 9. 04. 2023

# hydrolysis of nh4cl

consent of Rice University. 3: Determining the Acidic or Basic Nature of Salts. Therefore, NH4+ is a strong conjugate acid while Cl- is a weak conjugate base. 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. It works according to the reaction: $Mg(OH)_2(s)Mg^{2+}(aq)+2OH^-(aq) \nonumber$. $$\ce{Al(H2O)6^3+}(aq)+\ce{H2O}(l)\ce{H3O+}(aq)+\ce{Al(H2O)5(OH)^2+}(aq) \hspace{20px} K_\ce{a}=1.410^{5}$$. The reaction is: We are given two of three equilibrium concentrations and asked to find the missing concentration. Do Men Still Wear Button Holes At Weddings? Thus hydrolysis adds water to break down, whereas condensation builds up by removing water. In this video we will describe the equation NH4Cl + H2O and write what happens when NH4Cl is dissolved in water.When NH4Cl is dissolved in H2O (water) it will dissociate (dissolve) into NH4+ and Cl- ions. NH4Cl is ammonium chloride. Stock iron(II) solution (200Ug mL-1 Fe) ferrous ammonium sulfate hexahydrate mass= 0.1437g, transfer it to a 100 ml beaker. , A weak acid produces a strong conjugate base. 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. If you are redistributing all or part of this book in a print format, 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. We will not find a value of Ka for the ammonium ion in Table E1. As with other polyprotic acids, the hydrated aluminum ion ionizes in stages, as shown by: $\ce{Al(H2O)6^3+}(aq)+\ce{H2O}(l)\ce{H3O+}(aq)+\ce{Al(H2O)5(OH)^2+}(aq) \nonumber$, $\ce{Al(H2O)5(OH)^2+}(aq)+\ce{H2O}(l)\ce{H3O+}(aq)+\ce{Al(H2O)4(OH)2+}(aq) \nonumber$, $\ce{Al(H2O)4(OH)2+}(aq)+\ce{H2O}(l)\ce{H3O+}(aq)+\ce{Al(H2O)3(OH)3}(aq) \nonumber$. If Ka > Kb, the solution is acidic, and if Kb > Ka, the solution is basic. The bromide ion is the conjugate base of a strong acid, and so it is of negligible base strength (no appreciable base ionization). 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. Pickling is a method used to preserve vegetables using a naturally produced acidic environment. A byproduct of the pickling process changes the flavor of the vegetables with the acid making them taste sour. i) citrate buffer ii) HCO3 - + H2CO3 iii) NH4OH + NH4Cl 3) Derive the equation which implies that the degree of dissociation of weak acid. One example is the use of baking soda, or sodium bicarbonate in baking. It is a salt of a strong acid and a weak base. Home | About | Contact | Copyright | Report Content | Privacy | Cookie Policy | Terms & Conditions | Sitemap. 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 ). 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. When we neutralize a weak base with a strong acid, the product is a salt containing the conjugate acid of the weak base. A solution of this salt contains ammonium ions and chloride ions. These ions are not just loosely solvated by water molecules when dissolved, instead they are covalently bonded to a fixed number of water molecules to yield a complex ion (see chapter on coordination chemistry). It is isolated as aniline hydrochloride, $$\ce{[C6H5NH3+]Cl}$$, a salt prepared by the reaction of the weak base aniline and hydrochloric acid. Ion(s) expected to hydrolyze, spectator ion(s), and net ionic equation(s) for the hydrolysis of NaCl, NH4Cl, NaCH3COO, and (NH4)2CO3. NH4CL. Answer: Hydrolysis usually is a equilibrated reaction between ion from weak bases or acids and water. Biological macromolecules are ingested and hydrolyzed in the digestive tract to form smaller molecules that can be absorbed by cells and then further broken down to release energy. It is actually the concentration of hydrogen ions in a solution. Your email address will not be published. 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. 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 , The word neutralization seems to imply that a stoichiometrically equivalent solution of an acid and a base would be neutral. If we can find the equilibrium constant for the reaction, the process is straightforward. Calculate (i) the degree of hydrolysis (ii) the hydrolysis constant and (iii) N Calculate pOH of the solution add 15 ml approx of water and 15m1 'approx of dilute sulphuric acid (2M H2SO.). Hydrogen chloride being stronger, dissociated to give hydrogen ions and makes resulting solution acidic. not only neutralizes stomach acid, it also produces CO2(g), which may result in a satisfying belch. As we have seen in the section on chemical reactions, when an acid and base are mixed, they undergo a neutralization reaction. Solve for x and the equilibrium concentrations. 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. Potassium carbonate (K2CO3) is a white salt, soluble in water (insoluble in ethanol) which forms a strongly alkaline solution. However, the ammonium ion, the conjugate acid of ammonia, reacts with water and increases the hydronium ion concentration: $\ce{NH4+}(aq)+\ce{H2O}(l)\ce{H3O+}(aq)+\ce{NH3}(aq) \nonumber$. This is called cationic hydrolysis. 