{"id":1292,"date":"2021-02-19T14:51:34","date_gmt":"2021-02-19T14:51:34","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/suny-dutchess-introbio2\/?post_type=chapter&p=1292"},"modified":"2021-02-26T20:35:07","modified_gmt":"2021-02-26T20:35:07","slug":"check-your-knowledge-self-test-2","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/suny-dutchess-introbio2\/chapter\/check-your-knowledge-self-test-2\/","title":{"raw":"Check Your Knowledge: Self-Test","rendered":"Check Your Knowledge: Self-Test"},"content":{"raw":"
    \r\n \t
  1. Determine the molarity for each of the following solutions:\r\n
      \r\n \t
    1. 0.444 mol of CoCl2<\/sub> in 0.654 L of solution<\/li>\r\n \t
    2. 98.0 g of phosphoric acid, H3<\/sub>PO4<\/sub>, in 1.00 L of solution<\/li>\r\n \t
    3. 0.2074 g of calcium hydroxide, Ca(OH)2<\/sub>, in 40.00 mL of solution<\/li>\r\n \t
    4. 10.5 kg of Na2<\/sub>SO4<\/sub>\u202210H2<\/sub>O in 18.60 L of solution<\/li>\r\n \t
    5. [latex]7.0\\times {10}^{-3}\\text{mol}[\/latex] of I2<\/sub> in 100.0 mL of solution<\/li>\r\n \t
    6. [latex]1.8\\times {10}^{4}\\text{mg}[\/latex] of HCl in 0.075 L of solution<\/li>\r\n<\/ol>\r\n<\/li>\r\n \t
    7. What is the molarity of the diluted solution when each of the following solutions is diluted to the given final volume?\r\n
        \r\n \t
      1. 1.00 L of a 0.250-M<\/em> solution of Fe(NO3<\/sub>)3<\/sub> is diluted to a final volume of 2.00 L<\/li>\r\n \t
      2. 0.5000 L of a 0.1222-M<\/em> solution of C3<\/sub>H7<\/sub>OH is diluted to a final volume of 1.250 L<\/li>\r\n \t
      3. 2.35 L of a 0.350-M<\/em> solution of H3<\/sub>PO4<\/sub> is diluted to a final volume of 4.00 L<\/li>\r\n \t
      4. 22.50 mL of a 0.025-M<\/em> solution of C12<\/sub>H22<\/sub>O11<\/sub> is diluted to 100.0 mL<\/li>\r\n<\/ol>\r\n<\/li>\r\n \t
      5. What is the final concentration of the solution produced when 225.5 mL of a 0.09988-M<\/em> solution of Na2<\/sub>CO3<\/sub> is allowed to evaporate until the solution volume is reduced to 45.00 mL?<\/li>\r\n \t
      6. A throat spray is 1.40% by mass phenol, C6<\/sub>H5<\/sub>OH, in water. If the solution has a density of 0.9956 g\/mL, calculate the molarity of the solution.<\/li>\r\n \t
      7. Copper(I) iodide (CuI) is often added to table salt as a dietary source of iodine. How many moles of CuI are contained in 1.00 lb (454 g) of table salt containing 0.0100% CuI by mass?<\/li>\r\n \t
      8. Explain why the ions Na+<\/sup> and Cl\u2212<\/sup> are strongly solvated in water but not in hexane, a solvent composed of nonpolar molecules.<\/li>\r\n \t
      9. \r\n
        \r\n

        Which of the following statements is not true?<\/p>\r\n\r\n<\/div><\/li>\r\n<\/ol>\r\n

          \r\n \t
        • a. Water is polar.<\/li>\r\n \t
        • b. Water stabilizes temperature.<\/li>\r\n \t
        • c. Water is essential for life.<\/li>\r\n \t
        • d. Water is the most abundant molecule in the Earth\u2019s atmosphere.<\/li>\r\n<\/ul>\r\n7. [reveal-answer q=\"316195\"]Show Answer[\/reveal-answer]<\/span>\r\n
          \r\n

          [hidden-answer a=\"316195\"]4[\/hidden-answer]<\/p>\r\n\r\n

          \r\n

          8. When acids are added to a solution, the pH should ________.<\/p>\r\n\r\n

            \r\n \t
          1. decrease<\/li>\r\n \t
          2. increase<\/li>\r\n \t
          3. stay the same<\/li>\r\n \t
          4. cannot tell without testing<\/li>\r\n<\/ol>\r\n<\/div>\r\n
            \r\n

