NaCl (s) ⇌ Na+(aq) + Cl-(aq) When adding 6M HCl, the solid white precipitate is observed. When adding 0.1M HCl, no change is observed, no solid white precipitate is observed in the NaCl solution. Explain the similarities and differences by using Le Chatlier's principle.
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.
NaCl (s) ⇌ Na+(aq) + Cl-(aq)
When adding 6M HCl, the solid white precipitate is observed.
When adding 0.1M HCl, no change is observed, no solid white precipitate is observed in the NaCl solution.
Explain the similarities and differences by using Le Chatlier's principle.
When a ionic solute is dissolved in a solvent, the solute gets dissociated into ions in the solution. There will be an equilibrium existing between the dissolved ions and undissolved molecules.
The equilibrium constant of the dissolved ions in the solution is called the solubility product constant (Ksp). It is the product of the equilibrium concentration of the ions or the concentration of the ions in a saturated solution raised to the power of their dissolution reaction coefficient.
Here, the solution is made from the ionic solute NaCl dissolved in water. Therefore, the NaCl exists as Na+ and Cl- ions.
The dissolution of NaCl can be written as follows.
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