How many moles of sulfate ions are in 100 ml of a solution of .002 M Fe2(SO4)3?
How many mols Fe2(SO4)3 do you have? That's mols = M x L = ?
There are 3 SO4 ions for every 1 mol Fe2(SO4)3.
I don't know it thats the reason am asking the same question
To determine the number of moles of sulfate ions in the solution of Fe2(SO4)3, you first need to calculate the number of moles of Fe2(SO4)3 present in 100 ml of the solution.
The molarity (M) is defined as the number of moles of solute per liter of solution. Therefore, to calculate the number of moles in 100 ml, you need to convert 100 ml to liters:
100 ml = 100/1000 = 0.1 L
Next, you can use the formula for calculating the number of moles:
Number of moles = Molarity x Volume (in liters)
Number of moles of Fe2(SO4)3 = 0.002 mol/L x 0.1 L = 0.0002 mol
Since there are two sulfate (SO4) ions per formula unit of Fe2(SO4)3, you can multiply the number of moles of Fe2(SO4)3 by 2 to determine the number of moles of sulfate ions:
Number of moles of sulfate ions = 0.0002 mol x 2 = 0.0004 mol
Therefore, there are 0.0004 moles of sulfate ions in 100 ml of a solution with a concentration of 0.002 M Fe2(SO4)3.