Final answer:
To calculate the ionic strength of a 0.15 M solution of Fe₂(SO₄)₃, you need to determine the concentration of Fe³⁺ and (SO₄)²⁻ ions and then sum the products of their concentrations and charges. The ionic strength is 3.51 M.
Step-by-step explanation:
The ionic strength of a solution is a measure of the concentration of ions in the solution. To calculate the ionic strength, you need to determine the concentration of each ion present in the solution and then sum the products of the concentration of each ion and the square of its charge. In the case of Fe₂(SO₄)₃, it dissociates into Fe³⁺ and (SO₄)²⁻ ions. So, the ionic strength of a 0.15 M solution of Fe₂(SO₄)₃ can be calculated as follows:
Fe³⁺ concentration = 2 * 0.15 M = 0.30 M
(SO₄)²⁻ concentration = 3 * 0.15 M = 0.45 M
Now, calculate the ionic strength:
ionic strength = (0.30 M * (3²)) + (0.45 M * (2²)) = 3.51 M