Concentration of ions in the solution
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The document describes the electrolysis of a 1.0 mol/dm3 sodium chloride solution using carbon electrodes. During electrolysis, sodium and chloride ions move to the cathode and anode respectively. At the cathode, hydrogen ions are discharged to produce hydrogen gas while at the anode, chloride ions are discharged to produce chlorine gas. The solution becomes alkaline after electrolysis due to the presence of sodium hydroxide.
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This document describes the electrolysis of a copper(II) sulfate solution using copper electrodes. During electrolysis, copper ions and hydrogen ions move to the cathode where copper ions are discharged to form a brown copper deposit, while hydroxide and sulfate ions move to the anode where the copper electrode dissolves to release copper ions and electrons. The process results in the cathode gaining mass and thickness while the anode loses mass and becomes thinner, but the concentration and blue color of the copper ions in the solution remains unchanged.Electrolysis molten sodium chloride
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The document summarizes the process of electrolysis for two types of electrolytes: molten sodium chloride and aqueous electrolytes. For molten sodium chloride, sodium and chloride ions move to the cathode and anode, respectively, where they are discharged. Sodium forms at the cathode while chlorine gas forms at the anode. For aqueous electrolytes like dilute sulfuric acid, hydrogen, sulfate, and hydroxide ions are present and migrate to the electrodes where hydrogen gas forms at the cathode and oxygen gas forms at the anode.6.2 (b) molten compound2
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Here are the key steps to identify products of electrolysis in molten compounds:
1. Identify the ions present in the molten compound
2. Determine which ions are attracted to the cathode and anode based on being positive or negative
3. Write the products formed by the ions discharging at each electrode
4. Write balanced half reactions for the cathode and anode
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Electrochemistry-Dr. Surendran ParambadathSurendran Parambadath
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The document discusses different types of electrochemical cells including primary cells that produce electricity from non-reversible chemical reactions and secondary cells that can be recharged by passing electricity in the opposite direction of the spontaneous reaction. Examples of primary cells discussed include Daniel, mercury, dry, and alkaline cells, while examples of secondary cells include lead-acid, nickel-cadmium, nickel-metal hydride, and lithium-ion batteries. The working and reactions of common cells like lead-acid, alkaline, and dry cells are also explained.C3f Electrolysis
C3f ElectrolysisM F Ebden
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This document discusses several examples of electrolysis processes:
1) Electrolysis of sodium chloride solution produces chlorine gas at the anode and sodium hydroxide solution at the cathode. Chlorine is used to make chemicals and disinfect water.
2) Electrolysis of sulfuric acid produces hydrogen gas at the cathode and oxygen gas at the anode.
3) Aluminum is extracted from its ore, bauxite, through electrolysis. Molten aluminum oxide is electrolyzed to produce aluminum metal at the cathode and oxygen gas at the anode.C5b Electrolysis
C5b ElectrolysisM F Ebden
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The document discusses electrolysis of molten and aqueous compounds. During electrolysis, ions are attracted to the electrodes and gain or lose electrons to form elements or different compounds. For molten compounds to electrolyze, they must decompose into ions. The ions then move towards the positively charged anode, where they lose electrons, and towards the negatively charged cathode, where they gain electrons. For aqueous solutions, the ions from water may plate out at the electrodes instead of ions from the dissolved compound. The amount of product formed depends on the charge transferred, which is calculated using current and time.Electrolysis.pptx
Electrolysis.pptxSabrinaDeBellotte1
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This document discusses factors that determine which ions are discharged at the electrodes during electrolysis. For molten compounds containing one cation and one anion, the cation will be reduced at the cathode and the anion will be oxidized at the anode. For compounds in solution, the position of ions in the electrochemical series and concentration determine which ions are discharged. Ions higher in the anion series and lower in the metal series are preferentially discharged at the anode and cathode respectively. In dilute solutions, OH- and H+ ions are discharged but in concentrated solutions the ions from the compound may be discharged instead.Sodium group
