Note that any solid or liquid reactants or products , or solvents such as water are considered to be pure substances, and so have an activity that is equal to 1. Thus for the ionization of HF.
When you are dealing with acids, the equilibrium constant is generally called an acid dissociation constant , and is written as K a. The larger the value of K a , the greater the extent of ionization and the and the higher the resulting concentration of the hydronium ion.
Because the concentration of the hydronium ion is directly correlated with acidity, acids with a large value of K a are termed strong acids. Table 8. HNO 3. HClO 4. These metrics are regularly updated to reflect usage leading up to the last few days. Citations are the number of other articles citing this article, calculated by Crossref and updated daily. Find more information about Crossref citation counts.
The Altmetric Attention Score is a quantitative measure of the attention that a research article has received online. Clicking on the donut icon will load a page at altmetric. Find more information on the Altmetric Attention Score and how the score is calculated. HF may not be dissociated at 0 K solely by water molecules because the HF H bond is stronger than the OH H bond, against the expectation that the dissociated HF H 2 O n would be more stable than the undissociated one in the presence of a number of water molecules.
The dissociation would be possible for only a fraction of a number of hydrated HF clusters by the Boltzmann distribution at finite temperatures. Corresponding author.
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Videla , Javier Rodriguez , and Daniel Laria. The Journal of Physical Chemistry A , 36 , The Journal of Physical Chemistry A , 49 , The Journal of Physical Chemistry A , 41 , Zakharenko , S. Karthikeyan , and Kwang S. Journal of Chemical Theory and Computation , 7 10 , Re: Why is HF a weak acid? Post by Marisa Gaitan 2D » Wed Dec 02, pm Because the HF bond is so short, it is very strong and therefore makes it difficult for the bond to be broken.
In other words it won't dissociate completely. Stronger acids such as HCl and HBr have weaker bonds and are more likely to dissociate completely. None of the strong acids create hydronium-anion bonds like this. The hydronium can't act as an acid when it's bonded to the fluoride ion, so HF is not a strong acid. It's actually the only hydrohalic acid that isn't strong. It's considered a weak acid because it doesn't completely dissociate into its ions in water.
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