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Calculate the concentration of OH in a solution that contains 3910-4 M H30 at 25°C. Identify the solution as acidic, basic or neutral OA) 2.6 10-11 M, acidic OB)26 10-11 M. basic O c) 3.9 x 10-4 M, neutral OD) 2.7 * 10-2 M

Answer :

Answer : The correct option is, (A) [tex]2.6\times 10^{-11}M[/tex], acidic

Explanation:

pH : It is defined as the negative logarithm of hydrogen ion or hydronium ion concentration.

When the value of pH is less then 7 then the solution will be acidic.

When the value of pH is more then 7 then the solution will be basic.

When the value of pH is equal to 7 then the solution will be neutral.

First we have to calculate the pH.

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

[tex]pH=-\log (3.9\times 10^{-4})[/tex]

[tex]pH=3.41[/tex]

Now we have to calculate the pOH.

[tex]pH+pOH=14\\\\pOH=14-pH\\\\pOH=14-3.41=10.59[/tex]

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

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

[tex]10.59=-\log [OH^-][/tex]

[tex][OH^-]=2.6\times 10^{-11}M[/tex]

Therefore, the [tex]OH^-[/tex] concentration is, [tex]2.6\times 10^{-11}M[/tex]

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