{"id":3131,"date":"2019-04-22T18:51:46","date_gmt":"2019-04-22T18:51:46","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/suny-introductorychemistry\/chapter\/end-of-chapter-material-28\/"},"modified":"2019-04-29T12:57:39","modified_gmt":"2019-04-29T12:57:39","slug":"end-of-chapter-material-28","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/suny-introductorychemistry\/chapter\/end-of-chapter-material-28\/","title":{"raw":"End-of-Chapter Material","rendered":"End-of-Chapter Material"},"content":{"raw":"
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Additional Exercises<\/h3>\r\n
    \r\n \t
  1. \r\n
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    Write the balanced chemical equation between Zn metal and HCl(aq). The other product is ZnCl2<\/sub>.<\/p>\r\n\r\n<\/div><\/li>\r\n \t

  2. \r\n
    \r\n

    Write the neutralization reaction in which ZnCl2<\/sub>, also found in Exercise 1, is the salt product.<\/p>\r\n\r\n<\/div><\/li>\r\n \t

  3. \r\n
    \r\n

    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?)<\/p>\r\n\r\n<\/div><\/li>\r\n \t

  4. \r\n
    \r\n

    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.<\/p>\r\n\r\n<\/div><\/li>\r\n \t

  5. \r\n
    \r\n

    Write the balanced chemical equation between aluminum hydroxide and sulfuric acid.<\/p>\r\n\r\n<\/div><\/li>\r\n \t

  6. \r\n
    \r\n

    Write the balanced chemical equation between phosphoric acid and barium hydroxide.<\/p>\r\n\r\n<\/div><\/li>\r\n \t

  7. \r\n
    \r\n

    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.<\/p>\r\n\r\n<\/div><\/li>\r\n \t

  8. \r\n
    \r\n

    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.<\/p>\r\n\r\n<\/div><\/li>\r\n \t

  9. \r\n
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    Can an amphiprotic substance be a strong acid and a strong base at the same time? Explain your answer.<\/p>\r\n\r\n<\/div><\/li>\r\n \t

  10. \r\n
    \r\n

    Can an amphiprotic substance be a weak acid and a weak base at the same time? If so, explain why and give an example.<\/p>\r\n\r\n<\/div><\/li>\r\n \t

  11. \r\n
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    Under what conditions will the equivalence point of a titration be slightly acidic?<\/p>\r\n\r\n<\/div><\/li>\r\n \t

  12. \r\n
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    Under what conditions will the equivalence point of a titration be slightly basic?<\/p>\r\n\r\n<\/div><\/li>\r\n \t

  13. \r\n
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    Write the chemical equation for the autoionization of NH3<\/sub>.<\/p>\r\n\r\n<\/div><\/li>\r\n \t

  14. \r\n
    \r\n

    Write the chemical equation for the autoionization of HF.<\/p>\r\n\r\n<\/div><\/li>\r\n \t

  15. \r\n
    \r\n

    What is the pOH range for an acidic solution?<\/p>\r\n\r\n<\/div><\/li>\r\n \t

  16. \r\n
    \r\n

    What is the pOH range for a basic solution?<\/p>\r\n\r\n<\/div><\/li>\r\n \t

  17. \r\n
    \r\n

    The concentration of commercial HCl is about 12 M. What is its pH and pOH?<\/p>\r\n\r\n<\/div><\/li>\r\n \t

  18. \r\n
    \r\n

    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?<\/p>\r\n\r\n<\/div><\/li>\r\n<\/ol>\r\n<\/div>\r\n

    \r\n

    Answers<\/h3>\r\n
    \r\n\r\n1.<\/strong>\r\n\r\nZn +\u00a02HCl \u2192\u00a0ZnCl2<\/sub> +\u00a0H2<\/sub>3.<\/strong>\r\n\r\nThe O2\u2212<\/sup> ion would come from H2<\/sub>O, which is not considered a classic acid in the Arrhenius sense.\r\n\r\n<\/div>\r\n
    \r\n\r\n5.<\/strong>2Al(OH)3<\/sub> +\u00a03 H2<\/sub>SO4<\/sub> \u2192\u00a0Al2<\/sub>(SO4<\/sub>)3<\/sub> +\u00a06 H2<\/sub>O\r\n\r\n7.<\/strong>\r\n\r\nC8<\/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.\r\n\r\n9.<\/strong>\r\n\r\nAs 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.\r\n\r\n11.<\/strong>\r\n\r\nif the salt produced is an acidic salt\r\n\r\n13.<\/strong>\r\n\r\nNH3<\/sub> +\u00a0NH3<\/sub> \u2192\u00a0NH4<\/sub>+<\/sup> +\u00a0NH2<\/sub>\u2212<\/sup>15.<\/strong>\r\n\r\npOH > 7\r\n\r\n17.<\/strong>\r\n\r\npH = \u22121.08; pOH = 15.08\r\n\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>","rendered":"
    \n
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    \n

