The pH of 0.35 M of CH₃NH₂ is 12.09 and the for methylamine is 4.4 x 10⁻⁴.
<h3>What is pH?</h3>
pHis the quantitative measure of acidity and basicity of an aqueous or other liquid solution. The scale range goes from 0 to 14. Water has a pH of 7 and is neutral in nature.
<h3>What is dissociation constant?</h3>The dissociation constant is an equilibrium constant that describes the dissociation or ionization of a base or an acid
describes the dissociation of an acid
describes the dissociation of a base
For methylamine,
Initial concentration of methylamine = 0.35 M
Initial concentration of products = 0
Let, at equilibrium concentration of CH₃NH₂ = 0.35 - x
Then, concentration of CH₃NH₃⁺ and OH⁻ is x and x respectively
The dissociation constant for methylamine, = 4.4 x 10⁻⁴
pOH = -log[OH] = -log(0.0124) = 1.91
pH + pOH = 14
pH = 14 - 1.91 = 12.09
Thus, the pH of methylamine is 12.09 and is 4.4 x 10⁻⁴
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