Respuesta :
The Ka of a weak acid is the acid dissociation constant, which is a measure of the strength of the acid.
The Ka of a weak monoprotic acid is basically 1.80×10−5, which is a very weak acid.
To calculate the pH of a 0.0769 m solution of this acid, we first need to calculate the concentration of the hydrogen ions (H+). So, the Ka expression for a weak acid is:
Ka = [H+][A-] / [HA]
Where [H+] is the concentration of hydrogen ions, [A-] is the concentration of the conjugate base, and [HA] is the concentration of the acid.
As we know the Ka and the concentration of the acid (0.0769 M), we can rearrange the equation to solve for [H+]:
[H+] = Ka * [HA]
[H+] = 1.80 x 10-5 * 0.0769
[H+] = 1.38 x 10-6 M
Now that we have the concentration of hydrogen ions, we can calculate the pH of the solution using the equation:
pH = -log[H+]
pH = -log(1.38 x 10-6)
pH = 5.85
What is a Monoprotic acid?
In a chemical reaction, a monoprotic acid can donate one proton (H+) per molecule. A single hydrogen atom is typically bonded to an oxygen, sulfur, or nitrogen atom in these acids. Hydrochloric acid, acetic acid, and sulfuric acid are all examples of monoprotic acids. When a proton is donated, monoprotic acids can form conjugate bases. These conjugate bases are known as monobasic anions and are frequently used in acid-base equilibrium reactions as conjugate pairs.
What is pH?
The pH of a solution determines its acidity or alkalinity. It is measured on a scale of 0 to 14, with 7 representing neutral. Solutions with a pH less than 7 are considered acidic, while solutions with a pH greater than 7 are considered basic or alkaline. The lower the pH number, the greater the acidity, and the higher the pH number, the greater the alkalinity.
To know more about Monoprotic acid,
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