Final answer:
To find the pH of a 0.38 M solution of a monoprotic weak acid with a Ka of 1.1 × 10⁻⁶, we can use the equation Ka = [H+][A-]/[HA]. Rearranging the equation, we can find [H+] and then determine the pH.
Step-by-step explanation:
To find the pH of a 0.38 M solution of a monoprotic weak acid with a Ka of 1.1 × 10⁻⁶, we need to use the equation Ka = [H+][A-]/[HA]. In this equation, [H+] represents the concentration of hydrogen ions, [A-] represents the concentration of the conjugate base, and [HA] represents the concentration of the weak acid.
Since the Ka value is given and we are looking for the pH, we can rearrange the equation to solve for [H+]. [H+] = √(Ka[HA]). Plugging in the values, [H+] = √(1.1 × 10⁻⁶ × 0.38) = 1.74 × 10⁻⁴ M.
To find the pH, we take the negative logarithm of [H+]. pH = -log[H+]. Substituting the value, pH = -log(1.74 × 10⁻⁴) = 3.76.