Electrolysis of copper sulphate equation. The electrolyte used is copper sulfate solution. or. 7. (b) What is seen to happen to the colour of the copper sulphate solution 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. 1 19. Galvanic cell produce electricity from chemical reactions. At the positive electrode (anode) bromine gas is produced by the discharge of bromide ions: 2Br- – 2e– Br2. (iv) When dilute sodium chloride is electrolysed using graphite electrodes, the cation which is discharged at the cathode most readily. If we connect the zinc and copper by means of a metallic conductor, the excess electrons that remain when Zn 2 + ions emerge from the zinc in the left cell would be able to flow through the external circuit and into the right electrode, where they could be delivered to the Cu 2 + ions which become "discharged", that is, converted into Cu atoms The principles of the electrolysis of copper (II) sulphate or any other soluble copper (II) salt is an important aspect of electrolysis applied in the indust Slide 1 of 3, Beaker with pure and impure copper rods dipping into copper(II) sulfate solution. At the cathode, water is reduced to OHX− O H X − and makes the solution more alkaline. At the positive electrode (anode) chlorine gas is produced by the discharge of chloride ions: 2Cl– – 2e– Cl2 Oxidation. A dilute aqueous solution of copper sulfate and sulfuric acid is used as the electrolyte. Electrolysis can only be used if the compound can Ammeters (0-1 A), DC, 3. Method. To avoid confusion, electrolysis should be introduced at the basic level by looking at the electrolysis of molten substances, coupling the theory with a video or teacher negative terminal of the battery. 2 H 2 O (l) + electrical energy → 2 H 2 (g) + O 2 (g) Thus, the water electrolysis reaction shows the separation of hydrogen and oxygen from water. As far as the mechanism of the process is concerned, during electrolysis, a large chunk or slab of impure metal is used as the anode, with a thin strip of pure metal as the cathode. An electric current is provided by a 9 volt (V) battery. Pour copper sulfate solution into a beaker. For two moles of water, two moles of hydrogen and one mole of oxygen are liberated. Health & Safety and Technical Notes. Why are acids, bases and salts classified as Copper electrodes: 1. Electrolysis of molten lead (II)bromide. Aqueous sodium chloride solution using platinum electrodes. Electrolysis of the new solution. The half equation is: Cu2+ + 2e- → Cu . Mar 21, 2021 · In short, the aim of my experiment is to determine how the concentration of sulphuric acid in solution affects the mass liberated and deposited at copper electrodes, when copper sulphate is electrolysed. Some reactions will, instead, use electricity to get a reaction to occur. Explain your answer. The Oct 7, 2018 · In aqueous solution the anode will oxidize the water instead, as this reaction can be done at much lower potential than oxidizing the sulfate ion. charco Study Forum Helper. Technician notes and integrated instructions are offered for this experiment. The process of decomposing ionic compounds into their constituent components by passing an electric current through them in an aqueous or molten form is known as electrolysis. A. dime serves as the cathode (a dime, versus another penny, makes the movement of copper more obvious). It'll breakdown into CuO and SO3 before it melts. 5 g of copper. Saturated copper sulfate solution is harmful. When discussing copper sulfate, we can safely assume we are dealing C6 - Electrolysis Ionic equations Half equations can be combined to form an ionic equation, which shows the overall reaction. So if you got copper ions into solution at the anode, you The half-equations for the electrolysis of copper(II) sulfate solution. Top-pan chemical balance with a sensitivity of no less than 0. The electrolyte is a solution of copper (II) sulfate. In this setup, an electrolyte (metal salt aqueous solution The influence of concentration of the ions. At the positive electrode (anode) bromine gas is produced by the discharge of bromide ions: 2Br-– 2e – Br 2. Since solid pieces of copper are involved, Cu must be considered in the reduction potential as well. The above mentioned drawbacks do not occur with sodium sulfate. 32 × 106C. What equation shows the reaction at the anode during the electrolysis of copper sulfate solution using inert electrodes? S O S O + O + 2 e 2 – 4 2 2 – C u C u + 2 e 2 + – S O + O + 2 e S O 2 2 – 2 – 4; 4 O H 2 H O + O + 4 e – 2 2 – 2 H + 2 e H + – 2; Answer . 