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?
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Recently Asked Questions
- I was doing an experiment to determine the ionization constant, KIn, for an indicator, bromophenol blue solution. A set of test-tubes is prepared with pairs of tubes containing different concentrations of HIn or In, so they (each pair) differ in colour when viewed from the side. Then, a buffer solution with known pH is added to some bromophenol blue solution, which is then compared to the pairs of test-tubes to find out the set with the colour that is the closest. The ratio of (In) to (HIn) can then be used to calculate the pKIn value. My teacher says that the buffer solution used for the experiment should have a pKa value very close to the pKIn value of the indicator, otherwise the colour of the indicator in the buffer solution could never match that of the indicator solution prepared. I don't understand why these two values have to be close to each other, and why can't the colours be matched? 2220409
- Hello, I want to know how can we decide which indicator should be used in titration by viewing a pH curve? 180309
- I've prepared two buffer solutions of pH 5.2 and 8.8. The acidic buffer was ammonia with ammonium chloride; and the base buffer was ethanoic acid with sodium ethanoate. A pH meter was used to measure the values. I was wondering why the pH 8.8 buffer was less stable over a period of time than many other buffers? 180309
Tests
updated: 09 July 2003
