What is the pH of a 0.11 M solution of methylamine (CH₃NH₂,K_b = 4.4 $\times$ 10^-4)at 25^oC? (K_w = 1.01 $\times$ 10^-14)

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Quizplus · Accepted Answer

To find the pH, first calculate the pOH using the formula: pOH = -log[OH⁻]. Methylamine is a weak base, so use the Kb expression: Kb = [CH3NH3⁺][OH⁻]/[CH3NH2]. Assume [OH⁻] = x, then Kb = x²/0.11. Solve for x, then pOH = -log(x). Finally, pH = 14 - pOH. The calculated pH is approximately 11.83.

What Is the PH of a 0 ×\times× 10-4)at 25oC? (Kw = 1

What Is the PH of a 0 $\times$ 10^-4)at 25^oC? (K_w = 1