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.
![For many weak acid or weak base calculations, you can use a simplifying assumption to avoid solving quadratic equations.
Ka =
[HA] — х
[НА]
Classify these situations by whether the assumption is valid or the quadratic formula is required.
Assumption is valid
Quadratic formula is required
Answer Bank
[HA] = 0.001 M
[HA] = 0.01 M
Ka = 1 x 10¬4
[HA] = 0.1 M
[HA] = 1 M
[HA] = 0.01 M
Ka = 1 × 10–5
Ką = 1 × 10-3
Ka = 1 × 10–3
Ka = 1 × 10-5](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcbd14ffb-bc40-4ae3-8f40-cba31e255ccc%2Fd45d296b-ace0-40bd-a20e-e26c886a1bdc%2F0v13l06_processed.png&w=3840&q=75)
If the concentration of [HA] >> x then you can neglected x value then for this condition Assumption is valid. And also Ka value is very less then also assume this assumption
If the concentration of is very less [HA] < x then you can used quadratic equation formula.
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