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
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