), For example, dissolving ammonium chloride in water results in its dissociation, as described by the equation, The ammonium ion is the conjugate acid of the base ammonia, NH3; its acid ionization (or acid hydrolysis) reaction is represented by. If we want to determine a Kb value using one of these handbooks, we must look up the value of Ka for the conjugate acid and convert it to a Kb value. The reaction is: We are given two of three equilibrium concentrations and asked to find the missing concentration. The fourth column has the following: 0, x, x. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. A solution of this salt contains ammonium ions and chloride ions. Calculate (i) the degree of hydrolysis (ii) the hydrolysis constant and (iii) The conjugate acid of the strong base is a weaker acid than water and has no effect on the acidity of the resulting solution. The acetate ion behaves as a base in this reaction; hydroxide ions are a product. But NH4OH molecule formed ionises only partially as shown above. The vegetable, such as a cucumber, is placed in a sealed jar submerged in a brine solution. Without the harmful bacteria consuming the cucumbers they are able to last much longer than if they were unprotected. 3 What is salt hydrolysis explain with example? One example is the use of baking soda, or sodium bicarbonate in baking. AgNO3 (aq) + NH4Cl (aq) --> AgCl (s)+ NH4NO3 silver chloride is precipitated as it is very insoluble in. When we mix solutions of an acid and a base, an acid-base neutralization reaction occurs. 2 Dec 15, 2022 OpenStax. The conjugate acid of the strong base is a weaker acid than water and has no effect on the acidity of the resulting solution. TimesMojo is a social question-and-answer website where you can get all the answers to your questions. The acid strength of these complex ions typically increases with increasing charge and decreasing size of the metal ions. The acetate ion behaves as a base in this reaction; hydroxide ions are a product. A book which I am reading has this topic on hydrolysis of salts. The major use of ammonium chloride is in nitrogen-based fertilizers. 14.3: Relative Strengths of Acids and Bases, Example \(\PageIndex{1}\): pH of a Solution of a Salt of a Weak Base and a Strong Acid, Example \(\PageIndex{2}\): Equilibrium of a Salt of a Weak Acid and a Strong Base, Equilibrium in a Solution of a Salt of a Weak Acid and a Weak Base, Example \(\PageIndex{3}\): Determining the Acidic or Basic Nature of Salts, Example \(\PageIndex{4}\): Hydrolysis of [Al(H2O)6]3+, status page at https://status.libretexts.org, Predict whether a salt solution will be acidic, basic, or neutral, Calculate the concentrations of the various species in a salt solution, Describe the process that causes solutions of certain metal ions to be acidic, A strong acid and a strong base, such as HCl(. The dissociation chemical reaction is: NH4Cl(solid) = NH4+(aqueous) + Cl-(aqueous). We frequently see the formula of this ion simply as Al3+(aq), without explicitly noting the six water molecules that are the closest ones to the aluminum ion and just describing the ion as being solvated in water (hydrated). The sodium ion has no effect on the acidity of the solution. As shown in Figure 14.13, the This is the most complex of the four types of reactions. NaHCO3 is a base. It is odorless with a density of 1.519 gm/cm3, It has a pH value between 4.5 and 6 and its pKa value is 9.24. The first-step acid ionization equations for a few other acidic metal ions are shown below: An ICE table with the provided information is. The word neutralization seems to imply that a stoichiometrically equivalent solution of an acid and a base would be neutral. As an example, the dissolution of aluminum nitrate in water is typically represented as, However, the aluminum(III) ion actually reacts with six water molecules to form a stable complex ion, and so the more explicit representation of the dissolution process is. Ka = [NH3] x[H3O+] = 5.6 x 10-10 [NH4+] 2.3: Relative Strengths of Acids and Bases, Example \(\PageIndex{1}\): pH of a Solution of a Salt of a