{"id":602,"date":"2017-12-14T21:42:05","date_gmt":"2017-12-14T21:42:05","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/suny-mcc-introductorychemistry\/chapter\/bronsted-lowry-acids-and-bases\/"},"modified":"2018-09-02T00:48:36","modified_gmt":"2018-09-02T00:48:36","slug":"bronsted-lowry-acids-and-bases","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/suny-mcc-introductorychemistry\/chapter\/bronsted-lowry-acids-and-bases\/","title":{"raw":"10.2 Br\u00f8nsted-Lowry Acids and Bases","rendered":"10.2 Br\u00f8nsted-Lowry Acids and Bases"},"content":{"raw":"<div class=\"textbox learning-objectives\">\r\n<h3>Learning Objectives<\/h3>\r\nBy the end of this module, you will be able to:\r\n<ul>\r\n \t<li>Identify acids, bases, and conjugate acid-base pairs according to the Br\u00f8nsted-Lowry definition<\/li>\r\n \t<li>Use the ion-product constant for water to calculate hydronium and hydroxide ion concentrations<\/li>\r\n<\/ul>\r\n<\/div>\r\nAcids and bases have been known for a long time. When Robert Boyle characterized them in 1680, he noted that acids dissolve many substances, change the color of certain natural dyes (for example, they change litmus from blue to red), and lose these characteristic properties after coming into contact with alkalis (bases). In the eighteenth century, it was recognized that acids have a sour taste, react with limestone to liberate a gaseous substance (now known to be CO<sub>2<\/sub>), and interact with alkalis to form neutral substances. In 1815, Humphry Davy contributed greatly to the development of the modern acid-base concept by demonstrating that hydrogen is the essential constituent of acids. Around that same time, Joseph Louis Gay-Lussac concluded that acids are substances that can neutralize bases and that these two classes of substances can be defined only in terms of each other. The significance of hydrogen was reemphasized in 1884 when Carl Axel <strong>Arrhenius<\/strong> defined an acid as a compound that dissolves in water to yield hydrogen cations (now recognized to be hydronium ions) and a base as a compound that dissolves in water to yield hydroxide anions.\r\n\r\nIn an earlier module, we defined acids and bases as Arrhenius did: We identified an acid as a compound that dissolves in water to yield hydronium ions (H<sub>3<\/sub>O<sup>+<\/sup>) and a base as a compound that dissolves in water to yield hydroxide ions (OH<sup>\u2212<\/sup>). This definition is not wrong; it is simply limited.\r\n\r\nWe extend on the Arrhenius definition of an acid or a base using the more general definition proposed in 1923 by the Danish chemist Johannes Br\u00f8nsted and the English chemist Thomas Lowry. Their definition centers on the proton, H<sup>+<\/sup>. A proton is what remains when a normal hydrogen atom, [latex]{}_{1}{}^{1}\\text{H}[\/latex], loses an electron. A compound that donates a proton to another compound is called a <strong>Br\u00f8nsted-Lowry acid<\/strong>, and a compound that accepts a proton is called a <strong>Br\u00f8nsted-Lowry base<\/strong>. An acid-base reaction is the transfer of a proton from a proton donor (acid) to a proton acceptor (base).\r\n\r\nAcids may be compounds such as HCl or H<sub>2<\/sub>SO<sub>4<\/sub>, organic acids like acetic acid (CH<sub>3<\/sub>COOH) or ascorbic acid (vitamin C), or H<sub>2<\/sub>O. Anions (such as [latex]{\\text{HSO}}_{4}^{-}[\/latex], [latex]{\\text{H}}_{2}{\\text{PO}}_{4}^{-}[\/latex], HS<sup>\u2212<\/sup>, and [latex]{\\text{HCO}}_{3}^{-}[\/latex]) may also act as acids. Bases fall into the same two categories. Bases may be neutral molecules (such as H<sub>2<\/sub>O, NH<sub>3<\/sub>, and CH<sub>3<\/sub>NH<sub>2<\/sub>), anions (such as OH<sup>\u2212<\/sup>, HS<sup>\u2212<\/sup>, [latex]{\\text{HCO}}_{3}^{-}[\/latex], [latex]{\\text{CO}}_{3}^{2-}[\/latex], F<sup>\u2212<\/sup>, and [latex]{\\text{PO}}_{4}^{3-}[\/latex]). The most familiar bases are ionic compounds such as NaOH and Ca(OH)<sub>2<\/sub>, which contain the hydroxide ion, OH<sup>\u2212<\/sup>. The hydroxide ion in these compounds accepts a proton from acids to form water:\r\n<p style=\"text-align: center\">[latex]\\large{\\text{H}}^{\\text{+}}+{\\text{OH}}^{-}\\longrightarrow {\\text{H}}_{2}\\text{O}[\/latex]<\/p>\r\nWe call the product that remains after an acid donates a proton the <strong>conjugate base<\/strong> of the acid. This species is a base because it can accept a proton (to re-form the acid):\r\n<p style=\"text-align: center\">[latex]\\large\\begin{array}{l}\\text{acid}\\rightarrow \\text{proton}+\\text{conjugate base}\\\\ \\text{HF}\\rightarrow {\\text{H}}^{\\text{+}}+{\\text{F}}^{-}\\\\ {\\text{H}}_{2}{\\text{SO}}_{4}\\rightarrow {\\text{H}}^{+}+{\\text{HSO}}_{4}^{-}\\\\ {\\text{H}}_{2}\\text{O}\\rightarrow {\\text{H}}^{\\text{+}}+{\\text{OH}}^{-}\\\\ {\\text{HSO}}_{4}^{-}\\rightarrow {\\text{H}}^{\\text{+}}+{\\text{SO}}_{4}^{2-}\\\\ {\\text{NH}}_{4}^{+}\\rightarrow {\\text{H}}^{+}+{\\text{NH}}_{3}\\end{array}[\/latex]<\/p>\r\nWe call the product that results when a base accepts a proton the base\u2019s <strong>conjugate acid<\/strong>. This species is an acid because it can give up a proton (and thus re-form the base):\r\n<p style=\"text-align: center\">[latex]\\large\\begin{array}{l}\\text{base}+\\text{proton}\\rightarrow \\text{conjugate acid}\\\\ {\\text{OH}}^{-}+{\\text{H}}^{\\text{+}}\\rightarrow {\\text{H}}_{2}\\text{O}\\\\ {\\text{H}}_{2}\\text{O}+{\\text{H}}^{\\text{+}}\\rightarrow {\\text{H}}_{3}{\\text{O}}^{\\text{+}}\\\\ {\\text{NH}}_{3}+{\\text{H}}^{\\text{+}}\\rightarrow {\\text{NH}}_{4}{}^{\\text{+}}\\\\ {\\text{S}}^{2-}+{\\text{H}}^{\\text{+}}\\rightarrow {\\text{HS}}^{-}\\\\ {\\text{CO}}_{3}{}^{2-}+{\\text{H}}^{\\text{+}}\\rightarrow {\\text{HCO}}_{3}{}^{-}\\\\ {\\text{F}}^{-}+{\\text{H}}^{\\text{+}}\\rightarrow \\text{HF}\\end{array}[\/latex]<\/p>\r\nIn these two sets of equations, the behaviors of acids as proton donors and bases as proton acceptors are represented in isolation. In reality, all acid-base reactions involve the <em>transfer<\/em> of protons between acids and bases. For example, consider the acid-base reaction that takes place when ammonia is dissolved in water. A water molecule (functioning as an acid) transfers a proton to an ammonia molecule (functioning as a base), yielding the conjugate base of water, OH<sup>\u2212<\/sup>, and the conjugate acid of ammonia, [latex]{\\text{NH}}_{4}{}^{\\text{+}}:[\/latex]\r\n<img class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/887\/2015\/05\/23213723\/CNX_Chem_14_01_conjugate_img.jpg\" alt=\"This figure has three parts in two rows. In the first row, two diagrams of acid-base pairs are shown. On the left, a space filling model of H subscript 2 O is shown with a red O atom at the center and two smaller white H atoms attached in a bent shape. Above this model is the label \u201cH subscript 2 O (acid)\u201d in purple. An arrow points right, which is labeled \u201cRemove H superscript plus.\u201d To the right is another space filling model with a single red O atom to which a single smaller white H atom is attached. The label in purple above this model reads, \u201cO H superscript negative (conjugate base).\u201d Above both of these red and white models is an upward pointing bracket that is labeled \u201cConjugate acid-base pair.\u201d To the right is a space filling model with a central blue N atom to which three smaller white H atoms are attached in a triangular pyramid arrangement. A label in green above reads \u201cN H subscript 3 (base).\u201d An arrow labeled \u201cAdd H superscript plus\u201d points right. To the right of the arrow is another space filling model with a blue central N atom and four smaller white H atoms in a tetrahedral arrangement. The green label above reads \u201cN H subscript 3 superscript plus (conjugate acid).\u201d Above both of these blue and white models is an upward pointing bracket that is labeled \u201cConjugate acid-base pair.\u201d The second row of the figure shows the chemical reaction, H subscript 2 O ( l ) is shown in purple, and is labeled below in purple as \u201cacid,\u201d plus N H subscript 3 (a q) in green, labeled below in green as \u201cbase,\u201d followed by a double sided arrow arrow and O H superscript negative (a q) in purple, labeled in purple as \u201cconjugate base,\u201d plus N H subscript 4 superscript plus (a q)\u201d in green, which is labeled in green as \u201cconjugate acid.\u201d The acid on the left side of the equation is connected to the conjugate base on the right with a purple line. Similarly, the base on the left is connected to the conjugate acid on the right side.\" \/>\r\n\r\n&nbsp;\r\n<div class=\"textbox examples\">\r\n<h3>Example 1: Bronsted-Lowry Acids and Bases<\/h3>\r\nIdentify the Br\u00f8nsted-Lowry acid and the Br\u00f8nsted-Lowry base in this chemical equation:\r\n\r\n[latex]\\large{\\text{C}_{6}\\text{H}}_{5}\\text{OH}\\left(l\\right)+{\\text{NH}_{2}}^{-}\\left(aq\\right)\\longrightarrow {\\text{C}_{6}\\text{H}}_{5}\\text{O}^{-}\\left(aq\\right)+{\\text{NH}}_{3}\\left(aq\\right)[\/latex]\r\n\r\n[reveal-answer q=\"160586\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"160586\"]\r\n\r\nThe C<sub class=\"subscript\">6<\/sub>H<sub class=\"subscript\">5<\/sub>OH molecule is losing an H<sup class=\"superscript\">+<\/sup>; it is the proton donor and the Br\u00f8nsted-Lowry acid. The NH<sub class=\"subscript\">2<\/sub><sup class=\"superscript\">\u2212<\/sup> ion (called the amide ion) is accepting the H<sup class=\"superscript\">+<\/sup> ion to become NH<sub class=\"subscript\">3<\/sub>, so it is the Br\u00f8nsted-Lowry base.