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What is the [H+] in a solution with pOH of 0.253? 5.58 × 10−15 M 1.79 × 10−14 M 3.21 × 10−2 M 5.58 × 10−1 M

Respuesta :

jprincess1105
Okay so we know that pOH + pH = 14, so if pOH is 0.253 the pH would be 13.747. 

And pH = -log [H+], so [H+] = 10^(-pH) -->This is just the antillog... 

so [H+] = 1.791e-14, which would make sense for the strongly basic solution (so B is the correct answer) 

Hope this helps...

Answer: [tex]3.6\times 10^{-14}M[/tex]

Explanation:-

First we have to calculate the pOH.

[tex]pOH=-\log [OH^-][/tex]

[tex]0.253=-\log[OH^-][/tex]

[tex][OH^-]=0.558M[/tex]

Now we have to calculate the pH.

[tex]pH+pOH=14\\\\pH=14-0.558\\\\pH=13.442[/tex]

Now we have to calculate the [tex]OH^-[/tex] concentration.

[tex]pH=-\log [H^+][/tex]

[tex]13.442=-\log [H^+][/tex]

[tex][H^+]=3.6\times 10^{-14}M[/tex]

Therefore, the [tex]H^+[/tex] concentration is, [tex]3.6\times 10^{-14}M[/tex]

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