{"id":603,"date":"2017-12-14T21:42:06","date_gmt":"2017-12-14T21:42:06","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/suny-mcc-introductorychemistry\/chapter\/arrhenius-acids-and-bases\/"},"modified":"2018-08-24T03:00:05","modified_gmt":"2018-08-24T03:00:05","slug":"arrhenius-acids-and-bases","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/suny-mcc-introductorychemistry\/chapter\/arrhenius-acids-and-bases\/","title":{"raw":"10.1 Introduction to Acids and Bases","rendered":"10.1 Introduction to 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>Describe basic properties of acids and bases<\/li>\r\n \t<li>Identify an Arrhenius acid and an Arrhenius base<\/li>\r\n \t<li>Name binary acids and oxoacids<\/li>\r\n<\/ul>\r\n<\/div>\r\n<div id=\"ball-ch12_s01\" class=\"section\" lang=\"en\">\r\n\r\nAcids and bases have been known for a long time. When Robert <span class=\"no-emphasis\">Boyle<\/span> 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 <span class=\"no-emphasis\">Davy<\/span> 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 <span class=\"no-emphasis\">Arrhenius<\/span> 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\nAcids and bases are common solutions that exist everywhere. Almost every liquid that we encounter in our daily lives consists of acidic and basic properties, with the exception of water. They have completely different properties and are able to neutralize to form H<sub>2<\/sub>O, which will be discussed later in a subsection. Acids and bases can be defined by their physical and chemical observations (Table 1).\r\n<table id=\"fs-idp55860464\" class=\"span-all\" summary=\"none\">\r\n<thead>\r\n<tr valign=\"middle\">\r\n<th colspan=\"3\">Table 1. General Properties of Acids and Bases<\/th>\r\n<\/tr>\r\n<tr valign=\"middle\">\r\n<th colspan=\"2\">Acids<\/th>\r\n<th>Bases<\/th>\r\n<\/tr>\r\n<\/thead>\r\n<tbody>\r\n<tr valign=\"middle\">\r\n<td colspan=\"2\">produce a piercing pain in a wound<\/td>\r\n<td>give a slippery feel<\/td>\r\n<\/tr>\r\n<tr>\r\n<td colspan=\"2\">taste sour<\/td>\r\n<td>taste bitter<\/td>\r\n<\/tr>\r\n<tr>\r\n<td colspan=\"2\">are red on blue litmus paper (a pH indicator)<\/td>\r\n<td>are blue on red litmus paper (a pH indicator)<\/td>\r\n<\/tr>\r\n<tr valign=\"middle\">\r\n<td colspan=\"2\">have a pH &lt; 7<\/td>\r\n<td>have a pH &gt; 7<\/td>\r\n<\/tr>\r\n<tr>\r\n<td colspan=\"2\">Common example: lemons, oranges, vinegar, urine<\/td>\r\n<td>Common examples: soap, toothpaste, bleach, cleaning agents, limewater<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\nAcids and bases in aqueous solutions will conduct electricity because they contain dissolved ions. Therefore, acids and bases are <i>electrolytes<\/i>. Strong acids and bases will be strong <strong>electrolytes<\/strong>. Weak acids and bases will be weak electrolytes. This affects the amount of conductivity.\r\n<h2>The Arrhenius Definition of Acids and Bases<\/h2>\r\n<p id=\"ball-ch12_s01_p01\" class=\"para editable block\">Historically, the first chemical definition of an acid and a base was put forward by Svante Arrhenius, a Swedish chemist, in 1884. An <span class=\"margin_term\"><a class=\"glossterm\">Arrhenius acid<\/a><\/span>\u00a0is a compound that increases the H<sup class=\"superscript\">+<\/sup> ion concentration in aqueous solution. The H<sup class=\"superscript\">+<\/sup> ion is just a bare proton, and it is rather clear that bare protons are not floating around in an aqueous solution. Instead, chemistry has defined the <span class=\"margin_term\"><a class=\"glossterm\">hydronium ion<\/a><\/span>\u00a0(H<sub class=\"subscript\">3<\/sub>O<sup class=\"superscript\">+<\/sup>) as the actual chemical species that represents an H<sup class=\"superscript\">+<\/sup> ion. H<sup class=\"superscript\">+<\/sup> ions and H<sub class=\"subscript\">3<\/sub>O<sup class=\"superscript\">+<\/sup> ions are often considered interchangeable when writing chemical equations (although a properly balanced chemical equation should also include the additional H<sub class=\"subscript\">2<\/sub>O). This process is represented\u00a0in a chemical equation by adding H<sub>2<\/sub>O to the reactants side.<\/p>\r\n<p style=\"text-align: center\">[latex]\\text{HCl}\\left(aq\\right)+{\\text{H}}_{2}\\text{O}\\left(l\\right)\\longrightarrow {\\text{H}}^{\\text{+}}\\left(aq\\right)+{\\text{Cl}}^{-}\\left(aq\\right)[\/latex]<\/p>\r\nIn this reaction, hydrochloric acid (<span id=\"MathJax-Element-7-Frame\" class=\"MathJax\" role=\"presentation\"><span id=\"MathJax-Span-70\" class=\"math\"><span id=\"MathJax-Span-71\" class=\"mrow\"><span id=\"MathJax-Span-72\" class=\"mi\">H<\/span><span id=\"MathJax-Span-73\" class=\"mi\">C<\/span><span id=\"MathJax-Span-74\" class=\"mi\">l<\/span><\/span><\/span><\/span>) dissociates into hydrogen (<span id=\"MathJax-Element-8-Frame\" class=\"MathJax\" role=\"presentation\"><span id=\"MathJax-Span-75\" class=\"math\"><span id=\"MathJax-Span-76\" class=\"mrow\"><span id=\"MathJax-Span-77\" class=\"msubsup\"><span id=\"MathJax-Span-78\" class=\"mi\">H<\/span><span id=\"MathJax-Span-79\" class=\"mo\">+<\/span><\/span><\/span><\/span><\/span>) and