{"id":7637,"date":"2021-06-08T21:57:08","date_gmt":"2021-06-08T21:57:08","guid":{"rendered":"https:\/\/opentextbc.ca\/introductorychemistry\/chapter\/end-of-chapter-12-material\/"},"modified":"2021-06-24T22:50:44","modified_gmt":"2021-06-24T22:50:44","slug":"end-of-chapter-12-material","status":"publish","type":"chapter","link":"https:\/\/opentextbc.ca\/introductorychemistry\/chapter\/end-of-chapter-12-material\/","title":{"raw":"End-of-Chapter Material","rendered":"End-of-Chapter Material"},"content":{"raw":"
\r\n

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

\r\n
    \r\n \t
  1. Write the balanced chemical equation between Zn metal and HCl(aq). The other product is ZnCl2<\/sub>.<\/li>\r\n \t
  2. Write the neutralization reaction in which ZnCl2<\/sub>, also found in Exercise 1, is the salt product.<\/li>\r\n \t
  3. Why isn\u2019t an oxide compound like CaO considered a salt? (Hint: what acid-base combination would be needed to make it if it were a salt?)<\/li>\r\n \t
  4. Metal oxides are considered basic because they react with H2<\/sub>O to form OH compounds. Write the chemical equation for a reaction that forms a base when CaO is combined with H2<\/sub>O.<\/li>\r\n \t
  5. Write the balanced chemical equation between aluminum hydroxide and sulfuric acid.<\/li>\r\n \t
  6. Write the balanced chemical equation between phosphoric acid and barium hydroxide.<\/li>\r\n \t
  7. Write the equation for the chemical reaction that occurs when caffeine (C8<\/sub>H10<\/sub>N4<\/sub>O2<\/sub>) acts as a Br\u00f8nsted-Lowry base.<\/li>\r\n \t
  8. Citric acid (C6<\/sub>H8<\/sub>O7<\/sub>) is the acid found in citrus fruits. It can lose a maximum of three H+<\/sup> ions in the presence of a base. Write the chemical equations for citric acid acting stepwise as a Br\u00f8nsted-Lowry acid.<\/li>\r\n \t
  9. Can an amphiprotic substance be a strong acid and a strong base at the same time? Explain your answer.<\/li>\r\n \t
  10. Can an amphiprotic substance be a weak acid and a weak base at the same time? If so, explain why and give an example.<\/li>\r\n \t
  11. Under what conditions will the equivalence point of a titration be slightly acidic?<\/li>\r\n \t
  12. Under what conditions will the equivalence point of a titration be slightly basic?<\/li>\r\n \t
  13. Write the chemical equation for the autoionization of NH3<\/sub>.<\/li>\r\n \t
  14. Write the chemical equation for the autoionization of HF.<\/li>\r\n \t
  15. What is the pOH range for an acidic solution?<\/li>\r\n \t
  16. What is the pOH range for a basic solution?<\/li>\r\n \t
  17. The concentration of commercial HCl is about 12 M. What is its pH and pOH?<\/li>\r\n \t
  18. The concentration of concentrated H2<\/sub>SO4<\/sub> is about 18 M. Assuming only one H+<\/sup> comes off the H2<\/sub>SO4<\/sub> molecule, what is its pH and pOH? What would the pH and pOH be if the second H+<\/sup> were also ionized?<\/li>\r\n<\/ol>\r\n<\/div>\r\n<\/div>\r\n
    \r\n

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

    \r\n
      \r\n \t
    1. Zn +\u00a02HCl \u2192\u00a0ZnCl2<\/sub> +\u00a0H2<\/sub><\/li>\r\n<\/ol>\r\n
        \r\n \t
      1. The O2\u2212<\/sup> ion would come from H2<\/sub>O, which is not considered a classic acid in the Arrhenius sense.<\/li>\r\n<\/ol>\r\n
          \r\n \t
        1. 2Al(OH)3<\/sub> + 3H2<\/sub>SO4<\/sub> \u2192 Al2<\/sub>(SO4<\/sub>)3<\/sub> + 6H2<\/sub>O<\/li>\r\n<\/ol>\r\n
            \r\n \t
          1. C8<\/sub>H10<\/sub>N4<\/sub>O2<\/sub> +\u00a0H2<\/sub>O \u2192\u00a0C8<\/sub>H10<\/sub>N4<\/sub>O2<\/sub>H+<\/sup> +\u00a0OH\u2212<\/sup>; the H+<\/sup> ion attaches to one of the N atoms in the caffeine molecule.<\/li>\r\n<\/ol>\r\n
              \r\n \t
            1. As a strong acid or base, an amphiprotic substance reacts 100% as an acid or a base, so it cannot be a base or an acid at the same time.<\/li>\r\n<\/ol>\r\n
                \r\n \t
              1. if the salt produced is an acidic salt<\/li>\r\n<\/ol>\r\n
                  \r\n \t
                1. NH3<\/sub> +\u00a0NH3<\/sub> \u2192\u00a0NH4<\/sub>+<\/sup> +\u00a0NH2<\/sub>\u2212<\/sup><\/li>\r\n<\/ol>\r\n
                    \r\n \t
                  1. pOH > 7<\/li>\r\n<\/ol>\r\n
                      \r\n \t
                    1. pH = \u22121.08; pOH = 15.08<\/li>\r\n<\/ol>\r\n<\/div>\r\n<\/div>","rendered":"
                      \n
                      \n

