Answer:
3.1 × 10⁻⁶ M
Explanation:
One water molecule can react as a base while other water molecule acts as an acid to form and hydronium ion and a hydroxide ion.
H₂O(l) + H₂O(l) ⇄ H₃O⁺(aq) + OH⁻(aq)
The equilibrium constant (Kw), known as the ionic product of water, has the following form:
Kw = [H₃O⁺] × [OH⁻]
The value of Kw at 25°C is 1.0 × 10⁻¹⁴.
An aqueous solution at 25°C has a hydronium ion concentration of 3.2 × 10⁻⁹ M. The hydroxide concentration is:
Kw = [H₃O⁺] × [OH⁻]
1.0 × 10⁻¹⁴ = 3.2 × 10⁻⁹ × [OH⁻]
[OH⁻] = 3.1 × 10⁻⁶ M
When An aqueous solution at 25°C has a hydronium ion concentration of 3.2 × 10⁻⁹ M. The hydroxide concentration is = 3.1 × 10⁻⁶ M
One water molecule can react as a base while other water molecule acts as an acid to form and hydronium ion and a hydroxide ion.
After that, H₂O(l) + H₂O(l) ⇄ H₃O⁺(aq) + OH⁻(aq)
Then The equilibrium constant (Kw), known as the ionic product of water, has the following form:
Kw is = [H₃O⁺] × [OH⁻]
When The value of Kw at 25°C is 1.0 × 10⁻¹⁴.
Although, An aqueous solution at 25°C has a hydronium ion concentration of 3.2 × 10⁻⁹ M. The hydroxide concentration is:
Then Kw is = [H₃O⁺] × [OH⁻]
After that 1.0 × 10⁻¹⁴ is = 3.2 × 10⁻⁹ × [OH⁻]
Therefore, [OH⁻] is = 3.1 × 10⁻⁶ M
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