chlorine (<span id=\"MathJax-Element-9-Frame\" class=\"MathJax\" role=\"presentation\"><span id=\"MathJax-Span-80\" class=\"math\"><span id=\"MathJax-Span-81\" class=\"mrow\"><span id=\"MathJax-Span-82\" class=\"mi\">C<\/span><span id=\"MathJax-Span-83\" class=\"msubsup\"><span id=\"MathJax-Span-84\" class=\"mi\">l<\/span><sup><span id=\"MathJax-Span-85\" class=\"mo\">\u2212<\/span><\/sup><\/span><\/span><\/span><\/span>) ions when dissolved in water, thereby releasing H<sup>+<\/sup> ions into solution. Formation of the hydronium ion equation:\r\n<p style=\"text-align: center\">[latex]\\text{HCl}\\left(aq\\right)+{\\text{H}}_{2}\\text{O}\\left(l\\right)\\longrightarrow \\text{H}_{3}\\text{O}^{\\text{+}}\\left(aq\\right)+{\\text{Cl}}^{-}\\left(aq\\right)[\/latex]<\/p>\r\n<p class=\"para editable block\">Classic Arrhenius acids can be considered ionic compounds in which H<sup class=\"superscript\">+<\/sup> is the cation. Table 2 lists some Arrhenius acids and their names.<\/p>\r\n\r\n<div id=\"ball-ch12_s01_t01\" class=\"table block\">\r\n<table style=\"border-spacing: 0px\" cellpadding=\"0\">\r\n<thead>\r\n<tr style=\"height: 15px\">\r\n<th style=\"height: 15px;width: 312.483px\">Table 2 Some Arrhenius Acids<\/th>\r\n<th style=\"height: 15px;width: 154.983px\"><\/th>\r\n<\/tr>\r\n<tr style=\"height: 15px\">\r\n<th style=\"height: 15px;width: 312.483px\">Formula<\/th>\r\n<th style=\"height: 15px;width: 154.983px\">Name<\/th>\r\n<\/tr>\r\n<\/thead>\r\n<tbody>\r\n<tr style=\"height: 19px\">\r\n<td style=\"height: 19px;width: 312.483px\">HC<sub class=\"subscript\">2<\/sub>H<sub class=\"subscript\">3<\/sub>O<sub class=\"subscript\">2<\/sub> (also written CH<sub class=\"subscript\">3<\/sub>COOH)<\/td>\r\n<td style=\"height: 19px;width: 154.983px\">acetic acid<\/td>\r\n<\/tr>\r\n<tr style=\"height: 19px\">\r\n<td style=\"height: 19px;width: 312.483px\">HClO<sub class=\"subscript\">3<\/sub><\/td>\r\n<td style=\"height: 19px;width: 154.983px\">chloric acid<\/td>\r\n<\/tr>\r\n<tr style=\"height: 15px\">\r\n<td style=\"height: 15px;width: 312.483px\">HCl<\/td>\r\n<td style=\"height: 15px;width: 154.983px\">hydrochloric acid<\/td>\r\n<\/tr>\r\n<tr style=\"height: 15px\">\r\n<td style=\"height: 15px;width: 312.483px\">HBr<\/td>\r\n<td style=\"height: 15px;width: 154.983px\">hydrobromic acid<\/td>\r\n<\/tr>\r\n<tr style=\"height: 15px\">\r\n<td style=\"height: 15px;width: 312.483px\">HI<\/td>\r\n<td style=\"height: 15px;width: 154.983px\">hydriodic acid<\/td>\r\n<\/tr>\r\n<tr style=\"height: 15px\">\r\n<td style=\"height: 15px;width: 312.483px\">HF<\/td>\r\n<td style=\"height: 15px;width: 154.983px\">hydrofluoric acid<\/td>\r\n<\/tr>\r\n<tr style=\"height: 19px\">\r\n<td style=\"height: 19px;width: 312.483px\">HNO<sub class=\"subscript\">3<\/sub><\/td>\r\n<td style=\"height: 19px;width: 154.983px\">nitric acid<\/td>\r\n<\/tr>\r\n<tr style=\"height: 19px\">\r\n<td style=\"height: 19px;width: 312.483px\">H<sub class=\"subscript\">2<\/sub>C<sub class=\"subscript\">2<\/sub>O<sub class=\"subscript\">4<\/sub><\/td>\r\n<td style=\"height: 19px;width: 154.983px\">oxalic acid<\/td>\r\n<\/tr>\r\n<tr style=\"height: 19px\">\r\n<td style=\"height: 19px;width: 312.483px\">HClO<sub class=\"subscript\">4<\/sub><\/td>\r\n<td style=\"height: 19px;width: 154.983px\">perchloric acid<\/td>\r\n<\/tr>\r\n<tr style=\"height: 19px\">\r\n<td style=\"height: 19px;width: 312.483px\">H<sub class=\"subscript\">3<\/sub>PO<sub class=\"subscript\">4<\/sub><\/td>\r\n<td style=\"height: 19px;width: 154.983px\">phosphoric acid<\/td>\r\n<\/tr>\r\n<tr style=\"height: 19px\">\r\n<td style=\"height: 19px;width: 312.483px\">H<sub class=\"subscript\">2<\/sub>SO<sub class=\"subscript\">4<\/sub><\/td>\r\n<td style=\"height: 19px;width: 154.983px\">sulfuric acid<\/td>\r\n<\/tr>\r\n<tr style=\"height: 19px\">\r\n<td style=\"height: 19px;width: 312.483px\">H<sub class=\"subscript\">2<\/sub>SO<sub class=\"subscript\">3<\/sub><\/td>\r\n<td style=\"height: 19px;width: 154.983px\">sulfurous acid<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<\/div>\r\n<p id=\"ball-ch12_s01_p02\" class=\"para editable block\">An <span class=\"margin_term\"><a class=\"glossterm\">Arrhenius base<\/a><\/span>\u00a0is a compound that increases the OH<sup class=\"superscript\">\u2212<\/sup> ion concentration in aqueous solution. Ionic compounds of the OH<sup class=\"superscript\">\u2212<\/sup> ion are classic Arrhenius bases (Table 3).<\/p>\r\n\r\n<table cellpadding=\"0\">\r\n<thead>\r\n<tr>\r\n<th>Table 3 Some Arrhenius Bases<\/th>\r\n<th><\/th>\r\n<\/tr>\r\n<tr>\r\n<th>Formula<\/th>\r\n<th>Name<\/th>\r\n<\/tr>\r\n<\/thead>\r\n<tbody>\r\n<tr>\r\n<td>NaOH<\/td>\r\n<td>sodium hydroxide<\/td>\r\n<\/tr>\r\n<tr>\r\n<td><sub>KOH<\/sub><\/td>\r\n<td>potassium hydroxide<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Mg(OH)<sub>2<\/sub><\/td>\r\n<td>magnesium hydroxide<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>Ca(OH)<sub>2<\/sub><\/td>\r\n<td>calcium hydroxide<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\nAll of the bases listed in the table are solids at room temperature. Upon dissolving in water, each dissociates into a metal cation and the hydroxide ion.