            [reveal-answer q=\"124784\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"124784\"]1[\/hidden-answer]<\/p>\r\n9.\u00a0A molecule that binds up excess hydrogen ions in a solution is called a(n) ________.<\/span>\r\n

            \r\n
              \r\n \t
            1. acid<\/li>\r\n \t
            2. isotope<\/li>\r\n \t
            3. base<\/li>\r\n \t
            4. donator<\/li>\r\n<\/ol>\r\n<\/div>\r\n
              \r\n

              [reveal-answer q=\"988900\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"988900\"]3[\/hidden-answer]<\/p>\r\n10.\u00a0Which of the following statements is true?<\/span>\r\n

              \r\n
                \r\n \t
              1. Acids and bases cannot mix together.<\/li>\r\n \t
              2. Acids and bases will neutralize each other.<\/li>\r\n \t
              3. Acids, but not bases, can change the pH of a solution.<\/li>\r\n \t
              4. Acids donate hydroxide ions (OH\u2013<\/sup>); bases donate hydrogen ions (H+<\/sup>).<\/li>\r\n<\/ol>\r\n<\/div>\r\n
                \r\n

                [reveal-answer q=\"226242\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"226242\"]2[\/hidden-answer]<\/p>\r\n11.\u00a0Discuss how buffers help prevent drastic swings in pH.\r\n\r\n12.\u00a0Why can some insects walk on water?\r\n\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>","rendered":"

                  \n
                1. Determine the molarity for each of the following solutions:\n
                    \n
                  1. 0.444 mol of CoCl2<\/sub> in 0.654 L of solution<\/li>\n
                  2. 98.0 g of phosphoric acid, H3<\/sub>PO4<\/sub>, in 1.00 L of solution<\/li>\n
                  3. 0.2074 g of calcium hydroxide, Ca(OH)2<\/sub>, in 40.00 mL of solution<\/li>\n
                  4. 10.5 kg of Na2<\/sub>SO4<\/sub>\u202210H2<\/sub>O in 18.60 L of solution<\/li>\n
                  5. [latex]7.0\\times {10}^{-3}\\text{mol}[\/latex] of I2<\/sub> in 100.0 mL of solution<\/li>\n
                  6. [latex]1.8\\times {10}^{4}\\text{mg}[\/latex] of HCl in 0.075 L of solution<\/li>\n<\/ol>\n<\/li>\n
                  7. What is the molarity of the diluted solution when each of the following solutions is diluted to the given final volume?\n
                      \n
                    1. 1.00 L of a 0.250-M<\/em> solution of Fe(NO3<\/sub>)3<\/sub> is diluted to a final volume of 2.00 L<\/li>\n
                    2. 0.5000 L of a 0.1222-M<\/em> solution of C3<\/sub>H7<\/sub>OH is diluted to a final volume of 1.250 L<\/li>\n
                    3. 2.35 L of a 0.350-M<\/em> solution of H3<\/sub>PO4<\/sub> is diluted to a final volume of 4.00 L<\/li>\n
                    4. 22.50 mL of a 0.025-M<\/em> solution of C12<\/sub>H22<\/sub>O11<\/sub> is diluted to 100.0 mL<\/li>\n<\/ol>\n<\/li>\n
                    5. What is the final concentration of the solution produced when 225.5 mL of a 0.09988-M<\/em> solution of Na2<\/sub>CO3<\/sub> is allowed to evaporate until the solution volume is reduced to 45.00 mL?<\/li>\n
                    6. A throat spray is 1.40% by mass phenol, C6<\/sub>H5<\/sub>OH, in water. If the solution has a density of 0.9956 g\/mL, calculate the molarity of the solution.<\/li>\n
                    7. Copper(I) iodide (CuI) is often added to table salt as a dietary source of iodine. How many moles of CuI are contained in 1.00 lb (454 g) of table salt containing 0.0100% CuI by mass?<\/li>\n
                    8. Explain why the ions Na+<\/sup> and Cl\u2212<\/sup> are strongly solvated in water but not in hexane, a solvent composed of nonpolar molecules.<\/li>\n
                    9. \n
                      \n

