A buffer solution contains 0.368 M NaH₂PO4 and 0.232 M K₂HPO4. Determine the pH change when 0.055 mol HCIO4 is ad 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.
![A buffer solution contains 0.368 M NaH₂PO₄ and 0.232 M K₂HPO₄. Determine the pH change when 0.055 mol HClO₄ is added to 1.00 L of the buffer.
pH change = [ ]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F16140577-95fc-4112-8b0a-8e4365545066%2Ff3e3b148-a960-4163-8d93-91ddb523902c%2Fg1ncq2_processed.png&w=3840&q=75)
![A buffer solution contains 0.298 M \( \text{CH}_3\text{NH}_3\text{Br} \) and 0.350 M \( \text{CH}_3\text{NH}_2 \) (methylamine). Determine the pH change when 0.010 mol HI is added to 1.00 L of the buffer. (Assume \( K_b (\text{CH}_3\text{NH}_2) = 4.2 \times 10^{-4} \).)
pH after addition − pH before addition = pH change = [Input Box]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F16140577-95fc-4112-8b0a-8e4365545066%2Ff3e3b148-a960-4163-8d93-91ddb523902c%2F5xdgfoe_processed.png&w=3840&q=75)
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