{"id":7630,"date":"2021-06-08T21:57:06","date_gmt":"2021-06-08T21:57:06","guid":{"rendered":"https:\/\/opentextbc.ca\/introductorychemistry\/chapter\/arrhenius-acids-and-bases\/"},"modified":"2021-10-06T21:43:05","modified_gmt":"2021-10-06T21:43:05","slug":"arrhenius-acids-and-bases","status":"publish","type":"chapter","link":"https:\/\/opentextbc.ca\/introductorychemistry\/chapter\/arrhenius-acids-and-bases\/","title":{"raw":"Arrhenius Acids and Bases","rendered":"Arrhenius Acids and Bases"},"content":{"raw":"
\r\n

Learning Objectives<\/p>\r\n\r\n<\/header>\r\n

\r\n
    \r\n \t
  1. Identify an Arrhenius acid and an Arrhenius base.<\/li>\r\n \t
  2. Write the chemical reaction between an Arrhenius acid and an Arrhenius base.<\/li>\r\n<\/ol>\r\n<\/div>\r\n<\/div>\r\nHistorically, the first chemical definition of an acid and a base was put forward by Svante Arrhenius, a Swedish chemist, in 1884. An Arrhenius acid<\/strong>\u00a0is a compound that increases the H+<\/sup> ion concentration in aqueous solution. The H+<\/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 hydronium ion<\/strong>\u00a0(H3<\/sub>O+<\/sup>) as the actual chemical species that represents an H+<\/sup> ion. H+<\/sup> ions and H3<\/sub>O+<\/sup> ions are often considered interchangeable when writing chemical equations (although a properly balanced chemical equation should also include the additional H2<\/sub>O). Classic Arrhenius acids can be considered ionic compounds in which H+<\/sup> is the cation. Table 12.2 \"Some Arrhenius Acids\" lists some Arrhenius acids and their names.\r\n\r\n\r\n\r\n\r\n\r\n\r\n\r\n\r\n\r\n\r\n\r\n\r\n\r\n\r\n\r\n
    Table 12.2<\/span> Some Arrhenius Acids<\/caption>\r\n
    Formula<\/th>\r\nName<\/th>\r\n<\/tr>\r\n<\/thead>\r\n
    HC2<\/sub>H3<\/sub>O2<\/sub> (also written CH3<\/sub>COOH)<\/td>\r\nacetic acid<\/td>\r\n<\/tr>\r\n
    HClO3<\/sub><\/td>\r\nchloric acid<\/td>\r\n<\/tr>\r\n
    HCl<\/td>\r\nhydrochloric acid<\/td>\r\n<\/tr>\r\n
    HBr<\/td>\r\nhydrobromic acid<\/td>\r\n<\/tr>\r\n
    HI<\/td>\r\nhydriodic acid<\/td>\r\n<\/tr>\r\n
    HF<\/td>\r\nhydrofluoric acid<\/td>\r\n<\/tr>\r\n
    HNO3<\/sub><\/td>\r\nnitric acid<\/td>\r\n<\/tr>\r\n
    H2<\/sub>C2<\/sub>O4<\/sub><\/td>\r\noxalic acid<\/td>\r\n<\/tr>\r\n
    HClO4<\/sub><\/td>\r\nperchloric acid<\/td>\r\n<\/tr>\r\n
    H3<\/sub>PO4<\/sub><\/td>\r\nphosphoric acid<\/td>\r\n<\/tr>\r\n
    H2<\/sub>SO4<\/sub><\/td>\r\nsulfuric acid<\/td>\r\n<\/tr>\r\n
    H2<\/sub>SO3<\/sub><\/td>\r\nsulfurous acid<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\nAn Arrhenius base<\/strong>\u00a0is a compound that increases the OH\u2212<\/sup> ion concentration in aqueous solution. Ionic compounds of the OH\u2212<\/sup> ion are classic Arrhenius bases.\r\n
    \r\n

