{"id":242,"date":"2018-03-19T16:08:06","date_gmt":"2018-03-19T16:08:06","guid":{"rendered":"https:\/\/courses.lumenlearning.com\/suny-orgbiochemistry\/chapter\/formula-mass\/"},"modified":"2018-08-08T17:17:07","modified_gmt":"2018-08-08T17:17:07","slug":"formula-mass","status":"publish","type":"chapter","link":"https:\/\/courses.lumenlearning.com\/suny-monroecc-orgbiochemistry\/chapter\/formula-mass\/","title":{"raw":"3.5 Formula Mass","rendered":"3.5 Formula Mass"},"content":{"raw":"
\r\n
\r\n
\r\n

Learning Objectives<\/h3>\r\n
\r\n
    \r\n \t
  1. Determine the formula mass of an ionic compound.<\/li>\r\n<\/ol>\r\n<\/div>\r\n<\/div>\r\n

    One skill needed in future chapters is the ability to determine the mass of the formula of an ionic compound. This quantity is called the formula mass<\/strong>.\u00a0\u00a0<\/span>The sum of the masses of the elements in the formula of an ionic compound.<\/span><\/span>. The formula mass is obtained by adding the masses of each individual atom or ion in the formula of the compound. Because the mass of an electron is so small, the mass of an ion is considered to be the same as the mass of an atom of the same element.\u00a0 In addition, within a neutral compound, the electrons lost by the cation were taken in by the anion anyway.<\/p>\r\n

    Let us start by calculating the formula mass of sodium chloride (NaCl). This formula mass is the sum of the atomic masses of one sodium atom and one chlorine atom, which we find from the periodic table; here, we use the masses to two decimal places:<\/p>\r\n\r\n

    \r\n\r\n\r\n\r\n\r\n\r\n
    Na:<\/td>\r\n22.99 u<\/td>\r\n<\/tr>\r\n
    Cl:<\/td>\r\n+35.45 u<\/span><\/td>\r\n<\/tr>\r\n
    Total:<\/td>\r\n=58.44 u<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<\/div>\r\n

    To two decimal places, the formula mass of NaCl is 58.44 u.<\/p>\r\n

    When an ionic compound has more than one anion or cation, you must remember to use the proper multiple of the atomic mass for the element in question. For the formula mass of calcium fluoride (CaF2<\/sub>), we must multiply the mass of the fluorine atom by 2 to account for the two fluorine atoms in the chemical formula:<\/p>\r\n\r\n

    \r\n\r\n\r\n\r\n\r\n\r\n
    Ca:<\/td>\r\n1 \u00d7 40.08<\/td>\r\n40.08 u<\/td>\r\n<\/tr>\r\n
    F:<\/td>\r\n2 \u00d7 19.00 =<\/td>\r\n+38.00 u<\/span><\/td>\r\n<\/tr>\r\n
    Total:<\/td>\r\n<\/td>\r\n=78.08 u<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<\/div>\r\n

    The formula mass of CaF2<\/sub> is 78.08 u.<\/p>\r\n

    For ionic compounds with polyatomic ions, the sum must include the number and mass of each atom in the formula for the polyatomic ion. For example, potassium nitrate (KNO3<\/sub>) has one potassium atom, one nitrogen atom, and three oxygen atoms:<\/p>\r\n\r\n

    \r\n\r\n\r\n\r\n\r\n\r\n\r\n
    K:<\/td>\r\n1 \u00d7 39.10<\/td>\r\n39.10 u<\/td>\r\n<\/tr>\r\n
    N:<\/td>\r\n1 \u00d7 14.00<\/td>\r\n+ 14.00 u<\/td>\r\n<\/tr>\r\n
    O:<\/td>\r\n3 \u00d7 16.00 =<\/td>\r\n+ 48.00 u<\/span><\/td>\r\n<\/tr>\r\n
    Total:<\/td>\r\n<\/td>\r\n=101.10 u<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<\/div>\r\n

