Dssociation vs ionization.ppt
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This document discusses dissociation and ionization when substances dissolve in water. It explains that ionic compounds dissociate into their constituent ions, while molecular compounds either disperse as neutral particles (non-electrolytes) or ionize to form hydrogen ions (acids). Specifically, it states that dissociation involves the separation of pre-existing ions in ionic compounds or bases, while ionization produces new ions through the reaction of acids in water. Examples of dissociation and ionization equations are also provided.
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This document summarizes key concepts about aqueous solutions, including:
- Solutions contain a solvent and one or more solutes
- Ionic compounds generally dissolve well in water due to ion separation through solvation
- "Like dissolves like" - polar substances dissolve in water and nonpolar substances do not
- Electrolytes conduct electricity in solution while nonelectrolytes do not
- Hydrates contain water within their crystalline structure.Ln 5 electrolysis drew
Ln 5 electrolysis drewlohitkumardrawal
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Electrolysis is the process of using a direct electric current to drive nonspontaneous chemical reactions. It involves the decomposition of an electrolyte into its constituent ions by the removal or addition of electrons to the ions. During electrolysis, ions migrate to the electrodes where they undergo oxidation or reduction reactions. In the electrolysis of molten lead bromide, lead ions are reduced to metallic lead at the cathode, while bromide ions are oxidized to bromine gas at the anode. When an aqueous solution of copper sulfate is electrolyzed using copper electrodes, copper ions are reduced at the cathode to form metallic copper while oxygen gas forms at the anode. Electrolysis requires an electrolyte, electrodes, and a direct current powerAdvchemchapt4 101015123318-phpapp02
Advchemchapt4 101015123318-phpapp02Cleophas Rwemera
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This document provides information on types of chemical reactions and solution stoichiometry. It discusses the common water molecule and how water acts as a solvent. It describes different types of solutions, including strong and weak electrolytes, and nonelectrolytes. Precipitation, acid-base, and oxidation-reduction reactions are introduced. Methods for writing balanced and net ionic equations are presented. Finally, techniques for performing stoichiometric calculations on reactions in solution, including determining limiting reactants and amounts of products formed, are covered.Arrhenius theory.pptx
Arrhenius theory.pptxUnknown Unknown
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The document summarizes Arrhenius theory of acids and bases as proposed by Svante Arrhenius in 1887. The key points are:
1) Arrhenius proposed that acids donate H+ ions and bases donate OH- ions when dissolved in water.
2) Electrolytes conduct electricity in solution by dissociating into ions, while nonelectrolytes do not dissociate or conduct.
3) The theory explained several phenomena like heat of neutralization and differentiation of strong/weak electrolytes but had limitations like not explaining ion formation mechanisms.5.2.1
5.2.1Kenton Hemsing
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When salts dissolve in water, the polar water molecules interact with the positive and negative ions of the salt, attracting them and breaking apart the crystal structure. Electrolytes separate into ions that move freely in solution while maintaining net neutral charge. Dissociation equations represent electrolytes dissolving as solute separating into aqueous ions. These equations must be balanced and show correct ionic charges and physical states. Dissociation refers to ionic compounds breaking apart while ionization describes molecules breaking into separate particles.Acids, Bases, and Salts: Properties & Reactions
Acids, Bases, and Salts: Properties & ReactionsRejoshaRajendran
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Acids, Bases, and Salts
Acids
Taste sour and turn blue litmus red.
Release H (Hydrogen) ions in solution.
Example: HCl (Hydrochloric acid), HSO (Sulfuric acid).
Bases
Taste bitter and feel soapy, turn red litmus blue.
Release OH (Hydroxide) ions in solution.
Example: NaOH (Sodium hydroxide), KOH (Potassium hydroxide).
Neutralization Reaction
Acid + Base Salt + Water
Example: HCl + NaOH NaCl + HO
Salts
Formed from neutralization of an acid and a base.
Can be acidic, basic, or neutral.
Example: NaCl (Table salt), CuSO (Copper sulfate).
pH Scale
Measures acidity or basicity (0-14).
