Determine the sulfate ion concentration in a solution prepared by diluting 15.00mL of a 0.200M aluminum sulfate solution with 35.00mL of water. Assume the volumes are additive.

[Al2(SO4)3] = 0.200M x (15.00/50.00) = ?

Then [SO4^2-] = 3x that.

To determine the sulfate ion concentration in the final solution, we need to use the concept of dilution. Dilution is a process in which a solution of higher concentration is diluted with a solvent (in this case, water) to reduce the concentration.

First, let's calculate the number of moles of aluminum sulfate in the 15.00 mL of the original solution:
Number of moles = concentration × volume
Number of moles of aluminum sulfate = 0.200 M × 0.01500 L
Number of moles of aluminum sulfate = 0.003 moles

Since aluminum sulfate has a 1:1 ratio with sulfate ions, the number of moles of sulfate ions is also 0.003 moles.

Now, we need to calculate the volume of the final solution. Since the volumes of the original solution and water are additive, the total volume of the final solution is:
Total volume = volume of original solution + volume of water
Total volume = 15.00 mL + 35.00 mL
Total volume = 50.00 mL

Next, we calculate the concentration of sulfate ions in the final solution:
Concentration = moles/volume
Concentration of sulfate ions = 0.003 moles / 0.05000 L
Concentration of sulfate ions = 0.060 M

Therefore, the sulfate ion concentration in the final solution is 0.060 M.