    The formula mass of KNO3<\/sub> is 101.10 u.<\/p>\r\n\r\n

    \r\n\r\nWhen a formula contains more than one polyatomic unit in the chemical formula, as in Ca(NO<\/span>3<\/sub>)<\/span>2<\/sub>, don\u2019t forget to multiply the atomic mass of every atom inside the parentheses by the subscript outside the parentheses. This is necessary because the subscript refers to the <\/span>entire polyatomic ion<\/em>. Thus, for Ca(NO<\/span>3<\/sub>)<\/span>2<\/sub>, the subscript 2 implies two complete nitrate ions, so we must sum the masses of two (1 \u00d7 2) nitrogen atoms and six (3 \u00d7 2) oxygen atoms, along with the mass of a single calcium atom:<\/span>\r\n\r\n<\/div>\r\n
    \r\n\r\n\r\n\r\n\r\n\r\n\r\n
    Ca:<\/td>\r\n1 \u00d7 40.08<\/td>\r\n40.08 u<\/td>\r\n<\/tr>\r\n
    N:<\/td>\r\n2 \u00d7 14.00 =<\/td>\r\n+ 28.00 u<\/td>\r\n<\/tr>\r\n
    O:<\/td>\r\n6 \u00d7 16.00 =<\/td>\r\n+ 96.00 u<\/span><\/td>\r\n<\/tr>\r\n
    Total:<\/td>\r\n<\/td>\r\n=164.08 u<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<\/div>\r\n

    The key to calculating the formula mass of an ionic compound is to correctly count each atom in the formula and multiply the atomic masses of its atoms accordingly.<\/p>\r\n\r\n

    \r\n

    Example 9<\/h3>\r\n

    Use the atomic masses (rounded to two decimal places) from the inside cover of this book to determine the formula mass for each ionic compound.<\/p>\r\n\r\n

      \r\n \t
    1. FeCl3<\/sub><\/li>\r\n \t
    2. (NH4<\/sub>)3<\/sub>PO4<\/sub><\/li>\r\n<\/ol>\r\n

      Solution<\/p>\r\n[reveal-answer q=\"806287\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"806287\"]\r\n\r\n1.\r\n\r\n\r\n\r\n\r\n\r\n
      Fe:<\/td>\r\n<\/td>\r\n55.85 u<\/td>\r\n<\/tr>\r\n
      Cl:<\/td>\r\n3 x 35.45=<\/td>\r\n+106.35 u<\/td>\r\n<\/tr>\r\n
      Total<\/td>\r\n<\/td>\r\n=162.20 u<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\nThe formula mass of FeCl3<\/sub> is 162.20 u.\r\n\r\n2. When we distribute the subscript 3 through the parentheses containing the formula for the ammonium ion, we see that we have 3 nitrogen atoms and 12 hydrogen atoms. Thus, we set up the sum as follows:\r\n\r\n\r\n\r\n\r\n\r\n\r\n\r\n
      N<\/td>\r\n3x14.00=<\/td>\r\n42.00 u<\/td>\r\n<\/tr>\r\n
      H<\/td>\r\n12 x 1.00=<\/td>\r\n+12.00 u P<\/td>\r\n<\/tr>\r\n
      P<\/td>\r\n<\/td>\r\n+30.97 u<\/td>\r\n<\/tr>\r\n
      O<\/td>\r\n4 x 16.00=<\/td>\r\n+64.00 u<\/td>\r\n<\/tr>\r\n
      Total:<\/td>\r\n<\/td>\r\n148.97 u<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\nThe formula mass for (NH4<\/sub>)3<\/sub>PO4 is 148.97 u.[\/hidden-answer]\r\n\r\n<\/div>\r\n
      \r\n

      Skill-Building Exercises<\/h3>\r\nUse the atomic masses (rounded to two decimal places) from the inside cover of this book to determine the formula mass for each ionic compound.\r\n
        \r\n \t
      1. \r\n
        \r\n

        TiO2<\/sub><\/p>\r\n\r\n<\/div><\/li>\r\n \t

      2. \r\n
        \r\n

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

      3. \r\n
        \r\n

        Au(NO3<\/sub>)3<\/sub><\/p>\r\n\r\n<\/div><\/li>\r\n \t

      4. \r\n
        \r\n

        Fe3<\/sub>(PO4<\/sub>)2<\/sub><\/p>\r\n\r\n<\/div><\/li>\r\n<\/ol>\r\n<\/div>\r\n

        \r\n
        \r\n

        To Your Health: Hydrates<\/h3>\r\n

        Some ionic compounds have water (H2<\/sub>O) incorporated within their formula unit. These compounds, called hydrates<\/em>, have a characteristic number of water units associated with each formula unit of the compound. Hydrates are solids, not liquids or solutions, despite the water they contain.<\/p>\r\n

