Question

Amphetamine (c9h13n) is a weak base with a pkb of 4.2. calculate the ph of a solution containing an amphetamine concentration of 225 mg>l

Answer 1

Answer:

pH = 10.505

Explanation:

Molar mass of Amphetamine ( C9H13N) = 135 g/mol

Given that the concentration of Amphetamine = 225 mg/L

mass of Amphetamine in one Liter = $\frac{225}{ 1000}$ = 0.225 g

Number of moles of Amphetamine in one liter =$\frac {0.225 g} { 135g/mol}$

= 0.001667 mol

∴ molarity = 0.0017 M

              C₉H₁₃N          +        H₂O -------->       C₉H₁₃NH⁺  +      OH⁻

I(M)         0.001667   M                                                  0                 0

C(M)            -x                                                                  x                 x

E(M)         0.001667 - x                                                   x                 x

Pkb = -log Kb = 4.2

∴ Kb = 6.309 x 10⁻⁵

Kb = 6.309 x 10⁻⁵

Equilibrium constant  = [C₉H₁₃NH⁺][OH⁻]/ [C₉H₁₃N]

6.309 x 10⁻⁵  = x² / 0.001667-x

where 0.001667 -x ≅ 0.001667

Then;

x² = 6.309 x 10⁻⁵  × 0.001667

x² =  1.0517103 × 10⁻⁷

x = $\sqrt {1.0517103 * 10^{-7}$

x = 0.00032 M

x = [OH-] = 0.00032 M

∴ pOH = -log [OH-]

pOH = -log (0.00032)

pOH =3.495

pH = 14 - 3.495

= 10.505