Question

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: 

image.png


Calculate the molarity of the FeSCN2+ in the diluted solution.

2 0
Add a comment Improve this question Transcribed image text
Answer #1

Q-3 ( a ) Molarity of Fe3+

Millimole of Fe3+ = Molarity x volume ( mL ) = 0.5 M x 5 mL = 2.5 millimole

total volume = 5+2+3 = 10 mL

molarity in dilute solution = millimole of Fe3+ / total volume in mL = 2.5 Millimole/ 10 mL = 0.25 M

( b ) Molarity of SCN-

  = 2 x 10-4 millimole/ 10 mL = 2 x 10-5 M

( c ) Molarity of FeSCN2+

since SCN- is limiting reagent it will consume completely in reaction and same mole of FeSCN2+ will produce so Molarity of SCN- and FeSCN2+ will be same

[ FeSCN2+ ] = 2 x 10-5 M


Add a comment
Know the answer?
Add Answer to:
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
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

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. 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-] = ___...

  • Use the following procedure for answering questions given below: 3.00 mL of 2.00 x 10' M...

    Use the following procedure for answering questions given below: 3.00 mL of 2.00 x 10' M solution of Fe(NO3)3 was mixed with 4.00 mL of 2.5 x 10-3 M solution of KSCN and 1.00 mL of 0.5M HNO3. After equilibrium: Fe3+ + SCN FeSCN2+ = was established the equilibrium concentration of FeSCN2+ ions was read from the calibration curve as 5.00 x 10-4 M. 01. The initial concentration of Fe3+ ions (assuming no reaction took place) was: [20] a) 1.00...

  • 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.

  • 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...

  • 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...

  • 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.

  • A student mixes 5.00 mL of 2.00 times 10^-3 M Fe(NO_3)_3 with 5.00 mL of 2.00...

    A student mixes 5.00 mL of 2.00 times 10^-3 M Fe(NO_3)_3 with 5.00 mL of 2.00 times 10^-3 M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN2^+ is 1.40 times 10^-4 M. a) What is the initial concentration in solution of the Fe^3+ and SCN^-? b) What is the equilibrium constant for the reaction?

  • 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....

  • A student mixes 5.12 mL of 4.02 x 10 M Fe(NO3)3 with 4.88 mL 2.01 x...

    A student mixes 5.12 mL of 4.02 x 10 M Fe(NO3)3 with 4.88 mL 2.01 x 103 M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN2 is 1.40 x 10 M. 1. What is the initial concentration in solution of the Fe3 and SCN'? What is the equilibrium constant for the reaction? What happened to the K' and the NO3 ions in this solution? a. b. C. A student mixes 5.12 mL of 4.02 x 10...

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