        To write the chemical formula of a hydrate, write the number of water units per formula unit of compound after its chemical formula. The two chemical formulas are separated by a vertically centered dot. The hydrate of copper(II) sulfate has five water units associated with each formula unit, so it is written as CuSO4<\/sub>\u00b75H2<\/sub>O. The name of this compound is copper(II) sulfate pentahydrate, with the penta-<\/em> prefix indicating the presence of five water units per formula unit of copper(II) sulfate.<\/p>\r\n

        Hydrates have various uses in the health industry. Calcium sulfate hemihydrate (CaSO4<\/sub>\u00b7\u00bdH2<\/sub>O), known as plaster of Paris, is used to make casts for broken bones. Epsom salt (MgSO4<\/sub>\u00b77H2<\/sub>O) is used as a bathing salt and a laxative. Aluminum chloride hexahydrate is an active ingredient in antiperspirants. The accompanying table lists some useful hydrates.<\/p>\r\n\r\n<\/div>\r\n<\/div>\r\n

        \r\n
        Table 3.4<\/span> Names and Formulas of Some Widely Used Hydrates<\/strong><\/h5>\r\n\r\n\r\n\r\n\r\n\r\n\r\n\r\n\r\n\r\n\r\n\r\n
        Formula<\/th>\r\nName<\/th>\r\nUses<\/th>\r\n<\/tr>\r\n<\/thead>\r\n
        AlCl3<\/sub>\u00b76H2<\/sub>O<\/td>\r\naluminum chloride hexahydrate<\/td>\r\nantiperspirant<\/td>\r\n<\/tr>\r\n
        CaSO4<\/sub>\u00b7\u00bdH2<\/sub>O<\/td>\r\ncalcium sulfate hemihydrate (plaster of Paris)<\/td>\r\ncasts (for broken bones and castings)<\/td>\r\n<\/tr>\r\n
        CaSO4<\/sub>\u00b72H2<\/sub>O<\/td>\r\ncalcium sulfate dihydrate (gypsum)<\/td>\r\ndrywall component<\/td>\r\n<\/tr>\r\n
        CoCl2<\/sub>\u00b76H2<\/sub>O<\/td>\r\ncobalt(II) chloride hexahydrate<\/td>\r\ndrying agent, humidity indicator<\/td>\r\n<\/tr>\r\n
        CuSO4<\/sub>\u00b75H2<\/sub>O<\/td>\r\ncopper(II) sulfate pentahydrate<\/td>\r\nfungicide, algicide, herbicide<\/td>\r\n<\/tr>\r\n
        MgSO4<\/sub>\u00b77H2<\/sub>O<\/td>\r\nmagnesium sulfate heptahydrate (Epsom salts)<\/td>\r\nlaxative, bathing salt<\/td>\r\n<\/tr>\r\n
        Na2<\/sub>CO3<\/sub>\u00b710H2<\/sub>O<\/td>\r\nsodium carbonate decahydrate (washing soda)<\/td>\r\nlaundry additive\/cleaner<\/td>\r\n<\/tr>\r\n<\/tbody>\r\n<\/table>\r\n<\/div>\r\n
        \r\n
        \r\n

        Concept Review Exercises<\/h3>\r\n
          \r\n \t
        1. \r\n
          \r\n

          What is the relationship between atomic mass and formula mass?<\/p>\r\n\r\n<\/div><\/li>\r\n \t

        2. \r\n
          \r\n

          How are subscripts used to determine a formula mass when more than one polyatomic ion is present in a chemical formula?<\/p>\r\n\r\n<\/div><\/li>\r\n<\/ol>\r\n<\/div>\r\n<\/div>\r\n

          \r\n
          \r\n
          \r\n

          Answers<\/h3>\r\n[reveal-answer q=\"969288\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"969288\"]\r\n
            \r\n \t
          1. The formula mass is the sum of the atomic masses of the atoms in the formula.<\/li>\r\n \t
          2. The subscript is distributed throughout the parentheses to determine the total number of atoms in the formula.[\/hidden-answer]\r\n
            \r\n