\r\n<p style=\"text-align: center\">[latex]\\text{NaOH}\\left(aq\\right)+{\\text{H}}_{2}\\text{O}\\left(l\\right)\\longrightarrow {\\text{Na}}^{\\text{+}}\\left(aq\\right)+{\\text{OH}}^{-}\\left(aq\\right)[\/latex]<\/p>\r\n\r\n<h2>Nomenclature of Acids and Bases<\/h2>\r\n<p id=\"ball-ch03_s05_p02\" class=\"para editable block\">Acids have their own nomenclature system based off of the type of acid, a binary acid or oxoacid.<\/p>\r\n\r\n<h3 class=\"para editable block\">Binary Acids<\/h3>\r\n<p class=\"para editable block\">If an acid is composed of only hydrogen and one other element, the name is <em class=\"emphasis\">hydro-<\/em> +\u00a0the stem of the other element +\u00a0<em class=\"emphasis\">-ic acid<\/em>. For example, the compound HCl(aq) is hydrochloric acid, while H<sub class=\"subscript\">2<\/sub>S(aq) is hydrosulfuric acid. (If these acids were not dissolved in water, the compounds would be called hydrogen chloride and hydrogen sulfide, respectively. Both of these substances are well known as molecular compounds; when dissolved in water, however, they are treated as acids.)<\/p>\r\n\r\n<table cellpadding=\"0\">\r\n<thead>\r\n<tr>\r\n<th>Table 4. Names of Binary Acids<\/th>\r\n<th><\/th>\r\n<\/tr>\r\n<tr>\r\n<th>Formula<\/th>\r\n<th>Name<\/th>\r\n<\/tr>\r\n<\/thead>\r\n<tbody>\r\n<tr>\r\n<td>HCl<\/td>\r\n<td>hydrochloric acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>HBr<\/td>\r\n<td>hydrobromic acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>HI<\/td>\r\n<td>hydriodic acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>HF<\/td>\r\n<td>hydrofluoric acid<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<h3 class=\"para editable block\">Oxoacids<\/h3>\r\n<p id=\"ball-ch03_s05_p03\" class=\"para editable block\">If a compound is composed of hydrogen ions and a polyatomic anion, then the name of the acid is derived from the stem of the polyatomic ion\u2019s name (Figure 1). Typically, if the anion name ends in -ate, the name of the acid is the stem of the anion name plus <em class=\"emphasis\">-ic acid<\/em>; if the related anion\u2019s name ends in -ite, the name of the corresponding acid is the stem of the anion name plus <em class=\"emphasis\">-ous acid<\/em>. Table 4 lists the formulas and names of a variety of acids that you should be familiar with. You should recognize most of the anions in the formulas of the acids.<\/p>\r\n\r\n\r\n[caption id=\"attachment_1580\" align=\"aligncenter\" width=\"641\"]<img class=\"wp-image-1580 size-full\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/2835\/2017\/12\/24023504\/Oxoacids.jpg\" alt=\"Figure 1. Naming Oxoacids\" width=\"641\" height=\"300\" \/> Figure 1. Naming Oxoacids[\/caption]\r\n\r\n<\/div>\r\n<table cellpadding=\"0\">\r\n<thead>\r\n<tr>\r\n<th>Table 5. Names of Oxoacids<\/th>\r\n<th><\/th>\r\n<\/tr>\r\n<tr>\r\n<th>Formula<\/th>\r\n<th>Name<\/th>\r\n<\/tr>\r\n<\/thead>\r\n<tbody>\r\n<tr>\r\n<td>HNO<sub>2<\/sub><\/td>\r\n<td>nitrous acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>HNO<sub class=\"subscript\">3<\/sub><\/td>\r\n<td>nitric acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>H<sub class=\"subscript\">2<\/sub>CO<sub class=\"subscript\">3<\/sub><\/td>\r\n<td>carbonic acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>HNO<sub>2<\/sub><\/td>\r\n<td>nitrous acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>HNO<sub class=\"subscript\">3<\/sub><\/td>\r\n<td>nitric acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>HClO<\/td>\r\n<td>hypochloric acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>HClO<sub>2<\/sub><\/td>\r\n<td>chlorous acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>HClO<sub>3<\/sub><\/td>\r\n<td>chloric acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>HClO<sub class=\"subscript\">4<\/sub><\/td>\r\n<td>perchloric acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>H<sub class=\"subscript\">3<\/sub>PO<sub class=\"subscript\">4<\/sub><\/td>\r\n<td>phosphoric acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>H<sub class=\"subscript\">2<\/sub>SO<sub class=\"subscript\">4<\/sub><\/td>\r\n<td>sulfuric acid<\/td>\r\n<\/tr>\r\n<tr>\r\n<td>H<sub class=\"subscript\">2<\/sub>SO<sub class=\"subscript\">3<\/sub><\/td>\r\n<td>sulfurous acid<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\nBases are named using the same nomenclature rules as ionic compounds.\r\n<div id=\"ball-ch12_s01\" class=\"section\" lang=\"en\">\r\n<div id=\"ball-ch12_s01_n04\" class=\"key_takeaways editable block\">\r\n<div class=\"bcc-box bcc-success\">\r\n<h3>Key Takeaways<\/h3>\r\n<ul id=\"ball-ch12_s01_l06\" class=\"itemizedlist\">\r\n \t<li>An Arrhenius acid is a compound that increases the H<sup class=\"superscript\">+<\/sup> ion concentration in aqueous solution.<\/li>\r\n \t<li>An Arrhenius base is a compound that increases the OH<sup class=\"superscript\">\u2212<\/sup> ion concentration in aqueous solution.<\/li>\r\n \t<li>Acids are an important class of compounds containing hydrogen and having special nomenclature rules. Binary acids are named using the prefix <em>hydro-<\/em>, changing the \u2013<em>ide<\/em> suffix to \u2013<em>ic<\/em>, and adding \u201cacid;\u201d HCl is hydrochloric acid. Oxyacids are named by changing the ending of the anion to \u2013<em>ic<\/em>, and adding \u201cacid;\u201d H<sub>2<\/sub>CO<sub>3<\/sub> is carbonic acid.