Question

Calculate the hydronium ion concentration and $\mathrm{pH}$ for a $0.015 \mathrm{M}$ solution of sodium formate, $\mathrm{NaHCO}_2$.

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In this task, we need to calculate H$^+$ ion concentration and pH.

First we need to determine where the ion comes from.

If they are derived from a strong acid and a strong base they do not undergo hydrolysis and thus form neutral solutions ( no effect on solution pH ).

If they are derived from weak acid or weak base, they undergo hydrolysis.

Hydrolysis is the cleavage of molecules of covalent chemical compounds in a reaction with water, where the hydrogen atom of water combines with one, and the hydroxyl group with the other decomposition product

If a salt contains the ion of a weak acid, the ion produces an basic solution (OH$^-$ is formed):

$\text{A^-} + \text{H_2O} \rightleftharpoons \text{HA} + \text{OH^-}$

If a salt contains the ion of a weak base, the ion produces an acidic solution (H$_3$O$^+$ is formed):

$\text{BH^+} + \text{H_2O} \rightleftharpoons \text{B} + \text{H_3O^+}$