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Bronsted Lowry Theory

Which of the ...

Question

Which of the following acts as a self - indicator?

A

K_{2} C r_{2} O_{7}

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B

K M n O_{4}

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C

Oxalic acid

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D

Iodine

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Solution

The correct option is C $K M n O_{4}$
In the presence of a reducing agent, $K M n O_{4}$ acts as self-indicator and changes color from pink to colorless. Because in $M n O_{4}^{-}$ Mn is in +7 oxidation state and is in highest oxidation state. Thus will tend to get reduced and easily takes electrons and being a charge transfer complex, shows intense color. After titration it is $M n O_{2}$ in +4 state and has no electronic charge transfer, therefore colorless.

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Similar questions

0.5

K_{2} C r_{2} O_{7}

K M n O_{4}

was treated with excess of

K I

in acidic medium. Iodine liberated required

150 c m^{3}

0.10 N

solution of thiosulphate solution for titration. Find the percentage of

K_{2} C r_{2} O_{7}

in the mixture.

Q. Consider the following list of reagents.
Acidified

K_{2} C r_{2} O_{7}

K M n O_{4}, C u S O_{4}, H_{2} O_{2}, C l_{2}, O_{3}, F e C l_{3}, H N O_{3}

N a_{2} S_{2} O_{3}

.
Which of the given reagents can oxidise aqueous iodide to iodine?

Q. Consider the following list of reagents:

Acidified K_{2} C r_{2} O_{7}, Alkanline K M n O_{4}, C u S O_{4}, H_{2} O_{2}, C l_{2}, O_{3}, F e C l_{3}, H N O_{3}, a n d N a_{2} S_{2} O_{3}

Which of the following reagents can oxidise aqueous iodide to iodine

Q. A mixture containing

0.05 m o l e

K_{2} C r_{2} O_{7}

0.02 m o l e

K M n O_{4}

was treated with excess of

K I

in acidic medium. The liberated iodine required

1.0 L

N a_{2} S_{2} O_{3}

solution for titration. Concentration of

N a_{2} S_{2} O_{3}

Q. Consider the following list of reagents: Acidified

K_{2} C r_{2} O_{7}

K M n O_{4}

C u S O_{4}

H_{2} O_{2}

C l_{2}

O_{3}

F e C l_{3}

N a_{2} S_{2} O_{3}

. The total number of reagents that can oxidise aqueous iodide to iodine is:

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