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2 years ago

Calculate the poh of a solution at 25. 0 °C that contains 2. 95 × 10^-12 m hydronium ions.

Chemistry

1 answer:

lapo4ka [179]2 years ago

8 0

The pOH of a solution at 25. 0 °C that contains 2. 95 × 10^-12 M hydronium ions is 0.5.

pH is the concentration of the hydrogen ion released or gained by the species in the solution that depicts the acidity and basicity of the solution.

pOH is the concentration of the hydroxide ion in the solution and is dependent on the pH as an increase in pH decreases the pOH and vice versa.

Total H+ ions = 2.95 x 10⁻¹² M

pH is calculated as:

pH = -log[H+]

Substituting values in the equation:

log( 2.95 x 10⁻¹² M)= 13.5 pH

pOH is calculated as:

14 - pH = pOH

Substituting values in the equation above:

14 - 13.5 = 0.5 pOH

Therefore, pH is 13.5 and pOH is 0.5.

Learn more about pH and pOH here: brainly.com/question/2947041

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