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Standard XII

Chemistry

Redox Reactions

Iodate ion, ...

Question

Iodate ion, ${I O_{3}}^{-}$ oxidises ${S O_{3}}^{2 -}$ to ${S O_{4}}^{2 -}$ in acidic medium. If $100$ mL sample of solution containing $2.14$ g of $K I O_{3}$ reacts with $60$ mL of $0.5$ M $N a_{2} S O_{3}$ solution, then final oxidation state of iodine is:

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-1

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Solution

The correct option is D -1
Oxidation state of I in $K I O_{3}$ $= + 5$ .
S in ${S O_{3}}^{2 -}$ $= + 4$
S in ${S O_{4}}^{2 -}$ $= + 6$
${I O_{3}}^{-} (+ 5) + {S O_{3}}^{2 -} \to {S O_{4}}^{2 -} (+ 6) + I^{x}$
$x < 5$
Equivalent of ${S O_{3}}^{2 -} = \frac{60 \times 0.5 \times 2}{1000} =$ $0.06$ .
Equivalent ${I O_{3}}^{-} =$ $(5 - x)$ $\times \frac{2.14}{214} =$ $(5 - x) 0.01$ .
Now, $(5 - x) 0.01 = 0.06$
$5 - x = 6; x = - 1$

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Similar questions

Q. Iodate ion,

{I O_{3}}^{-}

, oxidises

{S O_{3}}^{2 -}

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

in acidic medium. If 100 mL sample of solution containing 2.14 g of

K I O_{3}

reacts with 60 mL of 0.5 M

N a_{2} S O_{3}

solution, then final oxidation state of Iodine is

- x

. The value of

x

is :

Q. An aqueous solution containing

2.14

K I O_{3}

was treated with

100

ml of

0.4 M K I

solution, the weight of

I_{2}

produced is :

12 g

of an impure sample of arsenious oxide was dissolved in water containing

7.5 g

of sodium bicarbonate and the resulting solution was diluted to

250 m L

25 m L

of this solution was completely oxidised by

22.4 m L

of a solution of iodine.

25 m L

of this iodine solution reacted with same volume of a solution containing

24.8 g

of sodium thiosulphate solution

(N a_{2} S_{2} O_{3} \cdot 5 H_{2} O)

in one litre. Calculate the percentage of arsenious oxide in the sample. (Atomic mass of

A s = 75)

12

g of an impure sample of arsenious oxide was dissolved in water containing

7 .5

g of sodium bicarbonate and the resulting solution was diluted to

250

mL.

25

mL of this solution was completely oxidized by

22.4

mL of solution of iodine.

25

mL of this iodine solution reacted with same volume of a solution containing

24.8

g of sodium was completely oxidized by

22.4 m L

of a solution thiosulphate

(N a_{2} S_{2} O_{3} 5 H_{2} O)

in one litre. Calculate the percentage of arsenious oxide in the sample. (Atomic mass of

A s = 75

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Q. What is the volume (in ml) of 0.1 M potassium permanganate solution required to completely oxidise 100 ml of 0.5 M ferrous sulphate solution in acidic medium?

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Iodate ion, IO3− oxidises SO32− to SO42− in acidic medium. If 100 mL sample of solution containing 2.14 g of KIO3 reacts with 60 mL of 0.5M Na2SO3 solution, then final oxidation state of iodine is:

The correct option is D -1Oxidation state of I in KIO3 =+5.S in SO32− =+4S in SO42− =+6IO3−(+5)+SO32−→SO42−(+6)+Ixx<5Equivalent of SO32−=60×0.5×21000= 0.06.Equivalent IO3−= (5−x) ×2.14214= (5−x)0.01.Now, (5−x)0.01=0.065−x=6;x=−1

Iodate ion, ${I O_{3}}^{-}$ oxidises ${S O_{3}}^{2 -}$ to ${S O_{4}}^{2 -}$ in acidic medium. If $100$ mL sample of solution containing $2.14$ g of $K I O_{3}$ reacts with $60$ mL of $0.5$ M $N a_{2} S O_{3}$ solution, then final oxidation state of iodine is: