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For example, ammonium chloride, NH4Cl, is a salt formed by the reaction of the weak base ammonia with the strong acid HCl: \[\ce{NH3}(aq)+\ce{HCl}(aq)\ce{NH4Cl}(aq) \nonumber \]. Introduction Equation for NH4Cl + H2O (Ammonium chloride + Water) Wayne Breslyn 626K subscribers Subscribe 168K views 4 years ago In this video we will describe the equation NH4Cl + H2O and. The hydrolysis constant of NH 4Cl would be: A 1.8010 19 B 5.5510 10 C 5.5510 9 D 1.810 5 Hard Solution Verified by Toppr Correct option is B) NH 4OHNH 4++OH K b= NH 4OH[NH 4+][OH ] NH 4Cl+H 2OHCl+NH 4OH K h= NH 4Cl[HCl][NH 4OH] K w=K bK h K h= K bK w= 1.810 5110 14 =5.5510 10 The solution will be acidic. 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. NH4Cl is ammonium chloride. 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. Additional examples of the first stage in the ionization of hydrated metal ions are: \[\ce{Fe(H2O)6^3+}(aq)+\ce{H2O}(l)\ce{H3O+}(aq)+\ce{Fe(H2O)5(OH)^2+}(aq) \hspace{20px} K_\ce{a}=2.74 \nonumber \], \[\ce{Cu(H2O)6^2+}(aq)+\ce{H2O}(l)\ce{H3O+}(aq)+\ce{Cu(H2O)5(OH)+}(aq) \hspace{20px} K_\ce{a}=~6.3 \nonumber \], \[\ce{Zn(H2O)4^2+}(aq)+\ce{H2O}(l)\ce{H3O+}(aq)+\ce{Zn(H2O)3(OH)+}(aq) \hspace{20px} K_\ce{a}=9.6 \nonumber \]. Determine the acetic acid concentration in a solution with \(\ce{[CH3CO2- ]}=0.050\:M\) and [OH] = 2.5 106 M at equilibrium. 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(. Textbook content produced by OpenStax is licensed under a Creative Commons Attribution License . 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) . It works according to the reaction: \[Mg(OH)_2(s)Mg^{2+}(aq)+2OH^-(aq) \nonumber \]. (CH Ionization increases as the charge of the metal ion increases or as the size of the metal ion decreases. The process involves the reaction of Ammonia, Sodium Chloride, and Carbon dioxide in water. However, practically all hydrated metal ions other than those of the alkali metals ionize to give acidic solutions. EMMY NOMINATIONS 2022: Outstanding Limited Or Anthology Series, EMMY NOMINATIONS 2022: Outstanding Lead Actress In A Comedy Series, EMMY NOMINATIONS 2022: Outstanding Supporting Actor In A Comedy Series, EMMY NOMINATIONS 2022: Outstanding Lead Actress In A Limited Or Anthology Series Or Movie, EMMY NOMINATIONS 2022: Outstanding Lead Actor In A Limited Or Anthology Series Or Movie. The beneficial bacteria feed on starches in the cucumber and produce lactic acid as a waste product in a process called fermentation. It occurs near the volcanoes and forms volcanic rocks near fumaroles. The word neutralization seems to imply that a stoichiometrically equivalent solution of an acid and a base would be neutral. K a of NH 4 + = 5.65 x 10 10.. It is actually the concentration of hydrogen ions in a solution. So, Is NH4Cl an acid or base? A weak acid plus a weak base can yield either an acidic, basic, or neutral solution. Acids and Bases in Aqueous Solutions. Many people like to put lemon juice or vinegar, both of which are acids, on cooked fish (Figure \(\PageIndex{1}\)). 2 As shown in Figure 14.13, the add 15 ml approx of water and 15m1 'approx of dilute sulphuric acid (2M H2SO.). One of the most common antacids is calcium carbonate, CaCO3. 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 chloride ion is the conjugate base of hydrochloric acid, and so its base ionization (or base hydrolysis) reaction is represented by. But this pH dependent reaction yields different products. It is also used as a feed supplement for cattle. This conjugate base is usually a weak base. 2 Ka, for the acid \(\ce{NH4+}\): \[\ce{\dfrac{[H3O+][NH3]}{[NH4+]}}=K_\ce{a} \nonumber \]. 