A level Chemistry help
Hi I have just met a question asking
by reading the standard electrode potentials, explain, by reference to the data given in the table opposite, why i) HCl ii)HNO2 should not be used to acidify the solution containg iron(II) ions
so the iron(II) ions after acidification is titrated with a standard solution of potassium mangante(VII)
potentials:
MnO4- + 8H+ +5e- => Mn2+ + 4H2O : +1.51
Cl2 + 2e- => 2Cl- :+1.36
NO3- + 3H+ + 2e- => HNO2 + H2O :+0.94
Fe3+ + e- => Fe2+ : +0.77
Model ans:
i) as MnO4- has E/V > Cl-, Cl- will be oxidised
ii)as NO3- has E/V > Fe2+, Fe2+ will be oxidised
So both Cl and NO3 are lower than MnO4, and both are higher than Fe2+
does it matter which answer I put in either question
by reading the standard electrode potentials, explain, by reference to the data given in the table opposite, why i) HCl ii)HNO2 should not be used to acidify the solution containg iron(II) ions
so the iron(II) ions after acidification is titrated with a standard solution of potassium mangante(VII)
potentials:
MnO4- + 8H+ +5e- => Mn2+ + 4H2O : +1.51
Cl2 + 2e- => 2Cl- :+1.36
NO3- + 3H+ + 2e- => HNO2 + H2O :+0.94
Fe3+ + e- => Fe2+ : +0.77
Model ans:
i) as MnO4- has E/V > Cl-, Cl- will be oxidised
ii)as NO3- has E/V > Fe2+, Fe2+ will be oxidised
So both Cl and NO3 are lower than MnO4, and both are higher than Fe2+
does it matter which answer I put in either question
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