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. Oct 27, 2022 · The amount of Cr is then. Predict the products of electrolysis in the following. Next, the copper ions from the electrolyte are deposited at the cathode. During the electrolysis of copper sulphate aqueous solution using copper electrode, the reaction taking place at the cathode is: Q. [Cu 2+ , OH 1- , SO 4 2- , H + ]. Jan 19, 2015 · During the electrolysis of copper (II) sulfate, or CuSO4, the deposition of copper can be seen on the cathode; at the same time, the anode will be dissolved by the process. Electroplating - A process in which electrolysis is used as a means of coating an object with a layer of metal. Additionally, the copper sulfate electrolyte solution contains copper in the form of positively-charged cations, which are also attracted to the negative electrode (the cathode, a dime). Attach one electrode to the negative terminal of a dc supply, and the other electrode to The overall balanced equation close balanced chemical equation A chemical equation written using the symbols and Practical- electrolysis of copper sulfate solution. A series of free IGCSE Chemistry Activities and Experiments (Cambridge IGCSE Chemistry). A dilute solution of sodium sulphate in water is electrolysed using Pt electrodes. The negative cathode electrode attracts C u 2 + ions (from copper sulfate) and H + ions (from water). 7–1. 56molCr. Aluminium came in contact with air. As before, we would expect hydrogen ion to be preferentially discharged at the cathode before the sodium ion: 2H + (aq) + 2e - → H 2 (g) Eθ = 0. For example in the electrolysis of copper chloride the two half equations are: At the negative electrode (cathode): 2+ + 2 e- —> Cu At the positive electrode (anode): 2Cl- —> Cl 2 + 2 e- Assertion: Starting from aq. Some of the impurities are metals such as Fe and Zn which are more easily oxidized than Cu. molCr = 237 gCr × 1molCr 52. c. In practice, the products of electrolysis are usually simpler than the reactants, hence the term electro- lysis. Copper(II) ions are deposited as copper on the cathode (for the electrode equation, see under the purification of copper below). aqueous solutions of ionic compounds close ionic compound An ionic compound occurs when a Apr 18, 2020 · These sulfate ions do not deliver electrons. 1. In the electrolysis of molten lead(II) bromide the half equation at the negative electrode (cathode) is: Pb 2+ + 2e – Pb. The total charge is then. Figure 11. Place two graphite rods into the copper sulfate solution. Protic hydrogen (or the metal in the cation if this metal is not highly electropositive like magnesium) is reduced more easily at the cathode, and water is more easily oxidized at the anode. Place the copper el ectrodes in the beaker (see figure 2). Answer: During electrolysis of aqueous copper sulphate using copper electrodes, the two anions OH – . Electrolysis. copper [II] sulphate solution, equations for the reactions at the cathode and anode during electrolysis of aq. Record the masses. In the electrolysis of molten lead (II) bromide the half equation at the negative electrode (cathode) is: Pb2+ + 2e– Pb. The reactions at each electrode are called half equations. Electrolysis of Copper (II) Sulphate Solution. Cu2+(aq) + 2e–), so deduce the quantity of electricity equivalent to one Write down the ionic equation for the reactions that take place at the cathode during the electrolysis of an aqueous solution of nickel sulfate. Observations at the anode and cathode. Previous page. Using electrolysis, the accumulation of Cu(I) in the plating solutions was also confirmed. Required current = 3860 C / (10*60 s) Total charge due to the flow of electrons= 6. 6. It is the metal of the anode, copper, that donates 2 electrons, producing a copper ion $\ce{Cu^{2+}}$ and this ion attracts the sulfate ion arriving at the anode. > After running for about half an hour Oct 6, 2018 · Electrolysis of copper sulfate solution, using inert, graphite electrodes. Oct 27, 2020 · So you better use a solution of sodium sulfate $\ce{Na2SO4}$ instead of sodium carbonate. It makes a solution of copper sulfate. Q. 2Br- Br2 + 2e–. The cathode increases in mass while the anode decreases Examples of Electrolysis [1-4] 1. 7) Predict how the concentration of the copper(II) sulfate solution changes, if at all, as the electrolysis takes place. Passing an electric current through a specially prepared copper chromate solution results in the migration of two coloured ions. Time for ten minutes ; remove and dry, weigh and record result ; Evaluation (iii) The ion which is discharged at the anode during the electrolysis of copper sulphate solution using copper electrodes as anode and cathode. 