mole of the anhydrous salt is actually bonded to five moles of water. Copper(I) Sulphate will be Cu2SO4 and may have water of hydration expressed as a. Hydrated copper sulfate 4. Virtual Lab Hydrate. IB Chemistry Lab: Hydrate Introduction: A salt with associated water of crystallization is known as a hydrate. This experiment will use ΔH and ΔS obtained electrochemically to calculate ΔG. Percent Water in a Hydrate PURPOSE To determine the percent water in a hydrate sample. If too much heat is applied, the anhydrous copper (II) sulfate (CuSO4), which has a grayish white color, can be decomposed to copper (II) sulfide, a black colored compound. The archaic name for copper(II) sulphate is “blue vitriol” or “bluestone”. The occurrence of the reaction will be obvious since the blue cupric sulfate solution turns green due to the iron going into solution. Analysis of Hydrated Sulfate Salts lab. CuSO4 is white, the pentahydrate crystal (CuSO4. Many crystalline compounds contain water as part of their structure. Problem #6: Determine the formula and name for the hydrate: 73. 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. This salt exists as a series of compounds that differ in their degree of hydration. The water molecules remain as molecules, but they are loosely bonded into the hydrated crystalline structure in the 5:1 ratio. Copper(II) sulfate is corrosive in both the solid and aqueous states; handle with caution. Lab 2 - Determination of the Empirical Formula of Magnesium Oxide Goal and Overview The quantitative stoichiometric relationships governing mass and amount will be studied using the combustion reaction of magnesium metal. Copper sulfate pentahydrate has water molecules as part of the chemical formula. Hypothesis: Hydrates are ionic compounds that have a definite amount of water as part of their structure. asked by A. IB Chemistry Lab: Hydrate Introduction: A salt with associated water of crystallization is known as a hydrate. 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. Start studying Lab 15- Hydrate Analysis. Why is it important to scour the magnesium strip with steel wool at the start of the experiment? 2. The “·5” does NOT mean times five (×5). We did a lab today in chem class and I need help solvng a problem. pdf] - Read File Online - Report Abuse. PURPOSE: To determine the percentage of water in a hydrate. An anhydrate is the substance that remains after the water from a hydrate has been removed through heating. EXPERIMENT 7 Pre-Lab Assignment Determining the Empirical Formula of a Compound Name Date 1. This A Reversible Reaction of Hydrated Copper (II) Sulfate Lab Resource is suitable for 6th - 12th Grade. How can removing water change the color of a substance? Lab partners remove the water of crystallization from hydrated copper (II) sulfate, record their observations, then rehydrate the solid. In this decomposition lesson, students will heat the Blue Copper Sulfate Crystals to remove the water. The compound's formula is CuSO 4. The follow up lecture is very dependent on how you arrange your curriculum. Lab: Analysis Of a Hydrated Compound. Calculate the following for the oxygen:. 00g of iron to 6. Notice that the 5:1 ratio is the maximum ratio of water molecules to copper(II) sulfate. Hydrated copper (II) sulfate has some water in the structure already. The enthalpy change for the following reaction cannot be measured directly. Then answer the following questions. Why is it important to scour the magnesium strip with steel wool at the start of the experiment? 2. a student obtained the following experimental results: (i) mass of hydrated copper (II) sulfate sample: 8. 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. Chemical Database Copper sulfate Identifications. Introduction: Hydrates are ionic compounds (salts) that have a definite amount of water as part of their structure. Increase the ntil all of the ad" the solid tirring rod. The hydrate of copper (II) sulfate in this experiment has the formula Cu(SO 4). 002moles The molar mass of anhydrous copper sulfate is 159. PRE-LAB (must be completed before the lab can be started in class) 1. I've tried with filtration and other method like reverse phase column chromatography, But still I didn't find. Break up any large crystals before placing them in the crucible. When copper (II) sulfate hydrate, a blue crystalline solid containing embedded water molecules (called a hydrate), is heated in air, it loses the water molecules and the blue solid is transformed to a white anhydrous (no water) crystal known as copper (II) sulfate. xH 2 O Determine "x", where x is a whole number. Determine the mass of the covered crucible and crystals to the nearest 0. Heat the beaker of copper (II) sulfate and water using the ring stand and bunsen burner. We offer qualified products for 10257-54-2(copper(ii) sulfate hydrate),please inquire us for 10257-54-2(copper(ii) sulfate hydrate). The pentahydrate (x = 5) is the most common form. I wanted to separate copper sulfate from water. Describe what happens on the DATA SHEET. Drawing conclusions Using your answers from items 3 and 4, determine the empirical formula for the copper sulfate hydrate. Problem #6: Determine the formula and name for the hydrate: 73. Copper(I) sulfate, also known as cuprous sulfate and dicopper sulfate, is the chemical compound with the chemical formula Cu 2 SO 4 and a molar mass of 223. Hint: step 1- Use the number of moles of water and copper sulfate calculated above. We systematically heated and cooled the copper sulfate three times. Calculating molar mass: What is the molar mass of this hydrated compound? 3. Learn vocabulary, terms, and more with flashcards, games, and other study tools.

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