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<div class=\"bcc-box bcc-info\">\r\n<h3>Exercises<\/h3>\r\n<div id=\"ball-ch12_s01_qs01\" class=\"qandaset block\">\r\n<ol id=\"ball-ch12_s01_qs01_qd01\" class=\"qandadiv\">\r\n \t<li id=\"ball-ch12_s01_qs01_qd01_qa01\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"ball-ch12_s01_qs01_p01\" class=\"para\">Define <em class=\"emphasis\">Arrhenius acid<\/em>.<\/p>\r\n\r\n<\/div><\/li>\r\n \t<li id=\"ball-ch12_s01_qs01_qd01_qa02\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"ball-ch12_s01_qs01_p03\" class=\"para\">Define <em class=\"emphasis\">Arrhenius base<\/em>.<\/p>\r\n\r\n<\/div><\/li>\r\n \t<li id=\"ball-ch12_s01_qs01_qd01_qa03\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"ball-ch12_s01_qs01_p05\" class=\"para\">What are some general properties of Arrhenius acids?<\/p>\r\n\r\n<\/div><\/li>\r\n \t<li id=\"ball-ch12_s01_qs01_qd01_qa04\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"ball-ch12_s01_qs01_p07\" class=\"para\">What are some general properties of Arrhenius bases?<\/p>\r\n\r\n<\/div><\/li>\r\n \t<li id=\"ball-ch12_s01_qs01_qd01_qa05\" class=\"qandaentry\">\r\n<div class=\"question\">\r\n<p id=\"ball-ch12_s01_qs01_p09\" class=\"para\">Identify each substance as an Arrhenius acid, an Arrhenius base, or neither.<\/p>\r\n\r\n<\/div><\/li>\r\n<\/ol>\r\n<p style=\"padding-left: 60px\">a) \u00a0NaOH<\/p>\r\n<p style=\"padding-left: 60px\">b) \u00a0C<sub class=\"subscript\">2<\/sub>H<sub class=\"subscript\">5<\/sub>OH<\/p>\r\n<p style=\"padding-left: 60px\">c) \u00a0H<sub class=\"subscript\">3<\/sub>PO<sub class=\"subscript\">4<\/sub><\/p>\r\n\r\n<div class=\"question\">\r\n<p id=\"ball-ch12_s01_qs01_p10\" class=\"para\" style=\"padding-left: 30px\">6. \u00a0Identify each substance as an Arrhenius acid, an Arrhenius base, or neither.<\/p>\r\n<p style=\"padding-left: 60px\">a) \u00a0C<sub class=\"subscript\">6<\/sub>H<sub class=\"subscript\">12<\/sub>O<sub class=\"subscript\">6<\/sub><\/p>\r\n<p style=\"padding-left: 60px\">b) \u00a0HNO<sub class=\"subscript\">2<\/sub><\/p>\r\n<p id=\"ball-ch03_s05_qs01_p1\" class=\"para\" style=\"padding-left: 30px\">7. Give the formula for each acid.<\/p>\r\n\r\n<div id=\"ball-ch03_s05_qs01\" class=\"qandaset block\">\r\n<p style=\"padding-left: 60px\">a) \u00a0perchloric acid<\/p>\r\n<p style=\"padding-left: 60px\">b) \u00a0hydriodic acid<\/p>\r\n\r\n<div class=\"question\">\r\n<p id=\"ball-ch03_s05_qs01_p2\" class=\"para\" style=\"padding-left: 30px\">8. Give the formula for each acid.<\/p>\r\n<p style=\"padding-left: 60px\">a) \u00a0hydrosulfuric acid<\/p>\r\n<p style=\"padding-left: 60px\">b) \u00a0phosphorous acid<\/p>\r\n\r\n<\/div>\r\n<div class=\"question\">\r\n<p id=\"ball-ch03_s05_qs01_p3\" class=\"para\" style=\"padding-left: 30px\">9. \u00a0Name each acid.<\/p>\r\n<p style=\"padding-left: 60px\">a) \u00a0HF(aq)<\/p>\r\n<p style=\"padding-left: 60px\">b) \u00a0HNO<sub class=\"subscript\">3<\/sub>(aq)<\/p>\r\n<p style=\"padding-left: 60px\">c) \u00a0H<sub class=\"subscript\">2<\/sub>C<sub class=\"subscript\">2<\/sub>O<sub class=\"subscript\">4<\/sub>(aq)<\/p>\r\n\r\n<\/div>\r\n<div class=\"question\">\r\n<p id=\"ball-ch03_s05_qs01_p4\" class=\"para\" style=\"padding-left: 30px\">10. \u00a0Name each acid.<\/p>\r\n<p style=\"padding-left: 60px\">a) \u00a0H<sub class=\"subscript\">2<\/sub>SO<sub class=\"subscript\">4<\/sub>(aq)<\/p>\r\n<p style=\"padding-left: 60px\">b) \u00a0H<sub class=\"subscript\">3<\/sub>PO<sub class=\"subscript\">4<\/sub>(aq)<\/p>\r\n<p style=\"padding-left: 60px\">c) \u00a0HCl(aq)<\/p>\r\n\r\n<\/div>\r\n<div class=\"question\">\r\n<p id=\"ball-ch03_s05_qs01_p5\" class=\"para\" style=\"padding-left: 30px\">11. \u00a0Name an acid found in food.<\/p>\r\n\r\n<\/div>\r\n<div class=\"question\">\r\n<p id=\"ball-ch03_s05_qs01_p7\" class=\"para\" style=\"padding-left: 30px\">12.\u00a0 Name some properties that acids have in common.<\/p>\r\n\r\n<\/div>\r\n<\/div>\r\n[reveal-answer q=\"742610\"]Show Answers to Select Problems[\/reveal-answer]\r\n[hidden-answer a=\"742610\"]\r\n\r\n1.\u00a0 a compound that increases the H<sup class=\"superscript\">+<\/sup> concentration in water\r\n\r\n3. sour taste, react with metals, and turn litmus red\r\n\r\n5. a) \u00a0Arrhenius base, b) \u00a0neither, c) \u00a0Arrhenius acid\r\n\r\n7. a) \u00a0HClO<sub class=\"subscript\">4<\/sub>(aq), b) \u00a0HI(aq)\r\n\r\n9. a) \u00a0hydrofluoric acid, b) \u00a0nitric acid, c) \u00a0oxalic acid\r\n\r\n11. oxalic acid (answers will vary)\r\n\r\n[\/hidden-answer]\r\n\r\n<\/div>\r\n<\/div>\r\n&nbsp;\r\n\r\n<\/div>\r\n<\/div>\r\n<\/div>","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>Describe basic properties of acids and bases<\/li>\n<li>Identify an Arrhenius acid and an Arrhenius base<\/li>\n<li>Name binary acids and oxoacids<\/li>\n<\/ul>\n<\/div>\n<div id=\"ball-ch12_s01\" class=\"section\" lang=\"en\">\n<p>Acids and bases have been known for a long time. When Robert <span class=\"no-emphasis\">Boyle<\/span> 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 <span class=\"no-emphasis\">Davy<\/span> 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 <span class=\"no-emphasis\">Arrhenius<\/span> 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>Acids and bases are common solutions that exist everywhere. Almost every liquid that we encounter in our daily lives consists of acidic and basic properties, with the exception of water. They have completely different properties and are able to neutralize to form H<sub>2<\/sub>O, which will be discussed later in a subsection. Acids and bases can be defined by their physical and chemical observations (Table 1).