hydrolysis of nh4cl hydrolysis of nh4cl

We recommend using a Find Net Ionic equation for hydrolysis , Expression for equilibrium Hence , the reaction is - NHCl NH + Cl We can conclude that NHCl can be formed from the ions , NH and Cl Hence , According to the reaction , NH + HO NH + HO Therefore , Ionization increases as the charge of the metal ion increases or as the size of the metal ion decreases. Dissolving sodium acetate in water yields a solution of inert cations (Na+) and weak base anions Arrhenius theory: A molecule that produces hydroxide ion (OH-) in a solution is a base and the molecule which is unable to produce hydroxide ions is an acid. If Ka > Kb, the solution is acidic, and if Kb > Ka, the solution is basic. pH of NH4Cl Acidic or Basic? - Techiescientist Textbook content produced by OpenStax is licensed under a Creative Commons Attribution License . The major use of ammonium chloride is in nitrogen-based fertilizers. This can also be justified by understanding further hydrolysis of these ions. The equilibrium equation for this reaction is simply the ionization constant. Net ionic equation for hydrolysis of nh4cl - Math Practice 2 They are characterized by the splitting of a water molecule into a hydrogen and a hydroxide group with one or both of these becoming attached to an organic starting product. 2.4: Hydrolysis of Salt Solutions - Chemistry LibreTexts One of the most common antacids is calcium carbonate, CaCO3. Ammonium chloride in water is acidic and it produces ammonia, H+ ions, Cl- ions and H2O. 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. NH4CL. However, in this case, the hydrated aluminum ion is a weak acid (Figure \(\PageIndex{2}\)) and donates a proton to a water molecule. ), some metal ions function as acids in aqueous solutions. What is the pH of a 0.233 M solution of aniline hydrochloride? 6 For both types of salts, a comparison of the Ka and Kb values allows prediction of the solutions acid-base status, as illustrated in the following example exercise. 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. However, the ammonium ion, the conjugate acid of ammonia, reacts with water and increases the hydronium ion concentration: \[\ce{NH4+}(aq)+\ce{H2O}(l)\ce{H3O+}(aq)+\ce{NH3}(aq) \nonumber \]. Ammonium Chloride (NH4Cl) - Ammonium chloride is an inorganic compound with formula NH4Cl. 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? 0 0 Similar questions The solution will be acidic. Save my name, email, and website in this browser for the next time I comment. This relation holds for any base and its conjugate acid or for any acid and its conjugate base. Determine the acetic acid concentration in a solution with \(\ce{[CH3CO2- ]}=0.050\:M\) and [OH] = 2.5 106 M at equilibrium. This is similar to the simplification of the formula of the hydronium ion, H3O+ to H+. A solution of this salt contains sodium ions and acetate ions. If you are redistributing all or part of this book in a print format, (CH This conjugate acid is a weak acid. However, even if we mix stoichiometrically equivalent quantities, we may find that the resulting solution is not neutral. When hydrogen chloride is readily available, a direct neutralization reaction may be used for the production of ammonium chloride. 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. When we neutralize a weak base with a strong acid, the product is a salt containing the conjugate acid of the weak base. NH3 + OH- + HClC. Bronsted-Lowry theory: A molecule that readily gives away protons in an aqueous solution is an acid while the molecule that takes up those protons, given away by another molecule, is a base. 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. The second column is blank. Ion(s) expected to hydrolyze, spectator ion(s), and net ionic equation(s) for the hydrolysis of NaCl, NH4Cl, NaCH3COO, and (NH4)2CO3. This is the most complex of the four types of reactions. The beneficial bacteria feed on starches in the cucumber and produce lactic acid as a waste product in a process called fermentation. The third column has the following: approximately 0, x, x. While basic salt is formed by the combination of weak acid along with a strong base. Home | About | Contact | Copyright | Report Content | Privacy | Cookie Policy | Terms & Conditions | Sitemap. 