Introduction

When a mixture of FeSO4 (ferrous sulfate) and Fe2(SO4)3 (ferric sulfate) is formed, it is important to determine the molar ratio of Fe to Fe2(SO4)3. In this case, the number of sulfate ions in both ferrous and ferric sulfate is equal. To calculate the molar ratio, we need to consider the molar masses of the compounds and the stoichiometry of the reaction.

Explanation

1. Write the balanced equations
- FeSO4 + H2SO4 → Fe2(SO4)3 + H2O
- In this reaction, one molecule of FeSO4 reacts with one molecule of H2SO4 to produce one molecule of Fe2(SO4)3 and one molecule of H2O.

2. Calculate the molar masses
- FeSO4: Fe (55.845 g/mol) + S (32.06 g/mol) + 4O (16 g/mol) = 151.91 g/mol
- Fe2(SO4)3: 2Fe (55.845 g/mol) + 3S (32.06 g/mol) + 12O (16 g/mol) = 399.88 g/mol

3. Determine the molar ratio
- The molar ratio of Fe to Fe2(SO4)3 can be calculated by comparing the coefficients in the balanced equation.
- From the equation, we can see that one molecule of FeSO4 reacts to form one molecule of Fe2(SO4)3.
- Therefore, the molar ratio of Fe to Fe2(SO4)3 is 1:1.

Conclusion

In a mixture of FeSO4 and Fe2(SO4)3, where the number of sulfate ions in both ferrous and ferric sulfate is equal, the molar ratio of Fe to Fe2(SO4)3 is 1:1. This means that for every one mole of FeSO4, one mole of Fe2(SO4)3 is formed.