Which one is balanced net ionic equations for the following reactions in acidic solution:
$H N O_{2} (a q) \to N O_{3}^{-} + N O (g)$

3 H N O_{2} (a q) \to N O_{3}^{-} (a q) + 2 N O (g) + H_{2} O + H^{+} (a q)

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4 H N O_{2} (a q) \to 3 N O_{3}^{-} + 2 N O (g) + H_{2} O + H^{+} + e^{-}

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3 H N O_{2} (a q) \to N O_{3}^{-} + 2 N O (g) + H_{2} O + H^{+} + e^{-}

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4 H N O_{2} (a q) \to N O_{3}^{-} + 2 N O (g) + H_{2} O + H^{+} + e^{-}

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Solution

The correct option is A $3 H N O_{2} (a q) \to N O_{3}^{-} (a q) + 2 N O (g) + H_{2} O + H^{+} (a q)$
Steps for Balancing redox reactions:

Identify the oxidation and reduction half .

Find the oxidising and reducing agent.

Find the n-factor of oxidising and reducing agent.

Balance atom undergoing oxidation and reduction.

Cross multiply the oxidising or reducing agent with n-factor.

Balance atoms other than oxygen and hydrogen.

Balancing oxygen atoms

Balancing hydrogen atoms

Balance charge

For acidic medium:
As soon as we add x $H_{2} O$ units, we add 2x $H^{+}$ ions on the opposite side.

$n_{f} = (| O . S ._{P r o d u c t} - O . S ._{R e a c t a n t} | \times number of atom$
$+ 3 H N O_{2} (a q) \to + 5 N O_{3}^{-} + + 2 N O (g)$
$+ 3 H N O_{2} (a q) \to + 5 N O_{3}^{-}$ oxidation
$n_{f} = (| 5 - 3 | \times 1 = 2$
$+ 3 H N O_{2} (a q) \to + 2 N O (g)$ reduction
$n_{f} = (| 2 - 3 | \times 1 = 1$

Balance atom undergoing oxidation and reduction.
$3 H N O_{2} (a q) \to N O_{3}^{-} + 2 N O (g)$

Balance oxygen atom.
$3 H N O_{2} (a q) \to N O_{3}^{-} (a q) + 2 N O (g) + H_{2} O$

Balance hydrogen.
$3 H N O_{2} (a q) \to N O_{3}^{-} (a q) + 2 N O (g) + H_{2} O + H^{+} (a q)$

balance charge
charge in reactant side = 0
charge in product side = 0
so the balanced equation is $3 H N O_{2} (a q) \to N O_{3}^{-} (a q) + 2 N O (g) + H_{2} O + H^{+} (a q)$

Suggest Corrections

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