635 g of copper. A similar change happens if you electrolyse copper (II) sulphate solution using copper electrodes. The answer key says that zinc would be formed at the cathode. 18 × 10-3 mol Determine the moles of Cu (s) produced using the balanced reduction reaction equation : During the electrolysis of aqueous copper sulphate using copper electrodes, copper ions are generated at the anode, that go into the copper sulphate solution used as electrolyte. Jul 11, 2018 · The formation and accumulation of Cu(I) in copper sulfate electroplating solutions are discussed. In a $\ce{Na2SO4}$ solution, the ions $\ce{Na+}$ are moving towards the negative electrode (cathode), and the ions $\ce{SO4^{2-}}$ are moving toward the positive electrode (anode). The negative cathode reaction with graphite electrodes. The half equation for the reaction at the anode is 4OH – O 2 + 2H 2 O + 4e – Using copper electrodes: Apparatus for the electrolysis of copper(II)sulfate using active copper electrodes. The salt bridge prevents the copper ions from migrating to the zinc compartment. Video:19. Oct 15, 2014 · Describe how zinc metal can be obtained from zinc sulfate solution by electrolysis. During the electrolysis of copper sulfate ( CuSO 4) solution using copper electrodes, the copper metal ( Cu) deposits at the cathode give reddish-pink color. When current is passed through the electrolyte Solution. (i) Which electrode to your left or right is known as the oxidizing electrode and why? (ii) Write the equation representing the reaction that occurs Assertion: Starting from aq. Demonstration of electrolysis of aqueous sodium sulfate (using universal indicator) and of aqueous potassium iodide (using phenolphthalein indicator) with inert electrodes. Slide 1 of 3, Beaker with pure and impure copper rods dipping into copper(II) sulfate solution. e. 00gCr = 4. Electrolysis of sodium chloride solution produces results at each electrode. Since the solution contains chromium (III) ions, 3 moles of electrons are required per mole of Cr. 4 years ago. The electrolytic refining of copper is done using the apparatus shown in the figure. The following questions refer to the electrolysis of copper sulphate solution with copper electrodes: (a) Compare the change in mass of the anode. 3. In this case, that's the copper, so start with the electrode equation. 19g cm3 = 237 gCr. Electrolysis involves passing an electric current through either a molten salt or an ionic solution. Reaction of sulfate ion in copper sulfate electrolysis. MathJax reference. Examples of such electrolytes are sulfuric acid (H 2 SO 4) and salt of sodium nitrate (NaNO 3 ). 2Br- Br 2 + 2e – The overall chemical reaction is. (Half equations only required. When a solution of copper(II) sulfate is electrolysed using graphite electrodes, copper metal is formed on the cathode by reduction of copper ions in the sol Write equations for the reactions taking place at the two electrodes (mentioning clearly the name of the electrode) during the electrolysis of: (i) Acidified copper sulphate solution with copper electrodes. Acidified copper sulphate solution with copper electrodes. The second part of this investigation covers the products formed during 5 days ago · - Electrolysis is the process in which an electrolyte, in this case copper sulphate solution, undergoes redox reactions at the electrodes due to the action of electric current. Electrolysis of molten lead(II)bromide. 2 x 96500 coulombs give 63. This page looks in detail at the electrolysis of copper (II) sulfate solution using copper electrodes and silver nitrate solution using a silver anode. Write down the important bits of this in words: 2 mol of electrons give 1 mol of copper, Cu. In such a cell a thin sheet of high-purity Cu serves as the cathode, and the anode is the impure Cu which is to be refined. They move Feb 15, 2021 · 3. Figure 17. Note the reduction in the blue colour of the solution, the change in colour of the litmus paper and the changes in the test solutions (KI(aq) and KBr(aq)). Electrolysis of alumina is done. 1 mol of electrons is 1 faraday. Now put the numbers in. Oct 21, 2018 · 1. 3 Deduce from 1 and 2 the charge required to remove one mole of copper. during the electrolysis of concentrated sodium sulfate Electrolysis. 