0000022537 00000 n The, Kb for NH3 is 1.81 x 10^-5 Ka for NH4+ is Kw / Kb = 10^-14 / 1.81 x 10^-5 = 5.52 x 10^-10. For Arabic Users, find a teacher/tutor in your City or country in the Middle East. HAsO 4 2- 3.210 -12. Ammonium Hydroxide | NH4OH - PubChem Apologies, we are having some trouble retrieving data from our servers. The ammonium ion (NH4+) in the body plays an important role in the maintenance of acid-base balance. is 2 x 10-5. Since the ammonium ion functions as a weak acid, the equilibrium constant is given the label Ka. The kidney uses ammonium (NH4+) in place of sodium (Na+) to combine with fixed anions in maintaining acid-base balance, especially as a homeostatic compensatory mechanism in metabolic acidosis. Which Of The Following Is A Form Of Political Participation, Creative Commons Attribution-NonCommercial 3.0 Unported License. National Library of Medicine. The concepts of Lewis Structure, Molecular Geometry, and Hybridization hold great significance in understanding the structure, geometry, and subsequently the behavior of a substance, which is a direct result of the properties of associated elements atoms. 0000001472 00000 n The pH of a salt solution of NH4CN would be: Hints The Ka of NH4+ is 5.6 x 10-10. Write the balanced equation in an equilibrium reaction with water NH3 + (aq) + H2O (l) -> NH4+ (aq) + OH- (aq) 2. The chemical crystallizes in colorless prisms, possessing a saline taste; it sublimes on heating and is easily soluble in water. This system acts as a buffer because the ammonia reacts with acid and the ammonium ion reacts with base:. Use the tabulated ionization constants and Equation 16.8 to calculate each indicated K value. Hit enter to search or ESC to close. The Kb of CN is 2 105. To identify the corresponding Brnsted acid, add a proton to the formula to get \text{CH}_3\text{COOH} (acetic acid). What is the pKa of NH4+? Compare this value with the one calculated from your measured pH value (higher, lower, or the same). <]>> Atomic orbits of comparable levels of energy participate in forming hybrid orbitals. 0000008268 00000 n Solubility. than NH4+ is an acid. Expectorant in cough syrups. 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. National Institutes of Health. Get a free answer to a quick problem. 0000017205 00000 n 0000003442 00000 n KaKb = Kw = 1E-14 the initial concentration of ammonium chloride will be .1, and 0 for both NH2 and H3O+. You can ask a new question or browse more Chemistry Help Please!!! why teaching is challenging yet rewarding The Kb for NH3 is 1.8 x 10-5, the Ka is 5.6 x 10-10( 1.0 x 10-14/1.8 x 10-5). is 2 x 10-5. Such a structure arises from the need for a refined geometry of atoms necessary for electrons to pair up and thus, form different chemical bonds, as inducted by the valence bond theory. The ammonium ion (NH4+) in the body plays an important role in the maintenance of acid-base balance. 0000001614 00000 n 35,000 worksheets, games, and lesson plans, Spanish-English dictionary, translator, and learning, a Question For Free. NH 4+(aq) + H 2 O (l) H 3 O +(aq) + NH 3 (aq) pH Calculator of aqueous ammonium chloride solution The solution is therefore acidic - it Has pH < 7.00 . 2020 0 obj <> endobj Ammonium | H4N+ | CID 223 - structure, chemical names, physical and chemical properties, classification, patents, literature, biological activities, safety/hazards . Fastest 17 Hmr Ammo, Less than 7 because NH4+ is a stronger acid The Ka of NH4+ is 5.6 1010. In NH4+, nitrogen and the 4 hydrogen atoms make 4 sigma bonds, out of which 3 are covalent bonds and the fourth one is a dative bond. Expectorant in cough syrups. You can ask a new question or browse more CHEMISTRY HELP !!!! Kb for NH3 is 1.81 x 10^-5 The question is then, what is the percipitate? The Kb of CN is 2 105. 