Weak Base and a Strong Acid, Example \(\PageIndex{2}\): Equilibrium of a Salt of a Weak Acid and a Strong Base, Equilibrium in a Solution of a Salt of a Weak Acid and a Weak Base, Example \(\PageIndex{3}\): Determining the Acidic or Basic Nature of Salts, Example \(\PageIndex{4}\): Hydrolysis of [Al(H2O)6]3+, status page at https://status.libretexts.org, Predict whether a salt solution will be acidic, basic, or neutral, Calculate the concentrations of the various species in a salt solution, Describe the process that causes solutions of certain metal ions to be acidic, A strong acid and a strong base, such as HCl(. As seen in the above equation on dissolving in aqueous solution NH4Cl releases hydronium ions due to the hydrolysis of ammonium ions. Solve for x and the equilibrium concentrations. If you are redistributing all or part of this book in a print format, Likewise, some salts contain a single ion that is amphiprotic, and so the relative strengths of this ions acid and base character will determine its effect on solution pH. This increases the amount of hydroxide ion in the solution produced in the reaction and renders it slightly basic. ----- NH4Cl. The first row for the first column does not have a heading and then has the following in the first column: Initial concentration ( M ), Change ( M ), Equilibrium concentration ( M ). The reaction, \[CaCO_3(s)+2HCl(aq)CaCl_2(aq)+H_2O(l)+CO_2(g) \nonumber \]. The lactic acid eventually increases the acidity of the brine to a level that kills any harmful bacteria, which require a basic environment. Which response gives the . CO For example, ammonium chloride, NH4Cl, is a salt formed by the reaction of the weak base ammonia with the strong acid HCl: \[\ce{NH3}(aq)+\ce{HCl}(aq)\ce{NH4Cl}(aq) \nonumber \]. When we mix solutions of an acid and a base, an acid-base neutralization reaction occurs. Write formula equations and net ionic equations for the hydrolysis of sodium carbonate in water. Data and Results Table 7b.1. Ka, for the acid \(\ce{NH4+}\): \[\ce{\dfrac{[H3O+][NH3]}{[NH4+]}}=K_\ce{a} \nonumber \]. Strong acids may also be hydrolyzed. Salts that form from a weak acid and a strong base are basic salts, like sodium bicarbonate (NaHCO3). Aside from the alkali metals (group 1) and some alkaline earth metals (group 2), most other metal ions will undergo acid ionization to some extent when dissolved in water. Ammonium Chloride naturally occurs as a mineral called sal ammoniac. The acetate ion, One way to ensure that math tasks are clear is to have students work in pairs or small groups to complete the task. (a) basic; (b) neutral; (c) acidic; (d) basic, Unlike the group 1 and 2 metal ions of the preceding examples (Na+, Ca2+, etc. The brine solution favors the growth of beneficial bacteria and suppresses the growth of harmful bacteria. Keep in mind that a salt will only be basic if it contains the conjugate base of a weak acid. HCl is a strong acid while NH3 is a weak base and NH4Cl is formed as the product of their neutralization reaction. The fluoride ion is capable of reacting, to a small extent, with water, accepting a . Substituting the expressions for the equilibrium concentrations into the equation for the ionization constant yields: \(=\dfrac{(x)(x)}{0.10x}=1.4 \times 10^{5}\), \[\ce{[H3O+]}=0+x=1.210^{3}\:M \nonumber \], \[\mathrm{pH=log[H_3O^+]=2.92(an\: acidic\: solution)} \nonumber \]. In anionic hydrolysis, the pH of the solution will be above 7. A strong acid and a weak base yield a weakly acidic solution, not because of the strong acid involved, but because of the conjugate acid of the weak base. Hydrolysis reactions break bonds and release energy. Ammonium chloride is used in veterinary medicine in the prevention of urinary stones in sheep, goats, and cattle. ---- pH of 0.1 M NH4Cl: 6.35 [H+] for NH4Cl [OH] for NH4Cl Hydrolysis Net Ionic Equation for hydrolysis of NH4Cl Ka or Some aquatic animals utilize ammonium chloride to maintain their buoyancy in seawater. Ammonium Chloride is commercially prepared by a reaction between ammonia and hydrogen chloride also known as hydrochloric acid