I'm trying to do a lab, and I need to find the concentration of FeSCN+2 in five solutions based the calibration curve and the absorption. I have a calibration curve, the number of mLs and initial moles of Fe+3 and SCN-, the transmittances, the absorbencies, and the equation. I've tried my textbook, but it doesn't have the topic.
If you have the calibration curve, I assume it is A vs concentration. Choose your A values for the unknown, read the concn from the graph. I don't know how your graph is calibrated; therefore, I don't know the concn units, but you will need to convert that concn you find to the initial values of the unknowns. You know the dilutions you made.I'm sorry to be so vague but you don't have any numbers for me to be more helpful.
This is for a lab about determining the equilibrium constant. Given: 5.00mL of .203M Fe(NO3)3 mixed with 100mL of .00205M KSCN in a .5M HNO3 solvent for both solutions. Resulting absorbance for solution is .315. How can i find the
We did a lab on equilibrium and this is one of the following questions: When Ag ions are added to FeSCN ions (which are red in colour), the colour disappears, and a white precipitate of AgSCN forms. The question is.. Explain why
Hi there, maybe dumb question but how would I find the initial concentration of Fe^3+?? In lab, we mixed these reactants into one test tube: -0.50mL of 0.0025M Fe(NO3)3 -0.50mL of 0.0025M KSCN -2.50mL of 0.10M HNO3 The net ionic
So there's this prelab assignment we're supposed to complete where we would fill out this table with [FeSCN^2+] in each of the test tubes. I'm not completely sure on how to do this? For example, on the first tube calculate the
I have 3 Questions: We actually did the lab experiment for this, but I have no idea whether my reasons are correct. 1) For the equilibrium system Fe+3 + SCN- FeSCN+2, what would happen if you add 2 drops of Fe No3?. Which way will
A student mixes 5 mL of 2.00 x 10^-3 M Fe(NO3)3 with 5 mL 2.00 x 10 ^-3 M KSCN. They find that in the equilibrium mixture concentration of FeSCN^2+ is 1.40 x 10^-4 M. Find each of the following: the initial concentration in
I completed a lab to find the determination of Kc. I have to find the concentrations of reactants at equilibrium using an ICE table. The equation that were are using is Fe^3+(aq) + SCN^-(aq) -> Fe(SCN)^2+(aq) I have to create 5
so i'm trying to finish my lab and im trying to solve for the concentration, and the lab handout says "remember all the cl- from the original sample ended up in 100 mL of solution" The concentration i solved for (from my graph)