<\/p>\n<table id=\"fs-idp55860464\" class=\"span-all\" summary=\"none\">\n<thead>\n<tr valign=\"middle\">\n<th colspan=\"3\">Table 1. General Properties of Acids and Bases<\/th>\n<\/tr>\n<tr valign=\"middle\">\n<th colspan=\"2\">Acids<\/th>\n<th>Bases<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr valign=\"middle\">\n<td colspan=\"2\">produce a piercing pain in a wound<\/td>\n<td>give a slippery feel<\/td>\n<\/tr>\n<tr>\n<td colspan=\"2\">taste sour<\/td>\n<td>taste bitter<\/td>\n<\/tr>\n<tr>\n<td colspan=\"2\">are red on blue litmus paper (a pH indicator)<\/td>\n<td>are blue on red litmus paper (a pH indicator)<\/td>\n<\/tr>\n<tr valign=\"middle\">\n<td colspan=\"2\">have a pH &lt; 7<\/td>\n<td>have a pH &gt; 7<\/td>\n<\/tr>\n<tr>\n<td colspan=\"2\">Common example: lemons, oranges, vinegar, urine<\/td>\n<td>Common examples: soap, toothpaste, bleach, cleaning agents, limewater<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p>Acids and bases in aqueous solutions will conduct electricity because they contain dissolved ions. Therefore, acids and bases are <i>electrolytes<\/i>. Strong acids and bases will be strong <strong>electrolytes<\/strong>. Weak acids and bases will be weak electrolytes. This affects the amount of conductivity.<\/p>\n<h2>The Arrhenius Definition of Acids and Bases<\/h2>\n<p id=\"ball-ch12_s01_p01\" class=\"para editable block\">Historically, the first chemical definition of an acid and a base was put forward by Svante Arrhenius, a Swedish chemist, in 1884. An <span class=\"margin_term\"><a class=\"glossterm\">Arrhenius acid<\/a><\/span>\u00a0is a compound that increases the H<sup class=\"superscript\">+<\/sup> ion concentration in aqueous solution. The H<sup class=\"superscript\">+<\/sup> ion is just a bare proton, and it is rather clear that bare protons are not floating around in an aqueous solution. Instead, chemistry has defined the <span class=\"margin_term\"><a class=\"glossterm\">hydronium ion<\/a><\/span>\u00a0(H<sub class=\"subscript\">3<\/sub>O<sup class=\"superscript\">+<\/sup>) as the actual chemical species that represents an H<sup class=\"superscript\">+<\/sup> ion. H<sup class=\"superscript\">+<\/sup> ions and H<sub class=\"subscript\">3<\/sub>O<sup class=\"superscript\">+<\/sup> ions are often considered interchangeable when writing chemical equations (although a properly balanced chemical equation should also include the additional H<sub class=\"subscript\">2<\/sub>O). This process is represented\u00a0in a chemical equation by adding H<sub>2<\/sub>O to the reactants side.<\/p>\n<p style=\"text-align: center\">[latex]\\text{HCl}\\left(aq\\right)+{\\text{H}}_{2}\\text{O}\\left(l\\right)\\longrightarrow {\\text{H}}^{\\text{+}}\\left(aq\\right)+{\\text{Cl}}^{-}\\left(aq\\right)[\/latex]<\/p>\n<p>In this reaction, hydrochloric acid (<span id=\"MathJax-Element-7-Frame\" class=\"MathJax\" role=\"presentation\"><span id=\"MathJax-Span-70\" class=\"math\"><span id=\"MathJax-Span-71\" class=\"mrow\"><span id=\"MathJax-Span-72\" class=\"mi\">H<\/span><span id=\"MathJax-Span-73\" class=\"mi\">C<\/span><span id=\"MathJax-Span-74\" class=\"mi\">l<\/span><\/span><\/span><\/span>) dissociates into hydrogen (<span id=\"MathJax-Element-8-Frame\" class=\"MathJax\" role=\"presentation\"><span id=\"MathJax-Span-75\" class=\"math\"><span id=\"MathJax-Span-76\" class=\"mrow\"><span id=\"MathJax-Span-77\" class=\"msubsup\"><span id=\"MathJax-Span-78\" class=\"mi\">H<\/span><span id=\"MathJax-Span-79\" class=\"mo\">+<\/span><\/span><\/span><\/span><\/span>) and chlorine (<span id=\"MathJax-Element-9-Frame\" class=\"MathJax\" role=\"presentation\"><span id=\"MathJax-Span-80\" class=\"math\"><span id=\"MathJax-Span-81\" class=\"mrow\"><span id=\"MathJax-Span-82\" class=\"mi\">C<\/span><span id=\"MathJax-Span-83\" class=\"msubsup\"><span id=\"MathJax-Span-84\" class=\"mi\">l<\/span><sup><span id=\"MathJax-Span-85\" class=\"mo\">\u2212<\/span><\/sup><\/span><\/span><\/span><\/span>) ions when dissolved in water, thereby releasing H<sup>+<\/sup> ions into solution. Formation of the hydronium ion equation:<\/p>\n<p style=\"text-align: center\">[latex]\\text{HCl}\\left(aq\\right)+{\\text{H}}_{2}\\text{O}\\left(l\\right)\\longrightarrow \\text{H}_{3}\\text{O}^{\\text{+}}\\left(aq\\right)+{\\text{Cl}}^{-}\\left(aq\\right)[\/latex]<\/p>\n<p class=\"para editable block\">Classic Arrhenius acids can be considered ionic compounds in which H<sup class=\"superscript\">+<\/sup> is the cation. Table 2 lists some Arrhenius acids and their names.