A buffer solution contains 0.368 M NaH₂PO4 and 0.232 M K₂HPO4. Determine the pH change when 0.055 mol HCIO4 is added to 1.00 L of the buffer. pH change = 0.05
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 0.298 M CH₃NH₃Br and 0.350 M CH₃NH₂ (methylamine). Determine the pH change when 0.089 mol HI is added to 1.00 L of the buffer. (Assume \( K_b \) (CH₃NH₂) = \( 4.2 \times 10^{-4} \).)
**Formula:**
\[ \text{pH after addition} - \text{pH before addition} = \text{pH change} = \underline{\qquad\qquad\qquad} \]
This formulation guides students through calculating the pH change in a buffer solution when a strong acid is introduced.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F30f1d269-be25-4568-9778-815e824582cd%2Fa7993b09-6d55-4c49-894a-311bf35f63a3%2Fuchmfui_processed.png&w=3840&q=75)
Step by step
Solved in 4 steps with 60 images