    Example 12.7<\/p>\r\n\r\n<\/header>\r\n

    \r\n\r\nIdentify each compound as an Arrhenius acid, an Arrhenius base, or neither.\r\n
      \r\n \t
    1. HNO3<\/sub><\/li>\r\n \t
    2. CH3<\/sub>OH<\/li>\r\n \t
    3. Mg(OH)2<\/sub><\/li>\r\n<\/ol>\r\nSolution<\/em>\r\n
        \r\n \t
      1. This compound is an ionic compound between H+<\/sup> ions and NO3<\/sub>\u2212<\/sup> ions, so it is an Arrhenius acid.<\/li>\r\n \t
      2. Although this formula has an OH in it, we do not recognize the remaining part of the molecule as a cation. It is neither an acid nor a base. (In fact, it is the formula for methanol, an organic compound.)<\/li>\r\n \t
      3. This formula also has an OH in it, but this time we recognize that the magnesium is present as Mg2+<\/sup> cations. As such, this is an ionic compound of the OH\u2212<\/sup> ion and is an Arrhenius base.<\/li>\r\n<\/ol>\r\nTest Yourself<\/em>\r\nIdentify each compound as an Arrhenius acid, an Arrhenius base, or neither.\r\n
          \r\n \t
        1. KOH<\/li>\r\n \t
        2. H2<\/sub>SO4<\/sub><\/li>\r\n \t
        3. C2<\/sub>H6<\/sub><\/li>\r\n<\/ol>\r\nAnswer<\/em>\r\n
            \r\n \t
          1. Arrhenius base<\/li>\r\n \t
          2. Arrhenius acid<\/li>\r\n \t
          3. neither<\/li>\r\n<\/ol>\r\n<\/div>\r\n<\/div>\r\nAcids have some properties in common. They turn litmus, a plant extract, red. They react with some metals to give off H2<\/sub> gas. They react with carbonate and hydrogen carbonate salts to give off CO2<\/sub> gas. Acids that are ingested typically have a sour, sharp taste. (The name acid<\/em> comes from the Latin word acidus<\/em>, meaning \u201csour.\u201d) Bases also have some properties in common. They are slippery to the touch, turn litmus blue, and have a bitter flavour if ingested.\r\n\r\nAcids and bases have another property: they react with each other to make water and an ionic compound called a salt. A salt<\/strong>, in chemistry, is any ionic compound made by combining an acid with a base. A reaction between an acid and a base is called a neutralization reaction<\/strong>\u00a0and can be represented as follows:\r\n

            acid +\u00a0base \u2192\u00a0H2<\/sub>O +\u00a0salt<\/p>\r\nThe stoichiometry of the balanced chemical equation depends on the number of H+<\/sup> ions in the acid and the number of OH\u2212<\/sup> ions in the base.\r\n

            \r\n

            Example 12.8<\/p>\r\n\r\n<\/header>\r\n

            \r\n\r\nWrite the balanced chemical equation for the neutralization reaction between H2<\/sub>SO4<\/sub> and KOH. What is the name of the salt that is formed?\r\n\r\nSolution<\/em>\r\nThe general reaction is as follows:\r\n

            H2<\/sub>SO4<\/sub> + KOH \u2192 H2<\/sub>O + salt<\/p>\r\nBecause the acid has two H+<\/sup> ions in its formula, we need two OH\u2212<\/sup> ions to react with it, making two H2<\/sub>O molecules as product. The remaining ions, K+<\/sup> and SO4<\/sub>2\u2212<\/sup>, make the salt potassium sulfate (K2<\/sub>SO4<\/sub>). The balanced chemical reaction is as follows:\r\n

            H2<\/sub>SO4<\/sub> + 2KOH \u2192 2H2<\/sub>O + K2<\/sub>SO4<\/sub><\/p>\r\nTest Yourself<\/em>\r\nWrite the balanced chemical equation for the neutralization reaction between HCl and Mg(OH)2<\/sub>. What is the name of the salt that is formed?\r\n\r\nAnswer<\/em>\r\n2HCl + Mg(OH)2<\/sub> \u2192 2 H2<\/sub>O + MgCl2<\/sub>; magnesium chloride\r\n\r\n<\/div>\r\n<\/div>\r\n

            \r\n

            Key Takeaways<\/p>\r\n\r\n<\/header>\r\n

            \r\n
              \r\n \t
            • An Arrhenius acid is a compound that increases the H+<\/sup> ion concentration in aqueous solution.<\/li>\r\n \t
            • An Arrhenius base is a compound that increases the OH\u2212<\/sup> ion concentration in aqueous solution.<\/li>\r\n \t
            • The reaction between an Arrhenius acid and an Arrhenius base is called neutralization and results in the formation of water and a salt.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<\/div>\r\n
              \r\n

              Exercises<\/p>\r\n\r\n<\/header>\r\n

              \r\n

              Questions<\/h1>\r\n
                \r\n \t
              1. Define Arrhenius acid<\/em>.<\/li>\r\n \t
              2. Define Arrhenius base<\/em>.<\/li>\r\n \t
              3. What are some general properties of Arrhenius acids?<\/li>\r\n \t
              4. What are some general properties of Arrhenius bases?<\/li>\r\n \t
              5. Identify each substance as an Arrhenius acid, an Arrhenius base, or neither.\r\n
                  \r\n \t
                1. NaOH<\/li>\r\n \t
                2. C2<\/sub>H5<\/sub>OH<\/li>\r\n \t
                3. H3<\/sub>PO4<\/sub><\/li>\r\n<\/ol>\r\n<\/li>\r\n \t
                4. Identify each substance as an Arrhenius acid, an Arrhenius base, or neither.\r\n
                    \r\n \t
                  1. C6<\/sub>H12<\/sub>O6<\/sub><\/li>\r\n \t
                  2. HNO2<\/sub><\/li>\r\n \t
                  3. Ba(OH)2<\/sub><\/li>\r\n<\/ol>\r\n<\/li>\r\n \t
                  4. Write the balanced chemical equation for the neutralization reaction between KOH and H2<\/sub>C2<\/sub>O4<\/sub>. What is the salt?<\/li>\r\n \t
                  5. Write the balanced chemical equation for the neutralization reaction between Sr(OH)2<\/sub> and H3<\/sub>PO4<\/sub>. What is the salt?<\/li>\r\n \t
                  6. Write the balanced chemical equation for the neutralization reaction between HCl and Fe(OH)3<\/sub>. What is the salt?<\/li>\r\n \t
                  7. Write the balanced chemical equation for the neutralization reaction between H2<\/sub>SO4<\/sub> and Cr(OH)3<\/sub>. What is the salt?<\/li>\r\n \t
                  8. CaCl2<\/sub> would be the product of the reaction of what acid and what base?<\/li>\r\n \t
                  9. Zn(NO3<\/sub>)2<\/sub> would be product of the reaction of what acid and what base?<\/li>\r\n \t
                  10. BaSO4<\/sub> would be product of the reaction of what acid and what base?<\/li>\r\n \t
                  11. Na3<\/sub>PO4<\/sub> would be product of the reaction of what acid and what base?<\/li>\r\n<\/ol>\r\n

                    Answers<\/h1>\r\n
                      \r\n \t
                    1. A compound that increases the H+<\/sup> concentration in water.<\/li>\r\n<\/ol>\r\n
                        \r\n \t
                      1. Sour taste, react with metals, and turn litmus red<\/li>\r\n<\/ol>\r\n
                          \r\n \t
                        1. \r\n
                            \r\n \t
                          1. Arrhenius base<\/li>\r\n \t
                          2. neither<\/li>\r\n \t
                          3. Arrhenius acid<\/li>\r\n<\/ol>\r\n<\/li>\r\n<\/ol>\r\n
                              \r\n \t
                            1. 2KOH + H2<\/sub>C2<\/sub>O4<\/sub> \u2192 2H2<\/sub>O + K2<\/sub>C2<\/sub>O4<\/sub>; K2<\/sub>C2<\/sub>O4<\/sub><\/li>\r\n<\/ol>\r\n
                                \r\n \t
                              1. 3HCl + Fe(OH)3<\/sub> \u2192 3H2<\/sub>O + FeCl3<\/sub>; FeCl3<\/sub><\/li>\r\n<\/ol>\r\n
                                  \r\n \t
                                1. HCl and Ca(OH)2<\/sub><\/li>\r\n<\/ol>\r\n
                                    \r\n \t
                                  1. H2<\/sub>SO4<\/sub> and Ba(OH)2<\/sub><\/li>\r\n<\/ol>\r\n<\/div>\r\n<\/div>","rendered":"
                                    \n
                                    \n

