2. A buffer solution contains H2CO3 and HCO3¯, resulting in the equilibrium shown by the reaction below. According to this reaction and LeChatelier's principle, what happens when the following is added to this buffer solution? H2CO3 + H2O = HCO3 + H3O* Reaction will go Which species will increase in concentration? Which species will decrease in concentration? Added component forward/backward (Right/left) (reactants/products) (reactants/products) Rigth Le ft Righ Reactants Product Reactants H2CO3 Product Reactants Product H3O* H2O
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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The equilibrium reaction given is,
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