                      Which of the following statements is not true?<\/p>\n<\/div>\n<\/li>\n<\/ol>\n

                        \n
                      • a. Water is polar.<\/li>\n
                      • b. Water stabilizes temperature.<\/li>\n
                      • c. Water is essential for life.<\/li>\n
                      • d. Water is the most abundant molecule in the Earth\u2019s atmosphere.<\/li>\n<\/ul>\n

                        7. <\/p>\n

                        Show Answer<\/span><\/span><\/p>\n
                        \n

                        \n

                        4<\/div>\n<\/div>\n
                        \n

                        8. When acids are added to a solution, the pH should ________.<\/p>\n

                          \n
                        1. decrease<\/li>\n
                        2. increase<\/li>\n
                        3. stay the same<\/li>\n
                        4. cannot tell without testing<\/li>\n<\/ol>\n<\/div>\n
                          \n

                          \n

                          Show Answer<\/span><\/p>\n
                          1<\/div>\n<\/div>\n

                          9.\u00a0A molecule that binds up excess hydrogen ions in a solution is called a(n) ________.<\/span><\/p>\n

                          \n
                            \n
                          1. acid<\/li>\n
                          2. isotope<\/li>\n
                          3. base<\/li>\n
                          4. donator<\/li>\n<\/ol>\n<\/div>\n
                            \n

                            \n

                            Show Answer<\/span><\/p>\n
                            3<\/div>\n<\/div>\n

                            10.\u00a0Which of the following statements is true?<\/span><\/p>\n

                            \n
                              \n
                            1. Acids and bases cannot mix together.<\/li>\n
                            2. Acids and bases will neutralize each other.<\/li>\n
                            3. Acids, but not bases, can change the pH of a solution.<\/li>\n
                            4. Acids donate hydroxide ions (OH\u2013<\/sup>); bases donate hydrogen ions (H+<\/sup>).<\/li>\n<\/ol>\n<\/div>\n
                              \n

                              \n

                              Show Answer<\/span><\/p>\n
                              2<\/div>\n<\/div>\n

                              11.\u00a0Discuss how buffers help prevent drastic swings in pH.<\/p>\n

                              12.\u00a0Why can some insects walk on water?<\/p>\n<\/div>\n<\/div>\n<\/div>\n<\/div>\n","protected":false},"author":57729,"menu_order":8,"template":"","meta":{"_candela_citation":"[]","CANDELA_OUTCOMES_GUID":"","pb_show_title":"on","pb_short_title":"","pb_subtitle":"","pb_authors":[],"pb_section_license":""},"chapter-type":[],"contributor":[],"license":[],"class_list":["post-1292","chapter","type-chapter","status-publish","hentry"],"part":877,"_links":{"self":[{"href":"https:\/\/courses.lumenlearning.com\/suny-dutchess-introbio2\/wp-json\/pressbooks\/v2\/chapters\/1292","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/courses.lumenlearning.com\/suny-dutchess-introbio2\/wp-json\/pressbooks\/v2\/chapters"}],"about":[{"href":"https:\/\/courses.lumenlearning.com\/suny-dutchess-introbio2\/wp-json\/wp\/v2\/types\/chapter"}],"author":[{"embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/suny-dutchess-introbio2\/wp-json\/wp\/v2\/users\/57729"}],"version-history":[{"count":4,"href":"https:\/\/courses.lumenlearning.com\/suny-dutchess-introbio2\/wp-json\/pressbooks\/v2\/chapters\/1292\/revisions"}],"predecessor-version":[{"id":1426,"href":"https:\/\/courses.lumenlearning.com\/suny-dutchess-introbio2\/wp-json\/pressbooks\/v2\/chapters\/1292\/revisions\/1426"}],"part":[{"href":"https:\/\/courses.lumenlearning.com\/suny-dutchess-introbio2\/wp-json\/pressbooks\/v2\/parts\/877"}],"metadata":[{"href":"https:\/\/courses.lumenlearning.com\/suny-dutchess-introbio2\/wp-json\/pressbooks\/v2\/chapters\/1292\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/courses.lumenlearning.com\/suny-dutchess-introbio2\/wp-json\/wp\/v2\/media?parent=1292"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/suny-dutchess-introbio2\/wp-json\/pressbooks\/v2\/chapter-type?post=1292"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/suny-dutchess-introbio2\/wp-json\/wp\/v2\/contributor?post=1292"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/courses.lumenlearning.com\/suny-dutchess-introbio2\/wp-json\/wp\/v2\/license?post=1292"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}