                                    Learning Objectives<\/p>\n<\/header>\n

                                    \n
                                      \n
                                    1. Identify an Arrhenius acid and an Arrhenius base.<\/li>\n
                                    2. Write the chemical reaction between an Arrhenius acid and an Arrhenius base.<\/li>\n<\/ol>\n<\/div>\n<\/div>\n

                                      Historically, the first chemical definition of an acid and a base was put forward by Svante Arrhenius, a Swedish chemist, in 1884. An Arrhenius acid<\/strong>\u00a0is a compound that increases the H+<\/sup> ion concentration in aqueous solution. The H+<\/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 hydronium ion<\/strong>\u00a0(H3<\/sub>O+<\/sup>) as the actual chemical species that represents an H+<\/sup> ion. H+<\/sup> ions and H3<\/sub>O+<\/sup> ions are often considered interchangeable when writing chemical equations (although a properly balanced chemical equation should also include the additional H2<\/sub>O). Classic Arrhenius acids can be considered ionic compounds in which H+<\/sup> is the cation. Table 12.2 “Some Arrhenius Acids” lists some Arrhenius acids and their names.<\/p>\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n\n
                                      Table 12.2<\/span> Some Arrhenius Acids<\/caption>\n
                                      Formula<\/th>\nName<\/th>\n<\/tr>\n<\/thead>\n
                                      HC2<\/sub>H3<\/sub>O2<\/sub> (also written CH3<\/sub>COOH)<\/td>\nacetic acid<\/td>\n<\/tr>\n
                                      HClO3<\/sub><\/td>\nchloric acid<\/td>\n<\/tr>\n
                                      HCl<\/td>\nhydrochloric acid<\/td>\n<\/tr>\n
                                      HBr<\/td>\nhydrobromic acid<\/td>\n<\/tr>\n
                                      HI<\/td>\nhydriodic acid<\/td>\n<\/tr>\n
                                      HF<\/td>\nhydrofluoric acid<\/td>\n<\/tr>\n
                                      HNO3<\/sub><\/td>\nnitric acid<\/td>\n<\/tr>\n
                                      H2<\/sub>C2<\/sub>O4<\/sub><\/td>\noxalic acid<\/td>\n<\/tr>\n
                                      HClO4<\/sub><\/td>\nperchloric acid<\/td>\n<\/tr>\n
                                      H3<\/sub>PO4<\/sub><\/td>\nphosphoric acid<\/td>\n<\/tr>\n
                                      H2<\/sub>SO4<\/sub><\/td>\nsulfuric acid<\/td>\n<\/tr>\n
                                      H2<\/sub>SO3<\/sub><\/td>\nsulfurous acid<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n

                                      An Arrhenius base<\/strong>\u00a0is a compound that increases the OH\u2212<\/sup> ion concentration in aqueous solution. Ionic compounds of the OH\u2212<\/sup> ion are classic Arrhenius bases.<\/p>\n

                                      \n
                                      \n

                                      Example 12.7<\/p>\n<\/header>\n

                                      \n

                                      Identify each compound as an Arrhenius acid, an Arrhenius base, or neither.<\/p>\n

                                        \n
                                      1. HNO3<\/sub><\/li>\n
                                      2. CH3<\/sub>OH<\/li>\n
                                      3. Mg(OH)2<\/sub><\/li>\n<\/ol>\n

                                        Solution<\/em><\/p>\n

                                          \n
                                        1. This compound is an ionic compound between H+<\/sup> ions and NO3<\/sub>\u2212<\/sup> ions, so it is an Arrhenius acid.<\/li>\n
                                        2. Although this formula has an OH in it, we do not recognize the remaining part of the molecule as a cation. It is neither an acid nor a base. (In fact, it is the formula for methanol, an organic compound.)<\/li>\n
                                        3. This formula also has an OH in it, but this time we recognize that the magnesium is present as Mg2+<\/sup> cations. As such, this is an ionic compound of the OH\u2212<\/sup> ion and is an Arrhenius base.<\/li>\n<\/ol>\n

                                          Test Yourself<\/em>
                                          \nIdentify each compound as an Arrhenius acid, an Arrhenius base, or neither.<\/p>\n

