| Weak Acid | Ka | Weak Base | Kb |
| CH3COOH (Acetic Acid) | 1.8 X 10-5 | NH3 (Ammonia) | 1.76 X 10-5 |
| C6H5COOH (Benzoic Acid) | 6.5 X 10-5 | C6H5NH2 (Aniline) | 3.9 X 10-10 |
| CH3CH2CH2COOH (Butanoic Acid) | 1.5 X 10-5 | (CH3CH2)2NH (Diethyl amine) | 6.9 X 10-4 |
| HCOOH (Formic Acid) | 1.8 X 10-4 | C5H5N (Pyridine) | 1.7 X 10-9 |
| HBrO (Hypobromous Acid) | 2.8 X 10-9 | CH3CH2NH2 (Ethyl amine) | 5.6 X 10-4 |
| HNO2 (Nitrous Acid) | 4.6 X 10-4 | (CH3)3N (Trimethyl amine) | 6.4 X 10-5 |
| HClO (Hypochlorous Acid) | 2.9 X 10-8 | (CH3)2NH (Dimethyl amine) | 5.4 X 10-4 |
| CH3CH2COOH (Propanoic Acid) | 1.3 X 10-5 | CH3CH2CH2NH2 (Propylamine | 3.5 X 10-4 |
| HCN (Hydrocyanic Acid) | 4.9 X 10-10 | |
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When you titrate 17.2 mL of a 0.14 M solution of(CH3)3N (trimethylamine), it required 17.0 mLof hydrochloric acid solution. Assuming that you have reached theequivalence point, what is the pH of the resulting solution?
