Answer :
Answer : The concentration of [tex]H_3O^+[/tex] and [tex]OH^-[/tex] are [tex]7.94\times 10^{-5}[/tex] and [tex]1.258\times 10^{-10}[/tex] respectively.
Solution : Given,
pH = 4.10
pH : pH is defined as the negative logarithm of hydronium ion concentration.
Formula used : [tex]pH=-log[H_3O^+][/tex]
First we have to calculate the hydronium ion concentration by using pH formula.
[tex]4.10=-log[H_3O^+][/tex]
[tex][H_3O^+]=antilog(-4.10)[/tex]
[tex][H_3O^+]=7.94\times 10^{-5}[/tex]
Now we have to calculate the pOH.
As we know, [tex]pH+pOH=14[/tex]
[tex]4.10+pOH=14[/tex]
[tex]pOH=9.9[/tex]
Now we have to calculate the hydroxide ion concentration.
[tex]pOH=-log[OH^-][/tex]
[tex]9.9=-log[OH^-][/tex]
[tex][OH^-]=antilog(-9.9)[/tex]
[tex][OH^-]=1.258\times 10^{-10}[/tex]
Therefore, the concentration of [tex]H_3O^+[/tex] and [tex]OH^-[/tex] are [tex]7.94\times 10^{-5}[/tex] and [tex]1.258\times 10^{-10}[/tex] respectively.