    Additional Exercises<\/h3>\n
      \n
    1. \n
      \n

      Write the balanced chemical equation between Zn metal and HCl(aq). The other product is ZnCl2<\/sub>.<\/p>\n<\/div>\n<\/li>\n

    2. \n
      \n

      Write the neutralization reaction in which ZnCl2<\/sub>, also found in Exercise 1, is the salt product.<\/p>\n<\/div>\n<\/li>\n

    3. \n
      \n

      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?)<\/p>\n<\/div>\n<\/li>\n

    4. \n
      \n

      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.<\/p>\n<\/div>\n<\/li>\n

    5. \n
      \n

      Write the balanced chemical equation between aluminum hydroxide and sulfuric acid.<\/p>\n<\/div>\n<\/li>\n

    6. \n
      \n

      Write the balanced chemical equation between phosphoric acid and barium hydroxide.<\/p>\n<\/div>\n<\/li>\n

    7. \n
      \n

      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.<\/p>\n<\/div>\n<\/li>\n

    8. \n
      \n

      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.<\/p>\n<\/div>\n<\/li>\n

    9. \n
      \n

      Can an amphiprotic substance be a strong acid and a strong base at the same time? Explain your answer.<\/p>\n<\/div>\n<\/li>\n

    10. \n
      \n

      Can an amphiprotic substance be a weak acid and a weak base at the same time? If so, explain why and give an example.<\/p>\n<\/div>\n<\/li>\n

    11. \n
      \n

      Under what conditions will the equivalence point of a titration be slightly acidic?<\/p>\n<\/div>\n<\/li>\n

    12. \n
      \n

      Under what conditions will the equivalence point of a titration be slightly basic?<\/p>\n<\/div>\n<\/li>\n

    13. \n
      \n

      Write the chemical equation for the autoionization of NH3<\/sub>.<\/p>\n<\/div>\n<\/li>\n

    14. \n
      \n

      Write the chemical equation for the autoionization of HF.<\/p>\n<\/div>\n<\/li>\n

    15. \n
      \n

      What is the pOH range for an acidic solution?<\/p>\n<\/div>\n<\/li>\n

    16. \n
      \n

      What is the pOH range for a basic solution?<\/p>\n<\/div>\n<\/li>\n

    17. \n
      \n

      The concentration of commercial HCl is about 12 M. What is its pH and pOH?<\/p>\n<\/div>\n<\/li>\n

    18. \n
      \n

      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?<\/p>\n<\/div>\n<\/li>\n<\/ol>\n<\/div>\n

      \n

      Answers<\/h3>\n
      \n

      1.<\/strong><\/p>\n

      Zn +\u00a02HCl \u2192\u00a0ZnCl2<\/sub> +\u00a0H2<\/sub>3.<\/strong><\/p>\n

      The O2\u2212<\/sup> ion would come from H2<\/sub>O, which is not considered a classic acid in the Arrhenius sense.<\/p>\n<\/div>\n

      \n

      5.<\/strong>2Al(OH)3<\/sub> +\u00a03 H2<\/sub>SO4<\/sub> \u2192\u00a0Al2<\/sub>(SO4<\/sub>)3<\/sub> +\u00a06 H2<\/sub>O<\/p>\n

      7.<\/strong><\/p>\n

      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.<\/p>\n

      9.<\/strong><\/p>\n

      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.<\/p>\n

      11.<\/strong><\/p>\n

      if the salt produced is an acidic salt<\/p>\n

      13.<\/strong><\/p>\n

      NH3<\/sub> +\u00a0NH3<\/sub> \u2192\u00a0NH4<\/sub>+<\/sup> +\u00a0NH2<\/sub>\u2212<\/sup>15.<\/strong><\/p>\n

      pOH > 7<\/p>\n

      17.<\/strong><\/p>\n

      pH = \u22121.08; pOH = 15.08<\/p>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n\n\t\t\t

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