2Cl– Cl2 + 2e–. It is very important to make a distinction between the labelling of the cathode in electrolysis and in galvanic cells, as most of the time this causes a bit of confusion. , Purifying copper by electrolysis 1. Applying an external potential of about 1. The half-equations for the electrolysis of copper(II) chloride solution (the electrolyte) (a) The negative cathode electrode reaction for the electrolysis of copper(II) chloride solution. Activities. This reaction can be represented as, \[CuS{{O}_{4}}\rightleftharpoons C{{u}^{2+}}+SO_{4}^{2-}\] A. Assertion: Starting from aq. $\endgroup$ Sulfate ions and hydroxide ions (from the water) arrive. Measure the mass of a copper electrode and attach to the negati ve terminal of the power supply. Electrolysis of water - why not pure water? 4. The sulfate ions are difficult to discharge, and so hydroxide ions are discharged to form oxygen gas. Copper hydroxide is a blue, bulky precipitate, feebly acidic, and soluble in concentrated alkali hydroxide solutions. Theoretically 1 Calculate the number of moles of copper removed from the anode (weight lost (g)/ Ar[Cu]). Potassium peroxydisulfate can be prepared by electrolyzing a solution of potassium bisulfate ($\ce{KHSO4}$) in sulfuric acid solvent. This involves setting up an electrolysis to investigate the effect of changing the current on the mass of the copper electrodes used in the electrolysis of copper sulfate solution. Study the diagram given alongside and answer the questions that follows. 00 V. The electrolysis of aqueous solutions of ionic compounds using non-inert electrodes. . and S0 4 2- migrate to the anode, but none of them get discharged because the copper of the This flash animation takes a fairly in-depth look at the electrolysis of aqueous copper (II) sulfate and its use to refine blister copper by electrolytic re Assertion: Starting from aq. Include all the products of this electrolysis. Ionic equation for the electrolysis of Copper(II) chloride. mass = volume × density = 33cm3 × 7. 1: The electrolytic purification of copper. 2. An electrolytic cell is in this sense the opposite of a galvanic cell. Repeat with a second copper electrode, attaching it to the positive terminal. The hydroxide ion is more reactive than the sulphate ion, therefore this forms water (H2O) and oxygen at the positive electrode. (iii) State two appropriate observations for the above electrolysis reaction. Distilling sulfates was the ancient method for making sulfuric acid (oil of vitriol) The ancient name for copper (II) sulfate was blue vitriol. The number of moles of hydrogen generated is twice the oxygen. (a) Give reason: The electrolysis of acidulated water is considered to be an example of catalysis. The accumulation rate and amount depend on the current density and electrolysis time and the dissolved gases. If you haven't recently done so you should first read the page about the electrolysis of solutions using Feb 23, 2024 · Question 16: During the electrolysis of aqueous copper sulphate, between copper electrodes, the sulphate and hydroxyl ions remain as spectator ions. 3. There are two copper blocks sitting in the Cu(NOX3)X2(aq) solution, a battery is attached onto both of them, providing enough energy to start the reaction. A beaker with pure and impure copper rods dipped into copper Write chemical equation for the following events. Read the following in conjunction with the 'concept diagram' for the electrolysis of copper sulfate solution with copper electrodes, after the electrode equations. b. This is a standard electrolysis setup, where the impure copper (the sample to be refined) is placed as anode and a thin strip of pure copper is placed as a cathode. Iron filings are dropped in aqueous solution of copper sulphate. Batteries, 12 V, 3. Oxygen will be form as Copper sulphate breaks down to give Copper oxide , Sulfur di oxide and O2. In the electrolysis of aqueous copper (II) sulfate the half equation at the negative electrode (cathode) is: Cu2+ + 2e– Cu Reduction. A labelled diagram is acceptable. Zinc oxide is dissolved in dilute hydrochloric acid. As current is passed through the solution, positive copper ions, Cu 2+, in the solution are attracted to the negative cathode, where they take Jul 20, 2016 · Use MathJax to format equations. Aqueous copper sulphate solution using platinum electrodes. Positive Anode (penny): Cu (solid) Cu2+ (aqueous) + 2 e- Negative Cathode (dime): Cu2+ (aqueous) + 2 e- Cu (solid) The electrolysis of copper (II) sulphate solution using a copper anode. The cathode is a sheet of very pure copper. Q4. In electrolysis of aqueous solutions sulfate ions just sit there. The ions are "forced" to undergo either oxidation (at the anode) or