What is the hydronium ion concentration of a solution of a solution with a poh of 8.3

1.28 x 10^-6
1.99 x 10 ^-6
2.34 x 10^-5
2.86 x 19^-5

[H₃O⁺] = 1.99x10⁻⁶

Explanation:

pH + pOH = 14

pH = 14 - 8.30

pH = 5.7

10*-pH = [H₃O⁺]

10⁻⁵°⁷ = 1.99x10⁻⁶

Let's see another way to solve

[H₃O⁺] . [OH⁻] = 1x10⁻¹⁴

10*-pOH = [OH⁻]

10⁻⁸°³ = 5.01x10⁻⁹ → [OH⁻]

[H₃O⁺] . 5.01x10⁻⁹ =  1x10⁻¹⁴

[H₃O⁺] = 1x10⁻¹⁴ /  5.01x10⁻⁹  = 1.99x10⁻⁶

The hydronium ion concentration is 1.99 * 10^-6 M

Explanation:

Step 1: pOH = 8.3

pOH + pH = 14

Step 2: Calculate [H3O+] = [H+]

pOH + pH = 14

pH = 14 - pOH

pH = 14 - 8.3 = 5.7

pH = -log[H+] = 5.7

[H+] 10^(-0.57) = 1.995 * 10^-6

[H+] = [H3O+] = 1.995 * 10^-6 M

The hydronium ion concentration is 1.99 * 10^-6 M

your answer would be “dry”