A buffer solution contains 0.316 M NaH₂PO4 and 0.209 M Na₂HPO4. Determine the pH change when 0.056 mol HBr is added to 1.00 L of the buffer. 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 Analysis**
A buffer solution contains concentrations of two compounds: **0.316 M NaH₂PO₄** and **0.209 M Na₂HPO₄**.
**Objective:**
Determine the pH change when **0.056 mol HBr** is added to **1.00 L** of the buffer.
**Task:**
Calculate the pH change.
**Input Field:**
pH change = [ ]
This setup involves adding a strong acid, hydrobromic acid (HBr), to a buffer solution. The challenge is to accurately compute the resulting change in pH, drawing upon concepts like buffer capacity and the Henderson-Hasselbalch equation.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1ae39ebd-5819-4f56-bd42-4d335d0770f9%2Fcfcd0a6c-5886-4e25-97e3-c6a9e2a7c274%2F4uojqmg_processed.png&w=3840&q=75)
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