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

            \r\n
            \r\n

            Key Takeaway<\/h3>\r\n<\/div>\r\n
            \r\n
              \r\n \t
            • Formula masses of ionic compounds can be determined from the masses of the atoms in their formulas.<\/li>\r\n<\/ul>\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n
              \r\n
              \r\n

              Exercises<\/h3>\r\n
                \r\n \t
              1. \r\n
                \r\n

                What is the formula mass for the ionic compound formed by each pair of ions?<\/p>\r\n\r\n

                  \r\n \t
                1. Na+<\/sup> and Br\u2212<\/sup><\/li>\r\n \t
                2. Mg2+<\/sup> and Br\u2212<\/sup><\/li>\r\n \t
                3. Mg2+<\/sup> and S2\u2212<\/sup><\/li>\r\n<\/ol>\r\n<\/div><\/li>\r\n \t
                4. \r\n
                  \r\n

                  What is the formula mass for the ionic compound formed by each pair of ions?<\/p>\r\n\r\n

                    \r\n \t
                  1. K+<\/sup> and Cl\u2212<\/sup><\/li>\r\n \t
                  2. Mg2+<\/sup> and Cl\u2212<\/sup><\/li>\r\n \t
                  3. Mg2+<\/sup> and Se2\u2212<\/sup><\/li>\r\n<\/ol>\r\n<\/div><\/li>\r\n \t
                  4. \r\n
                    \r\n

                    What is the formula mass for the ionic compound formed by each pair of ions?<\/p>\r\n\r\n

                      \r\n \t
                    1. Na+<\/sup> and N3\u2212<\/sup><\/li>\r\n \t
                    2. Mg2+<\/sup> and N3\u2212<\/sup><\/li>\r\n \t
                    3. Al3+<\/sup> and S2\u2212<\/sup><\/li>\r\n<\/ol>\r\n<\/div><\/li>\r\n \t
                    4. \r\n
                      \r\n

                      What is the formula mass for the ionic compound formed by each pair of ions?<\/p>\r\n\r\n

                        \r\n \t
                      1. Li+<\/sup> and N3\u2212<\/sup><\/li>\r\n \t
                      2. Mg2+<\/sup> and P3\u2212<\/sup><\/li>\r\n \t
                      3. Li+<\/sup> and P3\u2212<\/sup><\/li>\r\n<\/ol>\r\n<\/div><\/li>\r\n \t
                      4. \r\n
                        \r\n

                        What is the formula mass for each compound?<\/p>\r\n\r\n

                          \r\n \t
                        1. FeBr3<\/sub><\/li>\r\n \t
                        2. FeBr2<\/sub><\/li>\r\n \t
                        3. Au2<\/sub>S3<\/sub><\/li>\r\n \t
                        4. Au2<\/sub>S<\/li>\r\n<\/ol>\r\n<\/div><\/li>\r\n \t
                        5. \r\n
                          \r\n

                          What is the formula mass for each compound?<\/p>\r\n\r\n

                            \r\n \t
                          1. Cr2<\/sub>O3<\/sub><\/li>\r\n \t
                          2. CrO<\/li>\r\n \t
                          3. PbCl2<\/sub><\/li>\r\n \t
                          4. PbCl4<\/sub><\/li>\r\n<\/ol>\r\n<\/div><\/li>\r\n \t
                          5. \r\n
                            \r\n

                            What is the formula mass for each compound?<\/p>\r\n\r\n

                              \r\n \t
                            1. Cr(NO3<\/sub>)3<\/sub><\/li>\r\n \t
                            2. Fe3<\/sub>(PO4<\/sub>)2<\/sub><\/li>\r\n \t
                            3. CaCrO4<\/sub><\/li>\r\n \t
                            4. Al(OH)3<\/sub><\/li>\r\n<\/ol>\r\n<\/div><\/li>\r\n \t
                            5. \r\n
                              \r\n

                              What is the formula mass for each compound?<\/p>\r\n\r\n

                                \r\n \t
                              1. NH4<\/sub>NO3<\/sub><\/li>\r\n \t
                              2. H2<\/sub>Cr2<\/sub>O7<\/sub><\/li>\r\n \t
                              3. Cu2<\/sub>CO3<\/sub><\/li>\r\n \t
                              4. NaHCO3<\/sub><\/li>\r\n<\/ol>\r\n<\/div><\/li>\r\n \t
                              5. \r\n
                                \r\n