when present in an aqueous solution. ( acid and base. As with other polyprotic acids, the hydrated aluminum ion ionizes in stages, as shown by: \[\ce{Al(H2O)6^3+}(aq)+\ce{H2O}(l)\ce{H3O+}(aq)+\ce{Al(H2O)5(OH)^2+}(aq) \nonumber \], \[\ce{Al(H2O)5(OH)^2+}(aq)+\ce{H2O}(l)\ce{H3O+}(aq)+\ce{Al(H2O)4(OH)2+}(aq) \nonumber \], \[\ce{Al(H2O)4(OH)2+}(aq)+\ce{H2O}(l)\ce{H3O+}(aq)+\ce{Al(H2O)3(OH)3}(aq) \nonumber \]. What is the approximately pH of a 0.1M solution of the salt. NaCl is neutral. One example is the use of baking soda, or sodium bicarbonate in baking. The value of Ka for this acid is not listed in Table E1, but we can determine it from the value of Kb for aniline, C6H5NH2, which is given as 4.6 1010 : \[\mathrm{\mathit{K}_a(for\:C_6H_5NH_3^+)\mathit{K}_b(for\:C_6H_5NH_2)=\mathit{K}_w=1.010^{14}} \nonumber \], \[\mathrm{\mathit{K}_a(for\:C_6H_5NH_3^+)=\dfrac{\mathit{K}_w}{\mathit{K}_b(for\:C_6H_5NH_2)}=\dfrac{1.010^{14}}{4.610^{10}}=2.310^{5}} \nonumber \]. Some salts formed in neutralization reactions may make the product solutions slightly acidic or slightly basic. They only report ionization constants for acids. NH4Cl + H2O -> NH4OH + HCl HCl <=======> H+ + Cl- This equation is for easy generalization. This is similar to the simplification of the formula of the hydronium ion, H3O+ to H+. A weak acid and a strong base yield a weakly basic solution. Several antacids have aluminum hydroxide, Al(OH)3, as an active ingredient. The reaction, \[CaCO_3(s)+2HCl(aq)CaCl_2(aq)+H_2O(l)+CO_2(g) \nonumber \]. Im a mother of two crazy kids and a science lover with a passion for sharing the wonders of our universe. When you dissolve ammonium chloride crystals in water (H2O), the ammonium chloride compound decomposes into its component ions: NH4+ and Cl-. As Cl- is a weak conjugate base it cannot further accept a proton. The fourth column has the following: 0, x, x. K a of NH 4 + = 5.65 x 10 10.. Cooking is essentially synthetic chemistry that happens to be safe to eat. C) NH3 + H3O+ + Cl- DUHOXHCL E) NH3 + OH- + HCI 49) Which diagram best represents the products when equimolar amounts of HF (g) and NH3 (g) react? Occasionally the weak acid and the weak base will have the, Do the calculations and show that the hydronium ion concentration for a 0.233-, What is the hydronium ion concentration in a 0.100-, The \(\ce{NH4+}\) ion is acidic and the Cl, The \(\ce{NH4+}\) ion is listed as being acidic, and the F, \[K_\ce{a}=\ce{\dfrac{[H3O+][Al(H2O)5(OH)^2+]}{[Al(H2O)6^3+]}} \nonumber \]. A weak acid and a strong base yield a weakly basic solution. Solutions that contain salts or hydrated metal ions have a pH that is determined by the extent of the hydrolysis of the ions in the solution. Considering all the above-mentioned theories this can be easily deciphered that the properties of ammonium chloride molecule do not fit into the definition of the base, rendered by any of these theories, therefore, NH4Cl is not a base. Neutralization is the reaction between an acid and a base that results in the formation of a salt that derives its properties from its constituent i.e. A byproduct of the pickling process changes the flavor of the vegetables with the acid making them taste sour. However, the ionization of a cation carrying more than one charge is usually not extensive beyond the first stage. What this means is that the aluminum ion has the strongest interactions with the six closest water molecules (the so-called first solvation shell), even though it does interact with the other water molecules surrounding this \(\ce{Al(H2O)6^3+}\) cluster as well: \[\ce{Al(NO3)3}(s)+\ce{6H2O}(l)\ce{Al(H2O)6^3+}(aq)+\ce{3NO3-}(aq) \nonumber \]. are not subject to the Creative Commons license and may not be reproduced without the prior and express written As an Amazon Associate we earn from qualifying purchases. On the other hand, the NH4+ ion gives away its proton to form a hydronium ion with the water molecule. 2 Creative Commons Attribution License Additional examples of the first stage in the ionization of hydrated metal ions are: \[\ce{Fe(H2O)6^3+}(aq)+\ce{H2O}(l)\ce{H3O+}(aq)+\ce{Fe(H2O)5(OH)^2+}(aq) \hspace{20px} K_\ce{a}=2.74 \nonumber \], \[\ce{Cu(H2O)6^2+}(aq)+\ce{H2O}(l)\ce{H3O+}(aq)+\ce{Cu(H2O)5(OH)+}(aq) \hspace{20px} K_\ce{a}=~6.3 \nonumber \], \[\ce{Zn(H2O)4^2+}(aq)+\ce{H2O}(l)\ce{H3O+}(aq)+\ce{Zn(H2O)3(OH)+}(aq) \hspace{20px} K_\ce{a}=9.6 \nonumber \]. O) Determine the acetic acid concentration in a solution with \(\ce{[CH3CO2- ]}=0.050\:M\) and [OH] = 2.5 106 M at equilibrium. So the ions present in the Solution of NH4Cl, will be, NH4+ , Cl-, H+, OH-. Salts of weak acids and strong bases undergo anionic hydrolysis and yield basic solution. Answer: Hydrolysis usually is a equilibrated reaction between ion from weak bases or acids and water. Legal. This means that two of the solutions are basic (NH3 and NaF), one solution is neutral (NaCl), and the other is acidic (NH4Br). Ammonium Chloride is majorly manufactured as a by-product of the Solvay process which is used for the production of Sodium Carbonate. Example 2.4. Home | About | Contact | Copyright | Report Content | Privacy | Cookie Policy | Terms & Conditions | Sitemap. 2022 - 2023 Times Mojo - All Rights Reserved You'll get a detailed solution from a subject matter expert that helps you learn core concepts. Determine the degree of hydrolysis of this salt in 0.01 M solution and the pH of the solution. , is the conjugate base of acetic acid, CH3CO2H, and so its base ionization (or base hydrolysis) reaction is represented by. We determine Kb as follows: \[K_\ce{b}=\ce{\dfrac{[CH3CO2H][OH- ]}{[CH3CO2- ]}}=5.610^{10} \nonumber \], \[=\dfrac{[\ce{CH3CO2H}](2.510^{6})}{(0.050)}=5.610^{10} \nonumber \]. 0 0 Similar questions , NH and Cl . Substituting the available values into the Kb expression gives. This is the most complex of the four types of reactions. We will not find a value of Ka for the ammonium ion in Table E1. What is the pH of a 0.233 M solution of aniline hydrochloride? Dissolving a salt of a weak acid or base in water is an example of a hydrolysis reaction. The Hydronium Ion. A byproduct of the pickling process changes the flavor of the vegetables with the acid making them taste sour. There are a number of examples of acid-base chemistry in the culinary world. This may seem obvious from the ion's formula, which indicates no hydrogen or oxygen atoms, but some dissolved metal ions function as weak acids, as addressed later in this section. Similarly, NaF is basic (it is the salt of a strong base, NaOH, and a weak acid, HF). In cationic hydrolysis, the solution becomes slightly acidic (p H <7). The first column has the following: 0.10 (which appears in red), negative x, 0.10 minus x. NH4Cl is ammonium chloride. The pH value for NH4Cl lies between 4.5 and 6 and its pKa value is 9.24, therefore, it is mildly acidic. The Ka of HCO3HCO3 is 4.7 1011,and its Kb is 1.010144.3107=2.3108.1.010144.3107=2.3108. One of the most common antacids is calcium carbonate, CaCO3. Conjugates of weak acids or bases are also basic or acidic (reverse. Cationic hydrolysis refers to the hydrolysis of those salts that have strong acid and weak base components.In Cationic hydrolysis the resulting solution is acidic. \(\ce{Al(H2O)6^3+}(aq)+\ce{H2O}(l)\ce{H3O+}(aq)+\ce{Al(H2O)5(OH)^2+}(aq) \hspace{20px} K_\ce{a}=1.410^{5}\). A strong base produces a weak conjugate acid. The neutralization that occurs when aqueous solutions of acids and bases are combined results from the reaction of the hydronium and hydroxide ions to form water. A strong acid and a weak base yield a weakly acidic solution, not because of the strong acid involved, but because of the conjugate acid of the weak base. Several antacids have aluminum hydroxide, Al(OH)3, as an active ingredient. not only neutralizes stomach acid, it also produces CO2(g), which may result in a satisfying belch. It works according to the reaction: \[Mg(OH)_2(s)Mg^{2+}(aq)+2OH^-(aq) \nonumber \]. In the case of NH4Cl the dissociation equation can be written as: Here, the NH4Cl hydrolysis to form an NH4+ ion, which is the conjugate acid of ammonia, while the Cl- ion which is the conjugate base of ammonia. and you must attribute OpenStax. According to