a. Choose a chemical equation showing how the following species can behave as indicated when dissolved in water: HCO3 as an acid. ○ HCO3¯¯ (aq) + H₂O(1) ⇒ CO3² (aq) + H3O+ (aq) ○ HCO3¯¯(aq) + H₂O(1) ⇒ CO3² (aq) + H+ (aq) OHCO3¯¯(aq) + H₂O(1) ⇒ CO3¯(aq) + H+ (aq) O HCO3(aq) + H₂O(1) ⇒ H₂CO3(aq) + OH¯(aq) b. Choose a chemical equation showing how the following species can behave as indicated when dissolved in water: 2- CO3²- as a base. 2- CO3²- (aq) + H₂O(1) ⇒ H₂CO3(aq) + OH¯ (aq) CO3² (aq) + H₂O(1) ⇒ HCO3¯(aq) + OH¯(aq) CO3²- (aq) + H₂O(1) ⇒ H₂CO3(aq) + H+ (aq) O CO32- (aq) + H₂O(1) ⇒ HCO3¯(aq) + H+ (aq) c. Choose a chemical equation showing how the following species can behave as indicated when dissolved in water: HN₂O₂ as an acid. ○ HN₂O₂¯(aq) + H₂O(1) ⇒ H₂N2O₂ (aq) + OH¯(aq) ○HN₂O₂¯(aq) + H₂O(1) ⇒ H₂N2O2 (aq) + H3O+ (aq) ○ HN₂O₂¯¯ (aq) + H₂O(1) ⇒ N₂O₂² (aq) + H+ (aq) ○ HN₂O₂¯(aq) + H₂O(1) ⇒ N₂O₂² (aq) + H3O+ (aq)
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.
Bronsted-Lowry acid-base theory: The Bronsted-Lowry acid-base theory states that the acid is a substance that gives H+ ions and the base is a substance that accepts the H+ ions.
The species which are differing by the H+ are called conjugate acid-base pairs.
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