                                What is the formula mass for each compound?<\/p>\r\n\r\n

                                  \r\n \t
                                1. Al(HSO4<\/sub>)3<\/sub><\/li>\r\n \t
                                2. Mg(HSO4<\/sub>)2<\/sub><\/li>\r\n<\/ol>\r\n<\/div><\/li>\r\n \t
                                3. \r\n
                                  \r\n

                                  What is the formula mass for each compound?<\/p>\r\n\r\n

                                    \r\n \t
                                  1. Co(HCO3<\/sub>)2<\/sub><\/li>\r\n \t
                                  2. LiHCO3<\/sub><\/li>\r\n<\/ol>\r\n<\/div><\/li>\r\n<\/ol>\r\n<\/div>\r\n<\/div>\r\n
                                    \r\n
                                    \r\n

                                    Answers<\/h3>\r\n[reveal-answer q=\"986825\"]Show Answer[\/reveal-answer]\r\n[hidden-answer a=\"986825\"]\r\n\r\n1. a. 102.90 u b. 184.11 u c. 56.38 u\r\n\r\n3. a. 83.00 u b. 100.93 u c. 150.17 u\r\n\r\n5. a. 295.50 u b. 215.60 u c. 490.30 u d. 426.10 u\r\n\r\n7. a. 238.00 u b. 357.49 u c. 156.08 u d. 78.01 u\r\n\r\n9. a. 318.22 u b. 218.47 u[\/hidden-answer]\r\n\r\n \r\n\r\n<\/div>\r\n<\/div>\r\n<\/div>\r\n<\/div>","rendered":"
                                    \n
                                    \n
                                    \n

                                    Learning Objectives<\/h3>\n
                                    \n
                                      \n
                                    1. Determine the formula mass of an ionic compound.<\/li>\n<\/ol>\n<\/div>\n<\/div>\n

                                      One skill needed in future chapters is the ability to determine the mass of the formula of an ionic compound. This quantity is called the formula mass<\/strong>.\u00a0\u00a0<\/span>The sum of the masses of the elements in the formula of an ionic compound.<\/span><\/span>. The formula mass is obtained by adding the masses of each individual atom or ion in the formula of the compound. Because the mass of an electron is so small, the mass of an ion is considered to be the same as the mass of an atom of the same element.\u00a0 In addition, within a neutral compound, the electrons lost by the cation were taken in by the anion anyway.<\/p>\n

                                      Let us start by calculating the formula mass of sodium chloride (NaCl). This formula mass is the sum of the atomic masses of one sodium atom and one chlorine atom, which we find from the periodic table; here, we use the masses to two decimal places:<\/p>\n

                                      \n\n\n\n\n\n
                                      Na:<\/td>\n22.99 u<\/td>\n<\/tr>\n
                                      Cl:<\/td>\n+35.45 u<\/span><\/td>\n<\/tr>\n
                                      Total:<\/td>\n=58.44 u<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<\/div>\n

                                      To two decimal places, the formula mass of NaCl is 58.44 u.<\/p>\n

                                      When an ionic compound has more than one anion or cation, you must remember to use the proper multiple of the atomic mass for the element in question. For the formula mass of calcium fluoride (CaF2<\/sub>), we must multiply the mass of the fluorine atom by 2 to account for the two fluorine atoms in the chemical formula:<\/p>\n

                                      \n\n\n\n\n\n
                                      Ca:<\/td>\n1 \u00d7 40.08<\/td>\n40.08 u<\/td>\n<\/tr>\n
                                      F:<\/td>\n2 \u00d7 19.00 =<\/td>\n+38.00 u<\/span><\/td>\n<\/tr>\n
                                      Total:<\/td>\n<\/td>\n=78.08 u<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<\/div>\n

                                      The formula mass of CaF2<\/sub> is 78.08 u.<\/p>\n

                                      For ionic compounds with polyatomic ions, the sum must include the number and mass of each atom in the formula for the polyatomic ion. For example, potassium nitrate (KNO3<\/sub>) has one potassium atom, one nitrogen atom, and three oxygen atoms:<\/p>\n