                                            \n
                                          1. KOH<\/li>\n
                                          2. H2<\/sub>SO4<\/sub><\/li>\n
                                          3. C2<\/sub>H6<\/sub><\/li>\n<\/ol>\n

                                            Answer<\/em><\/p>\n

                                              \n
                                            1. Arrhenius base<\/li>\n
                                            2. Arrhenius acid<\/li>\n
                                            3. neither<\/li>\n<\/ol>\n<\/div>\n<\/div>\n

                                              Acids have some properties in common. They turn litmus, a plant extract, red. They react with some metals to give off H2<\/sub> gas. They react with carbonate and hydrogen carbonate salts to give off CO2<\/sub> gas. Acids that are ingested typically have a sour, sharp taste. (The name acid<\/em> comes from the Latin word acidus<\/em>, meaning \u201csour.\u201d) Bases also have some properties in common. They are slippery to the touch, turn litmus blue, and have a bitter flavour if ingested.<\/p>\n

                                              Acids and bases have another property: they react with each other to make water and an ionic compound called a salt. A salt<\/strong>, in chemistry, is any ionic compound made by combining an acid with a base. A reaction between an acid and a base is called a neutralization reaction<\/strong>\u00a0and can be represented as follows:<\/p>\n

                                              acid +\u00a0base \u2192\u00a0H2<\/sub>O +\u00a0salt<\/p>\n

                                              The stoichiometry of the balanced chemical equation depends on the number of H+<\/sup> ions in the acid and the number of OH\u2212<\/sup> ions in the base.<\/p>\n

                                              \n
                                              \n

                                              Example 12.8<\/p>\n<\/header>\n

                                              \n

                                              Write the balanced chemical equation for the neutralization reaction between H2<\/sub>SO4<\/sub> and KOH. What is the name of the salt that is formed?<\/p>\n

                                              Solution<\/em>
                                              \nThe general reaction is as follows:<\/p>\n

                                              H2<\/sub>SO4<\/sub> + KOH \u2192 H2<\/sub>O + salt<\/p>\n

                                              Because the acid has two H+<\/sup> ions in its formula, we need two OH\u2212<\/sup> ions to react with it, making two H2<\/sub>O molecules as product. The remaining ions, K+<\/sup> and SO4<\/sub>2\u2212<\/sup>, make the salt potassium sulfate (K2<\/sub>SO4<\/sub>). The balanced chemical reaction is as follows:<\/p>\n

                                              H2<\/sub>SO4<\/sub> + 2KOH \u2192 2H2<\/sub>O + K2<\/sub>SO4<\/sub><\/p>\n

                                              Test Yourself<\/em>
                                              \nWrite the balanced chemical equation for the neutralization reaction between HCl and Mg(OH)2<\/sub>. What is the name of the salt that is formed?<\/p>\n

                                              Answer<\/em>
                                              \n2HCl + Mg(OH)2<\/sub> \u2192 2 H2<\/sub>O + MgCl2<\/sub>; magnesium chloride<\/p>\n<\/div>\n<\/div>\n

                                              \n
                                              \n

                                              Key Takeaways<\/p>\n<\/header>\n

                                              \n
                                                \n
                                              • An Arrhenius acid is a compound that increases the H+<\/sup> ion concentration in aqueous solution.<\/li>\n
                                              • An Arrhenius base is a compound that increases the OH\u2212<\/sup> ion concentration in aqueous solution.<\/li>\n
                                              • The reaction between an Arrhenius acid and an Arrhenius base is called neutralization and results in the formation of water and a salt.<\/li>\n<\/ul>\n<\/div>\n<\/div>\n
                                                \n
                                                \n