11 Uses of Platinum Laboratory, Commercial, and Miscellaneous, CH3Br Lewis Structure, Geometry, Hybridization, and Polarity. Hydrolysis involves the reaction of an organic chemical with water to form two or more new substances and usually means the cleavage of chemical bonds by the addition of water. The value of Kb can be calculated from the value of the ionization constant of water, Kw, and Ka, the ionization constant of the conjugate acid of the anion using the equation: For the acetate ion and its conjugate acid we have: \[\mathrm{\mathit{K}_b(for\:\ce{CH_3CO_2^-})=\dfrac{\mathit{K}_w}{\mathit{K}_a(for\:CH_3CO_2H)}=\dfrac{1.010^{14}}{1.810^{5}}=5.610^{10}} \nonumber \]. The molecular and net ionic equations are shown below. 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. Keep in mind that a salt will only be basic if it contains the conjugate base of a weak acid. i) citrate buffer ii) HCO3 - + H2CO3 iii) NH4OH + NH4Cl 3) Derive the equation which implies that the degree of dissociation of weak acid. When you dissolve ammonium chloride crystals in water (H2O), the ammonium chloride compound decomposes into its component ions: NH4+ and Cl-. It is defined as the fraction (or percentage) of the total salt which is hydrolysed at equilibrium. The pH of the solutions may be calculated using familiar equilibrium techniques, or it may be qualitatively determined to be acidic, basic, or neutral depending on the relative Ka and Kb of the ions involved. The acetate ion behaves as a base in this reaction; hydroxide ions are a product. ----- NH4Cl. Lastly, the reaction of a strong acid with a strong base gives neutral salts. (a) basic; (b) neutral; (c) acidic; (d) basic, Unlike the group 1 and 2 metal ions of the preceding examples (Na+, Ca2+, etc. A book which I am reading has this topic on hydrolysis of salts. 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. Ammonium chloride is used in veterinary medicine in the prevention of urinary stones in sheep, goats, and cattle. \(\ce{Al(H2O)6^3+}(aq)+\ce{H2O}(l)\ce{H3O+}(aq)+\ce{Al(H2O)5(OH)^2+}(aq) \hspace{20px} K_\ce{a}=1.410^{5}\). One example is the use of baking soda, or sodium bicarbonate in baking. Determine the acetic acid concentration in a solution with \(\ce{[CH3CO2- ]}=0.050\:M\) and [OH] = 2.5 106 M at equilibrium. For example, if 90% of a salt solution is hydrolysed, its degree of hydrolysis is 0.90 or as 90%. No hydrolysis occurs.Please Explain.also what is hydrolysis?!!!! HF ( a q) + NaOH ( a q) NaF ( a q) + H 2 O ( l) HF ( a q) + OH ( a q) F ( a q) + H 2 O ( l) Since sodium fluoride is soluble, the sodium ion is a spectator ion in the neutralization reaction. Is the salt for hydrolysis of ammonium chloride acidic or basic? The pH value for 1 M solution of NH4Cl can now be calculated as: As the pH value of ammonium chloride is less than 7, therefore, NH4Cl is acidic. When the conjugate acid and the conjugate base are of unequal strengths, the solution can be either acidic or basic, depending on the relative strengths of the two conjugates. The OpenStax name, OpenStax logo, OpenStax book covers, OpenStax CNX name, and OpenStax CNX logo Creative Commons Attribution License A strong base produces a weak conjugate acid. Cooking is essentially synthetic chemistry that happens to be safe to eat. 3 NH4Cl is not a base as it does not fit into the definition of base given by any of the acid-base theory viz. Several antacids have aluminum hydroxide, Al(OH)3, as an active ingredient. We determine Kb as follows: \[K_\ce{b}=\ce{\dfrac{[CH3CO2H][OH- ]}{[CH3CO2- ]}}=5.610^{10} \nonumber \], \[=\dfrac{[\ce{CH3CO2H}](2.510^{6})}{(0.050)}=5.610^{10} \nonumber \]. When we mix solutions of an acid and a base, an acid-base neutralization reaction occurs. In the case of NH4Cl, we have already learned that it is an ionic salt formed by the neutralization of a strong acid and a weak base. NH4Cl is an acidic salt. Solution: 1) Here is the chemical reaction (net ionic) for the hydrolysis of NH 4 Cl: NH 4 + + H 2 O NH 3 + H 3 O +. HCl is a strong acid while NH3 is a weak base and NH4Cl is formed as the product of their neutralization reaction. In spite of the unusual appearance of the acid, this is a typical acid ionization problem. Ionization increases as the charge of the metal ion increases or as the size of the metal ion decreases. 