Arrheniuss theory of acids and bases, acids are the compounds that release hydrogen or hydronium ions upon their dissociation in an aqueous solution. In Leclanch cells, the aqueous solution of ammonium chloride was used as an electrolyte. Thus, the hydration becomes important and we may use formulas that show the extent of hydration: \[\ce{Al(H2O)6^3+}(aq)+\ce{H2O}(l)\ce{H3O+}(aq)+\ce{Al(H2O)5(OH)^2+}(aq) \hspace{20px} K_\ce{a}=1.410^{5} \nonumber \]. The reaction is: We are given two of three equilibrium concentrations and asked to find the missing concentration. However, the acetate ion, the conjugate base of acetic acid, reacts with water and increases the concentration of hydroxide ion: \[\ce{CH3CO2-}(aq)+\ce{H2O}(l)\ce{CH3CO2H}(aq)+\ce{OH-}(aq) \nonumber \]. This reduces the odor of the fish, and also adds a sour taste that we seem to enjoy. Now as explained above the number of H+ ions will be more than the number . As a salt acquires its pH based upon the acidic or basic strength of its constituent compounds, NH4Cl is acidic. This conjugate base is usually a weak base. (d) The NH4+NH4+ ion is acidic (see above discussion) and the F ion is basic (conjugate base of the weak acid HF). add 15 ml approx of water and 15m1 'approx of dilute sulphuric acid (2M H2SO.). The boiling point of ammonium chloride is 520C. Note that some of these aluminum species are exhibiting amphiprotic behavior, since they are acting as acids when they appear on the left side of the equilibrium expressions and as bases when they appear on the right side. In anionic hydrolysis, the solution becomes slightly basic (p H >7). Sodium chloride, for instance, contains chloride (Cl), which is the conjugate base of HCl. NH4Cl NH+ 4 +Cl N H 4 C l N H 4 + + C l The ammonium ion is a weak acid that reacts with water according to the chemical equation. Then we can observe that in the given question, the $C{H_3}COON{H_4}$ is therefore, a weak salt made by weak acid ( acetic acid ) and weak base ( ammonia ). The value of pH for different substances ranges from 1 to 14 on the pH scale in which 7 is the value of pH for the neutral solution. They only report ionization constants for acids. The \(\ce{C6H5NH3+}\) ion is the conjugate acid of a weak base. If Ka > Kb, the solution is acidic, and if Kb > Ka, the solution is basic. Assuming x << 0.233, the equation is simplified and solved for x: The ICE table defines x as the hydronium ion molarity, and so the pH is computed as. calculate the moles of ferrous ammonium sulfate hexahydrate solution in unit ug/mL. The Molecular mass of NH4Cl is 53.49 gm/mol. When we neutralize a weak acid with a strong base, we get a salt that contains the conjugate base of the weak acid. What is the pH of a 0.233 M solution of aniline hydrochloride? A) H H H H B) N + H H H H H-F H1 H D) H F " H E) 2+ 2- N H H H. You'll get a detailed solution from a subject matter expert that helps you learn core concepts. The word neutralization seems to imply that a stoichiometrically equivalent solution of an acid and a base would be neutral. (a) The K+ cation is inert and will not affect pH. We frequently see the formula of this ion simply as Al3+(aq), without explicitly noting the six water molecules that are the closest ones to the aluminum ion and just describing the ion as being solvated in water (hydrated). Calculate the pH of a 0.10-M solution of aluminum chloride, which dissolves completely to give the hydrated aluminum ion \(\ce{[Al(H2O)6]^3+}\) in solution. By the end of this section, you will be able to: Salts are ionic compounds composed of cations and anions, either of which may be capable of undergoing an acid or base ionization reaction with water. Jan 29, 2023. The second column is blank. A solution of this salt contains sodium ions and acetate ions. It is a salt of a strong acid and a weak base. Use 4.9 1010 as Ka for HCN. Occasionally the weak acid and the weak base will have the, Do the calculations and show that the hydronium ion concentration for a 0.233-, What is the hydronium ion concentration in a 0.100-, The \(\ce{NH4+}\) ion is acidic and the Cl, The \(\ce{NH4+}\) ion is listed as being acidic, and the F, \[K_\ce{a}=\ce{\dfrac{[H3O+][Al(H2O)5(OH)^2+]}{[Al(H2O)6^3+]}} \nonumber \]. 