Iron in the +2 oxidation state reacts with potassium dichromate toproduce Fe 3+

Question

Iron in the +2 oxidation state reacts with potassium dichromate toproduce Fe3+ and Cr3+ according to theequation 6Fe2+ +Cr2O72- + 14H+ 6Fe3+ + 2Cr3+ + 7H2O. How manymilliliters of 0.1658 M K2Cr2O7are required to titrate 200.0 mL of 0.2500 M Fe2+solution? Iron in the +2 oxidation state reacts with potassium dichromate toproduce Fe3+ and Cr3+ according to theequation 6Fe2+ +Cr2O72- + 14H+ 6Fe3+ + 2Cr3+ + 7H2O. How manymilliliters of 0.1658 M K2Cr2O7are required to titrate 200.0 mL of 0.2500 M Fe2+solution?

Explanation / Answer

6Fe2+ + Cr2O72- +14H+ 6Fe3+ + 2Cr3+ +7H2O No . of moles of Fe 2+ is = Molarity * Volume in L                                       = 0.25 * 0.2                                        =0.05 moles According to the Equation 1 mole ofK2Cr2O7 requires 6 moles of Fe 2+solution                                      X mole of K2Cr2O7requires 0.05 moles of Fe 2+ solution X = ( 0.05 * 1 ) / 6     = 0.0083 moles of K2Cr2O7 No . of moles = Molarity * Volume in L Volume in L = No . of moles / Molarity                    = 0.0083 / 0.1658                    = 0.05026 L Volume in mL = 50.26 mL

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