Question

FDD

Answer 1

Use the formula: \(K_w=[H_3O^+][OH^-]=1.0 \times 10^{-14}\)
\(K_w\) = self-ionization constant. Now, if you remember from your algebra, rearrange the formula, solving for \([H_3O^+]\). In which case you can then calculate it's pH! Remember: \(pH = -log[H^+]\)
NOTE: pH 0-6 = acidic; 7 = neutral; and 7> = basic.

Answer 2

what's with your picture?

Answer 3

haters gon hate.

Answer 4

@abb0t Will you solve the whole question please?

Answer 5

I'm not going to do your work for you. Try working it out yourself. I already gave you a very detailed step-by-step process of what to do

Answer 6

K

Answer 7

If you're unsure about your answer, you can check with me.