<\/p>\n<div id=\"ball-ch12_s01_t01\" class=\"table block\">\n<table style=\"border-spacing: 0px\" cellpadding=\"0\">\n<thead>\n<tr style=\"height: 15px\">\n<th style=\"height: 15px;width: 312.483px\">Table 2 Some Arrhenius Acids<\/th>\n<th style=\"height: 15px;width: 154.983px\"><\/th>\n<\/tr>\n<tr style=\"height: 15px\">\n<th style=\"height: 15px;width: 312.483px\">Formula<\/th>\n<th style=\"height: 15px;width: 154.983px\">Name<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr style=\"height: 19px\">\n<td style=\"height: 19px;width: 312.483px\">HC<sub class=\"subscript\">2<\/sub>H<sub class=\"subscript\">3<\/sub>O<sub class=\"subscript\">2<\/sub> (also written CH<sub class=\"subscript\">3<\/sub>COOH)<\/td>\n<td style=\"height: 19px;width: 154.983px\">acetic acid<\/td>\n<\/tr>\n<tr style=\"height: 19px\">\n<td style=\"height: 19px;width: 312.483px\">HClO<sub class=\"subscript\">3<\/sub><\/td>\n<td style=\"height: 19px;width: 154.983px\">chloric acid<\/td>\n<\/tr>\n<tr style=\"height: 15px\">\n<td style=\"height: 15px;width: 312.483px\">HCl<\/td>\n<td style=\"height: 15px;width: 154.983px\">hydrochloric acid<\/td>\n<\/tr>\n<tr style=\"height: 15px\">\n<td style=\"height: 15px;width: 312.483px\">HBr<\/td>\n<td style=\"height: 15px;width: 154.983px\">hydrobromic acid<\/td>\n<\/tr>\n<tr style=\"height: 15px\">\n<td style=\"height: 15px;width: 312.483px\">HI<\/td>\n<td style=\"height: 15px;width: 154.983px\">hydriodic acid<\/td>\n<\/tr>\n<tr style=\"height: 15px\">\n<td style=\"height: 15px;width: 312.483px\">HF<\/td>\n<td style=\"height: 15px;width: 154.983px\">hydrofluoric acid<\/td>\n<\/tr>\n<tr style=\"height: 19px\">\n<td style=\"height: 19px;width: 312.483px\">HNO<sub class=\"subscript\">3<\/sub><\/td>\n<td style=\"height: 19px;width: 154.983px\">nitric acid<\/td>\n<\/tr>\n<tr style=\"height: 19px\">\n<td style=\"height: 19px;width: 312.483px\">H<sub class=\"subscript\">2<\/sub>C<sub class=\"subscript\">2<\/sub>O<sub class=\"subscript\">4<\/sub><\/td>\n<td style=\"height: 19px;width: 154.983px\">oxalic acid<\/td>\n<\/tr>\n<tr style=\"height: 19px\">\n<td style=\"height: 19px;width: 312.483px\">HClO<sub class=\"subscript\">4<\/sub><\/td>\n<td style=\"height: 19px;width: 154.983px\">perchloric acid<\/td>\n<\/tr>\n<tr style=\"height: 19px\">\n<td style=\"height: 19px;width: 312.483px\">H<sub class=\"subscript\">3<\/sub>PO<sub class=\"subscript\">4<\/sub><\/td>\n<td style=\"height: 19px;width: 154.983px\">phosphoric acid<\/td>\n<\/tr>\n<tr style=\"height: 19px\">\n<td style=\"height: 19px;width: 312.483px\">H<sub class=\"subscript\">2<\/sub>SO<sub class=\"subscript\">4<\/sub><\/td>\n<td style=\"height: 19px;width: 154.983px\">sulfuric acid<\/td>\n<\/tr>\n<tr style=\"height: 19px\">\n<td style=\"height: 19px;width: 312.483px\">H<sub class=\"subscript\">2<\/sub>SO<sub class=\"subscript\">3<\/sub><\/td>\n<td style=\"height: 19px;width: 154.983px\">sulfurous acid<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<\/div>\n<p id=\"ball-ch12_s01_p02\" class=\"para editable block\">An <span class=\"margin_term\"><a class=\"glossterm\">Arrhenius base<\/a><\/span>\u00a0is a compound that increases the OH<sup class=\"superscript\">\u2212<\/sup> ion concentration in aqueous solution. Ionic compounds of the OH<sup class=\"superscript\">\u2212<\/sup> ion are classic Arrhenius bases (Table 3).<\/p>\n<table cellpadding=\"0\">\n<thead>\n<tr>\n<th>Table 3 Some Arrhenius Bases<\/th>\n<th><\/th>\n<\/tr>\n<tr>\n<th>Formula<\/th>\n<th>Name<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td>NaOH<\/td>\n<td>sodium hydroxide<\/td>\n<\/tr>\n<tr>\n<td><sub>KOH<\/sub><\/td>\n<td>potassium hydroxide<\/td>\n<\/tr>\n<tr>\n<td>Mg(OH)<sub>2<\/sub><\/td>\n<td>magnesium hydroxide<\/td>\n<\/tr>\n<tr>\n<td>Ca(OH)<sub>2<\/sub><\/td>\n<td>calcium hydroxide<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p>All of the bases listed in the table are solids at room temperature. Upon dissolving in water, each dissociates into a metal cation and the hydroxide ion.<\/p>\n<p style=\"text-align: center\">[latex]\\text{NaOH}\\left(aq\\right)+{\\text{H}}_{2}\\text{O}\\left(l\\right)\\longrightarrow {\\text{Na}}^{\\text{+}}\\left(aq\\right)+{\\text{OH}}^{-}\\left(aq\\right)[\/latex]<\/p>\n<h2>Nomenclature of Acids and Bases<\/h2>\n<p id=\"ball-ch03_s05_p02\" class=\"para editable block\">Acids have their own nomenclature system based off of the type of acid, a binary acid or oxoacid.<\/p>\n<h3 class=\"para editable block\">Binary Acids<\/h3>\n<p class=\"para editable block\">If an acid is composed of only hydrogen and one other element, the name is <em class=\"emphasis\">hydro-<\/em> +\u00a0the stem of the other element +\u00a0<em class=\"emphasis\">-ic acid<\/em>. For example, the compound HCl(aq) is hydrochloric acid, while H<sub class=\"subscript\">2<\/sub>S(aq) is hydrosulfuric acid. (If these acids were not dissolved in water, the compounds would be called hydrogen chloride and hydrogen sulfide, respectively. Both of these substances are well known as molecular compounds; when dissolved in water, however, they are treated as acids.)