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Accepted Answer
| Question: | 500 mL Acetic acid (CH3COOH) + 200 mL Ammonia (NH3) |
| Solution: | This is not a simple titration problem. It involves a reaction between a weak acid (acetic acid) and a weak base (ammonia). The resulting solution will contain ammonium acetate, which is a salt of a weak acid and a weak base. To determine the final pH, we would need the concentrations of the acetic acid and ammonia solutions. 🧮 |
| Chemical Equation: | CH₃COOH(aq) + NH₃(aq) ⇌ CH₃COO⁻(aq) + NH₄⁺(aq) |
| Explanation: | Acetic acid and ammonia react in an acid-base neutralization reaction 🧪. Acetic acid donates a proton (H⁺) to ammonia, forming acetate (CH₃COO⁻) and ammonium (NH₄⁺) ions. The pH of the resulting solution depends on the relative strengths of the acid and base and their initial concentrations. It's not a simple titration because we're mixing both acid and base without knowing their concentrations. 🫙 |
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