At 30.°C, the concentration of hydronium (H3O^+) ions in an aqueous solution is 1.1 ✕ 10^−9 M. (Note: At 30.°C, the ion-product constant for water is 1.46 ✕ 10^−14.)

Question

At 30.°C, the concentration of hydronium (H3O^+) ions in an aqueous solution is 1.1 ✕ 10^−9 M. (Note: At 30.°C, the ion-product constant for water is 1.46 ✕ 10^−14.)

(a) What is the concentration of hydroxide (OH^−) ions in this solution?

(b)is the solution acidic, basic, or neutral, and why?

DrBob222 · Answer

Amy, Dalton, Jamie, et al. You are skirting on not getting help if you can't follow us. You're making it twice as hard t hel you.
.......2HOH ==> H3O^+ + OH^-
I......liquid..0......0
C......liquid..x......x
E......liquid..x......x

Kw = 1.46E-14 = (H3O^+)(OH^-)
Solve for x = (H3O^+)(OH^-)

Post your work if you get stuck. By the way, look at your answer and tell me, is the solution acidic, basic, or neutral.