pH < 7 Acidic, pH = 7 Neutral, pH > 7 Basic.388770.pptx.ppt
388770.pptx.pptssuser9fae69
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This document provides an overview of electrolytes and solutions. It defines electrolytes as substances that dissociate into ions when dissolved in water, allowing them to conduct electricity. Strong electrolytes dissociate completely while weak electrolytes only partially dissociate. Arrhenius' theory of electrolytic dissociation explains how electrolytes break up into ions in solution. The degree of dissociation depends on factors like temperature and concentration. Ostwald's dilution law describes how the degree of dissociation changes with concentration for weak electrolytes. Ionic equations represent the dissociation of electrolytes into ions.11 bctopic6
11 bctopic6King Ali
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When solutions of ionic compounds are mixed, precipitation reactions can occur if the mixing produces an insoluble ionic compound. For example, when solutions of silver nitrate and sodium chloride are mixed, a precipitate of insoluble silver chloride will form. Only the ions that react (Ag+ and Cl-) are shown in the balanced net ionic equation, with any spectator ions (Na+ and NO3-) that do not react omitted. The precipitate can be isolated by filtering the mixture.General chemistry academic journal (sample)
General chemistry academic journal (sample)Vincentius Soesanto
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This document provides definitions and explanations of acids and bases according to different theories. It discusses the Arrhenius, Br淡nsted-Lowry and Lewis definitions. It also covers pH, ionization constants, and the auto-ionization of water. Key points include: 1) Arrhenius defined acids/bases as producing H+/OH- ions in water, while Br淡nsted-Lowry defined them as proton donors/acceptors; 2) Lewis defined them based on electron pair sharing; 3) pH is a measure of H3O+ concentration; 4) the product of [H3O+] and [OH-] is constant.Ionic Equilibrium
Ionic Equilibrium Ednexa
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This document discusses ionic equilibrium and electrolytes. It defines electrolytes as substances that conduct electricity when dissolved in water by dissociating into ions. Electrolytes are divided into strong and weak based on their degree of ionization. Strong electrolytes almost completely ionize while weak electrolytes ionize only partially. The document discusses Arrhenius theory of electrolytic dissociation and factors that affect the degree of ionization like concentration, temperature, and presence of a common ion. It also defines concepts like isohydric solutions and dissociation constants.ionicequilibrium-150530122047-lva1-app6891.pdf
ionicequilibrium-150530122047-lva1-app6891.pdfAtiyyaS
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This document provides an overview of electrolytes, acids, and bases according to different theories. It defines strong and weak electrolytes, and lists examples of each. It then summarizes the Arrhenius, Bronsted-Lowry, and Lewis theories of acids and bases. The Arrhenius theory defines acids as substances that produce hydrogen ions in water and bases as those that produce hydroxide ions. The Bronsted-Lowry theory broadened this to include proton donors and acceptors. The Lewis theory further expanded the definition to any electron pair acceptor or donor.Ionic equilibrium
Ionic equilibriumShivani Singh
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The document provides an overview of electrolytes, acids, and bases, detailing their classifications as strong and weak electrolytes according to their ionization in aqueous solutions. It discusses different theories of acids and bases, including the Arrhenius, Br淡nsted-Lowry, and Lewis definitions, along with their strengths and limitations. Key concepts such as ionic equilibrium, conjugate acid-base pairs, and the roles of various ions in biological systems are highlighted.ELECTROLYSIS PPT.pptxvghjkghjvhjcbbvhjmvgnb
ELECTROLYSIS PPT.pptxvghjkghjvhjcbbvhjmvgnbthesciencehubprg
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Electrolysis is a process that involves the decomposition of chemical compounds using direct electric current, facilitating the movement of ions in solutions. Electrolytes can be strong or weak, with strong electrolytes completely dissociating in solution, whereas weak electrolytes only partially dissociate. The document covers various aspects of electrolysis, including applications such as electroplating and the principles of selective discharge of ions at electrodes.Chapter 14.1 : Compounds in Aqueous Solutions
Chapter 14.1 : Compounds in Aqueous SolutionsChris Foltz
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1) Ionic compounds dissolve in water by dissociating into their constituent ions. For example, NaCl dissociates into Na+ and Cl- ions in water.
2) Aluminum sulfate, Al2(SO4)3, dissociates into 2 Al3+ and 3 SO42- ions when dissolved in water, producing a total of 5 moles of ions from 1 mole of the compound.
3) Precipitation reactions occur when opposite ions combine to form an insoluble ionic compound. For example, combining solutions of (NH4)2S and Cd(NO3)2 will produce the insoluble precipitate CdS.what are solutions.docx
what are solutions.docxSesirekhaRavinuthula
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This document discusses key concepts related to solutions and acid-base chemistry, including:
- Definitions of solutions, solvents, solutes, electrolytes, and nonelectrolytes. Common examples are provided.
- Dissociation and hydration of ionic compounds in solution. Equations are given to represent these processes.
- Precipitation reactions and how to write balanced molecular, ionic, and net ionic equations.
- Arrhenius definitions of acids and bases. Examples of strong and weak acids and bases ionizing in water are given through chemical equations.
- Key reactions include neutralization and acid-base reactions where examples of writing balanced equations are provided.Chemical reaction occurring in water (dadiq)
Chemical reaction occurring in water (dadiq)Lithlith Bernal
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This document discusses three types of chemical reactions that occur in water: precipitation reactions, acid-base reactions, and oxidation-reduction reactions. Precipitation reactions involve the formation of an insoluble ionic compound from ions in solution. Acid-base reactions involve acids donating protons and bases accepting protons to form water. Oxidation-reduction reactions involve the exchange of electrons between reactants, with one species being reduced and the other being oxidized.Adv chem chapt 4
Adv chem chapt 4bobcatchemistry
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This document summarizes key concepts about types of chemical reactions and solution stoichiometry. It discusses water as a solvent, solubility, strong and weak electrolytes, and precipitation, acid-base, and oxidation-reduction reactions in solution. Calculations involve determining moles and masses of reactants and products using molarity, volumes, and balanced equations. Common indicators like phenolphthalein are used in acid-base titrations.Ch4
Ch4spathman
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This document discusses various concepts related to aqueous reactions and solution stoichiometry including:
- Ionic compounds dissociate into ions when dissolved in water, allowing them to conduct electricity.
