A weak acid, HA, with a molarity = 0.115 M was found to have a pH = 3.87. Calculate the ionization constant, Ka. O 1.58 x 10-7 O 1.17 x 10-3 O 8.51 x 10-5 5.18 x 10-7
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.
![**Problem Statement:**
A weak acid, HA, with a molarity = 0.115 M was found to have a pH = 3.87. Calculate the ionization constant, \( K_a \).
**Options:**
○ 1.58 x 10^-7
○ 1.17 x 10^-3
○ 8.51 x 10^-5
○ 5.18 x 10^-7
**Explanation:**
This problem requires calculating the acid dissociation constant (\( K_a \)) for a given weak acid, HA, using its provided molarity and pH. The \( K_a \) value is a crucial parameter that indicates the strength of the weak acid in aqueous solution.
To solve this, steps involve:
1. Calculating the concentration of hydrogen ions \([H^+]\) from the given pH.
2. Using the given initial concentration of the weak acid.
3. Applying the formula for the acid dissociation constant.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4f14b19b-124e-4186-8aa7-13c05fb6d55d%2F7bce83ee-e635-456d-91fb-c900cf76d50c%2Fb1f4agd_processed.jpeg&w=3840&q=75)
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