What is the equilibrium constant of citric acid?
Citric acid falls into the category of polyprotic acids, which are acids that have more than one acidic hydrogen that can react with water to produce the hydronium ion,
Citric acid's molecular formula is
When placed in water, citric acid will ionize in a step-wise manner
For each of these three steps we have a different value for the acid's dissociation constant,
Step (1): Step (2): Step (3): Notice that all three dissociation constants are smaller than 1, which is characteristic of a weak acid. Another interesting observation is that the dissociation constant for step (3) is very, very small, which means that the number of acid molecules that undergo ionization in this stage is, for all intended purposes, zero.
By signing up, you agree to our Terms of Service and Privacy Policy
The equilibrium constant of citric acid, represented as ( K_a ), depends on the specific reaction involving citric acid. Citric acid can undergo multiple reactions, each with its own equilibrium constant. Therefore, without specifying the reaction involving citric acid, it is not possible to provide a single equilibrium constant.
By signing up, you agree to our Terms of Service and Privacy Policy
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
- How does solubility affect equilibrium?
- Why is Ka important in chemistry?
- How do we explain the normal boiling points of #"ethanol"# (#78.4# #""^@C#), #"methanol"# (#64.7# #""^@C#), #"ethane"# (#-89# #""^@C#), #"ethyl acetate"#, (#77.1# #""^@C#), and #"methyl acetate"# (#56.9# #""^@C#)?
- Does dissolution with dissociation only happen with salts?
- Given the reaction...#SO_2(g) + NO_2(g) rightleftharpoons SO_3(g) + NO(g)#...for which #K_"eq"=3.75#, what will be the equilibrium concentrations of products and reactants?

- 98% accuracy study help
- Covers math, physics, chemistry, biology, and more
- Step-by-step, in-depth guides
- Readily available 24/7