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)
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+?
3 answers
0.156 M Fe2+
How many moles of molybdenum are in 1.235 g
1 answer