This collection of over 200 practical activities demonstrates a wide range of chemical concepts and processes. Of course the situation here is even more "complex" (sorry) as you can end up with mixtures of the different copper complexes, as appears to be the case over the course of your experiment. The pentahydrate (n = 5), a bright blue crystal, is the most commonly encountered hydrate of copper(II) sulfate.Older names for the pentahydrate include blue vitriol, bluestone, vitriol of copper, and Roman vitriol. Learn more about Stack Overflow the company, and our products. Copper sulfate is commonly included in teenager chemistry sets and undergraduate experiments. Explain how the mass of a given substance is related to the amount of that substance in moles and vice versa. 5 H2O) is heated, it decomposes to the dehydrated form. . The copper(II) ions are removed again from the organic solvent by reaction with fresh sulfuric acid, producing a much more concentrated copper(II) sulfate solution than before. The blood is dropped into a solution of copper sulfate of known specific gravityblood with sufficient hemoglobin sinks rapidly due to its density, whereas blood which sinks slowly or not at all has an insufficient amount of hemoglobin. Stack Exchange network consists of 181 Q&A communities including Stack Overflow, the largest, most trusted online community for developers to learn, share their knowledge, and build their careers. Applying the same means of calculation for trials 2,3,4,5, the results can be seen below. Demonstrate how to lift the entire clamp stand and apparatus. The more observant should notice that the addition of water to anhydrous copper(II) sulfate is exothermic, as the tube becomes noticeably hot if the water is added very slowly. Lower the temperature probe into the solution. When the temperature probe is located closer to the bottom of the Styrofoam cup, the probe would naturally pick up higher temperature, while when it is closer to the top of the solution, the temperature would be lower. From the table of values, it can be seen that at 126 seconds, the temperature begins to rise; this From the table of values, it can be seen that at 126 seconds, the temperature begins to rise; this is the t1value. A typical example of a single displacement reaction where one metal displaces another is the reaction between iron and copper sulfate, given by the reaction Fe + CuSO 4 . Copper(II) sulfate, CuSO 4 (s), (HARMFUL, DANGEROUS TO THE ENVIRONMENT) - see CLEAPSS Hazcard HC027c. Copper sulfate is used in Fehlings and Benedicts solutions. Use this practical to investigate how solutions of the halogens inhibit the growth of bacteria and which is most effective. Demonstration of an exothermic and endothermic reaction. After 750 seconds has finished, discard the solution into the waste containers and save your data. Re-weigh the crucible and contents once cold. Add zinc powder to the solution and use a stirring chip on a magnetic stirrer to stir the contents of the cupt until a maximum temperature has been reached and the temperature starts to drop. Show Fullscreen. The reaction of aluminium and copper(II) sulfate - RSC Education There are many ways of introducing reversible reactions,eg heating hydrated salts such as copper sulfate or cobalt chloride. WS2.7 Evaluate methods and suggest possible improvements and further investigations. A Copper-Iron Replacement Reaction. Heat the crucible and contents, gently at first, over a medium Bunsen flame, so that the water of crystallisation is driven off steadily. [30] Copper sulfate is also used in firework manufacture as a blue coloring agent, but it is not safe to mix copper sulfate with chlorates when mixing firework powders. Act quickly to prevent suck-back if the level of water collecting in the test-tube reaches the end of the delivery tube. The equation for the dehydration of copper (II)sulfate is: CuSO4o5H2O --> CuSO4 + 5H2O On the reactant side the . The blue colour of the hydrated compound should gradually fade to the greyish-white of anhydrous copper(II) sulfate. $\ce{Cu(OH)2}$ itself should be a greenish to pale-blue insoluble precipitate. is the mass of Zn powder . Step 1: Small amount of copper sulphate crystals is taken dry boiling test tube. Este site coleta cookies para oferecer uma melhor experincia ao usurio. Weigh the empty crucible, and then weigh into it between 2 g and 3 g of hydrated copper(II) sulfate. Losing water of crystallization turns hydrated copper sulphate into anhydrous copper sulphate salt. [23] It is produced by mixing a water solution of copper sulfate and a suspension of slaked lime. You can add water to this to rehydrate the compound, and turn it back to blue. Practical Chemistry activities accompanyPractical PhysicsandPractical Biology. By donating a pair of electrons, ligands act as Lewis bases. [19] It is often used to grow crystals in schools and in copper plating experiments, despite its toxicity. Weigh out 6 grams of zinc powder in a weighing boat. [41][42] There are numerous other, more complex, copper(II) sulfate minerals known, with environmentally important basic copper(II) sulfates like langite and posnjakite.