Question

A pH scale is shown, fading from red at the left end to blue at the right. Above the scale, pOH is shown in even increments from 14 to zero, and below the scale, p H is shown in even increments from 0 to 14. Points marked are: A at 1 on the p H scale, B at 7 on the p O H scale, C at 13 on the p H scale, and D at 6 on the p H scale.

Based on log rules and the way pH is calculated, what is the difference in [OH– ] concentration between point A and point B.
101
105
106
107

Answer 1

C

Step-by-step explanation:

Answer 2

C

Step-by-step explanation:

We know that the pH of A is 1, which means that -㏒[H+] = 1. Solving for [H+], we see that it is equivalent to
`10^(-1)` M.

Since the concentrations of [OH-] and [H+] have a product of
`10^(-14)`, we can solve for the concentration of OH-:

[OH-] =
`(10^(-14))/(10^(-1)) =10^(-13)`

So the concentration of OH- in A is
`10^(-13)`.

Now, we see that the pOH of B is 7, which means that -㏒[OH-] = 7. Solving for [OH-], we see that it is equivalent to
`10^(-7)` M.

Finally, we can find the difference in concentration between point A and point B by dividing B by A:

`10^(-7)/10^(-13)=10^6`

Thus, the answer is C.

Hope this helps!