Although hydrofluoric acid, HF is a weak acid (Ka of HF is 7.1 × 10–4), its strength actually increases with concentration. One major reason for this behavior of HF is the following reaction, HF + F– ⇌ [F—H∙∙∙∙∙F]– K’ = 5.2 at 25°C which removes F– ions from a solution of HF that contains predominantly the undissociated HF. Write the chemical equation for the dissociation of HF in water. Then, calculate the appropriate equilibrium constant to demonstrate, or explain without performing the calculation, the increase in the strength of HF at high HF concentration. Use Le Chatelier’s principle. The “∙∙∙∙∙” line in the structure of HF2– represents hydrogen bonding, which in this case its strength is expected to be comparable to the H—F covalent bond!
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
- Although hydrofluoric acid, HF is a weak acid (Ka of HF is 7.1 × 10–4), its strength actually increases with concentration. One major reason for this behavior of HF is the following reaction,
HF + F– ⇌ [F—H∙∙∙∙∙F]– K’ = 5.2 at 25°C
which removes F– ions from a solution of HF that contains predominantly the undissociated HF. Write the chemical equation for the dissociation of HF in water. Then, calculate the appropriate equilibrium constant to demonstrate, or explain without performing the calculation, the increase in the strength of HF at high HF concentration. Use Le Chatelier’s principle. The “∙∙∙∙∙” line in the structure of HF2– represents hydrogen bonding, which in this case its strength is expected to be comparable to the H—F covalent bond!
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