Question

Use Table B in your Student Guide to answer the questions about ion concentrations.

A solution with a pH = 13 has approximately how many moles of OH ions per liter?
How many moles of H* would this same solution have per liter?
(Use the decimal form of your answer.)
A different solution with an H+ concentration of 1.0 x 10-4 would have a pH =

Answer 1

A solution with a pH of 13 has approximately 0.1 moles of OH- ions per liter. The same solution would have approximately 1.0 x 10-13 moles of H+ ions per liter.

Step-by-step explanation:

In order to determine the number of moles of OH- ions in a solution with a pH of 13, we can use the relationship between pH and pOH. The pOH is calculated by subtracting the pH from 14. Since the pH is 13, the pOH would be 14 - 13 = 1. Then, we can use the relationship between pOH and the concentration of hydroxide ions. A pOH of 1 corresponds to a hydroxide ion concentration of 0.1 M. Therefore, the solution with a pH of 13 has approximately 0.1 moles of OH- ions per liter.

The moles of H+ ions in the same solution can be calculated by using the equation Kw = [H+] * [OH-], where Kw is the ion product constant for water. At 25°C, Kw is equal to 1.0 x 10-14. Since we know the concentration of hydroxide ions, which is 0.1 M, we can rearrange the equation to solve for the concentration of hydrogen ions. [H+] = Kw / [OH-] = (1.0 x 10-14) / (0.1) = 1.0 x 10-13 M. Therefore, the solution with a pH of 13 would have approximately 1.0 x 10-13 moles of H+ ions per liter.