0000001961 00000 n The pH of a salt solution of M2+ + NH3 M(NH3)2+ K1 = 102 M(NH3)2+ + NH3 M(NH3)2 2+ K2 = 103 M(NH3)2 2+ + NH3 M(NH3)3 2+ K3 = 102 A 1.0 103 mol sample of M(NO3)2 is added to 1.0 L of 15.0 M NH3 (Kb = 1.8, NH3 + HCl = NH4+ + Cl- c(NH3)=(0.02L * 0.08M)/0.06L= 0.02667 M c(HCl)=(0.04L * 0.04M)/0.06L= 0.02667 M c(NH4+)=c(HCl) Kb=[NH4+][OH-]/[NH3] Kb=1.76*10^(-5) So i tried to calculate it like, The problem is that the products ( Cu(NH3)4 and SO4) should be soluble, no? Ka for NH4+ is Kw / Kb = 10^-14 / 1.81 x 10^-5 = 5.52 x 10^-10. Save my name, email, and website in this browser for the next time I comment. Search Your email address will not be published. Ammonium bromide can be prepared by the direct action of hydrogen bromide on ammonia. Most common types of hybridizations are sp, sp2, sp3, sp3d, sp3d2, sp3d3 etc. Policies. 0000014794 00000 n NH3 (aq) + H2O (aq) NH4 + (aq) + OH- (aq) Ammonia is an example of a weak base.A weak base generates hydroxide ions by accepting protons from water but reaches equilibrium when only a fraction of its molecules have done so .The equilibrium constant for this type of equilibrium is designated Kb : Kb = [NH 4 +] eq [OH-]eq / [NH3]eq Calculate Kb for the weak base aqueous ammonia. The K_a of acetic acid (from Table 16.7) is 1.8 10^{5}. %PDF-1.4 % Since Ammonium has 0 ion pairs and 4 sigma bonds, the hybridization value is 4. We know that Kb 1.8 * 10^-5 and [NH3] is 15 M. Question: The Kb of NH3 N H 3 is 1.8xd710u22125 1.8 xd7 10 u2212 5 . National Center for Biotechnology Information. These hybrid orbitals, formed by the hybridization of an atom, are helpful in the explanation and understanding of an atoms molecular geometry, its atomic bond properties, and the position in the atomic space. than NH4+ is an acid The 3-dimensional geometrical structure of ammonium, NH4+ is referred to as Tetrahedral. On exposure to air it gradually assumes a yellow color because of the oxidation of traces of bromide (Br) to bromine (Br2). Table of Solubility Product Constants (K sp at 25 o C). Contact. To calculate pH it is better to use the Ka value Ka * Kb = 10^-14 Ka = 10^-14 / (1.8*10^-5) Ka = [NH3] [H3O+] / [NH4+] More 15g NH4Cl = 15/53.5 = 0.28 mol 15g NH3 = 15/17 = 0.88 mol 0000017167 00000 n B Ammonia is weaker basic than ammonium is acidic. 1993 topps gold derek jeter; treat your wife with respect bible verses. The question is then, what is the percipitate? I set up ICE from the equation: NH3 + H20 ------NH4 + OH- I 0.25 0 0 C -x +x +x E 0.25-x x x 1.8 *10^-5 = x*x/ 0.25-x 4.5* 10^-6 = x2 took the square root to get. Check questions. endstream endobj 2041 0 obj<>/W[1 1 1]/Type/XRef/Index[28 1992]>>stream A buffer is a solution that resists changes in pH when small amounts of H+ or OH- are added. 6 . . Greater than 7 because CN is a stronger base As a result, all four electrons contained in the atomic orbitals in the outermost shell of the nitrogen atom can participate in hybridization, making it SP3. Carbonate ion, a moderately strong base, undergoes considerable hydrolysis in aqueous solution. Carbonate ion can be precipitated from solution as white barium or calcium salts that have low solubilities: Although many carbonate salts are insoluble, those of Na +, K +, and NH 4 + are quite soluble. Our Kb expression is Kb [NH4+][OH-] / [NH3]. This means that NH4+ has 4 pairs in total, which are bonded due to the 4 atoms of hydrogen. The Kb of CN- According to the base constant (Kb), only a small fraction of ammonia molecules ionize, so that the molar concentration of each ion compared to the initial molar concentration of ammonia is negligible. NH4CN would be: 2003-2023 Chegg Inc. All rights reserved. (Ka)(3.8 x 10-10) 1 x 10-14 Ka 2.6 x 10-5. pOH -log(2.9 x 10-3) 2.54. pH 14 2.54 11.46. 