Question

What is the maximum concentration of Fe3+ in a solution that contains 0.010 M K3[Fe(C2O4)3] and...

What is the maximum concentration of Fe3+ in a solution that contains 0.010 M K3[Fe(C2O4)3] and 0.010 M C2O42−?

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

[Fe(C2O4)3]3-(aq) ⇌ Fe3+(aq) + 3 C2O42-(aq)

[Fe(C2O4)3]3- on dissociation forms 1 mole of Fe3+ and 3 mol C2O42-.

So, 0.010 M of [Fe(C2O4)3]3- on dissociation forms 0.010 M of Fe3+ and 3 x 0.010=0.030 M C2O42-.

But our problem given C2O42- is 0.010 M

Total C2O42-= 0.010M +0.030M=0.040M

Mixture contains only 0.010 M of Fe3+.

Essentially all of the Fe+3 reacts to form an equal amount of [Fe(C2O4)3]3-(aq).
so
0.010 M Fe3+ forms 0.010 M [Fe(C2O4)3]3-(aq).

Maximum concentration of Fe3+ in a solution 0.010M

0 0
Know the answer?
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
Similar Questions
2) The dissociation constant for Fe(enterobactin)]3- at high pH is 10-49 M, a) Calculate the concentration...
2) The dissociation constant for Fe(enterobactin)]3- at high pH is 10-49 M, a) Calculate the concentration of free Fe3+ in a 10 µM solution of Fe(enterobactin)]3-. b) How many free iron ions are present in 1 L of such a solution?  
What is the cell potential for the spontaneous concentration cell with the reaction Fe3+(aq) + Fe(s)...
What is the cell potential for the spontaneous concentration cell with the reaction Fe3+(aq) + Fe(s) → Fe(s) + Fe3+(aq), with concentrations of Fe3+ of 0.873M and 0.342M at a temperature of 310. K? Ecell = E°cell −(RT/nF)lnQ
When 50.0 mL of a 1.00 M solution of Fe(NO3)3 are mixed with 50.0mL of a...
When 50.0 mL of a 1.00 M solution of Fe(NO3)3 are mixed with 50.0mL of a 1.00 M solution of NaOH, a precipitate forms. What Ions remain after the reaction is complete? Fe(NO3)3 (aq) + 3 NaOH (aq) -> Fe(OH)3 (s) + 3 NaNO3 (aq) A. Fe3+, OH-, Na+, and NO3- B. Fe3+ and OH- C. Na+ and NO3- D. Fe3+, Na+, and OH-
Taking the activity coefficient effect into consideration, calculate the concentration of Fe3+ in a solution that...
Taking the activity coefficient effect into consideration, calculate the concentration of Fe3+ in a solution that is saturated with Fe4[Fe(CN6]3 (Iron(III) ferrocyanide). The overall ionic strength of the solution is .01 M. Iron(III) ferrocyanide Ksp = 3.3*10-41. The answer starts with 5.90... please show ALL steps
Q1) Kf([Fe(SCN)]2+)=8.9*102. What is the equilibrium concentration of Fe3+ if the initial concentrations are [Fe3+]=2.0M, [SCN-]=2.5M,...
Q1) Kf([Fe(SCN)]2+)=8.9*102. What is the equilibrium concentration of Fe3+ if the initial concentrations are [Fe3+]=2.0M, [SCN-]=2.5M, and [Fe(SCN)-]=0M? Answer in M. Do NOT use scientific notation! Q2)25.00mL of 0.2104M acetic acid (HAc) with Ka=1.8*10-5 is titrated with 0.2000M KOH. What is the pH after 15mL of KOH is added? Do NOT use scientific notation!
What is the pH of 0.0800 M Fe(NO3)3 (Ka of Fe3+ = 3.00x10-3)? Express your answer...
What is the pH of 0.0800 M Fe(NO3)3 (Ka of Fe3+ = 3.00x10-3)? Express your answer to two decimal places.
1) A student mixes 5.00 mL of 2.00 x 10-3 M Fe(NO3)3 with 5.00 mL of...
1) A student mixes 5.00 mL of 2.00 x 10-3 M Fe(NO3)3 with 5.00 mL of 2.00 x 10-3 M KSCN. She finds that in the equilibrium mixture the concentration of FeSCN2+ is 1.40 x 10-4 M a) What is the initial concentration in solution of the Fe3+ and SCN- ? b) What is the equilibrium constant for the reaction? 2. Assume that the reaction studied is actually: Fe3+ (aq) + 2 SCN- (aq) ↔ Fe(SCN)2+ (aq) a) What is...
What is the equilibrium Fe3+ concentration when 2.65 L of a 0.149 M iron(III) chloride solution...
What is the equilibrium Fe3+ concentration when 2.65 L of a 0.149 M iron(III) chloride solution are mixed with 2.51 L of a 0.434 M potassium sulfide solution?
A solution contains 0.010 M Ba2+ and 0.010 M Ag+. If we add chromate (CrO42-) to...
A solution contains 0.010 M Ba2+ and 0.010 M Ag+. If we add chromate (CrO42-) to the solution: Which ion starts to precipitate first? Can 99.90% of either ion be precipitated by chromate without precipitating the other metal ion? pKsp BaCrO4 = 9.67, pKsp Ag2CrO4=11.92
Calculate the pre-equilibrium concentration of Fe3+(aq) in a solution made by mixing 1.7 mL of 2.0 ...
Calculate the pre-equilibrium concentration of Fe3+(aq) in a solution made by mixing 1.7 mL of 2.0 ✕ 10−3 M Fe(NO3)3 and 8.3 mL of 2.0 ✕ 10−3 M NaSCN. Assume the final volume is 10.0 mL. i wasnt suere on whether i should compose an ice table for this problem? An explaination of this problem through a solution would be helpful.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT