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a) determine the pH present in the solution that comes out of the leaching process and indicate if it is within the permissible range. data: kb hcn = 1.61 x 10 -5

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Answer to a math question a) determine the pH present in the solution that comes out of the leaching process and indicate if it is within the permissible range. data: kb hcn = 1.61 x 10 -5

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Cristian
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Para determinar el pH de la solución y ver si se encuentra en el rango permisible, necesitamos usar la constante de basicidad ($K_b$) del cianuro de hidrógeno (HCN).

La reacción de ionización del HCN en agua es la siguiente:
HCN + H_2O \rightleftharpoons CN^- + H_3O^+

La constante de basicidad ($K_b$) se relaciona con la constante de acidez ($K_a$) de la siguiente manera:
K_a \times K_b = K_w
Donde $K_w$ es el producto iónico del agua ($1.0 \times 10^{-14}$ a 25°C).

Dado que conocemos la constante de basicidad ($K_b = 1.61 \times 10^{-5}$), podemos calcular la constante de acidez ($K_a$):
K_a = \frac{K_w}{K_b}
K_a = \frac{1.0 \times 10^{-14}}{1.61 \times 10^{-5}} \approx 6.21 \times 10^{-10}

Ahora, podemos usar este valor de $K_a$ para calcular el pH de la solución. Nuestra solución será básica ya que el cianuro es la base conjugada del ácido cianhídrico (HCN).

pOH = -\log [OH^-]
pOH = -\log \sqrt{\frac{K_b}{M}}
pOH = -\log \sqrt{\frac{1.61 \times 10^{-5}}{M}}

Donde M es la molaridad de la solución. Si asumimos una molaridad hipotética de 0.1 M, podemos calcular el pOH y luego el pH:
pOH = -\log \sqrt{\frac{1.61 \times 10^{-5}}{0.1}} \approx 3.59
pH = 14 - pOH \approx 10.41

Entonces, el pH de la solución sería aproximadamente 10.41, lo cual indica que se encuentra en el rango de pH permisible para una solución básica.

\textbf{Respuesta:} El pH de la solución sería aproximadamente 10.41, lo cual está en el rango de pH permisible para una solución básica.

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