How will the amount of the unionized acid HA be affected (increased, decreased, unaffected can’t predict) for the weak acid, HA. HA + H2O <---> H3O+ + A- If the following changes are made: The solution is diluted with water A strong acid like HCl is added to the solution The soluble ionic salt, NaA, is added to the solution A strong soluble base such as NaOH is added to the solution What is the effect on the Ka for the weak acid, HA in question 3 if: The solution is diluted with water The soluble ionic salt, NaA is added to the solution A 0.2 M solution of the weak acid, HA, has a pH of 4.24 HA + H2O H3O+ + A- What is the [H3O+] of the solution Calculate the Ka for the weak acid Calculate the % ionization for the acid
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.
- How will the amount of the unionized acid HA be affected (increased, decreased, unaffected can’t predict) for the weak acid, HA.
HA + H2O <---> H3O+ + A-
If the following changes are made:
- The solution is diluted with water
- A strong acid like HCl is added to the solution
- The soluble ionic salt, NaA, is added to the solution
- A strong soluble base such as NaOH is added to the solution
- What is the effect on the Ka for the weak acid, HA in question 3 if:
- The solution is diluted with water
- The soluble ionic salt, NaA is added to the solution
- A 0.2 M solution of the weak acid, HA, has a pH of 4.24
HA + H2O H3O+ + A-
- What is the [H3O+] of the solution
- Calculate the Ka for the weak acid
- Calculate the % ionization for the acid
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