Sodium groupgiovanniveitch
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The document discusses the Downs Process for extracting sodium through the electrolysis of molten sodium chloride, where sodium ions are reduced to sodium atoms at the cathode and chlorine gas is produced at the anode. It also describes how sodium hydroxide is produced through the electrolysis of sodium chloride solutions, and lists some common uses of sodium and sodium hydroxide such as in soap production, as a drain cleaner, and for lighting.Electrolysis
ElectrolysisAmanSaini51077
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Electrolysis is a process that uses electricity to separate substances. When an ionic substance is melted or dissolved in water, ions are free to move and an electric current can break them down into elements. During electrolysis, positive ions move to the negative cathode where they gain electrons and negative ions move to the positive anode where they lose electrons. Electrolysis of brine produces chlorine gas, hydrogen gas, and sodium hydroxide solution which have important industrial uses.Water
Water Nidhi D
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The document discusses the molecular structure of water. It explains that a water molecule is formed by two hydrogen atoms and one oxygen atom bonded together at an angle of 104.5 degrees. The polarity of the water molecule arises from oxygen's higher electronegativity which gives it a partial negative charge and the hydrogen atoms a partial positive charge. This polar nature is an important feature of water and causes it to have unique properties.ELECTROLYSIS PPT.FDGFYD UDRSECVXF KYS GDTSUTS
ELECTROLYSIS PPT.FDGFYD UDRSECVXF KYS GDTSUTSMalikKalim2
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The document explains the process of electrolysis, detailing how ionic compounds can conduct electricity when dissolved in a solution due to the movement of charged ions. It outlines the roles of anodes and cathodes, and the chemical reactions that occur at each electrode during electrolysis, including oxidation and reduction processes. Additionally, it provides examples of various ionic compounds and the products formed at the electrodes during the electrolysis process.ELECTROLYSIS.pdf
ELECTROLYSIS.pdfBagalanaSteven
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1. Electricity can affect substances in different ways depending on whether they are conductors, insulators, electrolytes or non-electrolytes. Conductors allow electric current to pass through due to mobile electrons, while insulators do not due to electrons locked in bonds.
2. Electrolysis is the decomposition of an electrolyte solution or melt by passing an electric current through it. At the anode, oxidation occurs as ions lose electrons. At the cathode, reduction occurs as ions gain electrons. Common electrolytes decomposed include NaCl, CuSO4 and acidified water.
3. During the electrolysis of molten lead(II) bromide, lead metal deposits at the cathode while bromineAnswers
AnswersCikgu Shaiful Kisas
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The document discusses electrolysis experiments using two electrodes, P and Q. At electrode P/cathode, sodium and hydrogen ions are attracted due to their position in the electrochemical series. At electrode Q/anode, chloride and hydroxide ions are attracted due to their higher concentration, and chloride ions are selectively discharged. The explanation involves experiments comparing the reactivity of metals like silver, L, and M based on their positions in the electrochemical series.2012 topic 4.1 bonding - ionic
2012 topic 4.1 bonding - ionicDavid Young
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The document discusses ionic bonding. Ionic bonds form between elements when one atom loses electrons to become a positively charged cation and another atom gains those electrons to become a negatively charged anion. This transfer of electrons allows both atoms to achieve a stable noble gas electron configuration. The resulting ions are held together by electrostatic attraction in a crystal lattice structure. Ionic compounds have high melting points, are brittle, and do not conduct electricity as solids since the ions are tightly bound. They dissolve in water, allowing the ions to separate and move, making the solutions electrically conductive.Ionic theory and electrolysis
Ionic theory and electrolysisMussaOmary3
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1) Electrolysis is the decomposition of electrolytes by the passage of an electric current through it. During electrolysis, ions move to the oppositely charged electrodes - cations to the cathode and anions to the anode.
2) At the anode, anions lose electrons in an oxidation reaction. At the cathode, cations gain electrons in a reduction reaction.