- Strong electrolytes fully dissociate into ions while weak electrolytes only partially dissociate.
- Chemical equilibria exist for reactions that proceed in both the forward and backward directions.
- Precipitation reactions form insoluble products that drop out of solution.
- Acid-base reactions form water and salts by neutralizing hydrogen and hydroxide ions.
- Redox reactions involve the transfer of electrons and a change in oxidation states.Arrhenius theory of Electrolytic Dissociation.pptx
Arrhenius theory of Electrolytic Dissociation.pptxSarahJabbar6
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"Arrhenius theory of Ionization ,A fundamental concept in physical chemistry ,explain behaviours of electrolyte in solution, catogories of electrolytes degree of dissociation , process of dissociation , ionization constant and a brief introduction about conduction with concept of oxidation and reduction . When ionic solids dissolve in water theions that are adjacent to each.pdf
When ionic solids dissolve in water theions that are adjacent to each.pdfinbox5
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When ionic solids dissolve in water, their ions become surrounded by water molecules through a process called hydration, influenced by ion-dipole forces. The solubility of ionic compounds is governed by the balance of solute-solute, solvent-solvent, and solute-solvent interactions, primarily affected by lattice energy. A compound's solubility relates to its lattice energy, with higher lattice energies correlating with lower solubility, as demonstrated in the example of potassium iodide dissolving in water.Ad
Dssociation vs ionization.ppt
- 2. Dissociation In 1887, Svante August Arrhenius proposed that when a substance dissolves in water, particles of the substance separate from each other and disperse into the solution (called dissociation). Non-electrolytes disperse electrically neutral particles (therefore dont conduct electricity) Electrolytes disperse electrically charged particles called ions (therefore do conduct electricity)
- 3. Why do ionic compounds disperse electrically charged particles? The positive ions are surrounded by the negative end of the polar water molecules. The negative ions are surrounded by the positive end of the polar water molecules. RESULT: The ions at the edges of the ionic crystal are tugged and dislodged until each one is surrounded by water molecules and is floating around as an independent entity DISSOCIATION the separation of ions that occurs when an ionic compound dissolves in water
- 4. Dissociation Equations There are two requirements of dissociation: it must be soluble in water and must be ionic Dissociation Equations: shows the separation of ions in a chemical equation H20(l) is not shown because it is a solvent and is NOT consumed nor changed. It is shown in the aqueous states for the products (aq means dissolved in water) Examples: (you still need to make sure the equations are balanced) NaCl(s) Na + (aq) + Cl (aq) K3PO4(s) 3 K +(aq) + PO43- (aq)
- 5. Arrhenius acids and bases Arrhenius extended his dissociation theory to include acids and bases Bases ionic compounds containing the hydroxide ion (OH-) that dissolve into cations and OH (aq) in water Ba(OH)2 (s) Ba 2+ (aq) + 2 OH-(aq) NOTE: All bases are ionic, so all bases could dissociate if soluble in H2O Acids molecular compounds containing hydrogen that yield H+(aq) ions when they dissolve in water - Acids behave as molecular substances; CH3COOH (l) does not conduct electricity or change the color of litmus paper - As soon as acids are dissolved in water, their acid properties appear; CH3COOH (aq) will conduct electricity and changes litmus paper from blue to red NOTE: Acids are not ionic, so they DO NOT dissociate. They IONIZE.
- 6. Arrhenius came up with the idea of ionization to explain why acids are electrolytic: IONIZATION the reaction of neutral molecular compounds forming charged ions The non-electrolytic molecular compound separates into ions when dissolved in water, becoming electrolytic HCl(g) H+(aq) + Cl-(aq)
- 7. Dissociation vs. Ionization What is the difference between dissociation and ionization? Both produce (aq) ions... Dissociation, however, is the separation of ions that already exist before dissolving in water M+X-(s) M+ (aq) + X-(aq) Ionization involves the production of new ions, specifically hydrogen ions HX0(aq) H+ (aq) + X-(aq)
- 8. SUMMARY Substance Process General Equation XY (s/l/g) XY (aq) Molecular Disperse as individual, neutral molecules Ionic Dissociate into individual ions MX (s) M+ (aq) + X-(aq) Base (ionic hydroxide) Dissociate into positive ions and hydroxide ions MOH(s) M+ (aq) + OH-(aq) Acid Ionize to form hydrogen ions and anions HX (s/l/g) H+ (aq) + X-(aq)