<\/p>\n<table cellpadding=\"0\">\n<thead>\n<tr>\n<th>Table 4. Names of Binary Acids<\/th>\n<th><\/th>\n<\/tr>\n<tr>\n<th>Formula<\/th>\n<th>Name<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td>HCl<\/td>\n<td>hydrochloric acid<\/td>\n<\/tr>\n<tr>\n<td>HBr<\/td>\n<td>hydrobromic acid<\/td>\n<\/tr>\n<tr>\n<td>HI<\/td>\n<td>hydriodic acid<\/td>\n<\/tr>\n<tr>\n<td>HF<\/td>\n<td>hydrofluoric acid<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<h3 class=\"para editable block\">Oxoacids<\/h3>\n<p id=\"ball-ch03_s05_p03\" class=\"para editable block\">If a compound is composed of hydrogen ions and a polyatomic anion, then the name of the acid is derived from the stem of the polyatomic ion\u2019s name (Figure 1). Typically, if the anion name ends in -ate, the name of the acid is the stem of the anion name plus <em class=\"emphasis\">-ic acid<\/em>; if the related anion\u2019s name ends in -ite, the name of the corresponding acid is the stem of the anion name plus <em class=\"emphasis\">-ous acid<\/em>. Table 4 lists the formulas and names of a variety of acids that you should be familiar with. You should recognize most of the anions in the formulas of the acids.<\/p>\n<div id=\"attachment_1580\" style=\"width: 651px\" class=\"wp-caption aligncenter\"><img loading=\"lazy\" decoding=\"async\" aria-describedby=\"caption-attachment-1580\" class=\"wp-image-1580 size-full\" src=\"https:\/\/s3-us-west-2.amazonaws.com\/courses-images\/wp-content\/uploads\/sites\/2835\/2017\/12\/24023504\/Oxoacids.jpg\" alt=\"Figure 1. Naming Oxoacids\" width=\"641\" height=\"300\" \/><\/p>\n<p id=\"caption-attachment-1580\" class=\"wp-caption-text\">Figure 1. Naming Oxoacids<\/p>\n<\/div>\n<\/div>\n<table cellpadding=\"0\">\n<thead>\n<tr>\n<th>Table 5. Names of Oxoacids<\/th>\n<th><\/th>\n<\/tr>\n<tr>\n<th>Formula<\/th>\n<th>Name<\/th>\n<\/tr>\n<\/thead>\n<tbody>\n<tr>\n<td>HNO<sub>2<\/sub><\/td>\n<td>nitrous acid<\/td>\n<\/tr>\n<tr>\n<td>HNO<sub class=\"subscript\">3<\/sub><\/td>\n<td>nitric acid<\/td>\n<\/tr>\n<tr>\n<td>H<sub class=\"subscript\">2<\/sub>CO<sub class=\"subscript\">3<\/sub><\/td>\n<td>carbonic acid<\/td>\n<\/tr>\n<tr>\n<td>HNO<sub>2<\/sub><\/td>\n<td>nitrous acid<\/td>\n<\/tr>\n<tr>\n<td>HNO<sub class=\"subscript\">3<\/sub><\/td>\n<td>nitric acid<\/td>\n<\/tr>\n<tr>\n<td>HClO<\/td>\n<td>hypochloric acid<\/td>\n<\/tr>\n<tr>\n<td>HClO<sub>2<\/sub><\/td>\n<td>chlorous acid<\/td>\n<\/tr>\n<tr>\n<td>HClO<sub>3<\/sub><\/td>\n<td>chloric acid<\/td>\n<\/tr>\n<tr>\n<td>HClO<sub class=\"subscript\">4<\/sub><\/td>\n<td>perchloric acid<\/td>\n<\/tr>\n<tr>\n<td>H<sub class=\"subscript\">3<\/sub>PO<sub class=\"subscript\">4<\/sub><\/td>\n<td>phosphoric acid<\/td>\n<\/tr>\n<tr>\n<td>H<sub class=\"subscript\">2<\/sub>SO<sub class=\"subscript\">4<\/sub><\/td>\n<td>sulfuric acid<\/td>\n<\/tr>\n<tr>\n<td>H<sub class=\"subscript\">2<\/sub>SO<sub class=\"subscript\">3<\/sub><\/td>\n<td>sulfurous acid<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<p>Bases are named using the same nomenclature rules as ionic compounds.<\/p>\n<div id=\"ball-ch12_s01\" class=\"section\" lang=\"en\">\n<div id=\"ball-ch12_s01_n04\" class=\"key_takeaways editable block\">\n<div class=\"bcc-box bcc-success\">\n<h3>Key Takeaways<\/h3>\n<ul id=\"ball-ch12_s01_l06\" class=\"itemizedlist\">\n<li>An Arrhenius acid is a compound that increases the H<sup class=\"superscript\">+<\/sup> ion concentration in aqueous solution.<\/li>\n<li>An Arrhenius base is a compound that increases the OH<sup class=\"superscript\">\u2212<\/sup> ion concentration in aqueous solution.<\/li>\n<li>Acids are an important class of compounds containing hydrogen and having special nomenclature rules. Binary acids are named using the prefix <em>hydro-<\/em>, changing the \u2013<em>ide<\/em> suffix to \u2013<em>ic<\/em>, and adding \u201cacid;\u201d HCl is hydrochloric acid. Oxyacids are named by changing the ending of the anion to \u2013<em>ic<\/em>, and adding \u201cacid;\u201d H<sub>2<\/sub>CO<sub>3<\/sub> is carbonic acid.<\/li>\n<\/ul>\n<\/div>\n<div class=\"bcc-box bcc-info\">\n<h3>Exercises<\/h3>\n<div id=\"ball-ch12_s01_qs01\" class=\"qandaset block\">\n<ol id=\"ball-ch12_s01_qs01_qd01\" class=\"qandadiv\">\n<li id=\"ball-ch12_s01_qs01_qd01_qa01\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"ball-ch12_s01_qs01_p01\" class=\"para\">Define <em class=\"emphasis\">Arrhenius acid<\/em>.<\/p>\n<\/div>\n<\/li>\n<li id=\"ball-ch12_s01_qs01_qd01_qa02\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"ball-ch12_s01_qs01_p03\" class=\"para\">Define <em class=\"emphasis\">Arrhenius base<\/em>.<\/p>\n<\/div>\n<\/li>\n<li id=\"ball-ch12_s01_qs01_qd01_qa03\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"ball-ch12_s01_qs01_p05\" class=\"para\">What are some general properties of Arrhenius acids?<\/p>\n<\/div>\n<\/li>\n<li id=\"ball-ch12_s01_qs01_qd01_qa04\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"ball-ch12_s01_qs01_p07\" class=\"para\">What are some general properties of Arrhenius bases?<\/p>\n<\/div>\n<\/li>\n<li id=\"ball-ch12_s01_qs01_qd01_qa05\" class=\"qandaentry\">\n<div class=\"question\">\n<p id=\"ball-ch12_s01_qs01_p09\" class=\"para\">Identify each substance as an Arrhenius acid, an Arrhenius base, or neither.