In `Fe(II)-MnO_4^-` titration, `HNO_3` is not used because :

In Fe(II) - MnO_(4)^(-) "tirtration" HNO_(3) is not used beacause:

Conc. HNO_3 stains wood yellow because.

In the titration of NaHCO_(3) with HCl, indicator cannot be used

In a titration, H_(2)O_(2) is oxidised to O_(2) by MnO_(4)^(-) . 24 mL of 0.1M H_(2)O_(2) requires 16 mL of 0.1M MnO_(4)^(-) solution. Hence MnO_(4)^(-) changes to :

During titration H_2SO_4 is preferably used over HCl and HNO_3 to make the solution acidic because

In the permanganate titration, the solution of reductant is always made acidic by adding H_(2)So_(4) rather than HCl or HNO_(3) because :

A solution containing 2.7 xx 10^-3 mol of A^(2+) irons required 1.6 xx 10^(-3) mole of MnO_4^- for the oxidation of A^(2+) to AO_3^- the medium used is :

In Iodometric titration which indicator is used to detect end point of titration reaction?

[Cu(NH_3)_4]^(+2) reacts with HNO_3 in excess of water gives :

A 4.0 g sample contained Fe_2O_3,Fe_3O_4 , and inert material. It was treated with an excess of aq KI solution in acidic medium, which reduced all iron to Fe^(2+) ions along with the liberation of iodine . The resulting solution was diluted to 50 mL and a 10 mL sample of it was taken the iodine liberated in the small sample was titrated with 12.0 " mL of " 0.5 M Na_2S_2O_3 solution. The iodine from another 25 mL was extracted, after which the Fe^(2+) ions were titrated with 16 " mL of " 0.25 M MnO_4^(ɵ) ions in H_2SO_4 solution. Calculate the mass of two oxides in the original mixture.