Answer :
Final answer:
The concentration of H⁺ in a 8.00M nitrous acid (HNO₂) solution is approximately 3.16×10⁻⁴ M.
Explanation:
To calculate the concentration of H⁺ in a 8.00M nitrous acid (HNO₂) solution, we can use the acid dissociation constant (Kᵃ) and the initial concentration of nitrous acid.
The dissociation of nitrous acid can be represented by the equation: HNO₂ ⇌ H⁺ + NO₂⁻.
The Kᵃ expression for this reaction is: Kᵃ = [H⁺][NO₂⁻] / [HNO₂]
Since nitrous acid is a weak acid, we can assume that the concentration of H⁺ at equilibrium is much smaller than the initial concentration of nitrous acid. Therefore, we can approximate the concentration of H⁺ as x (where x is much smaller than 8.00M).
Using the given Kᵃ value of 4.00×10⁻⁴ and the initial concentration of nitrous acid (8.00M), we can set up the following equation:
4.00×10⁻⁴ = x * (8.00 - x) / 8.00
Simplifying the equation, we get:
4.00×10⁻⁴ = x * (8.00 - x)
Now, we can solve this quadratic equation to find the value of x, which represents the concentration of H⁺ in the solution.
After solving the equation, we find that the concentration of H⁺ in the 8.00M nitrous acid solution is approximately 3.16×10⁻⁴ M.
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