When a 20.0 mL sample of a 0.483 M aqueous nitrous acid solution is titrated with a 0.430 M aqueous potassium hydroxide solution, what is the pH at the midpoint in the titration? pH =
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.
![**Titration of Nitrous Acid with Potassium Hydroxide**
When a 20.0 mL sample of a 0.483 M aqueous nitrous acid solution is titrated with a 0.430 M aqueous potassium hydroxide solution, what is the pH at the midpoint in the titration?
**Calculation:**
pH = [Insert calculated pH value here based on details or class notes]
**Explanation:**
In the titration of a weak acid, such as nitrous acid, with a strong base, such as potassium hydroxide, the pH at the midpoint equals the pKa of the acid. This is because, at the midpoint, the concentrations of the acid and its conjugate base are equal, simplifying the Henderson-Hasselbalch equation to:
\[ \text{pH} = \text{pKa} + \log \left(\frac{[\text{Base}]}{[\text{Acid}]}\right) = \text{pKa} \]
Nitrous acid (\( \text{HNO}_2\)) is a weak acid and the \( \text{KOH} \) is a strong base that will completely dissociate in solution.
For educational purposes, this concept can demonstrate the utility of the Henderson-Hasselbalch equation in calculating the pH of buffer solutions and understanding acid-base equilibria.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9aca1772-1e0c-4e24-86a8-736d39b6760d%2F3a6ce2d0-d8cf-4b5d-83ca-81e31cb64ad3%2Fy2qwjrk_processed.jpeg&w=3840&q=75)
we need to calculate the pH of solution at titration midpoint
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