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. In anionic hydrolysis, the solution becomes slightly basic (p H >7). The chloride ion is the conjugate base of hydrochloric acid, and so its base ionization (or base hydrolysis) reaction is represented by Since HCl is a strong acid, Ka is immeasurably large and Kb 0 (chloride ions don't undergo appreciable hydrolysis). https://openstax.org/books/chemistry-2e/pages/1-introduction, https://openstax.org/books/chemistry-2e/pages/14-4-hydrolysis-of-salts, Creative Commons Attribution 4.0 International License, Predict whether a salt solution will be acidic, basic, or neutral, Calculate the concentrations of the various species in a salt solution, Describe the acid ionization of hydrated metal ions. , NH and Cl . This relation holds for any base and its conjugate acid or for any acid and its conjugate base. It is defined as the fraction (or percentage) of the total salt which is hydrolysed at equilibrium. To learn more about the Structure, Properties, Preparation, Uses and FAQs of Ammonium Chloride (NH4Cl), Visit BYJU'S for more content. Step-by-step answer: Salts which are made from strong acid and weak base undergo cationic hydrolysis. Salts that form from a weak acid and a strong base are basic salts, like sodium bicarbonate (NaHCO3). This conjugate acid is a weak acid. As discussed earlier, the combination of strong acid and weak base results in the formation of an acidic salt. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. What is salt hydrolysis explain with example? NH4Cl is not a base as it does not fit into the definition of base given by any of the acid-base theory viz. It is isolated as aniline hydrochloride, \(\ce{[C6H5NH3+]Cl}\), a salt prepared by the reaction of the weak base aniline and hydrochloric acid. Save my name, email, and website in this browser for the next time I comment. This page titled 14.4: Hydrolysis of Salt Solutions is shared under a CC BY license and was authored, remixed, and/or curated by OpenStax. When we neutralize a weak base with a strong acid, the product is a salt containing the conjugate acid of the weak base. 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. The reaction, \[CaCO_3(s)+2HCl(aq)CaCl_2(aq)+H_2O(l)+CO_2(g) \nonumber \]. The chloride ion has no effect on the acidity of the solution since HCl is a strong acid. 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. 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. If we can find the equilibrium constant for the reaction, the process is straightforward. Solve for x and the equilibrium concentrations. Therefore, NH4+ is a strong conjugate acid while Cl- is a weak conjugate base. Potassium acetate (CH3COOK) is the potassium salt of acetic acid. Dec 15, 2022 OpenStax. 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. 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. Hydrolysis of Salts NH4Cl is the salt of a strong acid (hydrochloric acid) and a weak base (ammonia) The NH4+ ions will react with water: NH4+(aq) + H2O(aq) Clarify math tasks. Without the harmful bacteria consuming the cucumbers they are able to last much longer than if they were unprotected. (a) basic; (b) neutral; (c) acidic; (d) basic, Unlike the group 1 and 2 metal ions of the preceding examples (Na+, Ca2+, etc. 3+ Ammonium Chloride is commercially prepared by a reaction between ammonia and hydrogen chloride also known as hydrochloric acid when present in an aqueous solution. The fourth column has the following: 0, x, x. 4) A buffer solution contains 0.3 mol dm -3 NH4OH ( = 1.8 x10-5) and 0.4 mol dm-3 of NH4Cl. 2 NH4CN is a salt of weak acid HCN (Ka = 6.2 10-10) and a w. When sodium carbonate dissolves in water, it will react with hydroxide ion and will form sodium hydroxide and form alkaline solution. Write formula equations and net ionic equations for the hydrolysis of sodium carbonate in water. not only neutralizes stomach acid, it also produces CO2(g), which may result in a satisfying belch. Cooking is essentially synthetic chemistry that happens to be safe to eat. Is salt hydrolysis possible in ch3coonh4? 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. Strong acid along with weak base are known to form acidic salt. The burning sensation associated with heartburn is a result of the acid of the stomach leaking through the muscular valve at the top of the stomach into the lower reaches of the esophagus. The reaction is: We are given two of three equilibrium concentrations and asked to find the missing concentration. Expression for equilibrium constant (Ka or Kb)? However, the ammonium ion, the conjugate acid of ammonia, reacts with water and increases the hydronium ion concentration: \[\ce{NH4+}(aq)+\ce{H2O}(l)\ce{H3O+}(aq)+\ce{NH3}(aq) \nonumber \]. Besides these there will be some unionised NH4OH. Example 2.4. Once Sodium bicarbonate precipitates it is filtered out from the solution. Home | About | Contact | Copyright | Report Content | Privacy | Cookie Policy | Terms & Conditions | Sitemap. 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. Ammonium Chloride is denoted by the chemical formula NH4Cl. The conjugate acid of the strong base is a weaker acid than water and has no effect on the acidity of the resulting solution. 0 0 Similar questions Chemistry Chemistry questions and answers Net-Ionic Equation for Hydrolysis? O) Ion(s) expected to hydrolyze, spectator ion(s), and net ionic equation(s) for the hydrolysis of NaCl, NH4Cl, NaCH3COO, and (NH4)2CO3. ( Keep in mind that a salt will only be basic if it contains the conjugate base of a weak acid. At the same time, the NH4Cl is a very different substance than NH4+ and Cl-.If you need to know how to balance chemical reactions, see my complete tutorial on balancing all types of chemical equations:Balancing Equations in 5 Easy Steps: https://youtu.be/zmdxMlb88FsMore Practice Balancing: https://youtu.be/Qci7hiBy7EQDrawing/writing done in InkScape. The dissociation chemical reaction is: NH4Cl(solid) = NH4+(aqueous) + Cl-(aqueous). A solution of this salt contains ammonium ions and chloride ions. Some handbooks do not report values of Kb. The new step in this example is to determine Ka for the \(\ce{C6H5NH3+}\) ion. Stock iron(II) solution (200Ug mL-1 Fe) ferrous ammonium sulfate hexahydrate mass= 0.1437g, transfer it to a 100 ml beaker. 44) What are the products of hydrolysis of NH4Cl? Thank you! Example 14.4. Dissolving sodium acetate in water yields a solution of inert cations (Na+) and weak base anions The acetate ion behaves as a base in this reaction; hydroxide ions are a product. Chloride is a very weak base and will not accept a proton to a measurable extent. 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). If you are redistributing all or part of this book in a print format, As a salt acquires its pH based upon the acidic or basic strength of its constituent compounds, NH4Cl is acidic. K b(NH 4OH)=1.810 5 Medium Solution Verified by Toppr Solve any question of Equilibrium with:- Patterns of problems > Was this answer helpful? 6 The brine solution favors the growth of beneficial bacteria and suppresses the growth of harmful bacteria. 3: Determining the Acidic or Basic Nature of Salts. The acetate ion, The second column is blank. The hydroxide ions generated in this equilibrium then go on to react with the hydronium ions from the stomach acid, so that : This reaction does not produce carbon dioxide, but magnesium-containing antacids can have a laxative effect. 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 ). A weak base produces a strong conjugate acid. The fluoride ion is capable of reacting, to a small extent, with water, accepting a . 3 What is the approximately pH of a 0.1M solution of the salt. This table has two main columns and four rows. , is the conjugate base of acetic acid, CH3CO2H, and so its base ionization (or base hydrolysis) reaction is represented by. As Cl- is a weak conjugate base it cannot further accept a proton. The HCl Molecule formed will completely ionises to form H+ ion, as shown above. HCl is a strong acid while NH3 is a weak base and NH4Cl is formed as the product of their neutralization reaction. It is isolated as aniline hydrochloride, \(\ce{[C6H5NH3+]Cl}\), a salt prepared by the reaction of the weak base aniline and hydrochloric acid. 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. 