The structural formula for acetic acid is shown in Table Replacing hydrogen atoms on the carbon with chlorine atoms causes an increase in acidity, as follows:
Acid | Formula | Ka(25 °C) |
Acetic | CH3COOH | 1.8 × 10-5 |
Chloroacetic | CH2ClCOOH | 1.4 × 10-3 |
Dichloroacetic | CHCl2COOH | 3.3 × 10-2 |
Trichloroacetic | CCl3COOH | 2 × 10-1 |
Using Lewis structures as the basis of your discussion, explain the observed trend in acidities in the series. Calculate the pH of a 0.010 M solution of each acid.
Table Some Weak Acids in Water at 25°c
Acid | Structural Formula* | Conjugate Base | Ka |
Chlorous (HClO2) | H- O- Cl- O | ClO2- | 1.0 × 10-2 |
Hydrofluoric (HF) | H-F | F- | 6.8 × 10-4 |
Nitrous (HNO2) | H- O- N= O | NO2- | 4.5 × 10-4 |
Benzoic (C6H5COOH) | C6H5COO- | 6.3 × 10-5 | |
Acetic (CH3COOH) |
| CH3COO- | 1.8 × 10-5 |
Hypochlorous (HOCl) | H- O- Cl | OCl- | 3.0 × 10-8 |
Hydrocyanic (HCN) | H -C ≡N | CN- | 4.9 × 10-10 |
Phenol (HOC6H5) |
| C6H5O- | 1.3 × 10-10 |
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