Question

2.3456 g of Mohr's salt, (NH₄)₂Fe(SO₄)₂∙6H₂O, dissolves in water to make 250.0 ml of solution. What is the molarity of the sulfate ion in the solution?

a. 0.01 M
b. 0.02 M
c. 0.03 M
d. 0.04 M

Answer 1

The molarity of sulfate ions in the solution made from dissolving 2.3456 g of Mohr's salt in 250.0 ml of water is 0.02 M, which is accomplished by calculating the moles of Mohr's salt and relating them to the sulfate ions provided by the compound per liter of solution.

Step-by-step explanation:

To calculate the molarity of the sulfate ion in the solution made from dissolving 2.3456 g of Mohr's salt, (NH₄)₂Fe(SO₄)₂⋅₆H₂O, in 250.0 ml of water, we need to follow these steps:

1. Calculate the molar mass of Mohr's salt.
2. Determine the number of moles of Mohr's salt dissolved.
3. Understand that each formula unit of Mohr's salt provides two sulfate ions.
4. Divide the moles of sulfate ions by the volume of the solution in liters to find the molarity.

After performing these steps, we can conclude that the correct answer is b. 0.02 M, indicating that the molarity of the sulfate ion is 0.02 M.