# Electrolysis Of Aqueous Cuso4 Using Platinum Electrodes

Question 18: Predict the products of electrolysis in each of the following: (i) An aqueous solution of AgNO 3 with silver electrodes. The number of electrons transferred was calculated by bulk electrolysis and rotating disc electrodes. 670 M CuSO4 solution is electrolyzed by passing 4. Sodium chlorate is best as the starting material - someone has already done most of the electrolyzing for you. During the electrolysis of copper (II) sulfate, or "CuSO"_4", the deposition of copper can be seen on the cathode; at the same time, the anode will be dissolved by the process. On loosing their charge they get deposited on the electrode or discharged as a gas. Lesson organisation This class experiment can be done by students working either in pairs or threes. A sample of 80. carbon) What happens:. Grove's gas voltaic battery constructed in 1839 had electrodes (anode, cathode) made of platinum sitting in glass tubes with their lower end immersed in dilute sulfuric acid (electrolyte) and their upper part exposed to hydrogen and oxygen inside the tubes. CuSO4 ==> Cu(++) + SO4(-. Magnesium sulfate electrolysis - posted in Chemistry: Ok so i am doing a little thinking with different types of solutions and the flames they produce. 5 M Na 2 SO 4 aqueous solution (pH 7. copper that needs to be purified. d) S 2 O 8 2-, H 2. Using a cell containing inert platinum electrodes, electrolysis of aqueous solutions of some salts leads to reduction of the cations (e. Two graphite electrodes were connected to a D. 5% sodium carbonate electrolyte with two graphite carbon anodes. Which of the following equations is the correct equation for the cathode half-reaction in this electrolytic cell?. Aqueous Electrolysis In the electrolysis of a “molten” salt, the only possible half -reactions involve the ions of the salt. Cu 2+ is reduced at the anode. At an inert platinum anode, two oxidations are possible: hydroxideto oxygen, and/or silver(I) to silver(III). Active electrodes participate in the redox reactions of the cell. The electrolysis is generally conducted with platinum electrodes, of which the cathode takes the form of a piece of foil bent into a cylindrical form, the necessary current being generated by one or more Daniell cells. ELECTROCHEMISTRY MCQS Q. carbon) What happens:. Fundamentals Reactions at the cathode or anode Electrons flow from the battery to the cathode. 20 The diagram shows an electrolysis experiment using metals X and Y as electrodes. 54 describe experiments to investigate electrolysis, using inert electrodes, of aqueous solutions such as sodium chloride, copper(II) sulfate and dilute sulfuric acid and predict the products. This has been suggested as a way of shifting society towards using hydrogen as an energy carrier for powering electric motors and internal combustion engines. The Model: A Battery Used as an “Electron Pump” If a battery is used to “pump” electrons from one electrode to a second electrode, it is possible to force a non-spontaneous reaction to occur. 05μmaluminaslurryandapolishingpad,rinsed withdistilledwater,andwipeddryusingaKimwipe. The equipment used for electrolysis of a compound consists of three parts: a source of DC (direct) current; two electrodes; and an electrolyte. My analysis catechism "How can Beer's law be acclimated to verify Faraday's Aboriginal law of electrolysis and to actuate Avogadro's cardinal and Faraday's affiliated by electrolysis of 1. Magnesium chloride must be heated until it is molten before it will conduct electricity. 0M in AgNO3 and Fe(NO3)2. Graphite and platinum are examples of inert electrodes. Apparatus and chemicals. An aqueous solution of a compound contains (a) anions and cations of the compound. MUNISH KAKAR’s INSTITUTE OF CHEMISTRY S. Type 2 Electrolytic Cells – Electrolysis of Aqueous Salts and Non-reactive Electrodes. 00 hr using inert electrodes. The electrolyte is concentrated aqueous sodium chloride and under these circumstances chloride ions are discharged at the anode to form chlorine, while Hydrogen ions are discharged at the cathode, forming. Chapter 03: Electrochemistry of Chemistry-I book - Objectives After studying this Unit, you will be able to • describe an electrochemical cell and differentiate between galvanic and electrolytic cells; • apply Nernst equation for calculating the emf of galvanic cell and define standard potential of the cell; • derive relation between standard potential of the cell, Gibbs energy of cell. 7 v) is energetically more difficult than the reduction of water (-1. It might seem logical that electricity passed through a solution may result in a chemical reaction. It is that the electrodes materials nature has an influence, not only over their lifespan, but also