3+ Potassium carbonate (K2CO3) is a white salt, soluble in water (insoluble in ethanol) which forms a strongly alkaline solution. A strong acid produces a weak conjugate base. My aim is to uncover unknown scientific facts and sharing my findings with everyone who has an interest in Science. Save my name, email, and website in this browser for the next time I comment. Our mission is to improve educational access and learning for everyone. Some salts formed in neutralization reactions may make the product solutions slightly acidic or slightly basic. The first column has the following: 0.10 (which appears in red), negative x, 0.10 minus x. Which Teeth Are Normally Considered Anodontia. This page titled 2.4: Hydrolysis of Salt Solutions is shared under a CC BY license and was authored, remixed, and/or curated by OpenStax. In spite of the unusual appearance of the acid, this is a typical acid ionization problem. One of the most common antacids is calcium carbonate, CaCO3. Salt hydrolysis is defined as the process in which a salt reacts with water to give back the acid and the base. KAl(SO4)2. . We recommend using a Screen capture done with Camtasia Studio 4.0. Dissociation constant of NH 4OH is 1.810 5. Explanation : Hydrolysis is reverse of neutralization. OpenStax is part of Rice University, which is a 501(c)(3) nonprofit. The equilibrium equation for this reaction is simply the ionization constant. When aluminum nitrate dissolves in water, the aluminum ion reacts with water to give a hydrated aluminum ion, \(\ce{Al(H2O)6^3+}\), dissolved in bulk water. The HCl Molecule formed will completely ionises to form H+ ion, as shown above. Milk of Magnesia is a suspension of the sparingly soluble base magnesium hydroxide, Mg(OH)2. No hydrolysis occurs.Please Explain.also what is hydrolysis?!!!! NH4OH + HClE. Substituting the expressions for the equilibrium concentrations into the equation for the ionization constant yields: \(=\dfrac{(x)(x)}{0.10x}=1.4 \times 10^{5}\), \[\ce{[H3O+]}=0+x=1.210^{3}\:M \nonumber \], \[\mathrm{pH=log[H_3O^+]=2.92(an\: acidic\: solution)} \nonumber \]. The aluminum ion is an example. The OpenStax name, OpenStax logo, OpenStax book covers, OpenStax CNX name, and OpenStax CNX logo The neutralization that occurs when aqueous solutions of acids and bases are combined results from the reaction of the hydronium and hydroxide ions to form water. In a solution of a salt formed by the reaction of a weak acid and a weak base, to predict the pH, we must know both the Ka of the weak acid and the Kb of the weak base. Is salt hydrolysis possible in ch3coonh4? Step-by-step answer: Salts which are made from strong acid and weak base undergo cationic hydrolysis. However, the conjugate base of the weak acid is a weak base and ionizes slightly in water. Hint: We will probably need to convert pOH to pH or find [H3O+] using [OH] in the final stages of this problem. The following four situations illustrate how solutions with various pH values can arise following a neutralization reaction using stoichiometrically equivalent quantities: Our stomachs contain a solution of roughly 0.03 M HCl, which helps us digest the food we eat. A solution of a weak acid reacts with a solution of a strong base to form the conjugate base of the weak acid and the conjugate acid of the strong base. 3: Determining the Acidic or Basic Nature of Salts. resulting in a basic solution. The hydrolysis of an acidic salt, such as ammonia. All the substances having a pH value below 7 are acidic while the substances having a pH value above 7 are basic. Stock iron(II) solution (200Ug mL-1 Fe) ferrous ammonium sulfate hexahydrate mass= 0.1437g, transfer it to a 100 ml beaker. 2) Here is the K a expression for NH 4 +: (CH Some handbooks do not report values of Kb. It is isolated as aniline hydrochloride, \(\ce{[C6H5NH3+]Cl}\), a salt prepared by the reaction of the weak base aniline and hydrochloric acid.
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