Acid-base theory

Broenstedt acid-base reaction

Exercise 1

   

Write the equations of the following reactions. In the case of reactions between weak acid and weak base, calculate the equilibrium constant. Which can be considered complete, incomplete or no?

a) Bromhydric acid and fluoride ion

$C_6H_5COOH$ $+$ $ F^-$ $ \rightleftarrows $ $C_6H_5COO^- $ $+$ $ HF$ $K = 9.33\cdot 10^{-2}$ (incomplète )

b) Formic acid and hypochlorite ion

$HCOOH$ $ +$ $ ClO^-$ $ \rightarrow $ $HCOO^-$ $ + $ $HClO$ $K = 3.55\cdot 10^3$ (complete.)

c) Chloric acid and dichloroethanoate ion

$HClO_3$ $ +$ $ CHCl_2COO^-$ $ \rightleftarrows $ $ClO_3^-$ $ + $ $CHCl_2COOH$ $K = 2.00 \cdot10^2$ (incomplete )

d) Iodoethanoic acid and fluoride ion

$CH_2ICOOH$ $ + $ $F^-$ $ \rightleftarrows $ $CH_2ICOO^-$ $ + $ $HF$ $K = 1.02$ (incomplete )

e) Perchloric acid and hydroxyde ion

$ H_3O^+$ $ +$ $ OH^-$ $\rightarrow $ $ H_2O$ $ + $ $H_2O $ (both strong/ complete)

f) Cyanhydric acid and chlorite ion

$HCN$ $ +$ $ ClO_2^-$ $ \leftarrow $ $ CN^-$ $ + $ $HClO_2$ $K = 4.90\cdot 10^{-8}$ (none)