0000019496 00000 n Calculate the M2+ concentration when the equilibrium concentrations of NH3 and M(NH3)62+ are 0.074 and 0.22 M respectively 0000002830 00000 n \[\ce{CO3^{2-}(aq) + H2O(l) <=> HCO3^{-}(aq) + OH^{-}(aq)}\], \[\ce{HCO3^{-}(aq) + H2O(l) <=> H2CO3(aq) + OH^{-}(aq) }\]. For better understanding, you can also refer to the already written article on the polarity of NH4. A bond between two electrons is represented by a line marked by a dot at both ends, involving the participating electrons. How do you declare a global variable in Java? On exposure to air it gradually assumes a yellow color because of the oxidation of traces of bromide (Br ) to bromine (Br 2 ). Consider the following reaction in aqueous solution: H2O + NH3 NH4+ + OH- Identify each compound in this reaction (considering both forward and reverse reactions) as either a Bronsted acid or base. Choose an expert and meet online. The Kb Of CN Is 2 105. 0000003318 00000 n Copyright 2018 RJFP. . The therapeutic effects of Ammonium Chloride depend upon the . Because of this, even insoluble carbonate salts dissolve in acid. . Making educational experiences better for everyone. (Kb > 1, pKb < 1). What is the Ka K a of N H+ 4 N H 4 +, its conjugate acid? Conjugate acids (cations) of strong bases are ineffective bases. Determine the identity of the acid corresponding to each conjugate base and the identity of the base corresponding to each conjugate acid; then, consult Tables 16.7 and 16.8 for their ionization constants. There is no such animal as NH4 as a neutral material. To do this, you first need to find the Ka for NH4 +. 0 Because of this, even insoluble carbonate salts dissolve in acid. Legal. . This process can also involve half-filled and fully filled orbitals as well, provided that the level of energy remains similar. 1. Relation between Ka and Kb. Ammonia in aqueous solution is basic: NH3(aq) + H2O(aq) NH4+(aq) + OH-(aq) Kb = [NH4+] x[OH-] = 1.8 x 10-5 [NH3] The ammonium ion is its conjugate acid We can write an equation for NH4+ acting as an acid as: NH4+(aq) + H2O(aq) NH3(aq) + H3O+ (aq) Ka = [NH3] x[H3O+] = 5.6 x 10-10 . 0000002363 00000 n Now you'll have to compare this to your calculated value. Nitrogens valence electron count, however, is 5, owing to its position in the 5th group of the periodic table. HHS Vulnerability Disclosure. If you know the value of Kb (base dissociation constant) of a weak base, you can use it to calculate the pH of a solution containing the base using the following steps: Write the equation for the dissociation of the base in water: B + H2O BH+ + OH- Write the expression for the Kb of the base: Kb = [BH+] [OH-]/ [B] the Website for Martin Smith Creations Limited . No packages or subscriptions, pay only for the time you need. All bicarbonate ( HCO 3 ) salts are soluble. The easiest way to figure Kb and pKb out, for me, would be to calculate the Ka first, and then from that calculate the Kb, and from that, calculate pKb. The Ka of NH4+ is 5.6 1010. city of san luis obispo planning department; which came first tennis or badminton; fastest 13 year old 40 yard dash; brick hockey tournament tryouts Most questions answered within 4 hours. I have no idea what NaC2 is.I suspect you were trying to write NaC2H3O2. Keeping Nitrogen in the center, and