Calculate the hydrogen-ion concentration [H+] for the aqueous solution in which [OH–] is 1 x 10–4 mol/L. Is this solution acidic, basic, or neutral? Show your work. (3 points)

[H+] = 1 x 10-10 mol/L

Basic

Explanation:

pOH = -log[OH-]

        = -log(1 x 10-4)

        = -(-4) = 4

pOH + pH = 14

4 + pH = 14

pH = 10

Now that we know pH is 10, we can solve for the [H+]. We also now know that this is a basic solution, because the pH > 7.

pH = -log[H+]

10 = -log[H+]

[H+] = 1 x 10-10 mol/L

The answer to your question is [H⁺] = 1 x 10⁻¹⁰ M

Explanation:

Data

[H⁺] = ?

[OH⁻] = 1 x 10⁻⁴ mol/L

Process

1.- Calculate the pOH

Formula

pOH = -log[OH⁻]

Substitution

pOH = -log [1 x 10⁻⁴]

Result

pOH = 4

2.- Calculate the pH

pH + pOH = 14

-Solve for pH

pH = 14 - pOH

-Substitution

pH = 14 - 4

-Result

pH = 10

3.- Calculate the [H⁺]

Formula

pH = -log [H⁺]

Substitution

10 = -log[H⁺]

-Solve for [H⁺]

[H⁺] = antilog (-pH)

-Substitution

[H⁺] = antilog(-10)

-Result

[H⁺] = 1 x 10⁻¹⁰ M

more infor would

a lot