chemistry

Iron(II) can be oxidized by an acidic K2Cr2O7 solution according to the net ionic equation.
Cr2O72− + 6 Fe2+ + 14 H+ 2 Cr3+ + 6 Fe3+ + 7 H2O
If it takes 44.0 mL of 0.0250 M K2Cr2O7 to titrate 25.0 mL of a solution containing Fe2+, what is the molar concentration of Fe2+?

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  1. moles Cr2O7^-2 = M x L = ??
    Using the coefficients in the balanced equation, convert moles Cr2O7^-2 to moles Fe(II).
    Then M Fe(II) = moles Fe(II)/L Fe(II)

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  2. 0.156 M Fe2+

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    2. 👎 0
  3. How many moles of molybdenum are in 1.235 g

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