Calculate the pH of the following buffer solution:

$0.0500 \mathrm{mol} {\mathrm{dm}}^{-3}$ methanoic acid and $0.100 \mathrm{mol} {\mathrm{dm}}^{-3}$ sodium methanoate. (${\mathrm{K}}_{\mathrm{a}}$ of methanoic acid = $1.60 \mathrm{x} {10}^{-4} \mathrm{mol} {\mathrm{dm}}^{-3}$)

Calculate the pH of the following buffer solution:

$0.0100 \mathrm{mol} {\mathrm{dm}}^{-3}$ benzoic acid and $0.0400 \mathrm{mol} {\mathrm{dm}}^{-3}$ sodiumbenzoate. (${\mathrm{K}}_{\mathrm{a}}$ of benzoic acid = $6.3 \mathrm{x} {10}^{-5} \mathrm{mol} {\mathrm{dm}}^{-3}$)

One of the buffers in blood plasma is a mixture of dihydrogen phosphate ions$\left({\mathrm{H}}_2{{\mathrm{PO}}_4}^{-}\right)$ and hydrogenphosphate ions $\left({{\mathrm{HPO}}_4}^{2-}\right)$.

Identify the conjugate acid and base in this buffer.

One of the buffers in blood plasma is a mixture of dihydrogen phosphate ions$\left({\mathrm{H}}_2{{\mathrm{PO}}_4}^{-}\right)$ and hydrogenphosphate ions $\left({{\mathrm{HPO}}_4}^{2-}\right)$.

Write a balanced equation for the equilibrium between these two ions.

Write equilibrium expressions for the solubility product of the following:

$\mathrm{Fe}{\left(\mathrm{OH}\right)}_2$

Write equilibrium expressions for the solubility product of the following:

${\mathrm{Fe}}_2{\mathrm{S}}_3$

Write equilibrium expressions for the solubility product of the following: