I would really appreciate some help in confirming a value computed in a prelab problem to be used in a lab for analytical chemistry! We're working on redox reactions and are looking at the reaction: Fe2+ + K2Cr2O7 + H+ = Fe3+ + K+ + Cr3+ + H2O The final questions asks, "calculate the amount of unknown sample needed to achieve about a 25.00 mL titration volume of 0.01600 M K2Cr2O7 if the %Fe of the unknown is approximately 8%. Make sure to use the coefficients from the balanced reaction" I have found the balanced equation; however, I was hoping to be able to confirm my values! Thank you in advance!
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I would really appreciate some help in confirming a value computed in a prelab problem to be used in a lab for
Fe2+ + K2Cr2O7 + H+ = Fe3+ + K+ + Cr3+ + H2O
The final questions asks,
"calculate the amount of unknown sample needed to achieve about a 25.00 mL titration volume of 0.01600 M K2Cr2O7 if the %Fe of the unknown is approximately 8%. Make sure to use the coefficients from the balanced reaction"
I have found the balanced equation; however, I was hoping to be able to confirm my values! Thank you in advance!
Given that the percent of Fe in the unknown sample is 8% and the unknown sample should consume 25.00 mL of 0.01600 M K2Cr2O7 in the titration.
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