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

                      \n
                        \n
                      1. Write the balanced chemical equation between Zn metal and HCl(aq). The other product is ZnCl2<\/sub>.<\/li>\n
                      2. Write the neutralization reaction in which ZnCl2<\/sub>, also found in Exercise 1, is the salt product.<\/li>\n
                      3. Why isn\u2019t an oxide compound like CaO considered a salt? (Hint: what acid-base combination would be needed to make it if it were a salt?)<\/li>\n
                      4. Metal oxides are considered basic because they react with H2<\/sub>O to form OH compounds. Write the chemical equation for a reaction that forms a base when CaO is combined with H2<\/sub>O.<\/li>\n
                      5. Write the balanced chemical equation between aluminum hydroxide and sulfuric acid.<\/li>\n
                      6. Write the balanced chemical equation between phosphoric acid and barium hydroxide.<\/li>\n
                      7. Write the equation for the chemical reaction that occurs when caffeine (C8<\/sub>H10<\/sub>N4<\/sub>O2<\/sub>) acts as a Br\u00f8nsted-Lowry base.<\/li>\n
                      8. Citric acid (C6<\/sub>H8<\/sub>O7<\/sub>) is the acid found in citrus fruits. It can lose a maximum of three H+<\/sup> ions in the presence of a base. Write the chemical equations for citric acid acting stepwise as a Br\u00f8nsted-Lowry acid.<\/li>\n
                      9. Can an amphiprotic substance be a strong acid and a strong base at the same time? Explain your answer.<\/li>\n
                      10. Can an amphiprotic substance be a weak acid and a weak base at the same time? If so, explain why and give an example.<\/li>\n
                      11. Under what conditions will the equivalence point of a titration be slightly acidic?<\/li>\n
                      12. Under what conditions will the equivalence point of a titration be slightly basic?<\/li>\n
                      13. Write the chemical equation for the autoionization of NH3<\/sub>.<\/li>\n
                      14. Write the chemical equation for the autoionization of HF.<\/li>\n
                      15. What is the pOH range for an acidic solution?<\/li>\n
                      16. What is the pOH range for a basic solution?<\/li>\n
                      17. The concentration of commercial HCl is about 12 M. What is its pH and pOH?<\/li>\n
                      18. The concentration of concentrated H2<\/sub>SO4<\/sub> is about 18 M. Assuming only one H+<\/sup> comes off the H2<\/sub>SO4<\/sub> molecule, what is its pH and pOH? What would the pH and pOH be if the second H+<\/sup> were also ionized?<\/li>\n<\/ol>\n<\/div>\n<\/div>\n
                        \n
                        \n

                        Answers<\/p>\n<\/header>\n

                        \n
                          \n
                        1. Zn +\u00a02HCl \u2192\u00a0ZnCl2<\/sub> +\u00a0H2<\/sub><\/li>\n<\/ol>\n
                            \n
                          1. The O2\u2212<\/sup> ion would come from H2<\/sub>O, which is not considered a classic acid in the Arrhenius sense.<\/li>\n<\/ol>\n
                              \n
                            1. 2Al(OH)3<\/sub> + 3H2<\/sub>SO4<\/sub> \u2192 Al2<\/sub>(SO4<\/sub>)3<\/sub> + 6H2<\/sub>O<\/li>\n<\/ol>\n
                                \n
                              1. C8<\/sub>H10<\/sub>N4<\/sub>O2<\/sub> +\u00a0H2<\/sub>O \u2192\u00a0C8<\/sub>H10<\/sub>N4<\/sub>O2<\/sub>H+<\/sup> +\u00a0OH\u2212<\/sup>; the H+<\/sup> ion attaches to one of the N atoms in the caffeine molecule.<\/li>\n<\/ol>\n
                                  \n
                                1. As a strong acid or base, an amphiprotic substance reacts 100% as an acid or a base, so it cannot be a base or an acid at the same time.<\/li>\n<\/ol>\n
                                    \n
                                  1. if the salt produced is an acidic salt<\/li>\n<\/ol>\n
                                      \n
                                    1. NH3<\/sub> +\u00a0NH3<\/sub> \u2192\u00a0NH4<\/sub>+<\/sup> +\u00a0NH2<\/sub>\u2212<\/sup><\/li>\n<\/ol>\n
                                        \n
                                      1. pOH > 7<\/li>\n<\/ol>\n
                                          \n
                                        1. pH = \u22121.08; pOH = 15.08<\/li>\n<\/ol>\n<\/div>\n<\/div>\n","protected":false},"author":90,"menu_order":8,"template":"","meta":{"pb_show_title":"on","pb_short_title":"","pb_subtitle":"","pb_authors":[],"pb_section_license":""},"chapter-type":[],"contributor":[],"license":[],"class_list":["post-7637","chapter","type-chapter","status-publish","hentry"],"part":7615,"_links":{"self":[{"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/pressbooks\/v2\/chapters\/7637","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":2,"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/pressbooks\/v2\/chapters\/7637\/revisions"}],"predecessor-version":[{"id":8500,"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/pressbooks\/v2\/chapters\/7637\/revisions\/8500"}],"part":[{"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/pressbooks\/v2\/parts\/7615"}],"metadata":[{"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/pressbooks\/v2\/chapters\/7637\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/wp\/v2\/media?parent=7637"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/pressbooks\/v2\/chapter-type?post=7637"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/wp\/v2\/contributor?post=7637"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/opentextbc.ca\/introductorychemistry\/wp-json\/wp\/v2\/license?post=7637"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}