                                      \n\n\n\n\n\n\n
                                      K:<\/td>\n1 \u00d7 39.10<\/td>\n39.10 u<\/td>\n<\/tr>\n
                                      N:<\/td>\n1 \u00d7 14.00<\/td>\n+ 14.00 u<\/td>\n<\/tr>\n
                                      O:<\/td>\n3 \u00d7 16.00 =<\/td>\n+ 48.00 u<\/span><\/td>\n<\/tr>\n
                                      Total:<\/td>\n<\/td>\n=101.10 u<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<\/div>\n

                                      The formula mass of KNO3<\/sub> is 101.10 u.<\/p>\n

                                      \n

                                      When a formula contains more than one polyatomic unit in the chemical formula, as in Ca(NO<\/span>3<\/sub>)<\/span>2<\/sub>, don\u2019t forget to multiply the atomic mass of every atom inside the parentheses by the subscript outside the parentheses. This is necessary because the subscript refers to the <\/span>entire polyatomic ion<\/em>. Thus, for Ca(NO<\/span>3<\/sub>)<\/span>2<\/sub>, the subscript 2 implies two complete nitrate ions, so we must sum the masses of two (1 \u00d7 2) nitrogen atoms and six (3 \u00d7 2) oxygen atoms, along with the mass of a single calcium atom:<\/span><\/p>\n<\/div>\n

                                      \n\n\n\n\n\n\n
                                      Ca:<\/td>\n1 \u00d7 40.08<\/td>\n40.08 u<\/td>\n<\/tr>\n
                                      N:<\/td>\n2 \u00d7 14.00 =<\/td>\n+ 28.00 u<\/td>\n<\/tr>\n
                                      O:<\/td>\n6 \u00d7 16.00 =<\/td>\n+ 96.00 u<\/span><\/td>\n<\/tr>\n
                                      Total:<\/td>\n<\/td>\n=164.08 u<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<\/div>\n

                                      The key to calculating the formula mass of an ionic compound is to correctly count each atom in the formula and multiply the atomic masses of its atoms accordingly.<\/p>\n

                                      \n

                                      Example 9<\/h3>\n

                                      Use the atomic masses (rounded to two decimal places) from the inside cover of this book to determine the formula mass for each ionic compound.<\/p>\n

                                        \n
                                      1. FeCl3<\/sub><\/li>\n
                                      2. (NH4<\/sub>)3<\/sub>PO4<\/sub><\/li>\n<\/ol>\n

                                        Solution<\/p>\n

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

                                        1.<\/p>\n\n\n\n\n\n
                                        Fe:<\/td>\n<\/td>\n55.85 u<\/td>\n<\/tr>\n
                                        Cl:<\/td>\n3 x 35.45=<\/td>\n+106.35 u<\/td>\n<\/tr>\n
                                        Total<\/td>\n<\/td>\n=162.20 u<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n

                                        The formula mass of FeCl3<\/sub> is 162.20 u.<\/p>\n

                                        2. When we distribute the subscript 3 through the parentheses containing the formula for the ammonium ion, we see that we have 3 nitrogen atoms and 12 hydrogen atoms. Thus, we set up the sum as follows:<\/p>\n\n\n\n\n\n\n\n
                                        N<\/td>\n3×14.00=<\/td>\n42.00 u<\/td>\n<\/tr>\n
                                        H<\/td>\n12 x 1.00=<\/td>\n+12.00 u P<\/td>\n<\/tr>\n
                                        P<\/td>\n<\/td>\n+30.97 u<\/td>\n<\/tr>\n
                                        O<\/td>\n4 x 16.00=<\/td>\n+64.00 u<\/td>\n<\/tr>\n
                                        Total:<\/td>\n<\/td>\n148.97 u<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n

                                        The formula mass for (NH4<\/sub>)3<\/sub>PO4 is 148.97 u.<\/div>\n<\/div>\n<\/div>\n

                                        \n

                                        Skill-Building Exercises<\/h3>\n

                                        Use the atomic masses (rounded to two decimal places) from the inside cover of this book to determine the formula mass for each ionic compound.<\/p>\n

                                          \n
                                        1. \n
                                          \n

