what is the ph of a solution with a 1.50 × 10−9 m hydroxide ion concentration? 0.176 5.18 8.82 9.20

5.17.

Explanation:

∵ [H₃O⁺][OH⁻] = 10⁻¹⁴.

[OH⁻] = 1.5  x 10⁻⁹ M.

∴ [H₃O⁺] = 10⁻¹⁴/[OH⁻] = 10⁻¹⁴/(1.5  x 10⁻⁹ M) = 6.66 × 10⁻⁶ M.

∵ pH = - log[H₃O⁺]

∴ pH = - log(6.66 × 10⁻⁶ M) = 5.17.

5.18

Explanation:

I hope this helps ;)

sure what is it? ^w^

the dependant variable is spilled water

the independent is the heat