<p>A solution is prepared by dissolving 10.5 g ammonium sulfate in enough water to make 150.9 mL of stock solution. A 17.57 mL sample of this stock solution is added to 60.00 mL of water. Calculate the concentration of ammonium ions and sulfate ions in the final solution.</p>
<p>Find the molecular weight of ammonium sulfate by adding up the individual atomic masses of each atom, and find out how many moles 10.5g is equal to. Using Molarity=moles of solute/liters of solution, find out the initial concentration of the stock solution after 150.9 mL are added.
The concentration for that solution will be the same no matter how much of it you take… so use CV=CV… (initial concentration)x(initial volume)=(final concentration)x(final volume).
17.57 mL will be the initial volume, and 60.00 mL plus that will be the final volume.</p>
<p>don’t forget to use the chemical formula to determine the concentration of the specific ions (NH4 & SO4), since that’s what the question asks for.</p>
<p>How exactly do you calculate the initial concentration?</p>
<p>What is the 150.9 ml added to?</p>