Answer:
[H₂O] > [H₃O⁺] ≳ [Cl⁻] > [OH⁻] > [HCl]
Explanation:
HCl + H₂O ⟶ H₃O⁺ + Cl⁻
HCl dissociates completely in solution.
[HCl] = 0 mol·L⁻¹
[H₃O⁺] = 1.0 × 10⁻⁶ mol·L⁻¹
[Cl⁻] = 1.0 × 10⁻⁶ mol·L⁻¹
[H₃O⁺] is slightly greater than [Cl⁻] because the autoionization of water also creates some hydronium ion.
1 L of water has a mass of 1000 g.
[tex]\text{Moles of H$_{2}$O} = \text{1000 g} \times \frac{\text{1 mol}}{\text{18.02 g}} = \text{55.49 mol}[/tex]
∴ [H₂O] = 55.49 mol·L⁻¹
[tex][\text{OH}^{-}] = \frac{K_{w} }{\text{[H}_{3}\text{O}^{+}]} = \frac{1.00 \times10^{-14} }{ 1.0 \times 10^{-6}}= 1.0 \times 10^{-8} \text{ mol/L}[/tex]
∴ [H₂O] > [H₃O⁺] ≳ [Cl⁻] > [OH⁻] > [HCl]
55.5 10⁻⁶ 10⁻⁶ 10⁻⁸ 0
The relative molar amounts of these species from most to least is; H2O > H3O+ ≈ Cl- > OH- > HCl
We know that the equation of the reaction is represented as follows;
HCl(aq) + H2O(l) ⇄ H3O^+(aq) + OH^-(aq) + Cl^-(aq)
We know that water is present in large excess.
Also; [H3O^+] = [Cl^-]
Since it is an acid, the concentration of hydronium ions exceeds the concentration of hydroxide ions.
It then follows that the molar amounts of the species is;
H2O > H3O+ ≈ Cl- > OH- > HCl
HCl is least because the acid dissociates completely in water.
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