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.
![**Identify the Conjugate Acid-Base Pairs in the Following Equation:**
\[ \text{NH}_4^+(aq) + \text{H}_2\text{O}(l) \rightleftharpoons \text{H}_3\text{O}^+(aq) + \text{NH}_3(aq) \]
In this equation, the process involves transferring protons between the reactants and products, identifying conjugate acid-base pairs. Here's a breakdown of the pairs:
- NH₄⁺ (ammonium) donates a proton to become NH₃ (ammonia). Therefore, NH₄⁺ is the conjugate acid, and NH₃ is its conjugate base.
- H₂O (water) accepts a proton to form H₃O⁺ (hydronium). Thus, H₂O acts as the base, and H₃O⁺ is its conjugate acid.
Understanding these relationships is essential for mastering acid-base chemistry, as it helps predict the direction of chemical equilibrium and the strength of acids and bases.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F551637be-7a52-44bd-9b06-307a09d9ac69%2Fcf2f2850-9ffe-4213-89a9-063ad5350b10%2Fb4lkoai_processed.jpeg&w=3840&q=75)
Given -
NH4+ (aq) +H2O (l) -> H3O+ (aq) +NH3(aq)
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