Respuesta :
Explanation:
When pH of the solution is 11.
[tex]pH=-\log[H^+][/tex]
[tex]11=-\log[H^+][/tex]
[tex][H^+]=1\times 10^{-11} M[/tex]..(1)
At pH = 11, the concentration of [tex]H^+[/tex] ions is [tex]1\times 10^{-11} M[/tex].
When the pH of the solution is 6.
[tex]pH=-\log[H^+]'[/tex]
[tex]6=-\log[H^+]'[/tex]
[tex][H^+]'=1\times 10^{-6} M[/tex]..(2)
At pH = 6, the concentration of [tex]H^+[/tex] ions is [tex]1\times 10^{-6} M[/tex].
On dividing (1) by (2).
[tex]\frac{[H^+]}{[H^+]'}=\frac{1\times 10^{-11} M}{1\times 10^{-6}}=1\times 10^{-5} [/tex]
The ratio of hydrogen ions in solution of pH equal to 11 to the solution of pH equal to 6 is [tex] 1\times 10^{-5}[/tex].
Difference between the [tex]H^+[/tex] ions at both pH:
[tex]1\times 10^{-6} M-1\times 10^{-11} M=9.99\time 10^{-7} M[/tex]
This means that Hydrogen ions in a solution at pH = 7 has [tex]9.99\time 10^{-7} M[/tex] ions fewer than in a solution at a pH = 6