12th Chemistry EngMed QueBank MSCERT | PDF | Crystal Structure | Chlorine The aluminum hydroxide tends to cause constipation, and some antacids use aluminum hydroxide in concert with magnesium hydroxide to balance the side effects of the two substances. The solution is neutral. Milk of Magnesia is a suspension of the sparingly soluble base magnesium hydroxide, Mg(OH)2. To learn more about the Structure, Properties, Preparation, Uses and FAQs of Ammonium Chloride (NH4Cl), Visit BYJU'S for more content. It turns out that fish have volatile amines (bases) in their systems, which are neutralized by the acids to yield involatile ammonium salts. The value of Kb can be calculated from the value of the ionization constant of water, Kw, and Ka, the ionization constant of the conjugate acid of the anion using the equation: For the acetate ion and its conjugate acid we have: \[\mathrm{\mathit{K}_b(for\:\ce{CH_3CO_2^-})=\dfrac{\mathit{K}_w}{\mathit{K}_a(for\:CH_3CO_2H)}=\dfrac{1.010^{14}}{1.810^{5}}=5.610^{10}} \nonumber \]. Except where otherwise noted, textbooks on this site The bromide ion is the conjugate base of a strong acid, and so it is of negligible base strength (no appreciable base ionization). 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. For example, dissolving sulfuric acid in water yields hydronium and bisulfate. Acids and Bases in Aqueous Solutions. What is degree hydrolysis? Milk of Magnesia is a suspension of the sparingly soluble base magnesium hydroxide, Mg(OH)2. A weak acid and a strong base yield a weakly basic solution. 6 CO (If this occurs in other solvents, it will be called 'solvolysis' or just the name of solvent plus -lysis such as ethanolysis.) K a of NH 4 + = 5.65 x 10 10.. Because acetic acid is a weak acid, its Ka is measurable and Kb > 0 (acetate ion is a weak base). Ammonium Chloride naturally occurs as a mineral called sal ammoniac. It is isolated as aniline hydrochloride, \(\ce{[C6H5NH3+]Cl}\), a salt prepared by the reaction of the weak base aniline and hydrochloric acid. It works according to the reaction: \[Mg(OH)_2(s)Mg^{2+}(aq)+2OH^-(aq) \nonumber \]. However, the ionization of a cation carrying more than one charge is usually not extensive beyond the first stage. 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 ). (d) The NH4+NH4+ ion is acidic (see above discussion) and the F ion is basic (conjugate base of the weak acid HF). Some salts formed in neutralization reactions may make the product solutions slightly acidic or slightly basic. 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(. and its Kb is 1.010146.2108=1.6107.1.010146.2108=1.6107. The word neutralization seems to imply that a stoichiometrically equivalent solution of an acid and a base would be neutral. A solution is neutral when it contains equal concentrations of hydronium and hydroxide ions. It could contain either an excess of hydronium ions or an excess of hydroxide ions because the nature of the salt formed determines whether the solution is acidic, neutral, or basic. So, Is NH4Cl an acid or base? It is soluble in liquid ammonia, hydrazine, and slightly soluble in acetone. 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 ). Ammonia is moderately basic; a 1.0 M aqueous solution has a pH of 11.6, and if a strong acid is added to such a solution until the solution is neutral (pH = 7), 99.4% of the ammonia molecules are protonated. When we have heartburn, it feels better if we reduce the excess acid in the esophagus by taking an antacid. 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. Because Kb >> Ka, the solution is basic. The vegetable, such as a cucumber, is placed in a sealed jar submerged in a brine solution. If we can find the equilibrium constant for the reaction, the process is straightforward. The `pH` of a `0.1` M solution of `NH_4Cl` is `5.127`. 3+ The pH of the solutions may be calculated using familiar equilibrium techniques, or it may be qualitatively determined to be acidic, basic, or neutral depending on the relative Ka and Kb of the ions involved. ), This table has two main columns and four rows. Chemistry Chemistry questions and answers Net-Ionic Equation for Hydrolysis? is dissolved in water (hint: NH4Cl + H2OF NH4 H THC Determine mathematic problems Determining mathematical problems can be difficult, but with practice it can become easier. However, practically all hydrated metal ions other than those of the alkali metals ionize to give acidic solutions. then you must include on every digital page view the following attribution: Use the information below to generate a citation. However, it is not difficult to determine Ka for \(\ce{NH4+}\) from the value of the ionization constant of water, Kw, and Kb, the ionization constant of its conjugate base, NH3, using the following relationship: \[K_\ce{w}=K_\ce{a}K_\ce{b} \nonumber \]. The sodium ion has no effect on the acidity of the solution. Now we have the ionization constant and the initial concentration of the weak acid, the information necessary to determine the equilibrium concentration of H3O+, and the pH: With these steps we find [H3O+] = 2.3 103 M and pH = 2.64, \(K_a\ce{(for\:NH4+)}=5.610^{10}\), [H3O+] = 7.5 106 M. \(\ce{C6H5NH3+}\) is the stronger acid (a) (b) . The aluminum ion is an example. A byproduct of the pickling process changes the flavor of the vegetables with the acid making them taste sour. Dec 15, 2022 OpenStax. 2 KAl(SO4)2. For example, sodium acetate, NaCH3CO2, is a salt formed by the reaction of the weak acid acetic acid with the strong base sodium hydroxide: \[\ce{CH3CO2H}(aq)+\ce{NaOH}(aq)\ce{NaCH3CO2}(aq)+\ce{H2O}(aq) \nonumber \]. As mentioned in the other answer, NH4Cl is an acidic salt, formed by the neutralization of a strong acid (HCl) with a weak base (NH3). Techiescientist is a Science Blog for students, parents, and teachers. A solution is neutral when it contains equal concentrations of hydronium and hydroxide ions. Ammonium Chloride is commercially prepared by a reaction between ammonia and hydrogen chloride also known as hydrochloric acid when present in an aqueous solution. What is \(\ce{[Al(H2O)5(OH)^2+]}\) in a 0.15-M solution of Al(NO3)3 that contains enough of the strong acid HNO3 to bring [H3O+] to 0.10 M? Solved What are the net ionic equations for the hydrolysis - Chegg HCl is a strong acid while NH3 is a weak base and NH4Cl is formed as the product of their neutralization reaction. Calculating the pH for 1 M NH4Cl Solution. The (aq) shows that they are aqueous dissolved in water.The equation for NH4Cl (Ammonium chloride) and H2O sometimes isnt considered a chemical reaction since it is easy to change the NH4+ and Cl- back to NH4Cl (just let the H2O evaporate). The brine solution favors the growth of beneficial bacteria and suppresses the growth of harmful bacteria. As an Amazon Associate we earn from qualifying purchases. When salt is added to the water, then cation, anion or both the ions of salt react with water and if the solution becomes either acidic or basic then it is hydrolysis process. This is called cationic hydrolysis. As seen in the above equation on dissolving in aqueous solution NH4Cl releases hydronium ions due to the hydrolysis of ammonium ions. There are a number of examples of acid-base chemistry in the culinary world. Glycine increased glucose absorption, while lysine decreased 32P absorption without affecting the 32P uptake by the tibia. What are the products of the hydrolysis of NH4Cl? | Homework.Study.com 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 HCl Molecule formed will completely ionises to form H+ ion, as shown above. It is also used for eliminating cough as it has an expectorant effect i.e. As you may have guessed, antacids are bases. In spite of the unusual appearance of the acid, this is a typical acid ionization problem. Why is an aqueous solution of NH4Cl Acidic? 3: Determining the Acidic or Basic Nature of Salts. Screen capture done with Camtasia Studio 4.0. When it reacts with an acid such as lemon juice, buttermilk, or sour cream in a batter, bubbles of carbon dioxide gas are formed from decomposition of the resulting carbonic acid, and the batter rises. Baking powder is a combination of sodium bicarbonate, and one or more acid salts that react when the two chemicals come in contact with water in the batter. 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 ). Lewis theory, Arrhenius theory, or Bronsted-Lowry theory. . 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. Salt hydrolysis is defined as the process in which a salt reacts with water to give back the acid and the base. The Molecular mass of NH4Cl is 53.49 gm/mol. 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. NH4OH + HClE. 2 It occurs near the volcanoes and forms volcanic rocks near fumaroles. 