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

C

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 M.

Since the concentrations of [OH-] and [H+] have a product of , we can solve for the concentration of OH-:

[OH-] =

So the concentration of OH- in A is .

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 M.

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

Thus, the answer is C.

Hope this helps!

"you start with 15.67 g mgco3-xh2o, when heated and all the water is removed, you are left with 7.58 g mgco3 only.

therefore, you had 15.67 - 7.58 = 8.09g h2o  

moles of each :

7.58g mgco3 = ? moles = 7.58g / 83.4g/mole = 0.09moles  

8 09g h2o = ? moles = 8.09g / 18g/mole = 0.44moles  

molar ratio between the two by dividing both numbers by the smallest number :

0.09 / 0.09 = 1  

0.44 / 0.09 = 4.8  

mgco3-5h2o"