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Orthoboric Acid

Iodimetric ti...

Question

Iodimetric titrations are usually performed in neutral or mildly alkaline ( $p H = 8$ ) or weakly acidic solution. Which of the following statements is not valid for this observation?

In strong alkaline solution,

I_{2}

disproportionates to

I^{-}

and

I O^{-}

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In strong acidic solutions, starch used to detect the end point tends to hydrolyse or decompose

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I^{-}

produced during titration tends to be oxidized by dissolved oxygen in acidic medium

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Reducing power of reducing agent is increased in strong acidic medium

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Solution

The correct option is D Reducing power of reducing agent is increased in strong acidic medium
Reducing power of the reducing agent increases in an acidic medium. This observation when if the pH is too acidic. The remaining options are observed during the titration in a weakly acidic solution.

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Similar questions

K M n O_{4}, K_{2} C r_{2} O_{7}, C u S O_{4}, H_{2} O_{2}

(I_{2})

K_{2} C r_{2} O_{7} + 6 K I + 7 H_{2} S O_{4} \to C r_{2} (S O_{4})_{3} + 4 K_{2} S O_{4} + 7 H_{2} O + I_{2}

2 C u C O_{4} + 4 K I \to C u_{2} I_{2} + 2 K_{2} S O_{4} + I_{2}

I_{2} + N a_{2} S_{2} O_{3} \to 2 N a I + N a_{2} S_{4} O_{6}

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

I_{2}

K I

C u S O_{4}

\begin{matrix} List - I (Salt solution) & List - II (pH) (I) 0.1 M K C N & (P) 7 (II) 0.1 M P h N H_{3} C l & (Q) 6.5+ \frac{1}{2} p K_{a} (III) 0.1 M K C l & (R) 7.5 - \frac{1}{2} p K_{b} (IV) 0.1 M C H_{3} C O O N H_{4} (K_{a} = K_{b}) & (S) 7.5 + \frac{1}{2} p K_{a} - \frac{1}{2} p K_{b} (T) 7.5 - \frac{1}{2} p K_{a} - \frac{1}{2} p K_{b} (U) 7.5 - \frac{1}{2} p K_{a} + \frac{1}{2} p K_{b} \end{matrix}

1 M

K M n O_{4}

20

33.4

100

{M n O_{4}}^{-}

M n^{2 +}

{M n O_{4}}^{-}

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