\r\n\r\n[\/hidden-answer]\r\n\r\n<\/div>\r\n<div class=\"textbox examples\">\r\n<h3>Example 2: Conjugate Acids and Conjugate Bases<\/h3>\r\nIdentify the conjugate acid-base pairs in this equation:\r\n\r\n[latex]\\large{(\\text{C}\\text{H}}_{3})_{3}\\text{N}\\left(l\\right)+{\\text{H}_{2}}\\text{O}\\left(l\\right)\\longrightarrow {(\\text{C}\\text{H}}_{3})_{3}\\text{NH}^{+}\\left(aq\\right)+{\\text{OH}}^{-}\\left(aq\\right)[\/latex]\r\n[reveal-answer q=\"1605861\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"1605861\"]\r\n\r\nOne pair is H<sub class=\"subscript\">2<\/sub>O and OH<sup class=\"superscript\">\u2212<\/sup>, where H<sub class=\"subscript\">2<\/sub>O has one more H<sup class=\"superscript\">+<\/sup> and is the conjugate acid, while OH<sup class=\"superscript\">\u2212<\/sup> has one less H<sup class=\"superscript\">+<\/sup> and is the conjugate base. The other pair consists of (CH<sub class=\"subscript\">3<\/sub>)<sub class=\"subscript\">3<\/sub>N and (CH<sub class=\"subscript\">3<\/sub>)<sub class=\"subscript\">3<\/sub>NH<sup class=\"superscript\">+<\/sup>, where (CH<sub class=\"subscript\">3<\/sub>)<sub class=\"subscript\">3<\/sub>NH<sup class=\"superscript\">+<\/sup> is the conjugate acid (it has an additional proton) and (CH<sub class=\"subscript\">3<\/sub>)<sub class=\"subscript\">3<\/sub>N is the conjugate base.\r\n\r\n[\/hidden-answer]\r\n<h4>Check Your Learning<\/h4>\r\nIdentify the conjugate acid-base pairs in this equation:\r\n\r\n[latex]\\large{\\text{NH}}_{2}^{-}\\left(aq\\right)+{\\text{H}_{2}}\\text{O}\\left(l\\right)\\longrightarrow {\\text{NH}}_{3}\\left(aq\\right)+{\\text{OH}}^{-}\\left(aq\\right)[\/latex]\r\n\r\n[reveal-answer q=\"366443\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"366443\"]\r\n\r\nH<sub class=\"subscript\">2<\/sub>O (acid) and OH<sup class=\"superscript\">\u2212<\/sup> (base); NH<sub class=\"subscript\">2<\/sub><sup class=\"superscript\">\u2212<\/sup> (base) and NH<sub class=\"subscript\">3<\/sub> (acid)\r\n\r\n[\/hidden-answer]\r\n\r\n<\/div>\r\n<div class=\"textbox key-takeaways\">\r\n<h3>Key Concepts and Summary<\/h3>\r\nA compound that can donate a proton (a hydrogen ion) to another compound is called a Br\u00f8nsted-Lowry acid. The compound that accepts the proton is called a Br\u00f8nsted-Lowry base. The species remaining after a Br\u00f8nsted-Lowry acid has lost a proton is the conjugate base of the acid. The species formed when a Br\u00f8nsted-Lowry base gains a proton is the conjugate acid of the base. Thus, an acid-base reaction occurs when a proton is transferred from an acid to a base, with formation of the conjugate base of the reactant acid and formation of the conjugate acid of the reactant base.\r\n\r\n<\/div>\r\n<div class=\"textbox exercises\">\r\n<h3>Exercises<\/h3>\r\n<ol>\r\n \t<li>Write equations that show NH<sub>3<\/sub> as both a conjugate acid and a conjugate base.<\/li>\r\n \t<li>Write equations that show [latex]{\\text{H}}_{2}{\\text{PO}}_{4}{}^{-}[\/latex] acting both as an acid and as a base.<\/li>\r\n \t<li>What is the conjugate acid of each of the following? What is the conjugate base of each?\r\n<ol style=\"list-style-type: lower-alpha\">\r\n \t<li>OH<sup>\u2212<\/sup><\/li>\r\n \t<li>H<sub>2<\/sub>O<\/li>\r\n \t<li>[latex]{\\text{HCO}}_{3}{}^{-}[\/latex]<\/li>\r\n \t<li>NH<sub>3<\/sub><\/li>\r\n \t<li>[latex]{\\text{HSO}}_{4}{}^{-}[\/latex]<\/li>\r\n \t<li>H<sub>2<\/sub>O<sub>2<\/sub><\/li>\r\n \t<li>HS<sup>\u2212<\/sup><\/li>\r\n \t<li>[latex]{\\text{H}}_{5}{\\text{N}}_{2}{}^{\\text{+}}[\/latex]<\/li>\r\n<\/ol>\r\n<\/li>\r\n \t<li>What is the conjugate acid of each of the following? What is the conjugate base of each?\r\n<ol style=\"list-style-type: lower-alpha\">\r\n \t<li>H<sub>2<\/sub>S<\/li>\r\n \t<li>[latex]{\\text{H}}_{2}{\\text{PO}}_{4}{}^{-}[\/latex]<\/li>\r\n \t<li>PH<sub>3<\/sub><\/li>\r\n \t<li>HS<sup>\u2212<\/sup><\/li>\r\n \t<li>[latex]{\\text{HSO}}_{3}{}^{-}[\/latex]<\/li>\r\n \t<li>[latex]{\\text{H}}_{3}{\\text{O}}_{2}{}^{\\text{+}}[\/latex]<\/li>\r\n \t<li>H<sub>4<\/sub>N<sub>2<\/sub><\/li>\r\n \t<li>CH<sub>3<\/sub>OH<\/li>\r\n<\/ol>\r\n<\/li>\r\n \t<li>Identify and label the Br\u00f8nsted-Lowry acid, its conjugate base, the Br\u00f8nsted-Lowry base, and its conjugate acid in each of the following equations:\r\n<ol style=\"list-style-type: lower-alpha\">\r\n \t<li>[latex]{\\text{HNO}}_{3}+{\\text{H}}_{2}\\text{O}\\longrightarrow {\\text{H}}_{3}{\\text{O}}^{\\text{+}}+{\\text{NO}}_{3}{}^{-}[\/latex]<\/li>\r\n \t<li>[latex]{\\text{CN}}^{-}+{\\text{H}}_{2}\\text{O}\\longrightarrow \\text{HCN}+{\\text{OH}}^{-}[\/latex]<\/li>\r\n \t<li>[latex]{\\text{H}}_{2}{\\text{SO}}_{4}+{\\text{Cl}}^{-}\\longrightarrow \\text{HCl}+{\\text{HSO}}_{4}{}^{-}[\/latex]<\/li>\r\n \t<li>[latex]{\\text{HSO}}_{4}{}^{-}+{\\text{OH}}^{-}\\longrightarrow {\\text{SO}}_{4}{}^{\\text{2-}}+{\\text{H}}_{2}\\text{O}[\/latex]<\/li>\r\n \t<li>[latex]{\\text{O}}^{2-}+{\\text{H}}_{2}\\text{O}\\longrightarrow 2{\\mathrm{OH}}^{-}[\/latex]<\/li>\r\n \t<li>[latex]{\\text{H}}_{2}\\text{S}+{\\text{NH}}_{2}{}^{-}\\longrightarrow {\\text{HS}}^{-}+{\\text{NH}}_{3}[\/latex]<\/li>\r\n<\/ol>\r\n<\/li>\r\n \t<li>Identify and label the Br\u00f8nsted-Lowry acid, its conjugate base, the Br\u00f8nsted-Lowry base, and its conjugate acid in each of the following equations:\r\n<ol style=\"list-style-type: lower-alpha\">\r\n \t<li>[latex]{\\text{NO}}_{2}{}^{-}+{\\text{H}}_{2}\\text{O}\\longrightarrow {\\text{HNO}}_{2}+{\\text{OH}}^{-}[\/latex]<\/li>\r\n \t<li>[latex]\\text{HBr}+{\\text{H}}_{2}\\text{O}\\longrightarrow {\\text{H}}_{3}{\\text{O}}^{\\text{+}}+{\\text{Br}}^{-}[\/latex]<\/li>\r\n \t<li>[latex]{\\text{HS}}^{-}+{\\text{H}}_{2}\\text{O}\\longrightarrow {\\text{H}}_{2}\\text{S}+{\\text{OH}}^{-}[\/latex]<\/li>\r\n \t<li>[latex]{\\text{H}}_{2}{\\text{PO}}_{4}{}^{-}+{\\text{OH}}^{-}\\longrightarrow {\\text{HPO}}_{4}{}^{\\text{2-}}+{\\text{H}}_{2}\\text{O}[\/latex]<\/li>\r\n \t<li>[latex]{\\text{H}}_{2}{\\text{PO}}_{4}{}^{-}+\\text{HCl}\\longrightarrow {\\text{H}}_{3}{\\text{PO}}_{4}+{\\text{Cl}}^{-}[\/latex]<\/li>\r\n \t<li>[latex]{\\text{CH}}_{3}\\text{OH}+{\\text{H}}^{-}\\longrightarrow {\\text{CH}}_{3}{\\text{O}}^{-}+{\\text{H}}_{2}[\/latex]<\/li>\r\n<\/ol>\r\n<\/li>\r\n<\/ol>\r\n[reveal-answer q=\"41360\"]Show Selected Answers[\/reveal-answer]\r\n[hidden-answer a=\"41360\"]\r\n\r\n1. One example for NH<sub>3<\/sub> as a conjugate acid: [latex]{\\text{NH}}_{2}{}^{-}+{\\text{H}}^{\\text{+}}\\longrightarrow {\\text{NH}}_{3}[\/latex]; as a conjugate base: [latex]{\\text{NH}}_{4}{}^{\\text{+}}\\left(aq\\right)+{\\text{OH}}^{-}\\left(aq\\right)\\longrightarrow {\\text{NH}}_{3}\\left(aq\\right)+{\\text{H}}_{2}\\text{O}\\left(l\\right)[\/latex]\r\n\r\n3. The conjugate acids and bases are as follows:\r\n<ol style=\"list-style-type: lower-alpha\">\r\n \t<li>H<sub>2<\/sub>O, O<sup>2\u2212<\/sup><\/li>\r\n \t<li>[latex]{\\text{H}}_{3}{\\text{O}}^{+}[\/latex], OH<sup>\u2212<\/sup><\/li>\r\n \t<li>H<sub>2<\/sub>CO<sub>3<\/sub>, [latex]{\\text{CO}}_{3}{}^{2-}[\/latex]<\/li>\r\n \t<li>[latex]{\\text{NH}}_{4}{}^{\\text{+}}[\/latex], [latex]{\\text{NH}}_{2}^{-}[\/latex]<\/li>\r\n \t<li>H<sub>2<\/sub>SO<sub>4<\/sub>, [latex]{\\text{SO}}_{4}^{2-}[\/latex]<\/li>\r\n \t<li>[latex]{\\text{H}}_{3}{\\text{O}}_{2}^{+}[\/latex], [latex]{\\text{HO}}_{2}^{-}[\/latex]<\/li>\r\n \t<li>H<sub>2<\/sub>S, S<sup>2\u2212<\/sup><\/li>\r\n \t<li>[latex]{\\text{H}}_{6}{\\text{N}}_{2}{}^{2+}[\/latex], H<sub>4<\/sub>N<sub>2<\/sub><\/li>\r\n<\/ol>\r\n5. The labels are Br\u00f8nsted-Lowry acid = BA; its conjugate base = CB; Br\u00f8nsted-Lowry base = BB; its conjugate acid = CA.\r\n<ol style=\"list-style-type: lower-alpha\">\r\n \t<li>HNO<sub>3<\/sub>(BA), H<sub>2<\/sub>O(BB), [latex]{\\text{H}}_{3}{\\text{O}}^{\\text{+}}\\left(\\text{CA}\\right)[\/latex], [latex]{\\text{NO}}_{3}{}^{-}\\left(\\text{CB}\\right)[\/latex]<\/li>\r\n \t<li>CN<sup>\u2212<\/sup>(BB), H<sub>2<\/sub>O(BA), HCN(CA), OH<sup>\u2212<\/sup>(CB)<\/li>\r\n \t<li>H<sub>2<\/sub>SO<sub>4<\/sub>(BA), Cl<sup>\u2212<\/sup>(BB), HCl(CA), [latex]{\\text{HSO}}_{4}{}^{-}\\left(\\text{CB}\\right)[\/latex]<\/li>\r\n \t<li>[latex]{\\text{HSO}}_{4}{}^{-}\\left(\\text{BA}\\right)[\/latex], OH<sup>\u2212<\/sup>(BB), [latex]{\\text{SO}}_{4}{}^{\\text{2-}}[\/latex] (CB), H<sub>2<\/sub>O(CA)<\/li>\r\n \t<li>O<sup>2\u2212<\/sup>(BB), H<sub>2<\/sub>O(BA) OH<sup>\u2212<\/sup>(CB and CA)<\/li>\r\n \t<li>[latex]{\\left[{\\text{Cu(H}}_{2}{\\text{O)}}_{3}\\text{(OH)}\\right]}^{\\text{+}}\\text{(BB)}[\/latex], [latex]{\\left[{\\text{Al(H}}_{2}{\\text{O)}}_{6}\\right]}^{3+}\\left(\\text{BA}\\right)[\/latex], [latex]{\\left[\\text{Cu}{\\left({\\text{H}}_{2}\\text{O}\\right)}_{4}\\right]}^{2+}\\left(\\text{CA}\\right)[\/latex], [latex]{\\left[\\text{Al}{\\left({\\text{H}}_{2}\\text{O}\\right)}_{5}\\left(\\text{OH}\\right)\\right]}^{2+}\\left(\\text{CB}\\right)[\/latex]<\/li>\r\n \t<li>H<sub>2<\/sub>S(BA), [latex]{\\text{NH}}_{2}{}^{-}\\left(\\text{BB}\\right)[\/latex], HS<sup>\u2212<\/sup>(CB), NH<sub>3<\/sub>(CA)<\/li>\r\n<\/ol>\r\n[\/hidden-answer]\r\n\r\n<\/div>\r\n<h2>Glossary<\/h2>\r\n<strong>Br\u00f8nsted-Lowry acid: <\/strong>proton donor\r\n\r\n<strong>Br\u00f8nsted-Lowry base: <\/strong>proton acceptor\r\n\r\n<strong>conjugate acid: <\/strong>substance formed when a base gains a proton\r\n\r\n<strong>conjugate base: <\/strong>substance formed when an acid loses a proton","rendered":"<div class=\"textbox learning-objectives\">\n<h3>Learning Objectives<\/h3>\n<p>By the end of this module, you will be able to:<\/p>\n<ul>\n<li>Identify acids, bases, and conjugate acid-base pairs according to the Br\u00f8nsted-Lowry definition<\/li>\n<li>Use the ion-product constant for water to calculate hydronium and hydroxide ion concentrations<\/li>\n<\/ul>\n<\/div>\n<p>Acids and bases have been known for a long time. When Robert Boyle characterized them in 1680, he noted that acids dissolve many substances, change the color of certain natural dyes (for example, they change litmus from blue to