When 0.016 moles of aluminum sulfate are dissolved in enough water to make 477 milliliters of solution, what is the molarity of sulfate ions?
See this post above.
http://www.jiskha.com/display.cgi?id=1378696606
To find the molarity of sulfate ions, we need to use the given information about the number of moles of aluminum sulfate and the volume of the solution.
First, let's calculate the number of moles of sulfate ions in 0.016 moles of aluminum sulfate. Aluminum sulfate has a chemical formula of Al2(SO4)3, which means for every one mole of Al2(SO4)3, we have three moles of sulfate ions (SO4^2-). So, the number of moles of sulfate ions in 0.016 moles of aluminum sulfate is 3 x 0.016 = 0.048 moles.
Next, we need to convert the volume of the solution from milliliters (ml) to liters (L) because the molarity is defined as moles of solute per liter of solution.
To convert milliliters to liters, we divide the volume by 1000:
477 ml รท 1000 = 0.477 L
Finally, we can calculate the molarity of sulfate ions by dividing the number of moles of sulfate ions by the volume of the solution in liters:
Molarity = Moles of solute / Volume of solution
Molarity of sulfate ions = 0.048 moles / 0.477 L = 0.1006 M (rounded to four decimal places)
Therefore, the molarity of sulfate ions in the solution is approximately 0.1006 M.