ZuoTi.Pro
Question

A 25.0 mL volume of 0.0200 M Fe(NO3)3 is mixed with 50.0 mL of 0.00200 M...

A 25.0 mL volume of 0.0200 M Fe(NO3)3 is mixed with 50.0 mL of 0.00200 M NaSCN and 25.0 mL of 0.100 HNO3. The blood-red FeSCN2+ ion forms and the equilibrium is established:

Fe3+(aq) + SCN-(aq) <---> FeSCN2+(aq)

The equilibrium concentration of FeSCN2+ ([FeSCN2+]) was measured spectrophotometrically and found to be 7.0 x 10-4 mol/L. To calculate the equilibrium constant (Kc) for thr equilibrium system, proceed through the following steps:

A. Moles of Fe3+, initial

B. Moles of SCN-, initial

C. Moles of FeSCN2+, at equilibrium

D. Moles of Fe3+, reacted

E. Moles of SCN-, reacted

F. Moles of unreacted Fe3+ (A - D)

G. Moles of unreacted SCN- (B - E)

H. [Fe3+] at equilibrium

I. [SCN-] at equilibrium

J. [FeSCN2+] at equilibrium

K. Kc of FeSCN2+

Please and thank you!

science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

0 0
Add a comment
Know the answer?
Add Answer to:
A 25.0 mL volume of 0.0200 M Fe(NO3)3 is mixed with 50.0 mL of 0.00200 M...
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for? Ask your own homework help question. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions

  • 4.81 mL of 0.00200 M Fe(NO3)3, 2.85 mL of 0.00200 M KSCN and 2.34 mL of...

    4.81 mL of 0.00200 M Fe(NO3)3, 2.85 mL of 0.00200 M KSCN and 2.34 mL of distilled water were mixed. The resulting solution was allowed to attain equilibrium at 24 oC. The absorbance of the equilibrium solution was recorded, and the [FeSCN2+] was determined graphically to be 7.58 x 10-5 M. Part A: Calculate the number of moles of Fe3+ initially added to the solution. Part B: Calculate the number of moles of FeSCN2+ formed in the solution at equilibrium....

  • 4. When 5.00 mL of 0.500 M Fe (NO3)3 are mixed with 5.00 mL of 0.250...

    4. When 5.00 mL of 0.500 M Fe (NO3)3 are mixed with 5.00 mL of 0.250 M NaSCN, the following reaction occurs: Fe3+ (aq) + SCN(aq) $ FeSCN2+(aq) At equilibrium the concentration of FeSCN2- is found to be 6.00 x 10-2 M. A. Fill in the table below with the proper numerical values. (Remember to take into account the effects of dilution when calculating the initial molarity of Fe3+ (aq) and SCN'(aq) Fes- (aq) SCN (aq) FeSCN-(aq) Initial Molarity Change...

  • Consider the following: A student mixes 5.00 mL 2.00 × 10−3 M Fe(NO3)3 with 3.00 mL...

    Consider the following: A student mixes 5.00 mL 2.00 × 10−3 M Fe(NO3)3 with 3.00 mL 2.00 × 10−3 M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN2+ is 1.28 × 10−4 M. Find Kc for the reaction Fe3+(aq) + SCN−(aq) ↔ FeSCN2+(aq). a. What is the initial concentration of Fe3+ in the reaction mixture? [Fe3+] = ___ x 10-3 M b. What is the initial concentration of SCN- in the reaction mixture? [SCN-] = ___...

  • Determination of an Equilibrium Constant 1) If 20.0 mL of 0.00200 M Fe(No3)3 is diluted to...

    Determination of an Equilibrium Constant 1) If 20.0 mL of 0.00200 M Fe(No3)3 is diluted to 50.0 mL, what is the concentration of Fe^+3 in the diluted solution? 2) Write the equilibrium for the following reaction. Co^+2 +4SCN^-1 <--> Co(SCN)4 ^-2 3) How many mmoles of SCN^-1 ion are there in 3.0 mL of 0.00200 M KSCN?

  • For the reaction Fe3+ + SCN 1- FeSCN2+ 9.00 mL of 0.00800M Fe(NO3)3 were diluted to...

    For the reaction Fe3+ + SCN 1- FeSCN2+ 9.00 mL of 0.00800M Fe(NO3)3 were diluted to a volume of 450.0 ml, then... 4.00 mL of the diluted Fe(NO3)3 were mixed with 4.00 mL of KSCN and 4.00 mL of HNO3. Calculate the initial concentration of Fe3+ at the time of mixing. Short answer LE- _ (no extra Scientific notation format spaces) How many mL of 0.00200 M Fe(NO3)3 are required to prepared 12.50 mL total volume with a concentration of...

  • Beers law solve for E3 and E4 showing work Part II. Equilibrium Constant Calculations Calculate the...

    Beers law solve for E3 and E4 showing work Part II. Equilibrium Constant Calculations Calculate the initial moles of Fe3+ and SCN- for solutions E2 through E6 and record these values in the table on your Data Sheet. You obtain the moles of the reactants by multiplying their molarity by the volume (in L) of their solution used. Determine the equilibrium concentration of FeSCN2+ for each of the solutions E2-E6 from your Beer’s Law plot. Using these equilibrium concentrations, the...

  • A student mixes 5.00 mL 4.00 x 10-3 M Fe(NO3)3 with 5.00 mL 4.00 x 10-3 M KSCN.

    A student mixes 5.00 mL 4.00 x 10-3 M Fe(NO3)3 with 5.00 mL 4.00 x 10-3 M KSCN. The student finds that the equilibrium concentration of FeSCN2+ is 5.6 x 10-4M. a. Set up the Kc expression for the following equation. Fe3+ + SCN-  ↔ FeSCN2+b. What is the total volume of the solution? _______ mL c. Fill in the following table for the moles of each species.d. Find the concentration for the above ions. e. Calculate Kc for the reaction.

  • 5.00 mL of 5.00 × 10-1M Fe(NO3)3 are mixed with 2.00 mL of 1.00 x 10-4M NASCN and 3.00 mL of 0.5M HNO3

    5.00 mL of 5.00 × 10-1M Fe(NO3)3 are mixed with 2.00 mL of 1.00 x 10-4M NASCN and 3.00 mL of 0.5M HNO3. A. Calculate the molarity of the Fe3+ in the diluted solution. B. Calculate the molarity of the SCN in the diluted solution. C. Assume that the following reaction goes to completion: Calculate the molarity of the FeSCN2+ in the diluted solution.

  • A mixture is prepared by combining 10.20 mL of 1.80 x 10-3 M Fe(NO3)3 with 10.00...

    A mixture is prepared by combining 10.20 mL of 1.80 x 10-3 M Fe(NO3)3 with 10.00 mL of 1.68 x 10-3 M KSCN. The solution turns red due to the formation of FeSCN2+. The absorbance is measured and, using a calibration plot, the [FeSCN2+] at equilibrium is found to be 2.20 x 10-4 M. Complete the following ICE table Fe3+   + SCN-     ⇌ FeSCN2+ initial (M) (A) (B) (C) change (M) (D) (E) (F) equilibrium (M) (G) (H) (I) What...

  • Prelab Question 12 (modified): If 5.00 mL of 0.00200 M Fe(NO3)3is mixed with 3.00 mL of...

    Prelab Question 12 (modified): If 5.00 mL of 0.00200 M Fe(NO3)3is mixed with 3.00 mL of 0.00200 M KSCN, calculate the initial concentration of Fe3+ and SCN1-in the solution.

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT