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Answer :
The value of KB for NO₂⁻ is 2.2 × 10⁻¹¹.
The first step is to calculate the molarity of the solution. We can do this by dividing the mass of Ba(NO₂)₂ by its molar mass and by the volume of the solution.
molarity = (37.9 g / 253.3 g/mol) / 0.500 L = 2.89 M
The second step is to write the equilibrium equation for the reaction of NO₂⁻ with water.
NO₂⁻(aq) + H₂O(l) ⇌ OH⁻(aq) + HNO₂(aq)
The third step is to use the Ka of HNO₂ to calculate the value of Kb for NO₂⁻.
Kw = Ka * Kb
1.0 × 10⁻¹⁴ = 4.5 × 10⁻⁴ * Kb
Kb = 1.0 × 10⁻¹⁴ / 4.5 × 10⁻⁴ = 2.2 × 10⁻¹¹
Therefore, the value of KB for NO₂⁻ is 2.2 × 10⁻¹¹.
To know more about molarity refer here :
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