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(. Substituting the expressions for the equilibrium concentrations into the equation for the ionization constant yields: \(=\dfrac{(x)(x)}{0.10x}=1.4 \times 10^{5}\), \[\ce{[H3O+]}=0+x=1.210^{3}\:M \nonumber \], \[\mathrm{pH=log[H_3O^+]=2.92(an\: acidic\: solution)} \nonumber \]. Do Men Still Wear Button Holes At Weddings? Here's the concept of strong and weak conjugate base/acid:- This is sometimes true, but the salts that are formed in these reactions may have acidic or basic properties of their own, as we shall now see. THe ammonium is acting as an acid (proton donor) hence the ammonia (NH3) is the conjugate base of the acid (ammonium). NaHCO3 is a base. What is the hydrolysis reaction for NH4Cl? This increases the amount of hydroxide ion in the solution produced in the reaction and renders it slightly basic. A solution of this salt contains ammonium ions and chloride ions. In its pure form, it is white crystalline salt. But because HCl is a strong acid, the Cl ion is not basic in solution, and it isnt capable of deprotonating water. The reaction is: We are given two of three equilibrium concentrations and asked to find the missing concentration. There are a number of examples of acid-base chemistry in the culinary world. 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. Thank you! TimesMojo is a social question-and-answer website where you can get all the answers to your questions. Potassium acetate (CH3COOK) is the potassium salt of acetic acid. Ka, for the acid \(\ce{NH4+}\): \[\ce{\dfrac{[H3O+][NH3]}{[NH4+]}}=K_\ce{a} \nonumber \]. The constants for the different stages of ionization are not known for many metal ions, so we cannot calculate the extent of their ionization. The acetate ion, Required fields are marked *. Which response gives the products of hydrolysis ofNH4Cl? A. NH4+ + HCl I am Savitri,a science enthusiast with a passion to answer all the questions of the universe. 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, \[K_\ce{a}=\ce{\dfrac{[H3O+][Al(H2O)5(OH)^2+]}{[Al(H2O)6^3+]}} \nonumber \]. The first column has the following: 0.10 (which appears in red), negative x, 0.10 minus x. Urea, equimolar to the NH4Cl, showed no effect on intestinal absorption or bone accumulation, indicating little or no hydrolysis of urea in the chick duodenum in the 20-minute test period. Why is NH4Cl acidic? Equation for NH4Cl + H2O (Ammonium chloride + Water) Legal. It is used for producing lower temperatures in cooling baths. The equilibrium equation for this reaction is the ionization constant, Kb, for the base \(\ce{CH3CO2-}\). 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. When an acid or base is dissolved in an aqueous solution it results in dissociation of its molecules resulting in the formation of ions, therefore, the acidity or basicity of a substance in an aqueous solution can be understood by drawing its dissociation equation. The reaction, \[CaCO_3(s)+2HCl(aq)CaCl_2(aq)+H_2O(l)+CO_2(g) \nonumber \]. The fourth column has the following: 0, x, x. If Ka > Kb, the solution is acidic, and if Kb > Ka, the solution is basic. Your email address will not be published. The new step in this example is to determine Ka for the \(\ce{C6H5NH3+}\) ion. Therefore, ammonium chloride is an acidic salt. Ammonium Chloride | NH4Cl - PubChem 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). These hydronium ions are responsible for the acidity of the aqueous solution of ammonium chloride. The new step in this example is to determine Ka for the \(\ce{C6H5NH3+}\) ion. It is an inorganic compound and a salt of ammonia. Calculate (i) the degree of hydrolysis (ii) the hydrolysis constant and (iii) Therefore, NH4+ is a strong conjugate acid while Cl- is a weak conjugate base. Ammonium Chloride is majorly manufactured as a by-product of the Solvay process which is used for the production of Sodium Carbonate. 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. 21.21: Hydrolysis of Salts - Equations - Chemistry LibreTexts Salts that form from a strong acid and a weak base are acid salts, like ammonium chloride (NH4Cl). As with other polyprotic acids, the hydrated aluminum ion ionizes in stages, as shown by: \[\ce{Al(H2O)6^3+}(aq)+\ce{H2O}(l)\ce{H3O+}(aq)+\ce{Al(H2O)5(OH)^2+}(aq) \nonumber \], \[\ce{Al(H2O)5(OH)^2+}(aq)+\ce{H2O}(l)\ce{H3O+}(aq)+\ce{Al(H2O)4(OH)2+}(aq) \nonumber \], \[\ce{Al(H2O)4(OH)2+}(aq)+\ce{H2O}(l)\ce{H3O+}(aq)+\ce{Al(H2O)3(OH)3}(aq) \nonumber \].