[42][43][44]. From the table, the initial temperature of 21.8 can be yielded. and that's how reaction $\eqref{two}$ proceeds. I tried reacting copper sulfate with sodium hydroxide to get copper hydroxide, which should precipitate, according to the following equation: \end{align}. I also tried to give a better description of the turquoise-ish color. It is possible that the original $\ce{Cu(OH)2}$ precipitate appeared more blue than green due to the blue $\ce{CuSO4}$ solution. A boy can regenerate, so demons eat him for years. Copper sulfate can be prepared by treating metallic copper with heated and concentrated sulphuric acid, or by treating the oxides of copper with dilute sulphuric acid. The structure of the solid pentahydrate reveals a polymeric structure wherein copper is again octahedral but bound to four water ligands. However, the latter is the preferred compound described by the term copper sulfate. When concentrated hydrochloric acid is added to a very dilute solution of copper sulfate, the pale blue solution slowly turns yellow-green on the formation of a copper chloride complex. C6.3.1 recall that some reactions may be reversed by altering the reaction conditions including: reversible reactions are shown by the symbol ; reversible reactions (in closed systems) do not reach 100% yield, C5 Monitoring and controlling chemical reactions, C5.3a recall that some reactions may be reversed by altering the reaction conditions, C6.3.1 recall that some reactions may be reversed by altering the reaction conditions including: reversible reactions are shown by the symbol ; reversible reactions (in closed systems) do not reach 100% yield, C5.2a recall that some reactions may be reversed by altering the reaction conditions. Hydrated copper(II) sulfate (HARMFUL, DANGEROUS FOR THE ENVIRONMENT), 23 g. Weigh the empty crucible, and then weigh into it between 2 g and 3 g of hydrated copper(II) sulfate. [48] It is still listed as an antidote in the World Health Organization's Anatomical Therapeutic Chemical Classification System. Copper sulfate can also be produced by slowly leaching low-grade copper ore in air; bacteria may be used to hasten the process. You must be very careful when you add the acid to the ammonia because very large quantities of ammonium chloride smoke are produced, hence use of a fume cupboard. If large crystals are used, these should be ground down before use by students. Carefully add the ammonia in the same way but initially without swirling. Quantitative chemistry | Review my learning | 1416 years, Demonstrating the diffusion of ammonia and hydrogen chloride, Gold coins on a microscale | 1416 years, Practical potions microscale | 1114 years, Antibacterial properties of the halogens | 1418 years, Crucibles may be of porcelain, stainless steel or nickel, of capacity about 15 cm. Do not heat too strongly, nor allow the white colour to darken, as the copper sulfate may decompose to produce toxic sulfur oxides. Copper (I) sulfate, Cu 2 SO 4, which is uncommonly used. [12] It exothermically dissolves in water to give the aquo complex [Cu(H2O)6]2+, which has octahedral molecular geometry. [28] The hydrated salt can be intimately mingled with potassium permanganate to give an oxidant for the conversion of primary alcohols.[29]. Use a related experiment from ourExhibition Chemistry series to demonstrate the reactivity of aluminium using hydrochloric acid and mercury. I tried reacting copper sulfate with sodium hydroxide to get copper hydroxide, which should precipitate, according to the following equation: $$\ce{2NaOH + CuSO4 -> Cu(OH)2(s) + Na2SO4}$$ I looked on Google Images, and the color of copper hydroxide is light-blue, but something interesting happened when I mixed these two solutions: the precipitate formed - and was originally light-blue, as . *Calculation of Average Change in Temperature, Tavg=45.3+44.2+42.8+43.9+44.7=220.9/5=44.18oC, Calculating the Enthalpy Change of Reaction. Reactions in solution involving potassium dichromate or bismuth trichloride are normally controlled by pH, and an example of a simple reversible gas reaction involves copper sulfate with hydrogen chloride and ammonia. The trick with this demonstration is doing it on a large enough scale for the whole class to see clearly. 