Why is HNO3 added to the Fe(NO3)3 solution used in chemical equilibrium experiment? How does the HNO3 accomplish its function?
HNO3 serves following purposes:
HNO3 accomplishes its function by releasing H+ ions which is the product of equilibrium reaction involved i.e.
Fe3+ + HSCN <-----> Fe(SCN)2+ + 3H+
This prevents formation of more Fe(SCN)2+ and hence, the absorbance remains in measurable range i.e. between 0.8 to 0.3 absorbance units and hence error is minimized.
Why is HNO3 added to the Fe(NO3)3 solution used in chemical equilibrium experiment? How does the...
If NH3 (ammonia, pKb=4.74) is added to a solution of Fe(NO3)3 such that right after the addition we have 50 mL of 5.0 M NH3 and 0.0040 M Fe(NO3)3 (right after addition) Find Kc for Fe2+(aq) + 2OH-(aq) ---> Fe(OH)2 (s) any type of explanation would be helpful please!
15. The pH of a solution of ferric nitrate, Fe(NO3)3, is not 7.00. This fact is best explained by the equation: A) NO3-(aq) + H2O(1) + HNO3(aq) + OH(aq) B) Fe3+(aq) + 6 H2O(1) Fe(OH)3(aq) + 3 H30+(aq) C) [Fe(OH2)6]3+(aq) + H20(1) 3 H3O+(aq) + [Fe(OH2)5(OH)]2+(aq) D) H3O+(aq) + OH-(aq) + 2 H2O(1) E) HNO3(aq) + H2O() H30+(aq) + NO3-(aq)
One drop of 2.5 M KSCN solution is added to 0.5 mL of 0.10 M Fe(NO3)3. After the solution is mixed, 1.0 mL of 0.125 M EDTA solution is added. Enter the chemical formula of the major iron complex in solution after the addition of EDTA
am confused how to start this. for my lab i obtained 24ml of 0.000075M Fe(NO3)3, 40ml of 1M KSCN and 45ml 0f 0.1M HNO3. i was asked to pipet different volumes into 12 testubes. testtube 1....4.00ml Fe(NO3)3, 3.00ml KSCN and 1.00ml HNO3. Calculate the molarity of the complex [Fe(SCN)]^2+ that was present at equilibrium. Am confusing my ideas please help
How do I find the moles of Fe in a .2M solution of Fe(NO3)3?
The actual concentration of the stock [Fe(NO3)3] solution you will use in lab will be posted on D2L. Be sure to record the concentration value matching YOUR lab room and use it in your laboratory worksheet! Consider test tube #5 that you will prepare in Part 1 of the laboratory (Table A). If your dilute solution of Fe(NO3)3 had a concentration of 0.00087 M, predict the initial concentration of the Fe3+ ions, [Fe3+]0 in test tube #5, once you have added...
Part A of lab: pour 30 ml of 0.150 M Fe(NO3)3 into a 50 ml beaker and pipette 10 ml of this solution into a 25 ml volumetric flask. This is the standard reagent blank Part B of lab: pour 30 ml of 1.50*10^-3 M Fe(NO3)3 into a 25 ml volumetric flask. This is the reagent blank. Why is a large excess of Fe3+ added to make the standard solution, and why do you NOT add a large excess of...
What is the chemical reaction of this equilibrium when different stressors are added to the reactants side? Include state Fe3+ + SCN1- ↔ FeSCN2+ 1. Fe(NO3)3 2. NH4NCS 3.AgNO3 4.SnCl2 5. NH3
Fe(NO3)3 (0.00100 mol) and KSCN (0.200 mol) are added to water to make exactly 1 liter of solution. The red complex ion FeSCN2+ is produced. Calculate the concentrations of Fe3+(aq) and FeSCN2+(aq) at equilibrium, if Kf of the FeSCN2+ is 8.9 × 102.
a student accidentally switches the set of KSCN and Fe(NO3)3/HNO3 solutions between part 1 and part 2 so that there is excess of Iron(III) in Part II (equilibrium solutions) instead of in Part I (standard solutions). Will his standard curve equation describe accurately the relation between the absorbance and the colored complex? Will the equilibrium constants be reliable? Rationalize your answers.