Chemistry help please?
Sorry, I really do not know how to do net ionic equations so I thought I could turn to you basilers for help.
-You created a standard solution where you dissolve 28.00 g of iron (III) sulfate in enough water to create a 350.0 mL solution.
a.) Create a balanced equation showing the dissociation of iron (III) sulfate into ions (consider the compound to be aqueous when dissociating).
b.)Determine the moles of iron (III) sulfate dissolved, and then determine the number of moles of each ion created.
c.) Determine the molarity of iron (III) sulfate, and then determine the molarities of each ion.
Also, can you guys explain it step by step how to do it? I'm really lost..
January 26, 2011
1 Comment • Newest first
A. Sulfur has a charge of 2-. The LCM of 2 and 3 is 6, so the number of Fe (III) and S in iron III sulfate must amount to +/- 6. 6/3=2, so that's 2 Fe (III), and 6/2=3, so that's 3 S.
So you end up with:
Fe2S3=>2 Fe (3+) and 3 S (2-)
B. Turn 28.00 g into moles using the periodic table.
C. Answer of b/0.350 L, since for molarity, the denominator must always be in L.