Question

A solution with a pH = 13 has approximately how many moles of OH– ions per liter?

How many molecules of H+ would this same solution have per liter?

A different solution with an H+ concentration of 1.0 × 10–4 would have a pH =

Answer 1

Part 1--0.1

Part 2--0.0000000000001

Part 3--4

Step-by-step explanation:

Answer 2

(A) The number of moles of
`OH^-` ions per liter is, 0.1 moles/L

(B) The number of molecules of
`H^+` ion is,
`6.022* 10^(10)`

(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,

`pH+pOH=14\\\\13+pOH=14\\\\pOH=1`

Now we have to calculate the moles of
`OH^-` ion per liter.

`pOH=-\log [OH^-]\\\\1=-\log [OH^-]`

`[OH^-]=0.1moles/L`

Solution for part B :

First we have to calculate the
`H^+` ion concentration.

`pH=-\log [H^+]\\\\13=-\log [H^+]`

`[H^+]=10^(-13)moles/L`

Now we have to calculate the number of molecules of
`H^+` ion

As, 1 mole contains
`6.022* 10^(23)` number of molecules of
`H^+` ion

So,
`10^(-13)` moles contains
`6.022* 10^(23)* 10^(-13)=6.022* 10^(10)` number of molecules of
`H^+` ion

Solution for part C :

`pH=-\log [H^+]\\\\pH=-\log (1* 10^(-4))`

`pH=4`