3 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. The beneficial bacteria feed on starches in the cucumber and produce lactic acid as a waste product in a process called fermentation. 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, $K_\ce{a}=\ce{\dfrac{[H3O+][Al(H2O)5(OH)^2+]}{[Al(H2O)6^3+]}} \nonumber$. When we mix solutions of an acid and a base, an acid-base neutralization reaction occurs. Salt hydrolysis is defined as the process in which a salt reacts with water to give back the acid and the base. calculate the moles of ferrous ammonium sulfate hexahydrate solution in unit ug/mL. Some handbooks do not report values of Kb. Check the work. What are the net ionic equations for the hydrolysis of the the following:NaC2H3O2Na2CO3NH4CLZnCl2KAl (SO4)2KAl (SO4)2 for 5 & 6 there are supposed to be 2 different hydrolysis reactions occuringAlso determine if each is Ka or Kb This problem has been solved! Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. Solving this equation we get [CH3CO2H] = 1.1 105 M. What is the pH of a 0.083-M solution of CN? Without the harmful bacteria consuming the cucumbers they are able to last much longer than if they were unprotected. This is similar to the simplification of the formula of the hydronium ion, H3O+ to H+. 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. In the preparation of metals, it is used for tin coating, where it is used for cleansing the metal surfaces of metal oxides. A weak acid plus a weak base can yield either an acidic, basic, or neutral solution. Aniline is an amine that is used to manufacture dyes. Screen capture done with Camtasia Studio 4.0. Pickling is a method used to preserve vegetables using a naturally produced acidic environment. However, the ammonium ion, the conjugate acid of ammonia, reacts with water and increases the hydronium ion concentration: $\ce{NH4+}(aq)+\ce{H2O}(l)\ce{H3O+}(aq)+\ce{NH3}(aq) \nonumber$. The second column is blank. , is the conjugate base of acetic acid, CH3CO2H, and so its base ionization (or base hydrolysis) reaction is represented by. 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. It is soluble in liquid ammonia, hydrazine, and slightly soluble in acetone. As an Amazon Associate we earn from qualifying purchases. NaHCO3 is a base. Since ammonia is a weak base, Kb is measurable and Ka > 0 (ammonium ion is a weak acid). The beneficial bacteria feed on starches in the cucumber and produce lactic acid as a waste product in a process called fermentation. 2 However, the ionization of a cation carrying more than one charge is usually not extensive beyond the first stage. Al 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. Save my name, email, and website in this browser for the next time I comment. Calculating the pH for 1 M NH4Cl Solution. However, the ionization of a cation carrying more than one charge is usually not extensive beyond the first stage. The chemical equation for the same is written as follows: Double decomposition of ammonium sulfate on reaction with sodium chloride also results in the formation of ammonium chloride. The Molecular mass of NH4Cl is 53.49 gm/mol. It turns out that fish have volatile amines (bases) in their systems, which are neutralized by the acids to yield involatile ammonium salts. 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. ---- pH of 0.1 M NH4Cl: 6.35 [H+] for NH4Cl [OH] for NH4Cl Hydrolysis Net Ionic Equation for hydrolysis of NH4Cl Ka or 2 Hint: We will probably need to convert pOH to pH or find [H3O+] using [OH] in the final stages of this problem. Write the net ionic equation for the hydrolysis reaction that occurs when ammonium chloride, NH.CI. The pH value of a substance is an indicator of the acidity or basicity of that substance in its aqueous solution. 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 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 : $\mathrm{\mathit{K}_a(for\:C_6H_5NH_3^+)\mathit{K}_b(for\:C_6H_5NH_2)=\mathit{K}_w=1.010^{14}} \nonumber$, $\mathrm{\mathit{K}_a(for\:C_6H_5NH_3^+)=\dfrac{\mathit{K}_w}{\mathit{K}_b(for\:C_6H_5NH_2)}=\dfrac{1.010^{14}}{4.610^{10}}=2.310^{5}} \nonumber$. As discussed earlier, the combination of strong acid and weak base results in the formation of an acidic salt. 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 . Use 4.9 1010 as Ka for HCN. One of the most common antacids is calcium carbonate, CaCO3. (2) If the acid produced is weak and the base produced is strong. The characteristic properties of aqueous solutions of Brnsted-Lowry acids are due to the presence of hydronium ions; those of aqueous solutions of Brnsted-Lowry bases are due to the presence of hydroxide ions. This reduces the odor of the fish, and also adds a sour taste that we seem to enjoy. NH4Cl is used as a urinary acidifying salt as it helps in maintaining the pH and exhibits a diuretic effect. 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. As Cl- is a weak conjugate base it cannot further accept a proton. Is salt hydrolysis possible in ch3coonh4? Example #1: What is the pH of a 0.0500 M solution of ammonium chloride, NH 4 Cl. ), This conjugate acid is a weak acid. Salts that form from a weak acid and a strong base are basic salts, like sodium bicarbonate (NaHCO3). As seen in the above equation on dissolving in aqueous solution NH4Cl releases hydronium ions due to the hydrolysis of ammonium ions. Some salts formed in neutralization reactions may make the product solutions slightly acidic or slightly basic. 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 acid strength of these complex ions typically increases with increasing charge and decreasing size of the metal ions. Jan 29, 2023. document.getElementById( "ak_js_1" ).setAttribute( "value", ( new Date() ).getTime() ); Welcome to Techiescientist.com. This relation holds for any base and its conjugate acid or for any acid and its conjugate base. 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 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). Responses Chemistry - DrBob222, Friday, April 24, 2009 at 10:50pm The hydrolysis of Na2CO3 ends us as the hydrolysis of the carbonate ion. Similarly, NaF is basic (it is the salt of a strong base, NaOH, and a weak acid, HF). OpenStax is part of Rice University, which is a 501(c)(3) nonprofit. If you could please show the work so I can understand for the rest of them. ( The acetate ion behaves as a base in this reaction; hydroxide ions are a product. If we can find the equilibrium constant for the reaction, the process is straightforward. Without the harmful bacteria consuming the cucumbers they are able to last much longer than if they were unprotected. It is found in the form of white crystalline salt which is highly soluble in water (about 37%). 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). A book which I am reading has this topic on hydrolysis of salts. Lastly, the reaction of a strong acid with a strong base gives neutral salts. Sort by: Use 4.9 1010 as Ka for HCN. (CH However, practically all hydrated metal ions other than those of the alkali metals ionize to give acidic solutions. Therefore, the pH of NH4Cl should be less than 7. As we have seen in the section on chemical reactions, when an acid and base are mixed, they undergo a neutralization reaction. Data and Results Table 7b.1. It is also used for eliminating cough as it has an expectorant effect i.e. Question: Which response gives the products of hydrolysis of NH4Cl?A. The third column has the following: approximately 0, x, x. Example 2.4. (b) The Na+ cation is inert and will not affect the pH of the solution; while the HCO3HCO3 anion is amphiprotic. The pH of a salt solution is determined by the relative strength of its conjugated acid-base pair. Techiescientist is a Science Blog for students, parents, and teachers. This can also be justified by understanding further hydrolysis of these ions. Dissolving sodium acetate in water yields a solution of inert cations (Na+) and weak base anions 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. However, as ammonium chloride is easily available as a by-product in double decomposition reactions, therefore, being cost-effective they are more favored. Why is NH4Cl acidic? NH3 + H+D. Except where otherwise noted, textbooks on this site When you dissolve ammonium chloride crystals in water (H2O), the ammonium chloride compound decomposes into its component ions: NH4+ and Cl-. 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. . 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. Determine the degree of hydrolysis of this salt in 0.01 M solution and the pH of the solution. $$\ce {RCN + 2H2O + HCl -> RCOOH + NH4Cl}$$. 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. The new step in this example is to determine Ka for the $$\ce{C6H5NH3+}$$ ion. Why Do Cross Country Runners Have Skinny Legs? 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: $\mathrm{\mathit{K}_b(for\:\ce{CH_3CO_2^-})=\dfrac{\mathit{K}_w}{\mathit{K}_a(for\:CH_3CO_2H)}=\dfrac{1.010^{14}}{1.810^{5}}=5.610^{10}} \nonumber$. Aniline is an amine that is used to manufacture dyes. it causes irritation in the mucous membrane. 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. The arithmetic checks; when 1.2 103 M is substituted for x, the result = Ka. The chloride ion has no effect on the acidity of the solution since HCl is a strong acid. How do you know if a salt will undergo hydrolysis? 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). The vegetable, such as a cucumber, is placed in a sealed jar submerged in a brine solution. Chemistry questions and answers. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. However, the conjugate base of the weak acid is a weak base and ionizes slightly in water. The reaction is: We are given two of three equilibrium concentrations and asked to find the missing concentration. The new step in this example is to determine Ka for the $$\ce{C6H5NH3+}$$ ion. then transfer FeII to 100 ml flask makeup to the mark with water. Ammonium chloride in its aqueous solution is acidic as it releases hydronium upon its dissociation in a solution. ), some metal ions function as acids in aqueous solutions. Cooking is essentially synthetic chemistry that happens to be safe to eat. 