<\/p>\n<\/div>\n<\/li>\n<\/ol>\n<p style=\"padding-left: 60px\">a) \u00a0NaOH<\/p>\n<p style=\"padding-left: 60px\">b) \u00a0C<sub class=\"subscript\">2<\/sub>H<sub class=\"subscript\">5<\/sub>OH<\/p>\n<p style=\"padding-left: 60px\">c) \u00a0H<sub class=\"subscript\">3<\/sub>PO<sub class=\"subscript\">4<\/sub><\/p>\n<div class=\"question\">\n<p id=\"ball-ch12_s01_qs01_p10\" class=\"para\" style=\"padding-left: 30px\">6. \u00a0Identify each substance as an Arrhenius acid, an Arrhenius base, or neither.<\/p>\n<p style=\"padding-left: 60px\">a) \u00a0C<sub class=\"subscript\">6<\/sub>H<sub class=\"subscript\">12<\/sub>O<sub class=\"subscript\">6<\/sub><\/p>\n<p style=\"padding-left: 60px\">b) \u00a0HNO<sub class=\"subscript\">2<\/sub><\/p>\n<p id=\"ball-ch03_s05_qs01_p1\" class=\"para\" style=\"padding-left: 30px\">7. Give the formula for each acid.<\/p>\n<div id=\"ball-ch03_s05_qs01\" class=\"qandaset block\">\n<p style=\"padding-left: 60px\">a) \u00a0perchloric acid<\/p>\n<p style=\"padding-left: 60px\">b) \u00a0hydriodic acid<\/p>\n<div class=\"question\">\n<p id=\"ball-ch03_s05_qs01_p2\" class=\"para\" style=\"padding-left: 30px\">8. Give the formula for each acid.<\/p>\n<p style=\"padding-left: 60px\">a) \u00a0hydrosulfuric acid<\/p>\n<p style=\"padding-left: 60px\">b) \u00a0phosphorous acid<\/p>\n<\/div>\n<div class=\"question\">\n<p id=\"ball-ch03_s05_qs01_p3\" class=\"para\" style=\"padding-left: 30px\">9. \u00a0Name each acid.<\/p>\n<p style=\"padding-left: 60px\">a) \u00a0HF(aq)<\/p>\n<p style=\"padding-left: 60px\">b) \u00a0HNO<sub class=\"subscript\">3<\/sub>(aq)<\/p>\n<p style=\"padding-left: 60px\">c) \u00a0H<sub class=\"subscript\">2<\/sub>C<sub class=\"subscript\">2<\/sub>O<sub class=\"subscript\">4<\/sub>(aq)<\/p>\n<\/div>\n<div class=\"question\">\n<p id=\"ball-ch03_s05_qs01_p4\" class=\"para\" style=\"padding-left: 30px\">10. \u00a0Name each acid.<\/p>\n<p style=\"padding-left: 60px\">a) \u00a0H<sub class=\"subscript\">2<\/sub>SO<sub class=\"subscript\">4<\/sub>(aq)<\/p>\n<p style=\"padding-left: 60px\">b) \u00a0H<sub class=\"subscript\">3<\/sub>PO<sub class=\"subscript\">4<\/sub>(aq)<\/p>\n<p style=\"padding-left: 60px\">c) \u00a0HCl(aq)<\/p>\n<\/div>\n<div class=\"question\">\n<p id=\"ball-ch03_s05_qs01_p5\" class=\"para\" style=\"padding-left: 30px\">11. \u00a0Name an acid found in food.<\/p>\n<\/div>\n<div class=\"question\">\n<p id=\"ball-ch03_s05_qs01_p7\" class=\"para\" style=\"padding-left: 30px\">12.\u00a0 Name some properties that acids have in common.<\/p>\n<\/div>\n<\/div>\n<div class=\"qa-wrapper\" style=\"display: block\"><span class=\"show-answer collapsed\" style=\"cursor: pointer\" data-target=\"q742610\">Show Answers to Select Problems<\/span><\/p>\n<div id=\"q742610\" class=\"hidden-answer\" style=\"display: none\">\n<p>1.\u00a0 a compound that increases the H<sup class=\"superscript\">+<\/sup> concentration in water<\/p>\n<p>3. sour taste, react with metals, and turn litmus red<\/p>\n<p>5. a) \u00a0Arrhenius base, b) \u00a0neither, c) \u00a0Arrhenius acid<\/p>\n<p>7. a) \u00a0HClO<sub class=\"subscript\">4<\/sub>(aq), b) \u00a0HI(aq)<\/p>\n<p>9. a) \u00a0hydrofluoric acid, b) \u00a0nitric acid, c) \u00a0oxalic acid<\/p>\n<p>11. oxalic acid (answers will vary)<\/p>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n<p>&nbsp;<\/p>\n<\/div>\n<\/div>\n<\/div>\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-603\">\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>Acids and Bases: A Brief Review. <strong>Authored by<\/strong>: Brown, LeMay, Busten, Murphy, and Woodward. <strong>Provided by<\/strong>: LibreTexts. <strong>Located at<\/strong>: <a target=\"_blank\" href=\"https:\/\/chem.libretexts.org\/Textbook_Maps\/General_Chemistry\/Map%3A_Chemistry_-_The_Central_Science_(Brown_et_al.)\/16%3A_Acid%E2%80%93Base_Equilibria\/16.01%3A_Acids_and_Bases%3A_A_Brief_Review\">https:\/\/chem.libretexts.org\/Textbook_Maps\/General_Chemistry\/Map%3A_Chemistry_-_The_Central_Science_(Brown_et_al.)\/16%3A_Acid%E2%80%93Base_Equilibria\/16.01%3A_Acids_and_Bases%3A_A_Brief_Review<\/a>. <strong>Project<\/strong>: Chemistry: The Central Science. <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><\/li><li>Naming Acids and Bases . <strong>Authored by<\/strong>: Averill and Eldredge. <strong>Provided by<\/strong>: LibreTexts. <strong>Located at<\/strong>: <a target=\"_blank\" href=\"https:\/\/chem.libretexts.org\/Textbook_Maps\/General_Chemistry\/Map%3A_Chemistry_(Averill_and_Eldredge)\/03%3A_Chemical_Reactions\/3.6b%3A_Naming_Acids_and_Bases\">https:\/\/chem.libretexts.org\/Textbook_Maps\/General_Chemistry\/Map%3A_Chemistry_(Averill_and_Eldredge)\/03%3A_Chemical_Reactions\/3.6b%3A_Naming_Acids_and_Bases<\/a>. <strong>Project<\/strong>: 3A_Chemistry. <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><\/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":1,"template":"","meta":{"_candela_citation":"[{\"type\":\"cc\",\"description\":\"Introductory Chemistry- 1st Canadian Edition \",\"author\":\"Jessie A. Key and David W. 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