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. Question: Which response gives the products of hydrolysis of NH4Cl?A. This salt does not undergo hydrolysis. The lactic acid eventually increases the acidity of the brine to a level that kills any harmful bacteria, which require a basic environment. HCl is a strong acid while NH3 is a weak base and NH4Cl is formed as the product of their neutralization reaction. As an Amazon Associate we earn from qualifying purchases. In spite of the unusual appearance of the acid, this is a typical acid ionization problem. A byproduct of the pickling process changes the flavor of the vegetables with the acid making them taste sour. When we mix solutions of an acid and a base, an acid-base neutralization reaction occurs. CO Salts of weak acids and strong bases undergo anionic hydrolysis and yield basic solution. If we can find the equilibrium constant for the reaction, the process is straightforward. Chloride is a very weak base and will not accept a proton to a measurable extent. This increases the amount of hydroxide ion in the solution produced in the reaction and renders it slightly basic. citation tool such as, Authors: Paul Flowers, Klaus Theopold, Richard Langley, William R. Robinson, PhD. They are given below: Lewis theory: A molecule that gives away an unshared pair of electrons to another molecule is known as a base while the molecule that accepts those electrons is termed an acid. The concentration of hydrogen ions is calculated as: As the value of Ka = NH4Cl is 5.6 X 10-10 at 25C, Also, we are calculating the hydrogen ion concentration for 1 M NH4Cl solution. not only neutralizes stomach acid, it also produces CO2(g), which may result in a satisfying belch. Required fields are marked *. The \(\ce{C6H5NH3+}\) ion is the conjugate acid of a weak base. A solution of this salt contains sodium ions and acetate ions. A weak acid plus a weak base can yield either an acidic, basic, or neutral solution. 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. Our mission is to improve educational access and learning for everyone. Hydrolysis reactions break bonds and release energy. 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, \[K_\ce{a}=\ce{\dfrac{[H3O+][Al(H2O)5(OH)^2+]}{[Al(H2O)6^3+]}} \nonumber \]. are licensed under a, Measurement Uncertainty, Accuracy, and Precision, Mathematical Treatment of Measurement Results, Determining Empirical and Molecular Formulas, Electronic Structure and Periodic Properties of Elements, Electronic Structure of Atoms (Electron Configurations), Periodic Variations in Element Properties, Relating Pressure, Volume, Amount, and Temperature: The Ideal Gas Law, Stoichiometry of Gaseous Substances, Mixtures, and Reactions, Shifting Equilibria: Le Chteliers Principle, The Second and Third Laws of Thermodynamics, Representative Metals, Metalloids, and Nonmetals, Occurrence and Preparation of the Representative Metals, Structure and General Properties of the Metalloids, Structure and General Properties of the Nonmetals, Occurrence, Preparation, and Compounds of Hydrogen, Occurrence, Preparation, and Properties of Carbonates, Occurrence, Preparation, and Properties of Nitrogen, Occurrence, Preparation, and Properties of Phosphorus, Occurrence, Preparation, and Compounds of Oxygen, Occurrence, Preparation, and Properties of Sulfur, Occurrence, Preparation, and Properties of Halogens, Occurrence, Preparation, and Properties of the Noble Gases, Transition Metals and Coordination Chemistry, Occurrence, Preparation, and Properties of Transition Metals and Their Compounds, Coordination Chemistry of Transition Metals, Spectroscopic and Magnetic Properties of Coordination Compounds, Aldehydes, Ketones, Carboxylic Acids, and Esters, Composition of Commercial Acids and Bases, Standard Thermodynamic Properties for Selected Substances, Standard Electrode (Half-Cell) Potentials, Half-Lives for Several Radioactive Isotopes. NaCl is neutral. 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. So the ions present in the Solution of NH4Cl, will be, NH4+ , Cl-, H+, OH-. 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 pH value for NH4Cl lies between 4.5 and 6 and its pKa value is 9.24, therefore, it is mildly acidic. The third column has the following: approximately 0, x, x. When an aluminum ion reacts with water, the hydrated aluminum ion becomes a weak acid. $$\ce {RCN + 2H2O + HCl -> RCOOH + NH4Cl}$$. 