The pH of a solution of Sr(OH)2 is 12.42. What is its pOH? What is its [H3O^+]? What is its (OH^-)? What is its [Sr(OH02]? Is the solution acidic or basic?

Refer to your post below.

pH = -log(H^+). Substitute and solve for (H^+).
pH<7 = acid
pH = 7 = neutral
pH >7 = basic.

To find the pOH of a solution, you can use the formula:

pOH = 14 - pH

Given that the pH of the solution is 12.42, we can substitute it into the formula:

pOH = 14 - 12.42
pOH = 1.58

The pOH of the solution is 1.58.

To find the [H3O+], you can use the formula:

[H3O+] = 10^(-pH)

Substituting the given pH of 12.42 into the formula:

[H3O+] = 10^(-12.42)

Using a calculator, you would find that [H3O+] is approximately 2.356 x 10^(-13) M (Molar).

The [OH-] (hydroxide ion concentration) can be found by taking the negative logarithm of the [H3O+]:

[OH-] = 10^(-pOH)

Substituting the given pOH of 1.58 into the formula:

[OH-] = 10^(-1.58)

Using a calculator, you would find that [OH-] is approximately 0.0215 M.

To find the concentration of Sr(OH)2, you need to know the amount of Sr(OH)2 dissolved in a certain volume of solution. If that information is not provided, we cannot determine the concentration of Sr(OH)2.

Finally, to determine if the solution is acidic or basic, we can look at the pH. A pH greater than 7 indicates a basic solution, while a pH less than 7 indicates an acidic solution. In this case, since the pH is 12.42, the solution is basic.