Questions: Write the empirical formula for at least four ionic compounds that could be formed from the following ions: SO4^2-, IO3^-, NH4^+, Fe^3+

Write the empirical formula for at least four ionic compounds that could be formed from the following ions: SO4^2-, IO3^-, NH4^+, Fe^3+
Transcript text: Write the empirical formula for at least four ionic compounds that could be formed from the following ions: \[ \mathrm{SO}_{4}^{2-}, \mathrm{IO}_{3}^{-}, \mathrm{NH}_{4}^{+}, \mathrm{Fe}^{3+} \]
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Solution

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Solution Steps

Step 1: Identify the possible cations and anions

The given ions are:

  • Anions: \(\mathrm{SO}_{4}^{2-}\), \(\mathrm{IO}_{3}^{-}\)
  • Cations: \(\mathrm{NH}_{4}^{+}\), \(\mathrm{Fe}^{3+}\)
Step 2: Pair the cations and anions to form neutral compounds

To form neutral ionic compounds, the total positive charge must equal the total negative charge.

Step 3: Formulate the empirical formulas

  1. Pairing \(\mathrm{NH}_{4}^{+}\) with \(\mathrm{SO}_{4}^{2-}\):

    • Two \(\mathrm{NH}_{4}^{+}\) ions are needed to balance one \(\mathrm{SO}_{4}^{2-}\) ion.
    • Empirical formula: \(\mathrm{(NH_4)_2SO_4}\)

  2. Pairing \(\mathrm{NH}_{4}^{+}\) with \(\mathrm{IO}_{3}^{-}\):

    • One \(\mathrm{NH}_{4}^{+}\) ion is needed to balance one \(\mathrm{IO}_{3}^{-}\) ion.
    • Empirical formula: \(\mathrm{NH_4IO_3}\)

  3. Pairing \(\mathrm{Fe}^{3+}\) with \(\mathrm{SO}_{4}^{2-}\):

    • Two \(\mathrm{Fe}^{3+}\) ions are needed to balance three \(\mathrm{SO}_{4}^{2-}\) ions.
    • Empirical formula: \(\mathrm{Fe_2(SO_4)_3}\)

  4. Pairing \(\mathrm{Fe}^{3+}\) with \(\mathrm{IO}_{3}^{-}\):

    • One \(\mathrm{Fe}^{3+}\) ion is needed to balance three \(\mathrm{IO}_{3}^{-}\) ions.
    • Empirical formula: \(\mathrm{Fe(IO_3)_3}\)

Final Answer

\[ \boxed{\mathrm{(NH_4)_2SO_4}} \] \[ \boxed{\mathrm{NH_4IO_3}} \] \[ \boxed{\mathrm{Fe_2(SO_4)_3}} \] \[ \boxed{\mathrm{Fe(IO_3)_3}} \]

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