8.7: Enthalpy: A Measure of the Heat Evolved or Absorbed in a Reaction; Chapter 9. Copper sulfate is used to test blood for anemia. Other rare copper sulfate minerals include bonattite (trihydrate),[39] boothite (heptahydrate),[40] and the monohydrate compound poitevinite. In some chemical reactions, the products of the reaction can react to produce the original reactants. IaS2.6 when processing data use an appropriate number of significant figures, IaS2.11 in a given context interpret observations and other data (presented in diagrammatic, graphical, symbolic or numerical form) to make inferences and to draw reasoned conclusions, using appropriate scientific vocabulary and terminology to communicat. Both ammonia and hydrochloric acid should be diluted before disposal down a sink. WS.2.7 Evaluate methods and suggest possible improvements and further investigations. [25] Copper ions are highly toxic to fish, however. The chemistry of aqueous copper sulfate is simply that of copper aquo complex, since the sulfate is not bound to copper in such solutions. What reactions occur when mixing copper sulfate and sodium hydroxide? C3.2 How are metals with different reactivities extracted? [citation needed], Anhydrous copper(II) sulfate can be produced by dehydration of the commonly available pentahydrate copper sulfate. The hydrated form is medium blue, and the dehydrated solid is light blue. Copper sulfate is produced industrially by treating copper metal with hot concentrated sulfuric acid or copper oxides with dilute sulfuric acid. The physics of restoration and conservation, RSC Yusuf Hamied Inspirational Science Programme, How to prepare for the Chemistry Olympiad, Read our standard health and safety guidance. This becomes whitish when anhydrous when it is not molecularly bound to water. There's for example. Slowly add the acid down the side of the flask and swirl vigorously. The chemical reaction is the breaking up of the bonds in the molecules of the reactants and the formation of new bonds in the molecules of resultants (the products) from the reaction, and the chemical reaction plays an important role in our daily life. Try this class practical or demonstration to illustrate the displacement of copper from copper(II) sulfate using aluminium foil. Ammonia contact with the eyes can cause serious, long-term damage. Also, a better lid with airtight and temperature retention ability can be used. Site design / logo 2023 Stack Exchange Inc; user contributions licensed under CC BY-SA. 5.6 The rate and extent of chemical change, 5.6.2 Reversible reactions and dynamic equilibruim, 5.6.2.2 Energy changes and reversible reactions, Topic 4 - Extracting metals and equilibria, 4.13 Recall that chemical reactions are reversible, the use of the symbol in equations and that the direction of some reversible reactions can be altered by changing the reaction conditions. Note: Water is dissolved in copper sulphate, heat is produced due to which the water present boils. Begin data collection, allowing the temperature probe to equilibrate for 90-120 seconds before adding the zinc. . Procedure. Este site coleta cookies para oferecer uma melhor experincia ao usurio. Combined Science. Copper(II) sulfate was used in the past as an emetic. Students will probably also have to be reminded about the need to allow the crucible and contents to cool thoroughly before weighing. Consider . It is toxic by inhalation - the concentrated solution releases dangerous quantities of hydrogen chloride vapour. In this case, the coordination number of the copper changes from six to four. is the temperature change. C5.3.5 explain how the mass of a given substance is related to the amount of that substance in moles and vice versa and use the relationship: number of moles = mass of substance (g) / relative formula mass (g), C5.3.6 deduce the stoichiometry of an equation from the masses of reactants and products and explain the effect of a limiting quantity of a reactant. These components are water, lime ammonium, and copper ions. Although a great deal of heat is generated, this has never been a problem. Preparing salts by neutralisation of oxides and carbonates Such reactions are called reversible reactions and are represented: A + B C + D. 4.7.4 The rate and extent of chemical change. 8.6: Limiting Reactant, Theoretical Yield, and Percent Yield from Chemistry Stack Exchange is a question and answer site for scientists, academics, teachers, and students in the field of chemistry. Yes, as noted by @airhuff, there is not one but two reactions involving, one is formation of greenish-pale blue copper sulfate, $\ce{CuSO4}$ and other one is formation of black-brown copper(II) oxide $\ce{CuO}$.