For the given options, the one that correctly shows the concentration of H₃O⁺ ions in pure water is the second option: 1.0x10⁻⁷ mol/L.
In pure water, we have the following dissociation reaction:
2H₂O ⇄ H₃O⁺ + OH⁻
The dissociation constant of the above reaction is:
[tex] K_{w} = [H_{3}O^{+}]*[OH^{-}] = 1.00\cdot 10^{-14} [/tex]
Where:
[tex]K_{w}[/tex]: is the dissociation constant of water = 1.00x10⁻¹⁴
[H₃O⁺]: is the concentration of hydronium ions
[OH⁻]: is the concentration of hydroxide ions
In pure water, we have that H₃O⁺ and OH⁻ concentrations are the same, so:
[tex] 1.00 \cdot 10^{-14} = x^{2} [/tex]
[tex] x = \sqrt{1.00 \cdot 10^{-14}} [/tex]
[tex] x = 1.00 \cdot 10^{-7} [/tex]
Therefore, the concentration of H₃O⁺ ions in pure water is 1.00x10⁻⁷ mol/L, so the correct option is the second.
To find more about water dissociation goes here: https://brainly.com/question/13378385?referrer=searchResults
I hope it helps you!