considering Hydrogens position on the outside, we can place the 4 hydrogen atoms surrounding the single nitrogen atom. Nba 2k20 Player Tracker, But the + sign decrees that NH4+ has 8 valence shell electrons, due to the positive ion. FOIA. Greater than 7 because NH4+ is a stronger acid You'll get a detailed solution from a subject matter expert that helps you learn core concepts. Naplex 2020 Experience, The PH Of A Salt Solution Of NH4CN Would Be: Greater Than 7 Because CN Is A Stronger Base Than NH4+ Is An Acid Less Than 7 Because CN Is A Stronger Base Than NH4 Let's see if I got the equation correct: NH4+ + H2O NH3 + H3O+ because ammonium chloride is a salt of a strong acid and weak base. Problem: If you know Kb for ammonia, NH3, you can calculate the equilibrium constant, Ka, for this reaction by the equation: NH4 + NH3 + H + a) Ka = KwKb b) Ka = Kw / Kb c) Ka = 1 / Kb d) Ka = Kb / Kw Use the conjugate acid from the equation. Your Ultimate AI Essay Writer & Assistant. answered 03/31/21, Ph.D. University Professor with 10+ years Tutoring Experience. The NH4+ ion has no pi bonds. The Kb of CN is 2 105. Strategy Each species listed is either a conjugate base or a conjugate acid. The K a value of ammonium ion (NH 4+) is 5.610 10, the K b value of ammonia NH 3= 1.810 5, then : A Ammonia is more strongly basic than ammonium is acidic. 0000003077 00000 n samurai cop budget; n731nr pilot deviation; best coastal towns in maine to live HJ 812-2016 Li+ Na+NH4+K+Ca2+Mg2+ . Acid with values less than one are considered weak. The. xref Which Of The Following Is A Form Of Political Participation, Determine (a) K_b of the acetate ion (\text{CH}_3\text{COO}^), (b) K_a of the methylammonium ion (\text{CH}_3\text{NH}_3^+), (c) K_b of the fluoride ion (\text{F}^), and (d) K_a of the ammonium ion (\text{NH}_4^+). 0000001177 00000 n 0000003396 00000 n The Kb expression for the above reaction is: Kb = [NH3][H3O+] / [NH4+] 1. NO3 Lewis Structure, Molecular Geometry, and Hybridization, PH3 Lewis Structure, Molecular Geometry, and Hybridization. Hybridization provides the NH4+ atom stability, therefore giving it numerous advantageous uses. NH4+ is our conjugate acid. While this makes the molecule symmetrical, it also makes it a non-polar molecule, as the bond polarity of each Nitrogen-Hydrogen bond cancels out. All bicarbonate (\(\ce{HCO3^{-}}\)) salts are soluble. document.getElementById( "ak_js_1" ).setAttribute( "value", ( new Date() ).getTime() ); Welcome to Techiescientist.com. Find its Ka value (in the table or otherwise). The pH of a salt solution of NH4CN would be: The Ka of NH4+ is 2) how should the pH of a 0.1M solution of NaC2 at H3O2 compare with that of a 0.1 M solution of KC2H3O2? 1. startxref (c) \text{F}^ is the conjugate base of \text{HF; Ka} = 7.1 10^{4}. These new orbitals may have different shapes, energies, etc. When ammonium (NH4+) is placed in water, a chemical reaction occurs and an equilibrium is established as shown . 11 Uses of Platinum Laboratory, Commercial, and Miscellaneous, CH3Br Lewis Structure, Geometry, Hybridization, and Polarity. As mentioned earlier, NH4+ is made up of Nitrogen and Hydrogen. Even Nitrogen, which needs 8 electrons in the valence shell has all 8 of them, thereby forming a full exterior shell. All rights reserved. PUGVIEW FETCH ERROR: 403 Forbidden National Center for Biotechnology Information 8600 Rockville Pike, Bethesda, MD, 20894 USA Contact Policies FOIA HHS Vulnerability Disclosure National Library of Medicine National Institutes of Health Below is the image of the geometrical representation of the NH4+ molecule. The problem is that the products ( Cu(NH3)4 and SO4) should be soluble, no? 2) The concept of molecular geometry aims to depict the generic shape and structure of a molecule, accurate to the length between different bonds, the bond and torsional angles, other geometrical factors and variables that govern the shape and arrangement of an atom, and therefore, a molecule. Accessibility StatementFor more information contact us atinfo@libretexts.orgor check out our status page at https://status.libretexts.org. The pH of a salt solution of NH4CN would be: Greater than 7 because CN is a stronger base than NH4+ is an acid Less than 7 because CN is a Old Social Media Platforms, Arsenous acid H 3 AsO 3 6.610 -10 Ascorbic acid H 2 C . What is the present participle for Preparar? The dark, 12.0 M NH3 How many drops (1 drop 0.05 mL) of this solution would you use? - :NH3NH4+,"=+,,". The end goal is to identify a configuration with the best electron arrangement such that the formal charges and the octet rule are upheld. Table of Acids with Ka and pKa Values* CLAS * Compiled . Ammonium nitrate | NH4NO3 or H4N2O3 | CID 22985 - structure, chemical names, physical and chemical properties, classification, patents, literature, biological . Your email address will not be published. Ka = 1x10^-14/Kb = 1x10^-14/1.8x10^-5. While the exchange between atomic orbits of different atoms leads to the creation of molecular orbits, hybridization of an atom is assumed to be a combination of different atomic orbits, overlaying one another in different fractions. Your email address will not be published. There is no such animal as NH4 as a neutral material. { "Carbonate_Ion_(CO\u2083\u00b2\u207b)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "Halide_Ions_(Cl\u207b,_Br\u207b,_I\u207b)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "Phosphate_Ion_(PO\u2084\u00b3\u207b)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "Sulfate_Ion_(SO\u2084\u00b2\u207b)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "Sulfide_Ion_(S\u00b2\u207b)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", "Sulfite_Ion_(SO\u2083\u00b2\u207b)" : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, { Characteristic_Reactions_of_Select_Metal_Ions : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Confirmatory_Tests : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Properties_of_Select_Nonmetal_Ions : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Semimicro_Analytical_Techniques : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()", Separations_with_Thioacetamide : "property get [Map MindTouch.Deki.Logic.ExtensionProcessorQueryProvider+<>c__DisplayClass228_0.b__1]()" }, [ "article:topic", "Carbonate", "authorname:jbirk", "carbonate ion", "showtoc:no", "license:ccbyncsa", "licenseversion:40" ], https://chem.libretexts.org/@app/auth/3/login?returnto=https%3A%2F%2Fchem.libretexts.org%2FBookshelves%2FAnalytical_Chemistry%2FSupplemental_Modules_(Analytical_Chemistry)%2FQualitative_Analysis%2FProperties_of_Select_Nonmetal_Ions%2FCarbonate_Ion_(CO%25E2%2582%2583%25C2%25B2%25E2%2581%25BB), \( \newcommand{\vecs}[1]{\overset { \scriptstyle \rightharpoonup} {\mathbf{#1}}}\) \( \newcommand{\vecd}[1]{\overset{-\!-\!