Question
Suppose 0.432g of zinc acetate is dissolved in 200.mL of a 16.0mM aqueous solution of ammonium sulfate.
Calculate the final molarity of acetate anion in the solution. You can assume the volume of the solution doesn't change when the zinc acetate is dissolved in it.
Calculate the final molarity of acetate anion in the solution. You can assume the volume of the solution doesn't change when the zinc acetate is dissolved in it.
Answers
DrBob222
Zn(C2H3O2)2 = Zn(Ac)2
0.432 g Zn(Ac)2/mol mass = moles Zn(Ac)2
mols Ac^- = 2 x moles Zn(Ac)2
M Ac^- = mols Ac^-/L soln.
0.432 g Zn(Ac)2/mol mass = moles Zn(Ac)2
mols Ac^- = 2 x moles Zn(Ac)2
M Ac^- = mols Ac^-/L soln.