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Which option correctly shows the concentration of H3O+ ions in pure water?


Which Option Correctly Shows The Concentration Of H3O Ions In Pure Water class=

Sagot :

Answer:the correct answer is 1.0* 10^-7 mol/L

Explanation:

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!                  

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