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If a buffer solution is 0.190 M in a weak acid ( a=3.6×10−5) and 0.480 M in its conjugate base, what is the pH?

Respuesta :

Solution :

[tex]pk_b = -log ( K_b)\\\\pk_b = - log ( 3.6 \times 10^{-5})\\\\pk_b = 4.44[/tex]

We know, pH of this solution :

[tex]pH = pK_a + log ( \dfrac{|conjugate\ base|}{|weak \ acid|}\\\\pH = 4.44 + log(\dfrac{0.480}{0.190})\\\\pH = 4.44 + 0.40\\\\pH =4.84[/tex]

Hence, this is the required solution.

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