red), and lose these characteristic properties after coming into contact with alkalis (bases). In the eighteenth century, it was recognized that acids have a sour taste, react with limestone to liberate a gaseous substance (now known to be CO<sub>2<\/sub>), and interact with alkalis to form neutral substances. In 1815, Humphry Davy contributed greatly to the development of the modern acid-base concept by demonstrating that hydrogen is the essential constituent of acids. Around that same time, Joseph Louis Gay-Lussac concluded that acids are substances that can neutralize bases and that these two classes of substances can be defined only in terms of each other. The significance of hydrogen was reemphasized in 1884 when Carl Axel <strong>Arrhenius<\/strong> defined an acid as a compound that dissolves in water to yield hydrogen cations (now recognized to be hydronium ions) and a base as a compound that dissolves in water to yield hydroxide anions.<\/p>\n<p>In an earlier module, we defined acids and bases as Arrhenius did: We identified an acid as a compound that dissolves in water to yield hydronium ions (H<sub>3<\/sub>O<sup>+<\/sup>) and a base as a compound that dissolves in water to yield hydroxide ions (OH<sup>\u2212<\/sup>). This definition is not wrong; it is simply limited.<\/p>\n<p>We extend on the Arrhenius definition of an acid or a base using the more general definition proposed in 1923 by the Danish chemist Johannes Br\u00f8nsted and the English chemist Thomas Lowry. Their definition centers on the proton, H<sup>+<\/sup>. A proton is what remains when a normal hydrogen atom, [latex]{}_{1}{}^{1}\\text{H}[\/latex], loses an electron. A compound that donates a proton to another compound is called a <strong>Br\u00f8nsted-Lowry acid<\/strong>, and a compound that accepts a proton is called a <strong>Br\u00f8nsted-Lowry base<\/strong>. An acid-base reaction is the transfer of a proton from a proton donor (acid) to a proton acceptor (base).<\/p>\n<p>Acids may be compounds such as HCl or H<sub>2<\/sub>SO<sub>4<\/sub>, organic acids like acetic acid (CH<sub>3<\/sub>COOH) or ascorbic acid (vitamin C), or H<sub>2<\/sub>O. Anions (such as [latex]{\\text{HSO}}_{4}^{-}[\/latex], [latex]{\\text{H}}_{2}{\\text{PO}}_{4}^{-}[\/latex], HS<sup>\u2212<\/sup>, and [latex]{\\text{HCO}}_{3}^{-}[\/latex]) may also act as acids. Bases fall into the same two categories. Bases may be neutral molecules (such as H<sub>2<\/sub>O, NH<sub>3<\/sub>, and CH<sub>3<\/sub>NH<sub>2<\/sub>), anions (such as OH<sup>\u2212<\/sup>, HS<sup>\u2212<\/sup>, [latex]{\\text{HCO}}_{3}^{-}[\/latex], [latex]{\\text{CO}}_{3}^{2-}[\/latex], F<sup>\u2212<\/sup>, and [latex]{\\text{PO}}_{4}^{3-}[\/latex]). The most familiar bases are ionic compounds such as NaOH and Ca(OH)<sub>2<\/sub>, which contain the hydroxide ion, OH<sup>\u2212<\/sup>. The hydroxide ion in these compounds accepts a proton from acids to form water:<\/p>\n<p style=\"text-align: center\">[latex]\\large{\\text{H}}^{\\text{+}}+{\\text{OH}}^{-}\\longrightarrow {\\text{H}}_{2}\\text{O}[\/latex]<\/p>\n<p>We call the product that remains after an acid donates a proton the <strong>conjugate base<\/strong> of the acid. This species is a base because it can accept a proton (to re-form the acid):<\/p>\n<p style=\"text-align: center\">[latex]\\large\\begin{array}{l}\\text{acid}\\rightarrow \\text{proton}+\\text{conjugate base}\\\\ \\text{HF}\\rightarrow {\\text{H}}^{\\text{+}}+{\\text{F}}^{-}\\\\ {\\text{H}}_{2}{\\text{SO}}_{4}\\rightarrow {\\text{H}}^{+}+{\\text{HSO}}_{4}^{-}\\\\ {\\text{H}}_{2}\\text{O}\\rightarrow {\\text{H}}^{\\text{+}}+{\\text{OH}}^{-}\\\\ {\\text{HSO}}_{4}^{-}\\rightarrow {\\text{H}}^{\\text{+}}+{\\text{SO}}_{4}^{2-}\\\\ {\\text{NH}}_{4}^{+}\\rightarrow {\\text{H}}^{+}+{\\text{NH}}_{3}\\end{array}[\/latex]<\/p>\n<p>We call the product that results when a base accepts a proton the base\u2019s <strong>conjugate acid<\/strong>. This species is an acid because it can give up a proton (and thus re-form the base):<\/p>\n<p style=\"text-align: center\">[latex]\\large\\begin{array}{l}\\text{base}+\\text{proton}\\rightarrow \\text{conjugate acid}\\\\ {\\text{OH}}^{-}+{\\text{H}}^{\\text{+}}\\rightarrow {\\text{H}}_{2}\\text{O}\\\\ {\\text{H}}_{2}\\text{O}+{\\text{H}}^{\\text{+}}\\rightarrow {\\text{H}}_{3}{\\text{O}}^{\\text{+}}\\\\ {\\text{NH}}_{3}+{\\text{H}}^{\\text{+}}\\rightarrow {\\text{NH}}_{4}{}^{\\text{+}}\\\\ {\\text{S}}^{2-}+{\\text{H}}^{\\text{+}}\\rightarrow {\\text{HS}}^{-}\\\\ {\\text{CO}}_{3}{}^{2-}+{\\text{H}}^{\\text{+}}\\rightarrow {\\text{HCO}}_{3}{}^{-}\\\\ {\\text{F}}^{-}+{\\text{H}}^{\\text{+}}\\rightarrow \\text{HF}\\end{array}[\/latex]<\/p>\n<p>In these two sets of equations, the behaviors of acids as proton donors and bases as proton acceptors are represented in isolation. In reality, all acid-base reactions involve the <em>transfer<\/em> of protons between acids and bases. For