Question

Calculate the concentration (in m) of hydronium ions in a solution at 25. 0 °C with a POH of 3. 58.

Answer 1

The concentration (in M) of hydronium ions in a solution at 25. 0 °C with a POH of 3. 58 Is 3.8× 10⁻¹¹ M

pOH is the measure of basic nature of a solution by evaluating the [OH⁻] concentration.

pH is measure of acidic nature of a solution by evaluating the [H⁺] concentration.  It is the negative logarithm of the hydroxide ion concentration. It gives hydronium ions on dissociation.

Given,

pOH = 3.58

Temperature = 25°C = 298K

We know that pH + pOH =14

pH + 3.58 = 14

pH = 10.42

pH is the negative logarithm of hydrogen ion concentration.

At 25°C, the relation of pH and [H⁺] concentration is as follows:

∴ pH = -log [H⁺]

⇒ 10.42 = -log [H⁺]

⇒log [H⁺] = -10.42

⇒ [H⁺] = antilog (-10.42)

⇒[H⁺] =3.8× 10⁻¹¹ M

The concentration (in m) of hydronium ions in a solution at 25. 0 °C with a POH of 3. 58 Is 3.8× 10⁻¹¹ M

Learn more about pH here, brainly.com/question/17144456

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