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. NH3 + OH- + HClC. O) 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? But this pH dependent reaction yields different products. The dissociation chemical reaction is: NH4Cl(solid) = NH4+(aqueous) + Cl-(aqueous). But because HCl is a strong acid, the Cl ion is not basic in solution, and it isnt capable of deprotonating water. When we have heartburn, it feels better if we reduce the excess acid in the esophagus by taking an antacid. What is the hydrolysis reaction for NH4Cl? 3 NaHCO3 is a base. As you may have guessed, antacids are bases. The Ka of HPO42HPO42 is 4.2 1013. The word neutralization seems to imply that a stoichiometrically equivalent solution of an acid and a base would be neutral. Thus, the hydration becomes important and we may use formulas that show the extent of hydration: $\ce{Al(H2O)6^3+}(aq)+\ce{H2O}(l)\ce{H3O+}(aq)+\ce{Al(H2O)5(OH)^2+}(aq) \hspace{20px} K_\ce{a}=1.410^{5} \nonumber$. What is the pH of a 0.233 M solution of aniline hydrochloride? 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 second column has the header of A l ( H subscript 2 O ) subscript 6 superscript 3 positive sign plus H subscript 2 O equilibrium arrow H subscript 3 O superscript positive sign plus A l ( H subscript 2 O ) subscript 5 ( O H ) superscript 2 positive sign. Under the second column is a subgroup of four columns and three rows. 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. $$\ce{NH4+ + H2O <=> NH4OH + H+}$$ Now for . This is the most complex of the four types of reactions. Ka, for the acid $$\ce{NH4+}$$: $\ce{\dfrac{[H3O+][NH3]}{[NH4+]}}=K_\ce{a} \nonumber$. One example is the use of baking soda, or sodium bicarbonate in baking. 6 However, even if we mix stoichiometrically equivalent quantities, we may find that the resulting solution is not neutral. Besides these there will be some unionised NH4OH. What is net ionic equation for the reaction of AGNO3 NH4CL? E is inversely proportional to the square root of its concentration. 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. { "2.1:_Brnsted-Lowry_Acids_and_Bases" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "2.2:_pH_and_pOH" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "2.3:_Relative_Strengths_of_Acids_and_Bases" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "2.4:_Hydrolysis_of_Salt_Solutions" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "2.5:_Polyprotic_Acids" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "2.6:_Buffers" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "2.7:_Acid-Base_Titrations" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "2.8:_Acid-Base_Equilibria_(Exercises)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "2.9.0:_Equilibria_of_Other_Reaction_Classes" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, { "00:_Front_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "1:_Tools_for_quantitative_chemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "2:_Acid-Base_Equilibria" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "3:_Kinetics" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "4:_Thermodynamics" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "5:_Electrochemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "6:_Advanced_Theories_of_Covalent_Bonding" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "7:_Transition_Metals_and_Coordination_Chemistry" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "zz:_Back_Matter" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, [ "article:topic", "Author tag:OpenStax", "authorname:openstax", "showtoc:no", "license:ccby", "transcluded:yes" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FCourses%2FUniversity_of_Minnesota_Rochester%2Fgenchem2%2F2%253A_Acid-Base_Equilibria%2F2.4%253A_Hydrolysis_of_Salt_Solutions, $$\newcommand{\vecs}{\overset { \rightharpoonup} {\mathbf{#1}}}$$ $$\newcommand{\vecd}{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}}$$$$\newcommand{\id}{\mathrm{id}}$$ $$\newcommand{\Span}{\mathrm{span}}$$ $$\newcommand{\kernel}{\mathrm{null}\,}$$ $$\newcommand{\range}{\mathrm{range}\,}$$ $$\newcommand{\RealPart}{\mathrm{Re}}$$ $$\newcommand{\ImaginaryPart}{\mathrm{Im}}$$ $$\newcommand{\Argument}{\mathrm{Arg}}$$ $$\newcommand{\norm}{\| #1 \|}$$ $$\newcommand{\inner}{\langle #1, #2 \rangle}$$ $$\newcommand{\Span}{\mathrm{span}}$$ $$\newcommand{\id}{\mathrm{id}}$$ $$\newcommand{\Span}{\mathrm{span}}$$ $$\newcommand{\kernel}{\mathrm{null}\,}$$ $$\newcommand{\range}{\mathrm{range}\,}$$ $$\newcommand{\RealPart}{\mathrm{Re}}$$ $$\newcommand{\ImaginaryPart}{\mathrm{Im}}$$ $$\newcommand{\Argument}{\mathrm{Arg}}$$ $$\newcommand{\norm}{\| #1 \|}$$ $$\newcommand{\inner}{\langle #1, #2 \rangle}$$ $$\newcommand{\Span}{\mathrm{span}}$$$$\newcommand{\AA}{\unicode[.8,0]{x212B}}$$, pH of a Solution of a Salt of a Weak Base and a Strong Acid, Equilibrium of a Salt of a Weak Acid and a Strong Base, Determining the Acidic or Basic Nature of Salts. Scroll To Top