example, consider the acid-base reaction that takes place when ammonia is dissolved in water. A water molecule (functioning as an acid) transfers a proton to an ammonia molecule (functioning as a base), yielding the conjugate base of water, OH<sup>\u2212<\/sup>, and the conjugate acid of ammonia, [latex]{\\text{NH}}_{4}{}^{\\text{+}}:[\/latex]<br \/>\n<img decoding=\"async\" class=\"aligncenter\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images-archive-read-only\/wp-content\/uploads\/sites\/887\/2015\/05\/23213723\/CNX_Chem_14_01_conjugate_img.jpg\" alt=\"This figure has three parts in two rows. In the first row, two diagrams of acid-base pairs are shown. On the left, a space filling model of H subscript 2 O is shown with a red O atom at the center and two smaller white H atoms attached in a bent shape. Above this model is the label \u201cH subscript 2 O (acid)\u201d in purple. An arrow points right, which is labeled \u201cRemove H superscript plus.\u201d To the right is another space filling model with a single red O atom to which a single smaller white H atom is attached. The label in purple above this model reads, \u201cO H superscript negative (conjugate base).\u201d Above both of these red and white models is an upward pointing bracket that is labeled \u201cConjugate acid-base pair.\u201d To the right is a space filling model with a central blue N atom to which three smaller white H atoms are attached in a triangular pyramid arrangement. A label in green above reads \u201cN H subscript 3 (base).\u201d An arrow labeled \u201cAdd H superscript plus\u201d points right. To the right of the arrow is another space filling model with a blue central N atom and four smaller white H atoms in a tetrahedral arrangement. The green label above reads \u201cN H subscript 3 superscript plus (conjugate acid).\u201d Above both of these blue and white models is an upward pointing bracket that is labeled \u201cConjugate acid-base pair.\u201d The second row of the figure shows the chemical reaction, H subscript 2 O ( l ) is shown in purple, and is labeled below in purple as \u201cacid,\u201d plus N H subscript 3 (a q) in green, labeled below in green as \u201cbase,\u201d followed by a double sided arrow arrow and O H superscript negative (a q) in purple, labeled in purple as \u201cconjugate base,\u201d plus N H subscript 4 superscript plus (a q)\u201d in green, which is labeled in green as \u201cconjugate acid.\u201d The acid on the left side of the equation is connected to the conjugate base on the right with a purple line. Similarly, the base on the left is connected to the conjugate acid on the right side.\" \/><\/p>\n<p>&nbsp;<\/p>\n<div class=\"textbox examples\">\n<h3>Example 1: Bronsted-Lowry Acids and Bases<\/h3>\n<p>Identify the Br\u00f8nsted-Lowry acid and the Br\u00f8nsted-Lowry base in this chemical equation:<\/p>\n<p>[latex]\\large{\\text{C}_{6}\\text{H}}_{5}\\text{OH}\\left(l\\right)+{\\text{NH}_{2}}^{-}\\left(aq\\right)\\longrightarrow {\\text{C}_{6}\\text{H}}_{5}\\text{O}^{-}\\left(aq\\right)+{\\text{NH}}_{3}\\left(aq\\right)[\/latex]<\/p>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q160586\">Show Answer<\/span><\/p>\n<div id=\"q160586\" class=\"hidden-answer\" style=\"display: none\">\n<p>The C<sub class=\"subscript\">6<\/sub>H<sub class=\"subscript\">5<\/sub>OH molecule is losing an H<sup class=\"superscript\">+<\/sup>; it is the proton donor and the Br\u00f8nsted-Lowry acid. The NH<sub class=\"subscript\">2<\/sub><sup class=\"superscript\">\u2212<\/sup> ion (called the amide ion) is accepting the H<sup class=\"superscript\">+<\/sup> ion to become NH<sub class=\"subscript\">3<\/sub>, so it is the Br\u00f8nsted-Lowry base.<\/p>\n<\/div>\n<\/div>\n<\/div>\n<div class=\"textbox examples\">\n<h3>Example 2: Conjugate Acids and Conjugate Bases<\/h3>\n<p>Identify the conjugate acid-base pairs in this equation:<\/p>\n<p>[latex]\\large{(\\text{C}\\text{H}}_{3})_{3}\\text{N}\\left(l\\right)+{\\text{H}_{2}}\\text{O}\\left(l\\right)\\longrightarrow {(\\text{C}\\text{H}}_{3})_{3}\\text{NH}^{+}\\left(aq\\right)+{\\text{OH}}^{-}\\left(aq\\right)[\/latex]<\/p>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q1605861\">Show Answer<\/span><\/p>\n<div id=\"q1605861\" class=\"hidden-answer\" style=\"display: none\">\n<p>One pair is H<sub class=\"subscript\">2<\/sub>O and OH<sup class=\"superscript\">\u2212<\/sup>, where H<sub class=\"subscript\">2<\/sub>O has one more H<sup class=\"superscript\">+<\/sup> and is the conjugate acid, while OH<sup class=\"superscript\">\u2212<\/sup> has one less H<sup class=\"superscript\">+<\/sup> and is the conjugate base. The other pair consists of (CH<sub class=\"subscript\">3<\/sub>)<sub class=\"subscript\">3<\/sub>N and (CH<sub class=\"subscript\">3<\/sub>)<sub class=\"subscript\">3<\/sub>NH<sup class=\"superscript\">+<\/sup>, where (CH<sub class=\"subscript\">3<\/sub>)<sub class=\"subscript\">3<\/sub>NH<sup class=\"superscript\">+<\/sup> is the conjugate acid (it has an additional proton) and (CH<sub class=\"subscript\">3<\/sub>)<sub class=\"subscript\">3<\/sub>N is the conjugate base.