Respuesta :
Answer :
(A) The number of moles of [tex]OH^-[/tex] ions per liter is, 0.1 moles/L
(B) The number of molecules of [tex]H^+[/tex] ion is, [tex]6.022\times 10^{10}[/tex]
(C) The pH of the solution will be, 4
Solution for part A :
First we have to calculate the pOH of the solution.
As we know that,
[tex]pH+pOH=14\\\\13+pOH=14\\\\pOH=1[/tex]
Now we have to calculate the moles of [tex]OH^-[/tex] ion per liter.
[tex]pOH=-\log [OH^-]\\\\1=-\log [OH^-][/tex]
[tex][OH^-]=0.1moles/L[/tex]
Solution for part B :
First we have to calculate the [tex]H^+[/tex] ion concentration.
[tex]pH=-\log [H^+]\\\\13=-\log [H^+][/tex]
[tex][H^+]=10^{-13}moles/L[/tex]
Now we have to calculate the number of molecules of [tex]H^+[/tex] ion
As, 1 mole contains [tex]6.022\times 10^{23}[/tex] number of molecules of [tex]H^+[/tex] ion
So, [tex]10^{-13}[/tex] moles contains [tex]6.022\times 10^{23}\times 10^{-13}=6.022\times 10^{10}[/tex] number of molecules of [tex]H^+[/tex] ion
Solution for part C :
[tex]pH=-\log [H^+]\\\\pH=-\log (1\times 10^{-4})[/tex]
[tex]pH=4[/tex]
Answer:
Part 1--0.1
Part 2--0.0000000000001
Part 3--4
Explanation:
