Acid-base equilibria
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The equilibrium law helps to make sense of the behaviour of acids and bases. The theory helps to account for the behaviour of strong and weak acids as well as explaining the the way that indicators and buffer solutions work.
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Tutorials
- Sorted FAQs on Acid-Base equilibria
- Ionisation constants for acids: audio tutorial
- Is calcium hydroxide a strong or a weak base?
Webguides
Recently Asked Questions
- I have just done an investigation of the equilibrium between ethanoic acid and propan-1-ol to give ester and water. We have been asked to find the equilibrium constant for the reaction. I know that we have to leave liquids and solids out of equilibrium constants, but why do we have to include all the concentrations in the calculation of the equilibrium constant when all the species involved in this reaction were liquids? The conc. sulfuric acid used as the catalyst for this reaction quite naturally contains some water, and water is one of the products of the esterification. I would like to know how the presence of a small amount of water will affect the position of the equilibrium , and how this water affects the value determined for the equilibrium constant? Could some other acid be used as the catalyst? 110310
- Q.1: What type of reaction is: acid + carbonate --> salt + water + carbon dioxide? Is there a name for it? I wanted to say this is a ??? reaction. Is it a neutralisation or is there no name for it? Q.2: Also, is solvation energy the same as the enthalpy of hydration - or are they opposites? Q.3: I’m looking at adding sodium carbonate to a solution of calcium ions, and trying to explain why calcium carbonate forms. Sodium ions are weakly attracted to water whereas calcium ions are strongly attracted to water, so why does calcium carbonate form - surely calcium ions are too strongly attracted to water, so sodium carbonate would remain as it is weakly attracted to water? 110310
- How can you determine the Ka of an indicator without using spectrophotometry? 1110310
Tests
updated: 09 July 2003
