The oxidation of 25 mL of a solution containing Fe2+ requires 29 mL of 0.0230 M...
The oxidation of 25 mL of a solution containing Fe2+ requires 29 mL of 0.0230 M K2Cr2O7 in acidic solution. Balance the following equation. Do NOT include the states of each species. Cr2O72− + Fe2+ + H+ → Cr3+ + Fe3+ → Calculate the molar concentration of Fe2+: M
Homework Answers
Answer
0.1601M
Explanation
The balanced chemical equation is
Cr2O72- + 6Fe2+ + 14H+ --------> 2Cr3+ + 6Fe3+ + 7H2O
Stoichiometrically , 1mole of Cr2O72- react with 6moles of Fe2+
Moles of Cr2O72- consumed = (0.0230mol/1000ml) × 29.0ml = 0.000667mol
moles of Fe2+ present in the solution = 6 × 0.000667mol =0.004002mol
Molar concentration of Fe2+ = ( 0.004002mol/25ml ) ×1000ml = 0.1601M
Add Answer to:
The oxidation of 25 mL of a solution containing Fe2+ requires 29
mL of 0.0230 M...
7.41 ml of a solution of Fe2+ (aq) is titrated with 19.3 ml of 0.367 M...
7.41 ml of a solution of Fe2+ (aq) is titrated with 19.3 ml of 0.367 M KMnO4 in acidic solution. The balanced Redox equation is: MnO4 (aq) + 5 Fe2+(aq) + 8 H(aq) --> 5 Fe3+(aq) + Mn2+(aq) + 4 H2O(1) Calculate the concentration, in M, of Fe2(aq) in the sample. Express your answer to the appropriate number of significant figures.
7.83 ml of a solution of Fe2+(aq) is titrated with 24.9 ml of 0.375 M KMnO4...
7.83 ml of a solution of Fe2+(aq) is titrated with 24.9 ml of 0.375 M KMnO4 in acidic solution. The balanced Redox equation is: MnO4 (aq) + 5 Fe2+(aq) + 8 H+(aq) --> 5 Fe3+(aq) + Mn2+(aq) + 4 H2O(1) Calculate the concentration, in M, of Fe2+(aq) in the sample. Express your answer to the appropriate number of significant figures.
• CIU TEXAS INSTRUM 2. A 50.00 ml sample of solution containing Fe?ions is titrated with a 0.0216 M KMnO4 solution....
• CIU TEXAS INSTRUM 2. A 50.00 ml sample of solution containing Fe?ions is titrated with a 0.0216 M KMnO4 solution. It required 20.62 ml of the KMnO4 solution to oxidize all the Fe? ions to Fe ions by the reaction: MnO4 (aq) + Fe? ) -------> Mn(ed) Felco (unbalanced) a) What was the concentration of Fel.ions in the sample solution? b) What volume of 0.0150 M K2Cr2O7 solution would it take to do the same titration? The reaction is:...
A 50.0 g sample of ore containing FeBr2 is dissolved in acid and titrated to an...
A 50.0 g sample of ore containing FeBr2 is dissolved in acid and titrated to an end point with 24.80 mL of 0.629 M Cr2O72−. The following redox reaction takes place: Cr2O72− (aq) + Fe2+ (aq) ⟶ Cr3+ (aq) + Fe3+ (aq) a. balance the reaction b. what % of the ore sample if FeBr2 (molar mass = 215.65 g/mol)
Consider a galvanic cell based in the reaction Fe2. cr02--> Fe3+ + Cr3+ in acidic solution....
Consider a galvanic cell based in the reaction Fe2. cr02--> Fe3+ + Cr3+ in acidic solution. Balance the equation and calculate the voltage of the standard cell carrying out this reaction 3.
The concentration of a Fe2+ solution is determined by titrating it with a 0.1462 M solution...
The concentration of a Fe2+ solution
is determined by titrating it with a 0.1462 M
solution of Ce4+. The balanced net
ionic equation for the reaction is shown below.
Ce4+(aq)
+ Fe2+(aq)
Ce3+(aq)
+ Fe3+(aq)
In one experiment, 16.48 mL of the
0.1462 M Ce4+ solution
is required to react completely with 25.00 mL of
the Fe2+ solution. Calculate the
concentration of the Fe2+ solution.
A sample of an unknown containing Fe2+ in the dissolved sample requires 23.15 mL of a...
A sample of an unknown containing Fe2+ in the dissolved sample requires 23.15 mL of a 0.0020 M KMnO4 solution to reach the end point of the titration. 1)Calculate the moles of KMnO4 reacted. 2) Based on the moles you calculated , calculate how many grams of Fe2+ are in the unknown solution.
A 250.0 mL sample of spring water was treated to convert any iron present to Fe2+...
A 250.0 mL sample of spring water was treated to convert any iron present to Fe2+ . Addition of 24.00 mL of 0.002543 M K2Cr2O7 resulted in the reaction 6Fe2+ + Cr2O7 2- + 14H+ 6Fe3+ + 2Cr3+ + 7H2O The excess K2Cr2O7 was back titrated with 8.02 mL of 0.00971 M Fe2+ solution. Calculate the concentration of iron in the sample in ppm. Please be specific and include details.
A chemist requires a solution of 2.00 M Fe2+ for an experiment. (The Ksp of Fe(OH)2...
