Brainstorm from class. potassium chloride Which substance, when dissolved in water, will conduct the most electricity? Electrolyte or Not? An electrolyte is any fluid that contains free ions. The common concept of water being an electrolyte is due to the impurities present, that make it ionize itself, leading to electrolysis and being an electrolyte. The cation and anion that are formed to conduct electricity will not stay back as such. government site. Important ions in physiology include sodium, potassium, calcium, chloride and phosphate. b. December 4, 2010 Types of Electrolytes. Dr. Helmenstine holds a Ph.D. in biomedical sciences and is a science writer, educator, and consultant. Chapter 2 Part 1: Levels of Organization - Introduction, 15. 2016 Apr;27(4):981-9. The nonelectrolytes are out of the discussion here as their aqueous solution would not conduct current due to the lack of charged species. Examples: lemon juice (2.3), and vinegar (2.9) pH 3 Concentration: 10,000. Phosphate is regulated simultaneously with calcium by Vitamin D3, PTH, and calcitonin. Helmenstine, Anne Marie, Ph.D. "Strong Electrolyte Definition and Examples." The equilibrium constants for the dissociation of an intermediate electrolyte salt MX are typically in the range of 1-200. For pure water, \(\ce{[H2O]}\) is a constant (1000/18 = 55.6 M), and we often use the ion product, Kw, for water, \(\mathrm{\mathit K_w = \mathit K [H_2O] [H^+] [OH^-]}\). Phosphorus is an extracellular fluid cation. With a greater understanding . For electrolytes, water is the most important solvent. \(\mathrm{Zn + Cu^{2+} \rightarrow Zn^{2+} + Cu}\). \(\mathrm{Zn | Zn^{2+} || Cu^{2+}| Cu}\). , Jessica Damian, No Comment, February 8, 2023 Electrolytes are essential for basic life functioning, such as maintaining electrical neutrality in cells, generating and conducting action potentials in the nerves and muscles. Examples of some salts as strong electrolytes: How to know if a chemical is an electrolyte? Strong electrolytes are good conductors of electricity, but only in aqueous solutions or in molten form. Weak electrolytes are solutions that have the substances dissolved in them in the form of molecules rather than ions. You can help Wikipedia by expanding it. CHecking serum calcium levels is a recommended test in post-thyroidectomy patients. For example, \(\ce{NaCl}\), \(\ce{HNO3}\), \(\ce{HClO3}\), \(\ce{CaCl2}\) etc. A solution is neutral if its pH is equal to 7.0. Aqueous solutions containing electrolytes conduct electricity. The solution will conduct electricity if it contains free and charged ions. Here's some extreme examples of what can happen with an imbalance of electrolytes: elevated potassium levels may result in cardiac arrhythmias; decreased extracellular potassium produces paralysis; excessive extracellular sodium causes fluid retention; and decreased plasma calcium and magnesium can produce muscle spasms of the extremities. The figure here illustrates a copper-zinc battery. HCl (hydrochloric acid), H2SO4 (sulfuric acid), NaOH (sodium hydroxide) and KOH (potassium hydroxide) are all strong electrolytes. Originally, a "strong electrolyte" was defined as a chemical that, when in aqueous solution, is a good conductor of electricity. sodium sulfate, Na2SO4 sulfurous acid, H2SO3 nitrous acid, HNO2 sucrose, C12H22011 ammonia, NH3. Since ions are the charge carriers, we might expect the conductivity of a solution to be directly proportional to their concentrations in the solution. Naming Alkenes with Examples, Electron Configuration: The Key to Chemical Reactivity, Braggs Law [n = 2d sin]: A Relationship Between (d & ), Memorizing the Periodic Table: 3 Easy & Proven Ways, Neutralization Reactions: The Acid Base Balancing, Strong electrolytes ionize completely when dissolved in water, Weak electrolytes ionize partially in water, There is 100% ionization, so the principal species are the ions of the electrolytes in the solution, The ionization is less, roughly 1-10%. Helmenstine, Anne Marie, Ph.D. "Chemistry Examples: Strong and Weak Electrolytes." When solutions of electrolytes are combined, the cations and anions will meet each other. Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. , No Comment, February 8, 2023 Because C is a non-metal and H, O is a. Example: soapy water pH 13 Concentration: 1/1,000,000. Nick Trigili NITRO-3D. Electrolytes Substances that give ions when dissolved in water are called electrolytes. Electrolytes are essential for life, but many people get too much (like too much sodium from salt in processed food), which can also disrupt proper physiological function. The reabsorption of potassium takes place at the proximal convoluted tubule and thick ascending loop of Henle. , No Comment, February 6, 2023 At the rather low concentration of 0.001 M, the strong electrolyte solutions conduct between 2500 and 10 000 times as much current as pure H 2 O and about 10 times as much as the weak electrolytes HC 2 H 3 O 2 (acetic acid) and NH 3 (ammonia). Electrolytes is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by LibreTexts. You said HCl is a weak electrolyte in the first paragraph and then a strong one in the second. Why cant pure water be used as an electrolyte? Ammonia, NH3 is a weak electrolyte because it is a weak base. Legal. Electrolytes come from our food and fluids. sharing sensitive information, make sure youre on a federal If a parent provides an oral electrolyte maintenance solution at the very start of the illness, dehydration can be prevented. Electrolytes are chemicals that break into ions in water. A salt solution is usually used, but solutions of acids and bases will be all right. Symptoms of hypernatremia include tachypnea, sleeping difficulty, and feeling restless. These are called metathesis reactons, which include: Redox reactions are also possible between the various ions. Ammonia in water is an example for weak electrolyte. https://en.wikipedia.org/w/index.php?title=Strong_electrolyte&oldid=1099031951, Creative Commons Attribution-ShareAlike License 3.0, This page was last edited on 18 July 2022, at 17:38. Electrolyte or Not? Examples: bleach, oven cleaner pH 14 Concentration: 1/10,000,000. Ethanol, ammonia, and acetic acid are some of the non-aqueous solvents that are able to dissolve electrolytes. The primary electrolytes required in the body fluid are cations (of calcium, potassium, sodium, and magnesium) and anions (of chloride, carbonates, aminoacetates, phosphates, and iodide). Covalent or Molecular Compound Properties, Calculate Concentration of Ions in Solution, Strong Electrolyte Definition and Examples, Acids and Bases - Calculating pH of a Strong Base. Expert Answer. It forms ammonium hydroxide (NH4OH), which is a base, and basic solutions are electrolytic. This stands in contrast to the large number of weak acids (as well as weak bases) whose dissociation constants typically range from 103 to smaller than 1010. Instead, new counter-ions are continually acquired on the leading edge of the motion, while existing ones are left behind on the opposite side. Helmenstine, Anne Marie, Ph.D. "Chemistry Examples: Strong and Weak Electrolytes." A concentrated solution of this strong electrolyte has a lower vapor pressure than that of pure water at the same temperature. The following ionization is not complete, \(\mathrm{H_2CO_{3\large{(aq)}} \rightleftharpoons H^+_{\large{(aq)}} + HCO^-_{3\large{(aq)}}}\). Water cannot be used as an electrolyte because pure water is not an electrolyte. The non-ideality of electrolytic solutions is also reflected in their colligative properties, especially freezing-point depression and osmotic pressure. Bethesda, MD 20894, Web Policies A strong electrolyte is a solute or solution that is an electrolyte that completely dissociates in solution. How to Name Alkenes? The resulting values are known as limiting equivalent conductances or sometimes as "equivalent conductances at infinite dilution", designated by . Most compounds that contain nitrogen are weak electrolytes. Is ch3oh a strong electrolyte - Electrolytes can be divided into the class of weak and strong electrolytes depending upon the tendency of the chemical compound . Sodium, potassium, and chloride are the significant electrolytes along with magnesium, calcium, phosphate, and bicarbonates. as in the case below of ammonia, which grabs a proton from the water forming the weak electrolyte ammonium hydroxide (Figure \(\PageIndex{4}\)). Unauthorized use of these marks is strictly prohibited. You can generalize the definition of K here to give the equilibrium constant expression for any weak electrolyte. \(\mathrm{Cu^{2+}_{\large{(aq)}} + 2 e^- \rightarrow Cu_{\large{(s)}}}\). NaHCO3 (Sodium hydrogen carbonate/baking soda), C12H22O11 (lactose) (lactose and sucrose have the same formula??? When the ions are indifferent of each other, there is no reaction. The more ionization, the stronger the electrolyte. Join AUS-e-TUTE! -, Ellison DH, Terker AS, Gamba G. Potassium and Its Discontents: New Insight, New Treatments. Strong electrolytes completely ionize when dissolved, and no neutral molecules are formed in solution. Substances that do not ionize when dissolved in water are called nonelectrolytes. Distinguish between strong and weak electrolytes. where || means a salt bridge, and \(\ce{CuSO4}\) is used to provide \(\ce{Cu^2+}\). Similarities Between Carbohydrates and Lipids, Similarities Between Ulcerative Colitis and Pregnancy, Similarities Between Autotrophs and Heterotrophs, Similarities Between Influenza A and Influenza B. Ann Clin Lab Sci. , Dr. Romisa, No Comment, February 24, 2023 In dry cells, the solution is replaced by a paste so that the solution will not leak out of the package. Sodium is exchanged along with potassium across cell membranes as part of active transport. { "Acids_and_Bases_-_Conjugate_Pairs" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "Balance_Reduction_and_Oxidation_(Redox)_Reactions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Chemical_Reactions_Overview : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "Conjugate_Acids_of_Bases_-_Ka_Kb_and_Kw" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Electrolytes : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Features_of_Chemical_Reaction : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Half_Reactions : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Metathesis_Reactions : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Oxidation_States : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "Revealing_the_Dates_of_Buffalo_Nickels_(Demo)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Solutions : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Solution_Stoichiometry : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, { Chemical_Reactions_Examples : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Limiting_Reagents : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Properties_of_Matter : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Reactions_in_Solution : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Stoichiometry : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Stoichiometry_and_Balancing_Reactions : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, [ "article:topic", "cations", "anions", "Electrolytes", "bases", "equilibrium constant", "acid", "base", "salt", "ionic solid", "electrolyte", "neutralization", "showtoc:no", "weak electrolytes", "strong electrolytes", "salts", "aqueous solutions", "Body Fluids", "Macrominerals", "Solid formation", "Gas formation", "license:ccbyncsa", "licenseversion:40" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FBookshelves%2FInorganic_Chemistry%2FSupplemental_Modules_and_Websites_(Inorganic_Chemistry)%2FChemical_Reactions%2FChemical_Reactions_Examples%2FElectrolytes, \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), status page at https://status.libretexts.org. Strong electrolytes break apart into ions completely. Unable to load your collection due to an error, Unable to load your delegates due to an error. Dissociation, of course, is a matter of degree. Eighty-five percent of the total body phosphorus is in the bones and teeth in the form of hydroxyapatite; the soft tissues contain the remaining 15%. High or low levels of electrolytes disrupt normal bodily functions and can lead to even life-threatening complications. Our body fluids are solutions of electrolytes and many other things. The kidneys predominantly regulate serum chloride levels. By clicking Accept All Cookies, you agree to the storing of cookies on your device to enhance site navigation, analyze site usage, and assist in our marketing efforts. [Electrolyte and acid-base balance disorders in advanced chronic kidney disease]. Strong acids, strong bases, and ionic salts that are not weak acids or bases are strong electrolytes. The solution will contain only ions and no molecules of the electrolyte. Carbonic acid (CH2O3), Ammonia (NH3), and Phosphoric acid (H3PO4) act as weak electrolytes. A strong electrolyte consists of a solute that dissociates into free ions in large quantity while a weak electrolyte does not release much of the free ions. Is HF (Hydrofluoric Acid) a Strong Acid or a Weak Acid? Electrolytes are substances that ionize in solutions and form ions whereas nonelectrolytes do not ionize when added into water or other solvents. Sodium hydroxide, NaOH is a strong base, so, it is a strong electrolyte as well. In terms of child health, oral electrolyte is need when a child is dehydrated due to diarrhea. An ionization can be represented by, \(\mathrm{NaCl_{\large{(s)}} \rightarrow Na^+_{\large{(aq)}} + Cl^-_{\large{(aq)}}}\). Reproductive Structures and Functions. Cell Division and Control of Cell Number, V. Chapter 2 Part 4: Higher Order Structures, 18. The simplest battery consists of two electrodes. Electrolyte is a solution and a medium that consists of free ions which help in the conduction of electricity. Salts much have high solubility in the solvent to act as strong electrolytes. It exists as molecule in water and to some extent get dissociated as ion. Sodium regulation occurs in the kidneys. In the above image, ammonia grabs a proton from water forming ammonium hydroxide . The solution will contain only ions and no molecules of the electrolyte. Sodium, which is an osmotically active cation, is one of the most important electrolytes in the extracellular fluid. The ionization is said to be complete. Hint: b. any copper salt February 9, 2023 This electrochemistry-related article is a stub. Strong electrolytes examples: Hydrochloric acid (HCl), Sulfuric acid (H2SO4), sodium hydroxide (NaOH), and potassium hydroxide (KOH). Hypercalcemia is when corrected serum total calcium levels exceed 10.7 mg/dl, as seen with primary hyperparathyroidism. The use of oral electrolyte maintenance solutions, which is responsible for saving millions of lives worldwide over the last 25 years, is one of the most important medical advances in protecting the health of children in the century, explains Juilus G.K. Goepp, MD, assistant director of the Pediatric Emergency Department of the Children's Center at Johns Hopkins Hospital. FOIA Ammonia in water is an electrolyte. Chloride is an anion found predominantly in the extracellular fluid. . will shift to the left as the concentration of the "free" ions increases. The .gov means its official. The light will glow dimly for each solution since each is a weak electrolyte. Hypernatremia presents when the serum sodium levels are greater than145 mmol/L. In the distal convoluted tubule, sodium undergoes reabsorption. Chapter 1: Introduction to Anatomy and Physiology, II. NITRO-3D is an unmatched, supercharged intra-workout formulated to help you push harder and further than ever during your workouts. The general form of the strong electrolyte equation is: strong electrolyte (aq) cation+ (aq) + anion- (aq). Ammonia is an electrolyte because it produces ions by the following reaction: NH 3 (aq) + H 2 O = NH 4+ (aq) + OH - (aq) Ammonia is a weak rather than strong electrolyte because this reaction runs both ways; ammonia reacts with water to produce ammonium and hydroxide ions, while hydroxide ions react with ammonium ions to produce ammonia and water. For carbonic acid, K = 4.2x10-7. , Jessica Damian solvated. Among the electrolyte disorders, hyponatremia is the most frequent. In: StatPearls [Internet]. ----- Classifying Electrolytes ------ Strong Electrolyte: completely dissociate in solution and conducts electricity. Experience heightened energy, delayed fatigue, amplified recovery, enhanced hydration, and improved muscle growth in an all-in-one delicious intra-workout supplement. Even so, the Debye-Huckel theory breaks down for concentrations in excess of about 103 M L1 for most ions. These electrolytes can have an imbalance, leading to either high or low levels. The core reaction involved in this process-the nitrogen reduction reaction (NRR) is a slow kinetic reaction, which requires efficient catalysts to improve the ammonia yield rate. Common examples include most carbon compounds, such as sugars, fats, and alcohols. Calculate ionization percentage of weak electrolytes. A strong electrolyte is a solute or solution that is an electrolyte that completely dissociates in solution . Endocrine Homeostasis and Integration of Systems, 59. Therefore, the equation which involves the ionization of weak electrolytes is represented with double-headed arrows, meaning, the reaction is reversible, such as. At higher temperatures, the pH is slightly less than 7, and at lower temperatures, the pH is greater than 7. In the case of hydrogen chloride, the hydrogen and chlorine get dissociated and form cation and anion. Which of the following is a strong electrolyte in aqueous solution ? Small fractions of weak electrolytes' molecules ionize when dissolve in water. The https:// ensures that you are connecting to the (d) Ammonia N H 3 is weak electrolyte. true or false: if something goes into solution but doesn't dissociate, it will still conduct electricity. Compounds can be Strong, Weak . Electrolytes dissociate into ions when added to water. How can you tell if an electrolyte is strong or weak? Find the state of plane stress at point CCC located 8in8\ \mathrm{in}8in. We get electrolytes through ingestion. What are the solute particles present in aqueous solutions of each compound? Ammonia, NH3, is a weak electrolyte. The LibreTexts libraries arePowered by NICE CXone Expertand are supported by the Department of Education Open Textbook Pilot Project, the UC Davis Office of the Provost, the UC Davis Library, the California State University Affordable Learning Solutions Program, and Merlot. Patients may present with headaches, confusion, nausea, delirium. Ethanol, ammonia, and acetic acid are some of the non-aqueous solvents that are able to dissolve electrolytes. Weak electrolytes only partially break into ions in water. But at such a high dilution, the conductivity would be so minute that it would be masked by that of water itself (that is, by the H+ and OH ions in equilibrium with the massive 55.6 M L1 concentration of water) making values of in this region virtually unmeasurable. O'Regan S, Carson S, Chesney RW, Drummond KN. Even though NH3 is an base, it is a weak base and. Dr. Helmenstine holds a Ph.D. in biomedical sciences and is a science writer, educator, and consultant. , No Comment. Example: battery acid pH 1 Concentration: 1,000,000. The quantitative applications of electrolysis imply colorimeters connected by salt bridges. These substances do not have a distinct ionized state. Answer. { "8.10.9A:_8.10.9A:_Electrolytes_and_Electrolytic_Solutions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "8.10.9B:_8.10.9B:_The_nature_of_ions_in_aqueous_solution" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "8.10.9C:_8.10.9C:__Weak_and_Strong_Electrolytes" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "8.10.9D:_8.10.9D:_Ionic_migration" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "8.10.9E:_8.10.9E:_Some_applications_of_electrolytic_conduction" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, { "8.01:_Solutions_and_their_Concentrations" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "8.02:_Thermodynamics_of_Solutions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "8.03:_Colligative_Properties-_Raoult\'s_Law" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "8.04:_Colligative_Properties-_Boiling_Point_Elevation_and_Freezing_Point_Depression" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "8.05:__Colligative_Properties_-_Osmotic_Pressure" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "8.06:__Reverse_Osmosis" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "8.07:_Colligative_Properties_and_Entropy" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "8.08:_Ideal_vs._Real_Solutions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "8.09:_Distillation" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "8.10:_Ions_and_Electrolytes" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, [ "article:topic", "authorname:lowers", "showtoc:no", "license:ccby", "licenseversion:30", "source@http://www.chem1.com/acad/webtext/virtualtextbook.html" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FBookshelves%2FGeneral_Chemistry%2FBook%253A_Chem1_(Lower)%2F08%253A_Solutions%2F8.10%253A_Ions_and_Electrolytes%2F8.10.9C%253A_8.10.9C%253A__Weak_and_Strong_Electrolytes, \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), The quantitative treatment of these effects was first worked out by P. Debye and W. Huckel in the early 1920's, and was improved upon by Ostwald a few years later.
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