Since the pH of this solution is 9.94, it is basic.
1. To calculate the pH, we use the formula:
pH = -log[H3O+]
Since we were given the concentration of the hydroxide ion, we can use the following relationship to find the concentration of the hydronium ion:
[H3O+] x [OH-] = 1 x 10^-14 M^2
[H3O+] = (1 x 10^-14 M^2) / [OH-]
[H3O+] = (1 x 10^-14 M^2) / (8.79 x 10^4 M)
[H3O+] = 1.14 x 10^-10 M
Now we can substitute this value into the pH formula:
pH = -log(1.14 x 10^-10)
pH = 9.94
Therefore, the pH of the solution is 9.94.
2. To calculate the pOH, we use the formula:
pOH = -log[OH-]
We were given the concentration of the hydroxide ion, so we can use that directly in the formula:
pOH = -log(8.79 x 10^4)
pOH = 4.06
Therefore, the pOH of the solution is 4.06.
3. We already calculated the concentration of the hydronium ion in part 1:
[H3O+] = 1.14 x 10^-10 M
4. To determine whether the solution is acidic, basic, or neutral, we can use the pH scale. A solution with a pH less than 7 is acidic, a solution with a pH greater than 7 is basic, and a solution with a pH of 7 is neutral.
Since the pH of this solution is 9.94, it is basic.