<\/p>\n<\/div>\n<\/div>\n<h4>Check Your Learning<\/h4>\n<p>Identify the conjugate acid-base pairs in this equation:<\/p>\n<p>[latex]\\large{\\text{NH}}_{2}^{-}\\left(aq\\right)+{\\text{H}_{2}}\\text{O}\\left(l\\right)\\longrightarrow {\\text{NH}}_{3}\\left(aq\\right)+{\\text{OH}}^{-}\\left(aq\\right)[\/latex]<\/p>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q366443\">Show Answer<\/span><\/p>\n<div id=\"q366443\" class=\"hidden-answer\" style=\"display: none\">\n<p>H<sub class=\"subscript\">2<\/sub>O (acid) and OH<sup class=\"superscript\">\u2212<\/sup> (base); NH<sub class=\"subscript\">2<\/sub><sup class=\"superscript\">\u2212<\/sup> (base) and NH<sub class=\"subscript\">3<\/sub> (acid)<\/p>\n<\/div>\n<\/div>\n<\/div>\n<div class=\"textbox key-takeaways\">\n<h3>Key Concepts and Summary<\/h3>\n<p>A compound that can donate a proton (a hydrogen ion) to another compound is called a Br\u00f8nsted-Lowry acid. The compound that accepts the proton is called a Br\u00f8nsted-Lowry base. The species remaining after a Br\u00f8nsted-Lowry acid has lost a proton is the conjugate base of the acid. The species formed when a Br\u00f8nsted-Lowry base gains a proton is the conjugate acid of the base. Thus, an acid-base reaction occurs when a proton is transferred from an acid to a base, with formation of the conjugate base of the reactant acid and formation of the conjugate acid of the reactant base.<\/p>\n<\/div>\n<div class=\"textbox exercises\">\n<h3>Exercises<\/h3>\n<ol>\n<li>Write equations that show NH<sub>3<\/sub> as both a conjugate acid and a conjugate base.<\/li>\n<li>Write equations that show [latex]{\\text{H}}_{2}{\\text{PO}}_{4}{}^{-}[\/latex] acting both as an acid and as a base.<\/li>\n<li>What is the conjugate acid of each of the following? What is the conjugate base of each?\n<ol style=\"list-style-type: lower-alpha\">\n<li>OH<sup>\u2212<\/sup><\/li>\n<li>H<sub>2<\/sub>O<\/li>\n<li>[latex]{\\text{HCO}}_{3}{}^{-}[\/latex]<\/li>\n<li>NH<sub>3<\/sub><\/li>\n<li>[latex]{\\text{HSO}}_{4}{}^{-}[\/latex]<\/li>\n<li>H<sub>2<\/sub>O<sub>2<\/sub><\/li>\n<li>HS<sup>\u2212<\/sup><\/li>\n<li>[latex]{\\text{H}}_{5}{\\text{N}}_{2}{}^{\\text{+}}[\/latex]<\/li>\n<\/ol>\n<\/li>\n<li>What is the conjugate acid of each of the following? What is the conjugate base of each?\n<ol style=\"list-style-type: lower-alpha\">\n<li>H<sub>2<\/sub>S<\/li>\n<li>[latex]{\\text{H}}_{2}{\\text{PO}}_{4}{}^{-}[\/latex]<\/li>\n<li>PH<sub>3<\/sub><\/li>\n<li>HS<sup>\u2212<\/sup><\/li>\n<li>[latex]{\\text{HSO}}_{3}{}^{-}[\/latex]<\/li>\n<li>[latex]{\\text{H}}_{3}{\\text{O}}_{2}{}^{\\text{+}}[\/latex]<\/li>\n<li>H<sub>4<\/sub>N<sub>2<\/sub><\/li>\n<li>CH<sub>3<\/sub>OH<\/li>\n<\/ol>\n<\/li>\n<li>Identify and label the Br\u00f8nsted-Lowry acid, its conjugate base, the Br\u00f8nsted-Lowry base, and its conjugate acid in each of the following equations:\n<ol style=\"list-style-type: lower-alpha\">\n<li>[latex]{\\text{HNO}}_{3}+{\\text{H}}_{2}\\text{O}\\longrightarrow {\\text{H}}_{3}{\\text{O}}^{\\text{+}}+{\\text{NO}}_{3}{}^{-}[\/latex]<\/li>\n<li>[latex]{\\text{CN}}^{-}+{\\text{H}}_{2}\\text{O}\\longrightarrow \\text{HCN}+{\\text{OH}}^{-}[\/latex]<\/li>\n<li>[latex]{\\text{H}}_{2}{\\text{SO}}_{4}+{\\text{Cl}}^{-}\\longrightarrow \\text{HCl}+{\\text{HSO}}_{4}{}^{-}[\/latex]<\/li>\n<li>[latex]{\\text{HSO}}_{4}{}^{-}+{\\text{OH}}^{-}\\longrightarrow {\\text{SO}}_{4}{}^{\\text{2-}}+{\\text{H}}_{2}\\text{O}[\/latex]<\/li>\n<li>[latex]{\\text{O}}^{2-}+{\\text{H}}_{2}\\text{O}\\longrightarrow 2{\\mathrm{OH}}^{-}[\/latex]<\/li>\n<li>[latex]{\\text{H}}_{2}\\text{S}+{\\text{NH}}_{2}{}^{-}\\longrightarrow {\\text{HS}}^{-}+{\\text{NH}}_{3}[\/latex]<\/li>\n<\/ol>\n<\/li>\n<li>Identify and label the Br\u00f8nsted-Lowry acid, its conjugate base, the Br\u00f8nsted-Lowry base, and its conjugate acid in each of the following equations:\n<ol style=\"list-style-type: lower-alpha\">\n<li>[latex]{\\text{NO}}_{2}{}^{-}+{\\text{H}}_{2}\\text{O}\\longrightarrow {\\text{HNO}}_{2}+{\\text{OH}}^{-}[\/latex]<\/li>\n<li>[latex]\\text{HBr}+{\\text{H}}_{2}\\text{O}\\longrightarrow {\\text{H}}_{3}{\\text{O}}^{\\text{+}}+{\\text{Br}}^{-}[\/latex]<\/li>\n<li>[latex]{\\text{HS}}^{-}+{\\text{H}}_{2}\\text{O}\\longrightarrow {\\text{H}}_{2}\\text{S}+{\\text{OH}}^{-}[\/latex]<\/li>\n<li>[latex]{\\text{H}}_{2}{\\text{PO}}_{4}{}^{-}+{\\text{OH}}^{-}\\longrightarrow {\\text{HPO}}_{4}{}^{\\text{2-}}+{\\text{H}}_{2}\\text{O}[\/latex]<\/li>\n<li>[latex]{\\text{H}}_{2}{\\text{PO}}_{4}{}^{-}+\\text{HCl}\\longrightarrow {\\text{H}}_{3}{\\text{PO}}_{4}+{\\text{Cl}}^{-}[\/latex]<\/li>\n<li>[latex]{\\text{CH}}_{3}\\text{OH}+{\\text{H}}^{-}\\longrightarrow {\\text{CH}}_{3}{\\text{O}}^{-}+{\\text{H}}_{2}[\/latex]<\/li>\n<\/ol>\n<\/li>\n<\/ol>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q41360\">Show Selected Answers<\/span><\/p>\n<div id=\"q41360\" class=\"hidden-answer\" style=\"display: none\">\n<p>1. One example for NH<sub>3<\/sub> as a conjugate acid: [latex]{\\text{NH}}_{2}{}^{-}+{\\text{H}}^{\\text{+}}\\longrightarrow {\\text{NH}}_{3}[\/latex]; as a conjugate base: [latex]{\\text{NH}}_{4}{}^{\\text{+}}\\left(aq\\right)+{\\text{OH}}^{-}\\left(aq\\right)\\longrightarrow {\\text{NH}}_{3}\\left(aq\\right)+{\\text{H}}_{2}\\text{O}\\left(l\\right)[\/latex]<\/p>\n<p>3. The conjugate acids and bases are as follows:<\/p>\n<ol style=\"list-style-type: lower-alpha\">\n<li>H<sub>2<\/sub>O, O<sup>2\u2212<\/sup><\/li>\n<li>[latex]{\\text{H}}_{3}{\\text{O}}^{+}[\/latex], OH<sup>\u2212<\/sup><\/li>\n<li>H<sub>2<\/sub>CO<sub>3<\/sub>, [latex]{\\text{CO}}_{3}{}^{2-}[\/latex]<\/li>\n<li>[latex]{\\text{NH}}_{4}{}^{\\text{+}}[\/latex], [latex]{\\text{NH}}_{2}^{-}[\/latex]<\/li>\n<li>H<sub>2<\/sub>SO<sub>4<\/sub>, [latex]{\\text{SO}}_{4}^{2-}[\/latex]<\/li>\n<li>[latex]{\\text{H}}_{3}{\\text{O}}_{2}^{+}[\/latex], [latex]{\\text{HO}}_{2}^{-}[\/latex]<\/li>\n<li>H<sub>2<\/sub>S, S<sup>2\u2212<\/sup><\/li>\n<li>[latex]{\\text{H}}_{6}{\\text{N}}_{2}{}^{2+}[\/latex], H<sub>4<\/sub>N<sub>2<\/sub><\/li>\n<\/ol>\n<p>5. The labels are Br\u00f8nsted-Lowry acid = BA; its conjugate base = CB; Br\u00f8nsted-Lowry base = BB; its conjugate acid = CA.<\/p>\n<ol style=\"list-style-type: lower-alpha\">\n<li>HNO<sub>3<\/sub>(BA), H<sub>2<\/sub>O(BB), [latex]{\\text{H}}_{3}{\\text{O}}^{\\text{+}}\\left(\\text{CA}\\right)[\/latex], [latex]{\\text{NO}}_{3}{}^{-}\\left(\\text{CB}\\right)[\/latex]<\/li>\n<li>CN<sup>\u2212<\/sup>(BB), H<sub>2<\/sub>O(BA), HCN(CA), OH<sup>\u2212<\/sup>(CB)<\/li>\n<li>H<sub>2<\/sub>SO<sub>4<\/sub>(BA), Cl<sup>\u2212<\/sup>(BB), HCl(CA), [latex]{\\text{HSO}}_{4}{}^{-}\\left(\\text{CB}\\right)[\/latex]<\/li>\n<li>[latex]{\\text{HSO}}_{4}{}^{-}\\left(\\text{BA}\\right)[\/latex], OH<sup>\u2212<\/sup>(BB), [latex]{\\text{SO}}_{4}{}^{\\text{2-}}[\/latex] (CB), H<sub>2<\/sub>O(CA)<\/li>\n<li>O<sup>2\u2212<\/sup>(BB), H<sub>2<\/sub>O(BA) OH<sup>\u2212<\/sup>(CB and CA)<\/li>\n<li>[latex]{\\left[{\\text{Cu(H}}_{2}{\\text{O)}}_{3}\\text{(OH)}\\right]}^{\\text{+}}\\text{(BB)}[\/latex], [latex]{\\left[{\\text{Al(H}}_{2}{\\text{O)}}_{6}\\right]}^{3+}\\left(\\text{BA}\\right)[\/latex], [latex]{\\left[\\text{Cu}{\\left({\\text{H}}_{2}\\text{O}\\right)}_{4}\\right]}^{2+}\\left(\\text{CA}\\right)[\/latex], [latex]{\\left[\\text{Al}{\\left({\\text{H}}_{2}\\text{O}\\right)}_{5}\\left(\\text{OH}\\right)\\right]}^{2+}\\left(\\text{CB}\\right)[\/latex]<\/li>\n<li>H<sub>2<\/sub>S(BA), [latex]{\\text{NH}}_{2}{}^{-}\\left(\\text{BB}\\right)[\/latex], HS<sup>\u2212<\/sup>(CB), NH<sub>3<\/sub>(CA)<\/li>\n<\/ol>\n<\/div>\n<\/div>\n<\/div>\n<h2>Glossary<\/h2>\n<p><strong>Br\u00f8nsted-Lowry acid: <\/strong>proton donor<\/p>\n<p><strong>Br\u00f8nsted-Lowry base: <\/strong>proton acceptor<\/p>\n<p><strong>conjugate acid: <\/strong>substance formed when a base gains a proton<\/p>\n<p><strong>conjugate base: <\/strong>substance formed when an acid loses a proton<\/p>\n\n\t\t\t <section class=\"citations-section\" role=\"contentinfo\">\n\t\t\t <h3>Candela Citations<\/h3>\n\t\t\t\t\t <div>\n\t\t\t\t\t\t <div id=\"citation-list-602\">\n\t\t\t\t\t\t\t <div class=\"licensing\"><div class=\"license-attribution-dropdown-subheading\">CC licensed content, Shared previously<\/div><ul class=\"citation-list\"><li>Introductory Chemistry- 1st Canadian Edition . <strong>Authored by<\/strong>: Jessie A. Key and David W. Ball. <strong>Provided by<\/strong>: BCCampus. <strong>Located at<\/strong>: <a target=\"_blank\" href=\"https:\/\/opentextbc.ca\/introductorychemistry\/\">https:\/\/opentextbc.ca\/introductorychemistry\/<\/a>. <strong>License<\/strong>: <em><a target=\"_blank\" rel=\"license\" href=\"https:\/\/creativecommons.org\/licenses\/by-nc-sa\/4.0\/\">CC BY-NC-SA: Attribution-NonCommercial-ShareAlike<\/a><\/em>. <strong>License Terms<\/strong>: Download this book for free at http:\/\/open.bccampus.ca<\/li><li>Chemistry. <strong>Provided by<\/strong>: OpenStaxCollege. <strong>Located at<\/strong>: <a target=\"_blank\" href=\"http:\/\/openstaxcollege.org\">http:\/\/openstaxcollege.org<\/a>. <strong>License<\/strong>: <em><a target=\"_blank\" rel=\"license\" href=\"https:\/\/creativecommons.org\/licenses\/by\/4.0\/\">CC BY: Attribution<\/a><\/em>. <strong>License Terms<\/strong>: Download for free at https:\/\/openstaxcollege.org\/textbooks\/chemistry\/get<\/li><\/ul><\/div>\n\t\t\t\t\t\t <\/div>\n\t\t\t\t\t <\/div>\n\t\t\t <\/section>","protected":false},"author":23485,"menu_order":2,"template":"","meta":{"_candela_citation":"[{\"type\":\"cc\",\"description\":\"Introductory Chemistry- 1st Canadian Edition \",\"author\":\"Jessie A. 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