Calculate the concentration of oh- in a solution that contains 3.9 x 10-4 m h3o+ at 25°c. identify the solution as acidic, basic or neutral. calculate the concentration of oh- in a solution that contains 3.9 x 10-4 m h3o+ at 25°c. identify the solution as acidic, basic or neutral. 3.9 × 10-4 m, neutral 2.7 × 10-2 m, basic 2.6 × 10-11 m, basic 2.7 × 10-2 m, acidic 2.6 × 10-11 m, acidic

[OH⁻] = 2,6x10⁻¹¹

Acidic

Explanation:

The kw in water is:

2 H₂O(l) ⇄ OH⁻(aq) + H₃O⁺(aq)

kw = [OH⁻] [H₃O⁺] = 1,00x10⁻¹⁴

If concentracion of H₃O⁺ is 3,9x10⁻⁴M:

[OH⁻] [3,9x10⁻⁴M] = 1,00x10⁻¹⁴

[OH⁻] = 2,6x10⁻¹¹

pH is defined as - log[H₃O⁺]. If pH>7,0 the solution is basic, if pH<7,0 solution is acidic, if pH=7,0 solution is neutral.

In this problem,

pH = - log [3,9x10⁻⁴M] = 3,4

As pH is < 7.0, the solution is acidic

I hope it helps!

for step 7 table c on the lab "newtons law of action"   the average time it took the car to travel .25 meters   was 1.92 seconds.

the average time it took the car to travel 0.50 meters was 2.61 seconds

hope this : )

i wish i could but this one is weird give me abc and i can solve it.