College Level Chemistry Problem
Posted: Mon Nov 10, 2008 5:30 pm
Hi- I was wondering if someone could help me solve this pre-lab question because i cant even get the balanced equation to do the IRE table.
Heres the question:
At a temperature significantly different than room temperature a solution was prepared by pipetting 10.00mL of 1.98 * 10 ^(-3) M Fe(NO3)3 solution (in 0.1 M nitric acid) and 4.00mL of 1.98 * 10 ^(-3) M NaSCN solution (in 0.1 M nitric acid) into a 25mL volumetric flask and filling to the mark with deionized water. calculate the equilibrium constant for this reaction at this temperature given that the equilibrium concentration of FeSCN2+ was found to be 1.03 * 10 ^(-4) M. ( Note: the answer is 700)
If anyone could help me solve this i will be forever grateful! thanks!
-sam
Heres the question:
At a temperature significantly different than room temperature a solution was prepared by pipetting 10.00mL of 1.98 * 10 ^(-3) M Fe(NO3)3 solution (in 0.1 M nitric acid) and 4.00mL of 1.98 * 10 ^(-3) M NaSCN solution (in 0.1 M nitric acid) into a 25mL volumetric flask and filling to the mark with deionized water. calculate the equilibrium constant for this reaction at this temperature given that the equilibrium concentration of FeSCN2+ was found to be 1.03 * 10 ^(-4) M. ( Note: the answer is 700)
If anyone could help me solve this i will be forever grateful! thanks!
-sam