The concentration of a Fe2 solution is determined by titrating it with a 0.1830 M solution of dichromate. The balanced net ionic equation for the reaction is shown below.. Cr₂0, (aq) + 6 Fe (aq)+14 H₂0 (aq) 2 Cr³(aq) + 6 Fe³+ (aq) +21 H₂O(l) In one experiment, 24.88 mL of the 0.1830 M Cr,0,? solution is required to react completely with 20.00 mL of the Fe solution. Calculate the concentration of the Fe? solution.

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Determine an unknown volume or concentration using an oxidation-reduction titration.
The concentration of a Fe2+ solution is determined by titrating it with a 0.1830 M solution of dichromate. The
balanced net ionic equation for the reaction is shown below..
Cr₂0, (aq) + 6 Fe2(aq)+14 H₂0 (aq)-2 Cr³+ (aq) + 6 Fe³+ (aq)+21 H₂0(1)
In one experiment, 24.88 ml. of the 0.1830 M Cr₂0,? solution is required to react completely with 20.00 mL of the
Fe solution. Calculate the concentration of the Fe? solution.
M
Transcribed Image Text:Determine an unknown volume or concentration using an oxidation-reduction titration. The concentration of a Fe2+ solution is determined by titrating it with a 0.1830 M solution of dichromate. The balanced net ionic equation for the reaction is shown below.. Cr₂0, (aq) + 6 Fe2(aq)+14 H₂0 (aq)-2 Cr³+ (aq) + 6 Fe³+ (aq)+21 H₂0(1) In one experiment, 24.88 ml. of the 0.1830 M Cr₂0,? solution is required to react completely with 20.00 mL of the Fe solution. Calculate the concentration of the Fe? solution. M
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