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At 5.0°C, the value of Kw for the equilibrium shown above is 1.9×10−15 and the value of pKw is 14.73. Based on this information, which of the following is correct for pure water at this temperature?

Respuesta :

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the answer should be either b or d but i’m not too sure

Answer:

A

Explanation:

Kw value is equal to [H30+][OH-]

In the pKw, p is -log, so we need to reverse the negative log via the following:

Kw= [tex]10^{-pKw}[/tex]

Kw=[tex]10^{-14.73}[/tex]

Kw= 1.9x [tex]10^{-15}[/tex]

Now in pure water, [H3O+]=[OH-]

We can derive the following equation from the given, Kw=[tex][H3O+] ^{2}[/tex]since both hydronium and hydroxide have equal concentrations.

Substitute:

[H3O+]=[tex]\sqrt{1.9 x 10^{-15} }[/tex]

(we use square root as [H3O+] is squared)

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