Respuesta :
Explanation:
the pH of the solution defined as negatuve logarithm of [tex]H^+[/tex] ion concentration.
[tex]pH=-\log[H^+][/tex]
1. Hydrogen ion concentration when pH of the solution is 11.
[tex]11=-\log[H^+][/tex]
[tex][H^+]=1\times 10^{-11} mol/L[/tex]..(1)
At pH = 11, the concentration of [tex]H^+[/tex] ions is [tex]1\times 10^{-11} mol/L[/tex].
2. Hydrogen ion concentration when the pH of the solution is 6.
[tex]6=-\log[H^+]'[/tex]
[tex][H^+]'=1\times 10^{-6} mol/L[/tex]..(2)
At pH = 6, the concentration of [tex]H^+[/tex] ions is [tex]1\times 10^{-6} mol/L[/tex].
3. On dividing (1) by (2).
[tex]\frac{[H^+]}{[H^+]'}=\frac{1\times 10^{-11} mol/L}{1\times 10^{-6} mol/L}=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].
4. Difference between the [tex]H^+[/tex] ions at both pH:
[tex]1\times 10^{-6} mol/L-1\times 10^{-11} mol/L=9.99\time 10^{-7} mol/L[/tex]
This means that Hydrogen ions in a solution at pH = 7 has [tex]9.99\time 10^{-7} mol/L[/tex] ions fewer than in a solution at a pH = 6
Answer:
for table C
Explanation:
What is the concentration of H+ ions at a pH = 11?
1. ⇒ 0.00000000001 mol/L
What is the concentration of H+ ions at a pH = 6?
2. ⇒ 0.000001 mol/L
How many fewer H+ ions are there in a solution at a
pH = 11 than in a solution at a pH = 6?
3. ⇒ 100,000