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? When water and salts react, there are many possibilities . \(\ce{Al(H2O)6^3+}(aq)+\ce{H2O}(l)\ce{H3O+}(aq)+\ce{Al(H2O)5(OH)^2+}(aq) \hspace{20px} K_\ce{a}=1.410^{5}\). The first column has the following: 0.10 (which appears in red), negative x, 0.10 minus x. The arithmetic checks; when 1.2 103 M is substituted for x, the result = Ka. Solving the above equation for the acetic acid molarity yields [CH3CO2H] = 1.1 105 M. Some salts are composed of both acidic and basic ions, and so the pH of their solutions will depend on the relative strengths of these two species. One example is the use of baking soda, or sodium bicarbonate in baking. When you dissolve ammonium chloride crystals in water (H2O), the ammonium chloride compound decomposes into its component ions: NH4+ and Cl-. Thus, dissolving ammonium chloride in water yields a solution of weak acid cations (NH4+NH4+) and inert anions (Cl), resulting in an acidic solution. resulting in a basic solution. Ammonium Chloride is an acidic salt. It turns out that fish have volatile amines (bases) in their systems, which are neutralized by the acids to yield involatile ammonium salts. 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. Some aquatic animals utilize ammonium chloride to maintain their buoyancy in seawater. It is used for producing lower temperatures in cooling baths. 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. See Answer Copper sulphate will form an acidic solution. The `pH` of a `0.1` M solution of `NH_4Cl` is `5.127`. The first-step acid ionization equations for a few other acidic metal ions are shown below: An ICE table with the provided information is. 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? : a chemical process of decomposition involving the splitting of a bond and the addition of the hydrogen cation and the hydroxide anion of water. This conjugate acid is a weak acid. Determine the degree of hydrolysis of this salt in 0.01 M solution and the pH of the solution. calculate the moles of ferrous ammonium sulfate hexahydrate solution in unit ug/mL. 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 : \[\mathrm{\mathit{K}_a(for\:C_6H_5NH_3^+)\mathit{K}_b(for\:C_6H_5NH_2)=\mathit{K}_w=1.010^{14}} \nonumber \], \[\mathrm{\mathit{K}_a(for\:C_6H_5NH_3^+)=\dfrac{\mathit{K}_w}{\mathit{K}_b(for\:C_6H_5NH_2)}=\dfrac{1.010^{14}}{4.610^{10}}=2.310^{5}} \nonumber \]. 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: \[\ce{Al(NO3)3}(s)+\ce{6H2O}(l)\ce{Al(H2O)6^3+}(aq)+\ce{3NO3-}(aq) \nonumber \]. 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? This is similar to the simplification of the formula of the hydronium ion, H3O+ to H+. 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). It appears as a hygroscopic white solid. The acetate ion behaves as a base in this reaction; hydroxide ions are a product. A weak acid and a strong base yield a weakly basic solution. Al The hydrolysis of an acidic salt, such as ammonia. When NH 4 Cl goes through the hydrolysis process, it split into two ions (NH 4+ + Cl - ). Substituting the expressions for the equilibrium concentrations into the equation for the ionization constant yields: \(=\dfrac{(x)(x)}{0.10x}=1.4 \times 10^{5}\), \[\ce{[H3O+]}=0+x=1.210^{3}\:M \nonumber \], \[\mathrm{pH=log[H_3O^+]=2.92(an\: acidic\: solution)} \nonumber \]. For example, if 90% of a salt solution is hydrolysed, its degree of hydrolysis is 0.90 or as 90%. 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 ). However, the conjugate base of the weak acid is a weak base and ionizes slightly in water. It is also used for eliminating cough as it has an expectorant effect i.e. If Ka > Kb, the solution is acidic, and if Kb > Ka, the solution is basic. The equilibrium equation for this reaction is the ionization constant, Kb, for the base \(\ce{CH3CO2-}\). \(\ce{Al(H2O)6^3+}(aq)+\ce{H2O}(l)\ce{H3O+}(aq)+\ce{Al(H2O)5(OH)^2+}(aq) \hspace{20px} K_\ce{a}=1.410^{5}\). Legal. The reaction for the preparation of NH4Cl is as follows: As clear from the above-mentioned chemical equation, NH4Cl is a neutralization product of hydrogen chloride, which is a strong acid and almost completely ionizes in the aqueous solution to form protons, and ammonia, which is known to be a weak base.