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12.53 ml of 0...

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12.53 ml of 0.051 M SeO2 reacted with 25.52 ml of 0.1M CrSO4 solution. In the reaction Cr+2 was oxidised to Cr+3 . The oxidation state at which selenium was converted is

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Q. 12.53 mL of 0.0509 M

S e O_{2}

reacted with 25.52 mL 0.1 M

C r S O_{4}

solution. In the reaction

C r^{2 +}

was oxidized to

C r^{3 +}

. To what oxidation state selenium was converted in the reaction? Write the redox change for

S e O_{2}

Q. 12.5 ml of 0.05 M

S e O_{2}

reacts with 25 ml of 0.1 M

C r S O_{4}

which is oxidised to

C r^{3 +}

. To what oxidation state was the selenium converted by the reaction?

12.5

0.05

S e O_{2}

25

C r S O_{4}

which is oxidised to

0.1

C r^{3 -}

The oxidation state at which selenium is converted by the reaction is_________.

12.53

mL of solution of

0.05093 M

S e O_{2}

reacted with exactly

25.52

1 M C r S O_{4}

. After the completion of the reaction what is the change of oxidation state of

S e

?

Q. In an experiment,

50

0.1

M solution of a metallic salt reacted exactly with

25

0.1

M solution of sodium sulphite. In the reaction,

{S O_{3}}^{-}

{S O_{4}}^{2 -}

. If the original oxidation number of the metal in the salt was

3

, what would be the new oxidation number of the metal?

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