A student mixes 5.00 mL of 2.00 x 10-3 M Fe(NO3)3, 4.00 mL of 2.00 x 10-3 M KSCN, and 1.00 mL of distilled water to form the complex ion FeSCN2+. The solution is left to reach equilibrium. The equilibrium concentration of FeSCN2+ was found to be 1.31 x 10-4 M.
Calculate the initial concentration for Fe3+ at the start of reaction (that is, the concentration after all ingredients are added together).
1.00 x 10-3 M
2.00 x 10-3 M
1.11 x 10-3 M
4.00 x 10-3 M
A student mixes 5.00 mL of 2.00 x 10-3 M Fe(NO3)3, 4.00 mL of 2.00 x 10-3 M KSCN, and 1.00 mL of distilled water to form the complex ion FeSCN2+. The solution is left to reach equilibrium. The equilibrium concentration of FeSCN2+ was found to be 1.31 x 10-4 M.
Calculate the initial concentration for SCN- at the start of reaction (that is, the concentration after all ingredients are added together).
A student mixes 5.00 mL of 2.00 x 10-3 M Fe(NO3)3, 4.00 mL of 2.00 x 10-3 M KSCN, and 1.00 mL of distilled water to form the complex ion FeSCN2+. The solution is left to reach equilibrium. The equilibrium concentration of FeSCN2+ was found to be 1.31 x 10-4 M.
Calculate the concentration for Fe3+ used up in making FeSCN2+.
8.00 x 10-4 M
1.31 x 10-4 M
1.00 x 10-3 M
1.31 x 10-5 M