The ph of an aqueous solution at 25.0°c is 10.66. what is the molarity of h+ in this solution? the ph of an aqueous solution at 25.0°c is 10.66. what is the molarity of h+ in this solution? 4.6 à 10-4 3.3 2.2 à 10-11 1.1 à 10-13 4.6 à 1010

The molarity of hydrogen ions, H⁺ in this solution is  2.2 * 10⁻¹¹

The molarity of a solution is a measure of the concentration in moles of a substance present in a liter of solution of that substance.

The pH of a solution is the negative logarithm in base 10 of the hydrogen ion concentration of the solution.

pH = -log[H⁺]

-pH = log[H⁺]

pH of solution = 10.66

-10.66 = log[H⁺]

taking antilogarithm of both sides

[H⁺] = 10⁻¹⁰°⁶⁶

[H⁺] = 2.2 * 10⁻¹¹

Therefore, the molarity of hydrogen ions, H⁺ in this solution is  2.2 * 10⁻¹¹

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The molarity of in this solution is

Explanation:

pH or pOH is the measure of acidity or alkalinity of a solution.

pH is calculated by taking negative logarithm of hydrogen ion concentration.

Given : pH = 10.66

Putting in the values:

Thus the molarity of in this solution is

the answer to this question is 3.

frequency, z, and the collision density, z, in carbon dioxide (co2), r 180 pm at 30 °c and 120 kpa