3) Which ion is discharged depends on factors like their position in the electrochemical series, concentration, and the electrode material. Ions higher in concentration or lower in the series will preferentially discharge.Acids and bases dr.surendran prambadath
Acids and bases dr.surendran prambadathSurendran Parambadath
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The document discusses acids and bases according to different theories including Arrhenius, Bronsted-Lowry, and Lewis concepts. It defines acids and bases, describes their properties, and explains neutralization reactions. Examples are provided of strong vs weak acids and bases as well as monoprotic, diprotic, and triprotic acids and bases based on their equivalent weights.Electrolysis of water
Electrolysis of watercgraham6
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The document describes an experiment on the electrolysis of water, detailing the process of decomposing water into oxygen and hydrogen using an electric current and sodium carbonate as a catalyst. It outlines pre-lab questions, step-by-step procedural instructions, and subsequent testing of the gases produced. Additionally, it includes reflection questions aimed at understanding the volumes of gases produced and their relationship to the composition of water.Electrolysis chemist
Electrolysis chemistHilmi Qimie
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Electrolysis is the process of using electricity to cause a non-spontaneous chemical reaction. During electrolysis, ions migrate towards the electrodes and undergo oxidation or reduction reactions. At the cathode, positively charged ions are reduced and neutral atoms are formed. At the anode, negatively charged ions are oxidized and neutral atoms or molecules are formed. The products of electrolysis depend on factors like the ions present in the electrolyte, their concentration and position in the reactivity series, and the nature of the electrodes. Electrolysis has applications in purifying and extracting metals, and in electroplating.Synthesis of Sodium metal
Synthesis of Sodium metalabdullahahmed223
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1. The Down's cell is an electrolytic cell that operates at 800属C to produce sodium metal through the electrolysis of molten sodium chloride.
2. It consists of a graphite anode and iron cathode separated by an iron screen inside a lined steel chamber. Molten sodium chloride mixed with calcium chloride and barium chloride is used as the electrolyte.
3. During electrolysis, chloride ions are oxidized at the anode to produce chlorine gas while sodium ions are reduced at the cathode to produce molten sodium metal. Some calcium is also produced but separates from the sodium due to differences in density.presentation1-190429202206.pdf
presentation1-190429202206.pdfJam Saeed Ahmed
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1. The Down's cell is an electrolytic cell that operates at 800属C to produce sodium metal through the electrolysis of molten sodium chloride.
2. It consists of a graphite anode and iron cathode separated by an iron screen inside a lined steel chamber. Molten sodium chloride mixed with calcium chloride and barium chloride is used as the electrolyte.
3. During electrolysis, chloride ions are oxidized at the anode to produce chlorine gas while sodium ions are reduced at the cathode to produce molten sodium metal. Some calcium is also produced but separates from the sodium due to differences in density.Electrolysis
Electrolysislisa14hazel
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Electrolysis is the decomposition of a substance by an electric current, where electrolytes carry current as ions in solution. During electrolysis, ions move to the electrodes and undergo oxidation or reduction reactions. At the cathode, electrons are gained and reduction occurs. At the anode, electrons are lost and oxidation occurs. The amount of substance deposited or gas produced can be calculated using Faraday's law, relating current, time, and moles of electrons in the electrode reactions.Ad
Concentration of ions in the solution
- 1. (b) Concentration of ions in the solution / electrolytes. Sodium chloride solution, 1.0 mol dm-3 Carbon electrodes Figure 3 Electrolysis of sodium chloride solution From sodium chloride Na+, Cl- From water H+ , OH- CATHODE: Na+ , H+ ANODE: Cl- , OH- Both types of cations are attracted to the Both ions are attracted to the anode, Chloride cathode, H+ ions are selected for discharged ions are discharged because the concentration as they are lower in the ES. of Cl- ions are higher than of OH- ions. 2H+ + 2e -- H2 (g) 2Cl- -- Cl2 (g) + 2e Gas bubbles are formed. When a lighted Bubbles pungent yellowish-green gas is wooden splinter is place near the mouth of produced. The gas changed the damp blue the test tube, a `pop` sound is produced. litmus paper to red and bleached it. Chlorine Hydrogen gas is evolved. gas is formed. Solution becomes alkaline by presence of sodium hydroxide. NaOH(aq)