lizardtrip
Answered

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

Verified Answer :

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: \(3.6\times 10^{-14}M\)

Explanation:-

First we have to calculate the pOH.

\(pOH=-\log [OH^-]\)

\(0.253=-\log[OH^-]\)

\([OH^-]=0.558M\)

Now we have to calculate the pH.

\(pH+pOH=14\\\\pH=14-0.558\\\\pH=13.442\)

Now we have to calculate the \(OH^-\) concentration.

\(pH=-\log [H^+]\)

\(13.442=-\log [H^+]\)

\([H^+]=3.6\times 10^{-14}M\)

Therefore, the \(H^+\) concentration is, \(3.6\times 10^{-14}M\)

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