                                                Exercises<\/p>\n<\/header>\n

                                                \n

                                                Questions<\/h1>\n
                                                  \n
                                                1. Define Arrhenius acid<\/em>.<\/li>\n
                                                2. Define Arrhenius base<\/em>.<\/li>\n
                                                3. What are some general properties of Arrhenius acids?<\/li>\n
                                                4. What are some general properties of Arrhenius bases?<\/li>\n
                                                5. Identify each substance as an Arrhenius acid, an Arrhenius base, or neither.\n
                                                    \n
                                                  1. NaOH<\/li>\n
                                                  2. C2<\/sub>H5<\/sub>OH<\/li>\n
                                                  3. H3<\/sub>PO4<\/sub><\/li>\n<\/ol>\n<\/li>\n
                                                  4. Identify each substance as an Arrhenius acid, an Arrhenius base, or neither.\n
                                                      \n
                                                    1. C6<\/sub>H12<\/sub>O6<\/sub><\/li>\n
                                                    2. HNO2<\/sub><\/li>\n
                                                    3. Ba(OH)2<\/sub><\/li>\n<\/ol>\n<\/li>\n
                                                    4. Write the balanced chemical equation for the neutralization reaction between KOH and H2<\/sub>C2<\/sub>O4<\/sub>. What is the salt?<\/li>\n
                                                    5. Write the balanced chemical equation for the neutralization reaction between Sr(OH)2<\/sub> and H3<\/sub>PO4<\/sub>. What is the salt?<\/li>\n
                                                    6. Write the balanced chemical equation for the neutralization reaction between HCl and Fe(OH)3<\/sub>. What is the salt?<\/li>\n
                                                    7. Write the balanced chemical equation for the neutralization reaction between H2<\/sub>SO4<\/sub> and Cr(OH)3<\/sub>. What is the salt?<\/li>\n
                                                    8. CaCl2<\/sub> would be the product of the reaction of what acid and what base?<\/li>\n
                                                    9. Zn(NO3<\/sub>)2<\/sub> would be product of the reaction of what acid and what base?<\/li>\n
                                                    10. BaSO4<\/sub> would be product of the reaction of what acid and what base?<\/li>\n
                                                    11. Na3<\/sub>PO4<\/sub> would be product of the reaction of what acid and what base?<\/li>\n<\/ol>\n

                                                      Answers<\/h1>\n
                                                        \n
                                                      1. A compound that increases the H+<\/sup> concentration in water.<\/li>\n<\/ol>\n
                                                          \n
                                                        1. Sour taste, react with metals, and turn litmus red<\/li>\n<\/ol>\n
                                                            \n
                                                          1. \n
                                                              \n
                                                            1. Arrhenius base<\/li>\n
                                                            2. neither<\/li>\n
                                                            3. Arrhenius acid<\/li>\n<\/ol>\n<\/li>\n<\/ol>\n
                                                                \n
                                                              1. 2KOH + H2<\/sub>C2<\/sub>O4<\/sub> \u2192 2H2<\/sub>O + K2<\/sub>C2<\/sub>O4<\/sub>; K2<\/sub>C2<\/sub>O4<\/sub><\/li>\n<\/ol>\n
                                                                  \n
                                                                1. 3HCl + Fe(OH)3<\/sub> \u2192 3H2<\/sub>O + FeCl3<\/sub>; FeCl3<\/sub><\/li>\n<\/ol>\n
                                                                    \n
                                                                  1. HCl and Ca(OH)2<\/sub><\/li>\n<\/ol>\n
                                                                      \n
                                                                    1. H2<\/sub>SO4<\/sub> and Ba(OH)2<\/sub><\/li>\n<\/ol>\n<\/div>\n<\/div>\n","protected":false},"author":90,"menu_order":4,"template":"","meta":{"pb_show_title":"on","pb_short_title":"","pb_subtitle":"","pb_authors":[],"pb_section_license":""},"chapter-type":[],"contributor":[],"license":[],"class_list":["post-7630","chapter","type-chapter","status-publish","hentry"],"part":7615,"_links":{"self":[{"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/pressbooks\/v2\/chapters\/7630","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/pressbooks\/v2\/chapters"}],"about":[{"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/wp\/v2\/types\/chapter"}],"author":[{"embeddable":true,"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/wp\/v2\/users\/90"}],"version-history":[{"count":6,"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/pressbooks\/v2\/chapters\/7630\/revisions"}],"predecessor-version":[{"id":8923,"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/pressbooks\/v2\/chapters\/7630\/revisions\/8923"}],"part":[{"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/pressbooks\/v2\/parts\/7615"}],"metadata":[{"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/pressbooks\/v2\/chapters\/7630\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/wp\/v2\/media?parent=7630"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/pressbooks\/v2\/chapter-type?post=7630"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/wp\/v2\/contributor?post=7630"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/wp\/v2\/license?post=7630"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}