The pH of monoacidic base is 10 . Calculate its percentage dissociation in 0.01 M solution at 298 K ?

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Percentage dissociation of monoacidic base Given a monoacidic base with concentration C = 0.01 M at 298 K and solution pH = 10, calculate the percentage dissociation. The pOH is determined from the pH relationship at 298 K: pH + pOH = 14 pOH = 14 - 10 = 4 The hydroxide ion concentration is then: [ OH ^-] = 10⁻⁴ M For the dissociation equilibrium BOH B ^+ + OH ^- with initial concentration C , the hydroxide concentration relates to the degree of dissociation as: [ OH ^-] = C Solving for : = [ OH ^-] C = 10⁻⁴ 10⁻² =