A chemist requires a solution of 2.00 M Fe2+ for an experiment. (The Ksp of Fe(OH)2 is 4.9x10-17) a) Will the precipitation of Fe(OH)2 (s) be an issue if the solution is prepared with pure water at 25°C? b) [1 pt] What might the chemist do to prepare this Fe2+ solution to the desired concentration?
1. A solid sample containing some Fe2+ weighs 2.360 g. It required 36.44 mL 0.0244 M...
1. A solid sample containing some Fe2+ weighs 2.360 g. It required 36.44 mL 0.0244 M KMnO, to titrate the Fe- in the dissolved sample to a pink end point. The balanced redox reaction is shown below. 8 H + MnO4 + 5 Fe2+ + Mn2+ + 5 Fe3+ + 4H20 Calculate each of the following quantities. 2. (2 points) Calculate the percentage of Fe in pure iron(II) ammonium sulfate hexahydrate: (NH4)2[Fe(SO4)2]• 6 H20.
7.41 ml of a solution of Fe2+ (aq) is titrated with 19.3 ml of 0.367 M KMnO4 in acidic solution. The balanced Redox equation is: MnO4 (aq) + 5 Fe2+(aq) + 8 H(aq) --> 5 Fe3+(aq) + Mn2+(aq) + 4 H2O(1) Calculate the concentration, in M, of Fe2(aq) in the sample. Express your answer to the appropriate number of significant figures.
7.83 ml of a solution of Fe2+(aq) is titrated with 24.9 ml of 0.375 M KMnO4 in acidic solution. The balanced Redox equation is: MnO4 (aq) + 5 Fe2+(aq) + 8 H+(aq) --> 5 Fe3+(aq) + Mn2+(aq) + 4 H2O(1) Calculate the concentration, in M, of Fe2+(aq) in the sample. Express your answer to the appropriate number of significant figures.
• CIU TEXAS INSTRUM 2. A 50.00 ml sample of solution containing Fe?ions is titrated with a 0.0216 M KMnO4 solution. It required 20.62 ml of the KMnO4 solution to oxidize all the Fe? ions to Fe ions by the reaction: MnO4 (aq) + Fe? ) -------> Mn(ed) Felco (unbalanced) a) What was the concentration of Fel.ions in the sample solution? b) What volume of 0.0150 M K2Cr2O7 solution would it take to do the same titration? The reaction is:...
Consider a galvanic cell based in the reaction Fe2. cr02--> Fe3+ + Cr3+ in acidic solution. Balance the equation and calculate the voltage of the standard cell carrying out this reaction 3.
The concentration of a Fe2+ solution
is determined by titrating it with a 0.1462 M
solution of Ce4+. The balanced net
ionic equation for the reaction is shown below.
Ce4+(aq)
+ Fe2+(aq)
Ce3+(aq)
+ Fe3+(aq)
In one experiment, 16.48 mL of the
0.1462 M Ce4+ solution
is required to react completely with 25.00 mL of
the Fe2+ solution. Calculate the
concentration of the Fe2+ solution.
A chemist requires a solution of 2.00 M Fe2+ for an experiment. (The Ksp of Fe(OH)2 is 4.9x10-17) a) Will the precipitation of Fe(OH)2 (s) be an issue if the solution is prepared with pure water at 25°C? b) [1 pt] What might the chemist do to prepare this Fe2+ solution to the desired concentration?
1. A solid sample containing some Fe2+ weighs 2.360 g. It required 36.44 mL 0.0244 M KMnO, to titrate the Fe- in the dissolved sample to a pink end point. The balanced redox reaction is shown below. 8 H + MnO4 + 5 Fe2+ + Mn2+ + 5 Fe3+ + 4H20 Calculate each of the following quantities. 2. (2 points) Calculate the percentage of Fe in pure iron(II) ammonium sulfate hexahydrate: (NH4)2[Fe(SO4)2]• 6 H20.
Most questions answered within 3 hours.
-
List and compare different forms of passive transport and active
transport.
asked 9 seconds from now -
In Netherland Dwarf rabbits, dwarf size is determined by allele
N, and normal-size by allele n....
asked 6 minutes ago -
During Heaton Company’s first two years of operations, it
reported absorption costing net operating income as...
asked 20 minutes ago -
Consider testing the
hypotheses:
H0: p = 0.56
H1: p > 0.56
where p is
the...
asked 23 minutes ago -
In a two-factor analysis of variance a main effect is defined as
____.
a. the unique...
asked 31 minutes ago -
A bank's loan officer rates applicants for credit. The ratings
are normally distributed with a mean...
asked 31 minutes ago -
Fill in the following information for Adipic Acid: molecular
weight, g or ml, mole, melting point,...
asked 36 minutes ago -
how
to use a for loop to iterate over the string below and print each
character...
asked 38 minutes ago -
Please type answer, Thanks.
Respond to the following in a minimum of 175
words:
Research industry...
asked 38 minutes ago -
Assume that all interest rates in the economy increase from 9
percent to 10 percent. Which...
asked 48 minutes ago -
Describe the function of a Change Control Board.
When calculating Planned Value (PV), what is the...
asked 54 minutes ago -
The customer help center in your company receives calls from
customers who need help with some...
asked 1 hour ago