on the hydrogen production and the energy consumption. Set-Up A: Inert Electrodes such as. the non-aqueous solvents acetonitrile and 1,2-dimethoxyethane. Explain why the blue colour of the copper sulphate solution does not fade during its electrolysis using Cu electrodes. Electrolysis of Copper(II) Sulphate Solution This experiment is designed to demonstrate the different products obtained when the electrolysis of copper(II) sulfate solution is carried out first with inert graphite electrodes and then with copper electrodes. An aqueous solution of copper sulphate, CuSO 4 was electrolysed between platinum electrodes using a current of 0. Quantitative electrolysis of aqueous copper(II) sulfate Demonstration This demonstration is designed to find the value of the Faraday constant – the amount of electric charge carried by one mole of electrons - from the electrolysis of aqueous copper(II) sulfate solution, using weighed copper electrodes. See Section 10. These electrodes do not interfere with the reactions occuring at the surface of the electrode, they simply act as a point of connection between the electrical circuit and the solution. This can be explained as follows:. The Electrolysis of Copper Sulphate Essay - The Electrolysis of Copper Sulphate Aim Analyse and evaluate the quantity of Copper (Cu) metal deposited during the electrolysis of Copper Sulphate solution (CuSo4) using Copper electrodes, when certain variables were changed. (iii) A dilute solution of H 2 SO 4 with platinum electrodes. Please explain the electrolysis of copper sulphate solution using platinum electrodes ,and explain why copper ion was preferencially discharged rather than hydrogen ion,and also were the hydrogen came from. Inert Electrodes are electrodes which do not react with electrolyte or products during electrolysis. The power supply was switched on and a potential difference of 12 volts was applied. For example, if you heat sodium chloride until it melts, it is called molten sodium chloride, but if you dissolve sodium chloride in water, it is called aqueous sodium chloride. Data are obtained in fields of up to 6 T. (b) hydrogen ions, H+ and hydroxide ions, OH- from the partial dissociation of water molecules. Type 112 silver / silver chloride reference electrode 0. In the electrolysis of aqueous sodium chloride using platinum electrodes, hydrogen ions are usually discharged preferentially. In the electrolytic cell (or electrolysis cell), the driving force is the electric current. Looking at the. CuSO4 using copper electrodes At the anode Cu Cu2+ + 2e- copper anode dissolves At the cathode Cu2+ + 2e- Cu copper metal deposited Electrolysis of Copper(II) Sulphate Solution. An aqueous solution of a compound contains (a) anions and cations of the compound. For each half-cell, the metal, which is called an electrode, is placed in the solution and connected to an external wire. However, the standard hydrogen electrode is often inconvenient to use as a reference electrode experimentally. The chorine gas is from the chloride in the salt. Instead, water molecules undergo reduction to give hydrogen gas. The important part of this demonstration of the electrolysis of water is that the volume of hydrogen produced is twice that of the oxygen. So can we use any other electrolyte instead of CuSO4?Since w. Note that the blue colour of the solution does not change. While inert and all those features that make it a perfect electrode, it is way too expensive to use platinum as an electrode for commercial purposes. It is difficult to maintain 1 atm pressure of H2 gas. Standard electrode potential When doing an electrolysis, you have to choose a qualified material used as electrodes. For example, if you heat sodium chloride until it melts, it is called molten sodium chloride, but if you dissolve sodium chloride in water, it is called aqueous sodium chloride. Solid copper is deposited on the cathodeD. Oxidation half-reaction:. Electrolysis of concentrated potassium chloride solution, Ag 2 SO 4 using silver electrode as anode and carbon electrode as. This is the case for producing sodium, potassium, calcium and aluminium metals. Describe experiments to investigate electrolysis, using inert electrodes, of aqueous solutions such as sodium chloride, copper(II) sulfate and dilute sulfuric acid and predict the products Place inert electrodes (ones that wont react) into an aqueous solution. The electrolysis of sodium hydroxide gives exactly the same products, hydrogen and. Electr­olysis is the process of using electr­icity to break down or decompose a compound (usually an ionic compound in the molten state or aqueous solution). Fundamentals Reactions at the cathode or anode Electrons flow from the battery to the cathode. One example of reactive electrodes changing the ionic discharge will be the electrolysis of Copper (II) sulphate using copper electrodes. Electrolysis of copper (II) sulphate solution using copper electrodes Ions present in the solution are Cu² + (aq), SO 4 ² - (aq), H+ (aq) and OH- (aq). At an inert platinum anode, two oxidations are possible: hydroxideto oxygen, and/or silver(I) to silver(III). Which changes are observed during the electrolysis of aqueous copper(II) sulfate using copper electrodes? 