ZuoTi.Pro
Question

1801. -- + Fe — ortho-phenanthroline Ferrous tris-o-phenanthroline |Calculate the amount of Iron(II) sulfate and the amount of phenanthroline that needs to be weighed out and added to 100 mL of deionised water to make a stock solution of the iron-phenanthroline complex which has an iron concentration of 150 mg/L. Show your workings.

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

Homework Answers

Answer #1

Molar mass of Phenanthroline = 180.21 g/mol ( 1₂ HqN2. 3 henanthro Phenanthroline & Fe 2+ Complex . Conc-of the 2t in complexNow, using Reaction : mole of Phenanthroline = 3x mole of feet - 3x 15 x 10 3 56 mass of Phananthro line = 3x15 x 10 x 180 2

0 0
Add a comment
Know the answer?
Add Answer to:
Calculate the amount of Iron(II) sulfate and the amount of phenanthroline that needs to be weighed...
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

  • An unknown solution containing iron at a concentration between 10 and 50 mg/L is now to...

    An unknown solution containing iron at a concentration between 10 and 50 mg/L is now to be analyzed. 25 mL of this unknown solution is diluted to 250 mL with the appropriate reagents to form the ferrous - phenanthroline complex. The diluted solution has an absorption of 0.795. What is the concentration in (mg/L) of ferrous ion in the diluted solution? Enter a numeric answer only, do not include units with your answer. part 2 ) What is the concentration...

  • Can you answer question 4 & 5? The experiment and porcedure is posted below Question 4...

    Can you answer question 4 & 5? The experiment and porcedure is posted below Question 4 & 5 CHM3120C Analytical Chemistry Lab Lab 7. Spectrophotometric Determination of Iron in Mohr's Salt with o-Phenanthroline Required Reagents and Supplies: 50 mL of 0.0005M -0.0006 M of Mohr's solution (unknown), 10 g of Hydroxylamine hydrochloride (NH2OH, HCI), 500 mL of o-phenanthroline solution (contains 0.5 g of o-phenanthroline monohydrate), 83 g of sodium acetate (NaOAc. 3H20) in 500 mL of water (for 1.2 M...

  • 1. When iron(II) ammonium sulfate is dissolved in water, it dissociates into its component ions. ()...

    1. When iron(II) ammonium sulfate is dissolved in water, it dissociates into its component ions. () → () + ( ) + ( ) 2. When oxalic acid is added, the iron (II) ions precipitate as iron(II) oxalate dihydrate. Fe2+ (aq) + (aq) + __H20 (1) ► ( ) + _ H(aq) 3. Next, potassium oxalate is added to the washed precipitate. Potassium oxalate dissociates into its ions in solution. At high oxalate concentrations, iron (II) oxalate combines with another...

  • A solution of iron (II) sulfate was prepared by dissolving 10.00g of FeSO4-7H20 (FW= 277.9) in...

    A solution of iron (II) sulfate was prepared by dissolving 10.00g of FeSO4-7H20 (FW= 277.9) in water and diluting up to a total volume of 250 ml. The solution was left to stand, exposed to air, and some of the iron (II) ions became oxidized to Iron (III) ions. a 25.0 ml sample of this partially oxidized solution required 23.70 ml of 0.0100M potassium dichromate K2Cr2O7 solution for complete reaction in the presence of dilute sulfuric acid. Calculate the percentage...

  • THE DETERMINATION OF IRON BY SPECTROPHOTOMETRY INTRODUCTION In this experiment, the red-orange colored complex formed between...

    THE DETERMINATION OF IRON BY SPECTROPHOTOMETRY INTRODUCTION In this experiment, the red-orange colored complex formed between iron(II) and 1,10- phenanthroline (Eqn.) is used in determination of iron by spectrophotometry. Fe+3PhenH Fe(Phen)2 +3H red-orange (A 512 nm) An excess of reducing reagent, such as hydroxylamine or hydroquinone, is often used to reduce and maintain iron in +2 oxidation state. The complex, once formed, is very stable, and can be stored for a long time. Required Reading: Skoog and West (9E): Chapter...

  • Iron tablets may be used in the treatment of anaemia. To analyse the iron(II) content of...

    Iron tablets may be used in the treatment of anaemia. To analyse the iron(II) content of commercially available iron tablets, a student used four tablets, each of mass 0.360 g to make up 250 mL of solution in a volumetric flask using dilute sulfuric acid and deionized water. About 15.0 mL of dilute sulfuric acid was added to a 25.0 mL portion of this iron(II) solution and the mixture then titrated with a 0.01025 M solution of potassium manganite(VII), KMnO4....

  • (10 pts) The iron content of a well water sample is determined by UV-Vis spectroscopy. A...

    (10 pts) The iron content of a well water sample is determined by UV-Vis spectroscopy. A 10.00 mL aliquot of well water is transferred to a 100.0-mL volumetric flask and 20 mL of 0.10 M nitric acid is added to oxidize iron (II) to iron (II). Next 30 mL of a 0.1 M sodium thiocyanate solution is added to form the deep red complex iron (II) thiocyanate. The solution is diluted to volume with DI water. A reagent blank is...

  • 2) ( ) An acidic potassium dichromate can be used to titrate a solution of iron(II)...

    2) ( ) An acidic potassium dichromate can be used to titrate a solution of iron(II) ions since it reacts according to the following equation: Cr2O72 (aq) +6 Fe* (aq) +14 H30' (aq) - 2 Cr* (aq) + 6 Fe" (aq) + 21 H20 (1) a. What is the oxidizing agent in the above reaction? b. A dichromate stock solution is made by dissolving 2.567 g of K Cr2O, (294.2 g/mol) in a total of 50.0 ml. What is the...

  • calculate the concentration of iron in a solution prepared by diluting 10 mL of 240 mg...

    calculate the concentration of iron in a solution prepared by diluting 10 mL of 240 mg Fe/L solution to 100 mL

  • used to titrate a solution of iron(II) ions., with which it reacts according to Cerium(IV) sulfate...

    used to titrate a solution of iron(II) ions., with which it reacts according to Cerium(IV) sulfate Ce4(aq)Fe2 (aq)>Ce3*(aq) + Fe3 (aq) A cerium(IV) sulfate solution is prepared by dissolving 40.47 g of Ce(SO42 in water and diluting to a total volume of 1.000 L. A total of 19.41 mL of this solution is required to reach the endpoint in a titration of a 100.0-mL sample containing Fe(aq). Determine the concentration of Fe2 in the original solution It is desired precipitate,...

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