24.3cm3 of 0.02M KMnO4 reacted with 20.0cm3 of an iron(ii)solution
a) given the half ionic equations:
MnO4^-1 (aq) + 8H ^1+(aq) + 5e gives you Mn^2+ (aq) + 4H2O (L)
Fe^2+ (aq) -2e give you Fe^3+ (aq)
write a balanced equation for the reaction that takes place
b)determine:
i) number of moles of KMnO4 used
ii) number of moles of iron(ii) used
iii) concentration of iron(ii)solution in moles per litre
please explain detailed, step by step, the way a 17 year old would understand 🙂
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