Answer:
a. pH = 2.22.
b. [H+] = 2.588 x 10⁻⁴ mol/L.
Step-by-step explanation:
Acids and Bases => Calculating pH of Acids and Bases.
As we saw before, the formulas to find the pH based on the hydrogen ion concentration [H+], and to find the hydrogen ion concentration [H+] based on the pH are the following, respectively:
![\begin{gathered} pH=-log\lbrack H^+], \\ \\ [H^+]=10^(-pH). \end{gathered}](https://img.qammunity.org/2023/formulas/chemistry/high-school/ftfcom5kr5bim5xkb7u6rn0odcvdh63ul0.png)
So let's see each case:
a. To find the pH of an H+ concentration of 6.02 x 10⁻³ mol/L we use the pH formula:
![\begin{gathered} pH=-log\lbrack6.02\cdot10^(-3)], \\ \\ pH=2.220\approx2.22. \end{gathered}](https://img.qammunity.org/2023/formulas/chemistry/high-school/umku96uayxy65xrz9ew86hglel0rwbpqq0.png)
The answer would be that the pH is 2.22.
b. To find the H+ concentration of a pH of 3.587, we use the [H+] formula:
![\begin{gathered} \lbrack H{}^+]=10^(-3.587), \\ \\ [H^+]=2.5882\cdot10^(-4)\text{ mol/L}\approx2.588\cdot10^(-4)\text{ mol/L.} \end{gathered}](https://img.qammunity.org/2023/formulas/chemistry/high-school/e6l34ucp34koz7uowohnbd3wtlg93dh4e4.png)
The answer would be that the hydrogen ion concentration [H+] = 2.588 x 10⁻⁴ mol/L.