                                          TiO2<\/sub><\/p>\n<\/div>\n<\/li>\n

                                        2. \n
                                          \n

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

                                        3. \n
                                          \n

                                          Au(NO3<\/sub>)3<\/sub><\/p>\n<\/div>\n<\/li>\n

                                        4. \n
                                          \n

                                          Fe3<\/sub>(PO4<\/sub>)2<\/sub><\/p>\n<\/div>\n<\/li>\n<\/ol>\n<\/div>\n

                                          \n
                                          \n

                                          To Your Health: Hydrates<\/h3>\n

                                          Some ionic compounds have water (H2<\/sub>O) incorporated within their formula unit. These compounds, called hydrates<\/em>, have a characteristic number of water units associated with each formula unit of the compound. Hydrates are solids, not liquids or solutions, despite the water they contain.<\/p>\n

                                          To write the chemical formula of a hydrate, write the number of water units per formula unit of compound after its chemical formula. The two chemical formulas are separated by a vertically centered dot. The hydrate of copper(II) sulfate has five water units associated with each formula unit, so it is written as CuSO4<\/sub>\u00b75H2<\/sub>O. The name of this compound is copper(II) sulfate pentahydrate, with the penta-<\/em> prefix indicating the presence of five water units per formula unit of copper(II) sulfate.<\/p>\n

                                          Hydrates have various uses in the health industry. Calcium sulfate hemihydrate (CaSO4<\/sub>\u00b7\u00bdH2<\/sub>O), known as plaster of Paris, is used to make casts for broken bones. Epsom salt (MgSO4<\/sub>\u00b77H2<\/sub>O) is used as a bathing salt and a laxative. Aluminum chloride hexahydrate is an active ingredient in antiperspirants. The accompanying table lists some useful hydrates.<\/p>\n<\/div>\n<\/div>\n

                                          \n
                                          Table 3.4<\/span> Names and Formulas of Some Widely Used Hydrates<\/strong><\/h5>\n\n\n\n\n\n\n\n\n\n\n\n
                                          Formula<\/th>\nName<\/th>\nUses<\/th>\n<\/tr>\n<\/thead>\n
                                          AlCl3<\/sub>\u00b76H2<\/sub>O<\/td>\naluminum chloride hexahydrate<\/td>\nantiperspirant<\/td>\n<\/tr>\n
                                          CaSO4<\/sub>\u00b7\u00bdH2<\/sub>O<\/td>\ncalcium sulfate hemihydrate (plaster of Paris)<\/td>\ncasts (for broken bones and castings)<\/td>\n<\/tr>\n
                                          CaSO4<\/sub>\u00b72H2<\/sub>O<\/td>\ncalcium sulfate dihydrate (gypsum)<\/td>\ndrywall component<\/td>\n<\/tr>\n
                                          CoCl2<\/sub>\u00b76H2<\/sub>O<\/td>\ncobalt(II) chloride hexahydrate<\/td>\ndrying agent, humidity indicator<\/td>\n<\/tr>\n
                                          CuSO4<\/sub>\u00b75H2<\/sub>O<\/td>\ncopper(II) sulfate pentahydrate<\/td>\nfungicide, algicide, herbicide<\/td>\n<\/tr>\n
                                          MgSO4<\/sub>\u00b77H2<\/sub>O<\/td>\nmagnesium sulfate heptahydrate (Epsom salts)<\/td>\nlaxative, bathing salt<\/td>\n<\/tr>\n
                                          Na2<\/sub>CO3<\/sub>\u00b710H2<\/sub>O<\/td>\nsodium carbonate decahydrate (washing soda)<\/td>\nlaundry additive\/cleaner<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<\/div>\n
                                          \n
                                          \n

                                          Concept Review Exercises<\/h3>\n
                                            \n
                                          1. \n
                                            \n

                                            What is the relationship between atomic mass and formula mass?<\/p>\n<\/div>\n<\/li>\n

                                          2. \n
                                            \n

                                            How are subscripts used to determine a formula mass when more than one polyatomic ion is present in a chemical formula?<\/p>\n<\/div>\n<\/li>\n<\/ol>\n<\/div>\n<\/div>\n

                                            \n
                                            \n
                                            \n

                                            Answers<\/h3>\n
                                            Show Answer<\/span><\/p>\n
                                            \n
                                              \n
                                            1. The formula mass is the sum of the atomic masses of the atoms in the formula.<\/li>\n
                                            2. The subscript is distributed throughout the parentheses to determine the total number of atoms in the formula.<\/div>\n<\/div>\n
                                              \n

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

                                              \n
                                              \n

                                              Key Takeaway<\/h3>\n<\/div>\n
                                              \n