A buffer solution contains 0.366 M C,H5NH3CI and 0.229 M C,H5NH2 (aniline). Determine the pH change when 0.064 mol KOH is added to 1.00 L of the buff pH after addition – pH before addition = pH change =
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.
![### Buffer Solution pH Change Calculation
A buffer solution contains **0.366 M C6H5NH3Cl** and **0.229 M C6H5NH2 (aniline)**. Determine the pH change when **0.064 mol KOH** is added to **1.00 L** of the buffer.
**Expression for pH Change:**
\[ \text{pH after addition} - \text{pH before addition} = \text{pH change} = \text{______} \]
In this scenario, you will calculate how the addition of a strong base (KOH) affects the pH of the buffer solution containing aniline and its conjugate acid (C6H5NH3+). Utilize the buffer equation and stoichiometric changes to determine the overall pH shift.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F03ba95c9-584b-483d-8f8a-8f0f9c4c55b7%2F9aed30d4-7c3e-4ea7-9384-875854934510%2Fcebv56_processed.png&w=3840&q=75)
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