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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.
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CB stands for "Conjugate Base." In the context of acid-base chemistry, when an acid loses a proton (H+), it forms a conjugate base. For example, in the reaction HCl + H2O→ H3O+ + Cl-, H2O is the base and it accepts a proton (H+) from HCl to form its conjugate acid, H3O+. Likewise, HCl loses a proton (H+) to form its conjugate base, Cl-. The conjugate base of an acid is always one less proton than the original acid.
acidity increases with the stability of the conjugate base (CB). This is because the stability of the CB indicates how well it can accommodate the negative charge that results from the removal of a proton( H+) from the acid. The more stable the CB, the better it can stabilize the negative charge, making the loss of the proton more favorable and the acid stronger. Conversely, if the CB is unstable, it will not be able to stabilize the negative charge as effectively, and the acid will be weaker.
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