reduction (at the cathode). penny acts as the copper source/anode and a U. Nov 13, 2022 · In electrolysis, an external power source supplies the free energy required to drive a cell reaction in its non-spontaneous direction. ) Jul 19, 2023 · 1. OR. The overall balanced equation close balanced chemical equation A chemical during the electrolysis of copper chloride solution. Electrolysing close electrolysis The decomposition (breakdown) of a compound using an electric current. - When copper sulphate dissociates to form cupric ions and sulphate ions. 1: This 2:54 minute video shows the spontaneous reaction between copper ions and zinc. The balanced half equation is: Al 3+ + 3e-→ Al (because three negatively charged electrons are 6) Write the equation for the reaction occurring at the cathode. The electrolysis equation describes the relation: m = Z × Q. 3: The Electrolysis of Water. 9 V to two inert electrodes immersed in an aqueous solution of an electrolyte such as H 2 SO 4 or Na 2 SO 4 drives the thermodynamically nonspontaneous decomposition of water into H 2 at the cathode and O 2 at the anode. Where: m is the mass in kg (kilogram); Q is the charge in C (coulomb); and Electrolysis - A chemical reaction brought about by an electric current. Electrolyte: saturated solution of copper sulfate to which is added 5 per cent IM sulfuric acid. Sulfate ion (actually, bisulfate ion) can be oxidized electrolytically at the anode if Scrub copper electrodes with wire wool ; Rinse in distilled water ; Dry with propanone ; Weigh and record anode and cathode ; Put into circuit ate set current value, with crocodile clips, making sure the clips are not touching the copper sulphate. It is the same copper sulfate that has been dissolved in the solution to be electrolyzed. Q = 4. 01 g. Jun 16, 2017 · Figure 2: Microscale electrolysis of copper(II) chloride solution, before (left) and after (middle). Only the copper ion is discharged, being reduced to copper metal. Reasoning Based Questions. The half-equations for the electrolysis of copper(II) sulfate solution. a. The copper sulfate solution decomposes, and copper ions visibly collect at the cat Aug 3, 2022 · Electrolysis of copper (II) sulphate solution. Pour some copper sulfate solution into a beaker. 43 A; A copper sulphate solution (100 cm 3) is electrolyzed using graphite electrodes. Over all data points, what I observed is that the mass deposited at the cathode was lower than the mass liberated at the anode. Rheostats (10-15 ohms), 3, rated to carry at least 1 A. However, looking at the half reaction for copper: Cu(s) CuX2 + (aq) + 2eX − (E ∘ Jun 30, 2007 · The electrolysis of copper(II) chromate(VI) Copper chromate is a dark green solid, which can be bought or made by mixing copper sulfate with potassium chromate. Copper is deposited at the cathode as you would expect, but instead of oxygen being given off at the anode, copper (II) ions go into solution. 56molCr × 3mole − 1molCr × 96485C mole − = 1. C u S O 4 using active copper electrodes is; In a spontaneous reaction electrons leave the zinc, go through the wire and are then taken up by the copper ions. The electrolysis of sodium chloride solution provides an illustration of the influence of concentration on the products discharged. In this experiment, a U. (ii) Molten lead bromide with inert electrodes. S. 8) Why is it better to use the loss in weight of the anode as opposed to the gain in weight of the cathode? Assertion: Starting from aq. 2 Calculate the charge which has been passed through the electrolyte in Coulombs (current (A) x time (s)). The electrolysis is similar to that of copper (II) sulfate solution with inert electrodes. A reaction was brought about between ferric oxide and aluminium. Step 3: Calculate current by using the equation of Q = It; Q = Charge , I = current , t = time of electrolysis. Copper sulphate solution is electrolysed using copper electrodes. Ans. View Solution. Electrolysis is the process by which a compound can be broken down or split into its elements by passing an electrical current through the sample. Electrolytic refining is a process of refining a metal (mainly copper) by the process of electrolysis. Apr 19, 2021 · (c) Write equations for the reactions taking place at the two electrodes (mentioning clearly the name of the electrode) during the electrolysis of : 1. The positive copper(II) ions Cu 2+ (from copper sulfate) and the H + ions (from water) are attracted to the negative cathode. Molten lead bromide with inert electrodes. C u S O 4 using active copper electrodes is; at