A volume of 12.5 mL of 0.05 M `SeO_(2)` reacts with 25 mL of 0.1 M `CrSO_(4)` which is oxidised to `Cr^(3+)`. To what oxidation state was the selenium converted by the reaction ?

12.53 mL of 0.0509MSeO_(2) reacted with 25.52 mL 0.1M CrSO_(4) solution. In the raeaction Cr^(2+) was oxidised to Cr^(3+) . To what oxidation state selenium was converted in the reaction? Write the redox change for SeO_(2) .

15.0 mL of 0.05 M SeO_2 reacts with 30.6 mL of 0.1 M CrSO_4 solution . If during the reaction CrSO_4 gets oxidised to Cr_2(SO_4)_3 to what oxidation state does selenium get converted ?

Volume of 0.1 M K_(2)Cr_(2)O_(7) required to oxidize 35 mL of 0.5 M FeSO_(4) solution is

Volume of 0.1M K_(2)Cr_(2)O_(7) required to oxidise 35 mL of 0.5M FeSO_(4) solution is