1 2 3 A pink solid is deposited on the negative electrode. 1, 23-29, 2005 0 2005 Electrochemical Polymerization of Furfural on a Platinwn Electrode in Aqueous Solutions of Potassiwn Biphthalate Jorge Luiz Joaquim Hallal, Alzira Maria Serpa Lucho, Reinaldo Simões Gonçalves* Institute of Chemistry, Federal University of Rio Grande do Sul. Consider the electrolysis of a neutral nickel(II) chloride aqueous solution using inert platinum electrodes, predict the electrode reactions VCE tutoring professionals in Mathematics, Chemistry, and Physics. An aqueous solution of copper sulphate, CuSO 4 was electrolysed between platinum electrodes using a current of 0. A dilute solution of sodium sulfate, Na 2 SO 4, was electrolyzed using inert platinum electrodes. Question 18: Predict the products of electrolysis in each of the following: (i) An aqueous solution of AgNO 3 with silver electrodes. (iii) A dilute solution of H­2SO4 with platinum electrodes. Predict the products of electrolysis in each of the following: (i) An aqueous solution of AgNO 3 with silver electrodes. I have an aqueous solution of. (b) hydrogen ions, H+ and hydroxide ions, OH– from the partial dissociation of water molecules. the reaction that occurs at the anode and the cathode are respectively. Electrolysis of aqueous sodium chloride yields hydrogen and chlorine, with aqueous sodium hydroxide remaining in solution. Sodium is made by the electrolysis of a molten mixture of about. Peak currents (i p) were measured with respect to the. reaction occurs (loss of electrons). (iv) An aqueous solution of CuCl 2 with platinum electrodes. (a) Electrolysis : The process due to which a chemical compound in the fused state or in aqueous state conducts direct electric current, resulting in the discharge of ions of an electrolyte into neutral atoms at the electrodes is called electrolysis. The bulb is lighted indicates that copper (II) sulphate is an electrolyte which can conduct electricity. electricity. The reference electrode the auxiliary electrode was a platinum wire counter electrode. Thus, reaction intermediates could desorb a bit more. In this process of electrolysis, we use a block of impure copper as anode or positive electrode, copper sulfate acidified with sulfuric acid, as electrolyte and pure copper plates coated with graphite, as cathode or negative electrode. If during electrolysis of copper sulfate, we use carbon electrode instead of copper or other metal electrodes, then electrolysis reactions will be little bit different. I assume you are referring to the electrolysis of copper (II) sulfate with copper electrodes. Using a cell containing inert platinum electrodes, electrolysis of aqueous solutions of some salts leads to reduction of the cations (e. 10 oxygen oxygen hydrogen hydrogen chlorine sodium chlorine- hydrogen sodium chlorine hydrogen chlorine The electrolysis of concentrate' hydrochloric acid using platinum electrodes is shown. Predict the products of electrolysis in each of the following: (i) An aqueous solution of AgNO 3 with silver electrodes. 10 volt (d) none of these. (i) Write equations for the oxidation and reduction half-reactions. 00 hr using inert electrodes. During the electrolysis of aqueous KCl solution using inert electrodes, gaseous hydrogen is evolved at one electrode and gaseous chlorine at the other electrode. Electrolysis Na2SO4 So there really isn't too much information out there on Na2SO4 in terms of reduction potential. Electrolysis of copper sulphate solution: inert electrodes. (a) LiCl(aq) (b) CuSO4(aq) (c) NaCl(l) (d) H2SO4(aq), using platinum as electrodes. (c) When aqueous copper(II) sulfate is electrolysed using platinum electrodes, copper(II) ions are reduced to copper at the negative electrode. With an inert anode, the sulfuric acid (or sulfate ion if using a reasonably alkaline salt) is oxidized to persulfuric acid (S2O8(2-) or SO5(2-) as the case may be). The electrode in the left half-cell is the anode because oxidation occurs here. Magnesium chloride must be heated until it is molten before it will conduct electricity. 0 A was passed through the electrolyte for 3 hours. 65 x 10 4 C mol-1 (or 96500 C mol-1 if you prefer). , metal deposition with, e. the electrolysis products of the aqueous salt solution are hydrogen at the negative (-) cathode electrode and oxygen at the positive (+) anode with inert electrodes such as carbon or platinum. efficiency in the electrolysis of pure zinc sulfate solu­ tions (65 gpl Zn++ - 200 gpl H2so4> were determined. 20 Case 3 Electrolysis of dilute sodium chloride solution using carbon electrodes 21. An electrode which participates in chemical reactions during Electrolysis is called Reactive Electrode. I have on many occasions electrolized an aqueous royal blue copper sulphate solution with my students to observe changes such as reduction of copper onto cathode and evolution of oxygen from anode. 001 mol dm −3 NaCl (aq) 1. A solution is 1. These electrodes do not interfere with the reactions occuring at the surface of the electrode, they simply act as a point of connection between the electrical circuit and the solution. 5 M Na 2 SO 4 aqueous solution (pH 7. 12/27/08 Electrolysis* Electrolysis _ - the use of electric energy to drive a nonspontaneous chemical. , applied voltage) is reached. using chemical equations, half-reactions, and diagrams. The name refers to the flow of anions in the salt bridge toward it. is present. Unformatted text preview: Timeline History of Fuel cells In 1748 Benjamin Franklin coined the term battery to describe an array of charged glass plates In the 1860s Georges Leclanche of France developed a carbon zinc wet cell nonrechargeable it was rugged manufactured easily and had a reasonable shelf life Also in the 1860s Raymond Gaston Plant invented the lead acid battery 1881 mile Alphonse. The reaction is catalysed by the platinum. When a solution of copper sulphate is electrolyzed using platinum electrodes, the products of electrolysis are copper at cathode and oxygen gas at anode. Sethuraman,1,* and John W. At the end of the electrolysis, the electrolyte was acidified with sulfuric acid and was titrated with an aqueous solution of potassium permanganate. In many processes that occur at metal inter-faces, such as electrolysis, corrosion and electrocataly-. The experiment is demonstrated and the results discussed. 0 A was passed through the electrolyte for 3 hours. Oxygen is formed at the positive electrode. Chapter 03: Electrochemistry of Chemistry-I book - Objectives After studying this Unit, you will be able to • describe an electrochemical cell and differentiate between galvanic and electrolytic cells; • apply Nernst equation for calculating the emf of galvanic cell and define standard potential of the cell; • derive relation between standard potential of the cell, Gibbs energy of cell. Rather, steel, graphite and titanium electrodes are used. Questions 18. Electrolysis of copper sulphate solution using platinum or carbon electrodes. electricity. Examples of reactive electrodes are copper, silver and gold. 2 electrodes - one is nichrome wire and the other is platinum wire and foil. The counter (auxiliary) electrode was a Pt wire, and the working electrodes were glassy carbon (0. POSSIBLE FACTORS WHICH COULD AFFECT THE MASS OF COPPER DEPOSITED OR LOST: There are in fact many factors that could affect the mass of Copper lost or deposited on the electrodes: * The current intensity or. % and maintaining a. You don't need specific metals for electrolysis, just a metal that conducts electricity, and the two electrodes don't need to be different metals (as they do if you were creating an acid battery). This is the equilibrium that we are going to compare all the others with. 20 The diagram shows an electrolysis experiment using metals X and Y as electrodes. ELECTROCHEMISTRY MCQS Q. a) Write the equation for the reaction which took place at the anode b) Calculate the mass of silver deposited. 1 Answer to in the electrolysis of dilute sulphuric acid using platinum electrodes, the product obtained at the anode and cathode are - 15963 Home » Questions » Management » Supply Chain Management / Operations Management » Linear Programming » electrolysis: In the electrolysis of dilute. Hydrogen Production by Water Electrolysis Effects of the Electrodes Materials Nature on the Solar Water Electrolysis Performances 2. What are the electrolysis product of CuSO4 using platinum electrode and using copper electrode? Platinum is a non- attacked type electrode In this case at cathode Cu+2 + 2e- Cu At anode 4OH- 2H2O + O2 + 4e-In this case concentration will change. 