anode: C u + 2 + 2 e − → C u at cathode: C u → C u + 2 + 2 e − Reason: Oxidation always take place at anode and reduction at cathode. Electrolysis separates the molten ionic compound into its elements. Water (H 2 O) Water can undergo electrolysis in the presence of an electrolyte like acid or base. Chemical equation : CuSO 4 ( aq) → Cu 2 + ( aq) + SO 4 2 - ( aq) copper Write the reduction reaction equation for the production of copper metal from molten copper sulfate: Cu 2+ + 2e-→ Cu (s) Calculate the moles of electrons, n(e-): n(e-) = Q ÷ F = 500 ÷ 96,500 = 5. Therefore, for each copper ion discharged at the cathode, a copper ion is generated at the anode. Attach one electrode to the negative terminal of a dc supply, and the The practical experiment shown in this video is the electrolysis of aqueous copper (II) sulfate. The power is switched on and adjusted to deliver a small current. Copper sulphate solution is electrolyzed using copper electrodes. Suitable solutions include copper sulfate, copper chloride, sodium chloride, sodium nitrate, sodium The electrolysis of copper sulfate solution can easily be done in the lab using the set-up shown in Figure 2: > Before setting up the experiment, the two copper electrodes are weighed accurately. (i) At the positive ( +ve ) anode , the process is an oxidation , electron loss from copper atoms, as the copper atoms of the positive anode electrode dissolve to form blue copper(II Learn about and revise electrolysis with this BBC Bitesize GCSE Chemistry (AQA) study guide. > Copper sulfate is used as the electrolyte. On electrolysis of aqueous N a C l solution using platinum (P t) electrodes, the product obtained at anode will be Q. A beaker with pure and impure copper rods dipped into copper(II In the electrolytic refining of copper, the impure copper is made from the anode in an electrolyte bath of copper sulfate, CuSO 4, and sulfuric acid H 2 SO 4. The overall balanced equation close balanced chemical equation A chemical equation written using the symbols and Practical- electrolysis of copper sulfate solution. Balance the half equation for the formation of aluminium during electrolysis: Al 3+ + e-→ Al. Electrolysis Electrolysis of aqueous copper (II) chloride. Electrolysis oxygen gas will form at the positive electrode: 4OH - (aq) → 2H 2 O (l) + O 2 (g) + 4e -. Electrolysis is a process in which a compound gets dissociates into ions in the aqueous or molten state. 1 17. The half equations are written so that the same number of electrons occur in each equation. Potassium chloride must be heated until it is molten before it will conduct electricity. d. Explain, why during the electrolysis of copper sulphate using copper electrodes, the colour of solution does not fade. Electrolysis of (i) copper sulfate solution with copper electrodes and (ii) acidified water with inert electrodes. Cu 2 + (aq) + 2 Cl-(aq) → Cu (s) + Cl 2 (g) The reaction at the cathode: The Copper ions Cu 2 + have the Aug 18, 2021 · Copper is less reactive than hydrogen, so copper (Cu) is produced at the negative electrode. Right: a close up of the copper metal deposited on the carbon fibre negative electrode Concepts covered in ICSE Class 10 Chemistry Part 2 chapter 6 Electrolysis are Preferential Or Selective Discharge of Ions at Electrodes, Examples of Electrolysis, Electrolysis of Molten Lead Bromid, Electrolysis of Acidified Water Using Platinum Electrodes, Electrolysis of Copper Sulphate Solution Using Platinum Anode and Copper Or Platinum Electrolysis of Potassium Chloride. (b) During the electrolysis of copper [II] sulphate solution using platinum as cathode and carbon as anode (i) State what you observe at the cathode and at the anode (ii) State the change noticed in the electrolyte Jan 18, 2024 · The first Faraday's law for electrolysis is an equation that links the mass of a chemical species added or removed at an electrode and the charge in an electrolytic cell. 5. 4OH-(aq) O 2 (g) + 2H 2 O(l) + 4e-If you let this electrolysis run for a long time, the colour of the copper(II) sulfate fades, and eventually bubbles of hydrogen are formed at the cathode. Sulfates can be oxidized if you take the water away. ‘Electro’ refers to the use of electricity and ‘lysis’ refers to breaking down or splitting. Most electrolysis problems are really stoichiometry problems with the addition of an amount of electric current. You need to work out how many coulombs give 0. The presence of acid improves the electrical conductivity by increasing the hydrogen ion (H +) concentration. dk ka ka vg vh uj fr cc lk fz