Determine the [H+], [OH-], pH, and pOH for

0.045 M HBr

The answer to your question is below

Explanation:

Data

[HBr] = 0.045 M

[H⁺] = ?

[OH⁻] = ?

pH = ?

pOH = ?

Process

1.- Determine the [H⁺]

The [H⁺] is equal to the [HBr] then, [H⁺] = 0.045 M

2.- Determine the pH

pH = -log[H⁺]

-Substitution

pH = -log[0.045]

-Result

pH = 1.35

3.- Determine the pOH

Formula

pH + pOH = 14

-Solve for pOH

pOH = 14 - pH

-Substitution

pOH = 14 - 1.35

-Result

pOH = 12.65

4.- Determine the [OH⁻]

pOH = -log[OH⁻]

-Solve for [OH⁻]

[OH⁻] = antilog(-pOH)

-Substitution

[OH⁻] = antilog (-12.65)

-Result

[OH⁻] = 2.22 x 10⁻¹³

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