7 ampere is passed for 6 hours between platinum electrodes in 0. The electrodes use metals that are not easily corroded, such as gold, platinum or carbon. H2 at the cathode and O2 at the anode. Electrolysis of copper sulphate solution: inert electrodes. A SIMPLE explanation of Electrolysis of Copper Sulphate Using Copper Electrodes. Sodium is made by the electrolysis of a molten mixture of about. (The salt is needed to produce ions. Mass of the cathode decreasesC. When an electrolyte is dissolved in water, it splits up into charged particles called ions. 500 ampere was passed for 16 minutes and 5 seconds. Aqueous zinc chloride is electrolysed using platinum electrodes. Salt's chemical formula is NaCl - sodium chloride. HICKLING AND M. Whereas, the K + ions cannot be reduced in presence of water. The products of electrolysis can be predicted for a given electrolyte. [AFMC 1995]Use of electrolysis is (a) Electroplating (b) Electrorefining (c) (a) and (b) both (d) None of these 30. 02 cm 2 ) in disc or microelectrode (10 μm diameter or 7. De Castro, Y. 1 Standard hydrogen electrode. 000 mol dm-3 chestnut sulfate (CuSO4) band-aid application graphite electrodes?" is an aberrant catechism to the investigation. Solution: What mass of platinum could be plated on an electrode from the electrolysis of a Pt(NO3)2 solution with a current of 0. Considering that pure neutral water is usually electrolysed in PEM electrolysers, neutral electrolyte, 0. Explain why the blue colour of the copper sulphate solution does not fade during its electrolysis using Cu electrodes. 7 v) is energetically more difficult than the reduction of water (-1. During the electrolysis of an aqueous solution of CuSO4 using inert electrodes. The electrodes were immersed into a small beaker with 20 mL of 2 to 20 mM HAuCl 4 in deionized water. Materials: Hoffman electrolysis apparatus. Photoreduction of CO/sub 2/ and its aqueous forms to organic products is a challenging subject as a means of mimicking photosynthesis and solar energy conversion and storage. Electrolysis of Copper(II) Sulphate Solution This experiment is designed to demonstrate the different products obtained when the electrolysis of copper(II) sulfate solution is carried out first with inert graphite electrodes and then with copper electrodes. In this report the thermodynamic potential for the anode, E° OH-/O 2) 0. 65 x 10 4 C mol-1 (or 96500 C mol-1 if you prefer). Active Electrodes are electrodes which react with products of electrolysis, affecting the course of electrolysis. 2Cl- - 2e- Cl 2 (chlorine gas at the (+)anode). An aqueous solution of Na2SO4 is electrolysed by using inert electrodes, the products at cathode and anode are respectively [BPKIHS 2005] a. 500 ampere was passed for 16 minutes and 5 seconds. The Electrolysis of Aqueous NaCl The figure below shows an idealized drawing of a cell in which an aqueous solution of sodium chloride is electrolyzed. 7th Jul, 2018 2-The composition of the aqueous solution. 15mol/l CuSO4 solution using platinum electrodes, 0,16g of oxygen gas evolved at the anode. That difference in the positions of equilibrium causes the number of electrons which build up on the metal electrode and the platinum of the hydrogen electrode to be different. Martelli, and F. Electrolysis of CuSO 4 Using Inert Electrodes (e. Electrolysis definition is - the producing of chemical changes by passage of an electric current through an electrolyte. stop one oxygen gas 40H(aq) - anode + cathode — Microsoft Word - Electrolysis_inert_electrodes. However, in the particular case of aqueous HCl electrolysis, the use of a platinum-based catalyst as the cathode poses some serious drawbacks. The activation of the Pt electrode was tested by cyclic voltammetry (CV) in 0. I know that the sulfate ions will remain in the solution, but aren't the \$\ce{H+}\$ ions of \$\ce{H2SO4}\$ reduced at the cathode as well?. a) the anode loses mass and the cathode gains mass b) the mass of the anode decreases but the mass of the cathode remains constant c) the mass of the anode remains the same, but the cathode gains mass d) the anode and the cathode neither gain nor lose mass. Which changes are observed during the electrolysis of aqueous copper(II) sulfate using copper electrodes? 1 2 3 A pink solid is deposited on the negative electrode. The magnitude of these overvoltages varies with current and also with the composition of the electrode, and is frequently high enough to inhibit the gas discharge. • Copper(II) sulphate, CuSO4 solution consists of Cu2+ ions, H+ ions, Cl2- ions and OH- ions that move freely. Therefore, an electrolytic cell arranged concentrically with extended cathode surface areas was designed to improve the rate of mass transfer. 