Which of the following are valid iodometric titrations?

H C l O + 2 I^{-} + H^{+} ⟶ C l^{-} + I_{2} + H_{2} O

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O_{3} + 2 I^{-} + 2 H^{+} ⟶ O_{2} + I_{2} + H_{2} O

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2 H N O_{2} + 2 I^{-} ⟶ I_{2} + 2 N O + H_{2} O

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8 H N O_{3} + 6 I^{-} ⟶ 6 {N O}_{3}^{-} + 2 N O + 3 I_{2} + 4 H_{2} O

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Solution

The correct options are
A $O_{3} + 2 I^{-} + 2 H^{+} ⟶ O_{2} + I_{2} + H_{2} O$
B $H C l O + 2 I^{-} + H^{+} ⟶ C l^{-} + I_{2} + H_{2} O$
D $2 H N O_{2} + 2 I^{-} ⟶ I_{2} + 2 N O + H_{2} O$
Iodometric titrations are defined as those iodine titrations in which some oxidizing agent liberates iodine from an iodine solution and then liberated iodine is titrated with a standard solution of a reducing agent added from a burette. In such titrations, a neutral or an acidic solution of oxidizing agent is employed. The amount of iodine liberated from an iodide (KI) is equivalent to the quantity of the oxidizing agent present.
The following reactions are iodometric titrations:
$O_{3} + 2 I^{-} + 2 H^{+} ⟶ O_{2} + I_{2} + H_{2} O$
$2 H N O_{2} + 2 I^{-} ⟶ I_{2} + 2 N O + H_{2} O$
$H C l O + 2 I^{-} + H^{+} ⟶ C l^{-} + I_{2} + H_{2} O$

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Similar questions

Which of the following reaction shows the reduction reaction of $H_{2}$ $O_{2}$ ?

H_{2} O_{2} \to H_{2} O + (o)

H_{2} O_{2} + 2 I^{-} \to I_{2} + 2 O H^{-}, H_{2} O_{2}

H_{3} P O_{2} + I_{2} + H_{2} O ⟶ H_{3} P O_{3} + 2 I^{-} + 2 H^{+} H_{3} P O_{3} + I_{2} + 2 O H^{-} ⟶ H_{3} P O_{4} + 2 I^{-} + H_{2} O

H C l O

H C l O + 2 l^{-} + H^{+} ⟶ C l^{-} + I_{2} + H_{2} O

H_{2} O

10

H N O_{3}

10

C u

3 C u + 8 H N O_{3} ⟶ 3 C u (N O_{3})_{2} + 2 N O + 4 H_{2} O

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