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.
![**Question:**
What is the pH of a 1.7 M solution of HClO₄?
**Response:**
pH = \( 4.75 \times 10^{-2} \)
**Feedback:**
Incorrect
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*Explanation:*
This question asks for the calculation of the pH of a 1.7 M solution of perchloric acid (HClO₄), which is a strong acid and completely dissociates in water. The provided answer, \( 4.75 \times 10^{-2} \), is incorrect. To find the correct pH, you would calculate it from the concentration of hydronium ions directly:
For strong acids:
\[ \text{pH} = -\log [H^+] \]
Since HClO₄ is a strong acid, the concentration of \( [H^+] \) is equal to the concentration of HClO₄, which is 1.7 M. Therefore, the correct calculation should be:
\[ \text{pH} = -\log(1.7) \]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Faf8dd5bb-1368-4a10-9929-9294802d0b74%2F7264116b-81bd-4a98-b4f1-e2d2444661a7%2Fix07bdj_processed.png&w=3840&q=75)
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