1 Electrolysis is the process in which a chemical reaction takes place at the expense of (a) chemical energy (b) electrical energy (c) heat energy (d) none of these Q. electrolytic cell that has inert electrodes. Because only the electrodes are shown in the videos, it is important to show these still images. Active vs Inactive electrodes : Electrolysis of aq NaBr solution (initially PH = 7) Cathode : Na+(aq) + eŒ 0 Na(s) E = Œ 2 V 2eŒ + 2H. Predict the products of electrolysis in each of the folloiwng: (i) An aqueous solution of AgNO3 with silver electrodes (ii) An aqueous solution of AgNO3 with plantinum electrodes (iii) A dilute solution of H2SO4 with platinum electrodes - Chemistry - Electrochemistry. Active Electrodes are electrodes which react with products of electrolysis, affecting the course of electrolysis. Researchers have boosted the efficiency of water electrolysis. Abstract Electrolysis of metal ions in dilute solutions using vertical planar electrodes results in low recovery. Red metal copper deposits at the cathode and colourless odourless gas oxygen at the anode. Solutions for Chapter 10 End-of-Chapter Problems Problem 10. Brine (concentrated aqueous NaCl) using inert graphite electrodes The experiment is demonstrated and the results explained in detail. If the negative ion from the ionic compound is simple (eg Cl-or Br-), then that element is produced. the reaction that occurs at the anode and the cathode are respectively. 1 Standard hydrogen electrode. Graphite or platinum is usually used as electrodes because they are inert (do not react with electrolytes or products of electrolysis). When a solution of copper sulphate is electrolyzed using platinum electrodes, the products of electrolysis are copper at cathode and oxygen gas at anode. Does an oxide layer form on the anode during the electrolysis of aqueous NaOH solution ? as an anode and a platinum electrode as cathode. It has good corrosion-resistance, high overpotential for the oxygen evolution reaction, strong ability of oxidation in aqueous solution electrolysis, big current density, suitable for all kinds of oxygen evolution system conditions, which now has been widely used in electroplating, hydrometallurgy. The platinum electrode is easily poisoned by traces of impurities. Thin platinum or gold wire electrodes have been made down to micron diameters. H2 at the cathode and I2 at the anode. Similar to the steel anode experiment, bubbles quickly formed on both the anode and the cathode. 2H 2 O → 2H 2 + O 2. An aqueous solution of Na2SO4 is electrolysed by using inert electrodes, the products at cathode and anode are respectively [BPKIHS 2005] a. Pour 1 M K I solution in Petri dish. Two types of electrodes are in common use, namely, (1) thin-film electrodes made by coating a transparent substrate with metals (platinum, gold, silver, mer­ cury)4-6 or doped oxides (tin oxide or indium. The only change at the cathode was a slight change in the color of the solution. The conductance of aqueous liquids is a constant for brief measurements at low voltage. The electrolysis of dilute aqueous solution of Na 2 SO 4 produces at anode and cathode respectively using Platinum electrodes. Usually, inert electrodes such as graphite or platinum are used for electrolysis. It is also an extremely stable material even in the. C O P Cu2 P e r H. 001 mol dm −3 NaCl (aq) 1. Therefore, prolonged exposure to organic solvents should typically be avoided, and the stability of the reference potential should be regularly checked (by using an internal reference or by comparing with another reference electrode). Pi Bond Model Kit : This molecular model kit is large enough to be visible by a large lecture class. In electroplating the cathode may be the metal that needs to be plated and in purification of metals, the anode may be an impure metal- e. (a) When a concentrated aqueous solution of Sodium Chloride is electrolysed using inert electrodes, a different gas is produced at each electrode. At cathode, copper (II) ions are preferentially discharged than H+ ions to give copper metal since copper (II) ions are of lower reactivity than hydrogen ions. 01 V During the electrolysis of an aqueous solution of Na2SO4, which reaction occurs at the (platinum) anode?. During the electrolysis of an aqueous solution of CuSO4 with inert electrodes (A) the anode loses mass and the cathode gains mass. depolarizing electrode an electrode that has a resistance greater than that of the portion of the body enclosed in the circuit. evolution of bromine with bromides). Electrolysis of aqueous solution of using Cu electrodes: Thus ionisation of CuSO4 may be given as: It is the concept of electroplating that Cu-metal is liberated at cathode. In cell notation the electrode is written as:. electrolysis - (chemistry) a chemical decomposition reaction produced by passing an electric current through a solution containing ions. The electrolysis of sodium chloride solution (brine) Aqueous solutions with inert electrodes (carbon or platinum) The products of electrolysing aqueous sodium chloride solution are hydrogen gas, chlorine gas and sodium hydroxide solution. 2 Br - - 2 e - Br 2 ( bromine gas at the ( +) anode ). Electrolysis Of Aqueous Cuso4 Using Platinum Electrodes.