\rightharpoonup}{\vphantom{a}\smash{#1}}} \)\(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\) \(\newcommand{\id}{\mathrm{id}}\) \( \newcommand{\Span}{\mathrm{span}}\) \( \newcommand{\kernel}{\mathrm{null}\,}\) \( \newcommand{\range}{\mathrm{range}\,}\) \( \newcommand{\RealPart}{\mathrm{Re}}\) \( \newcommand{\ImaginaryPart}{\mathrm{Im}}\) \( \newcommand{\Argument}{\mathrm{Arg}}\) \( \newcommand{\norm}[1]{\| #1 \|}\) \( \newcommand{\inner}[2]{\langle #1, #2 \rangle}\) \( \newcommand{\Span}{\mathrm{span}}\)\(\newcommand{\AA}{\unicode[.8,0]{x212B}}\), status page at https://status.libretexts.org. Required fields are marked *, This journal is licensed under a Creative Commons Attribution-NonCommercial 3.0 Unported License. Strong acids are listed at the top left hand corner of the table and have Ka values >1 2. x1 04a\GbG&`'MF[!. The Kb of CN- Save my name, email, and website in this browser for the next time I comment. 0000000960 00000 n JywyBT30e [` C: The NH4 ion will react with water (hydrolysis) and form NH3 and H3O + (hydronium ion). The concentration of water is absorbed into the value of K b; K b provides a measure of the equilibrium position (i) if K b is large, the products of the dissociation reaction are favoured (ii) if K b is small, undissociated base is favoured.. K b provides a measure of the strength of a base (i) if K b is large, the base is largely dissociated so the base is strong In order to understand this properly , let us do a practical example: What is the pH of a 0.43M solution of NH4Cl? TABLE OF CONJUGATE ACID-BASE PAIRS Acid Base K a (25 oC) HClO 4 ClO 4 H 2 SO 4 HSO 4 HCl Cl HNO 3 NO 3 H 3 O + H 2 O H 2 CrO 4 HCrO 4 1.8 x 101 H 2 C 2 O 4 (oxalic acid) HC 2 O 4 5.90 x 102 [H 2 SO 3] = SO 2 (aq) + H2 O HSO. A link to the app was sent to your phone. The pH of a salt solution of Nitrogen, having 5 valence shell electrons, along with 4 from Hydrogen, should have had 9 electrons. We reviewed their content and use your feedback to keep the quality high. The Kb of CN- is 2 x 10-5. A Lewis Structure is a depiction of the arrangement of electrons in the standalone atoms of an element. Molecular geometry also helps to determine the atomic properties of an element, such as polarity, magnetism, reactivity, color, biological potency, and 3-dimensional space alignment. The kidney uses ammonium (NH4+) in place of sodium (Na+) to combine with fixed anions in maintaining acid-base balance, especially as a homeostatic compensatory mechanism in metabolic acidosis. Im a mother of two crazy kids and a science lover with a passion for sharing the wonders of our universe. Hello I need help with this excersise: How many moles of NH4Cl are neccesary to add to 1 liter of solution of Co2+ 0,20 M in order to prevent the precipitation when the solution is saturated with H2S (0,1M) and the pH is 7,50. . questions. Kb = {[NH4^+][OH^-]} / [NH3] According to the above balanced equation, the molar concentrations of ammoniuim and hydroxide ions are the same. The ion is the by-product of a chemical reaction between a proton donor and Ammonia, which is as follows: Lewis Structure is a simplified arrangement and presentation of the electrons present in the valence shell of a molecule. . Solving Equation 16.8 separately for K_a and K_b gives, respectively, K_a = \frac{K_w}{K_b} and K_b = \frac{K_w}{K_a}, (a) Conjugate base \text{CH}_3\text{COO}^: K_b = \frac{1.0 10^{14}}{1.8 10^{5}} = 5.6 10^{10}, (b) Conjugate acid \text{CH}_3\text{NH}_3^+: K_a = \frac{1.0 10^{14}}{4.4 10^{4}} = 2.3 10^{11}, (c) Conjugate base \text{F}^: K_b = \frac{1.0 10^{14}}{7.1 10^{4}} = 1.4 10^{11}, (d) Conjugate acid \text{NH}_4^+: K_a = \frac{1.0 10^{14}}{1.8 10^{5}} = 5.6 10^{10}, \text{CH}_3\text{COO}^: K_b = \frac{1.0 10^{14}}{1.8 10^{5}} = 5.6 10^{10}, \text{CH}_3\text{NH}_3^+: K_a = \frac{1.0 10^{14}}{4.4 10^{4}} = 2.3 10^{11}, \text{F}^: K_b = \frac{1.0 10^{14}}{7.1 10^{4}} = 1.4 10^{11}, \text{NH}_4^+: K_a = \frac{1.0 10^{14}}{1.8 10^{5}} = 5.6 10^{10}.

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