Given that Kw for water is 2.4 x 10-14 at 37 °C, calculate the pH of a neutral aqueous solution at 37 °C, which is the normal human body temperature. pH = Is a pH = 7.00 solution acidic, basic, or neutral at 37 °C?
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.
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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.
![**Educational Content on pH Calculation**
**Problem Statement:**
Given that \( K_w \) for water is \( 2.4 \times 10^{-14} \) at 37 °C, calculate the pH of a neutral aqueous solution at 37 °C, which is the normal human body temperature.
**Calculation:**
\[ \text{pH} = \]
**Question:**
Is a pH = 7.00 solution acidic, basic, or neutral at 37 °C?
- ○ acidic
- ○ basic
- ○ neutral
**Instruction:**
To determine the pH, use the formula for the water dissociation constant \( K_w \), which is the product of the hydrogen ion concentration \([H^+]\) and the hydroxide ion concentration \([OH^-]\) in water:
\[ K_w = [H^+][OH^-] \]
For a neutral solution at 37 °C, \([H^+]\) and \([OH^-]\) are equal, so:
\[ K_w = [H^+]^2 \]
Solve for \([H^+]\) and subsequently calculate the pH using the formula:
\[ \text{pH} = -\log([H^+]) \]
Once calculated, compare the pH value with 7.00 to determine if the solution is acidic, basic, or neutral under these conditions.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0e989a36-a976-4f9a-8f93-2801096d9bdd%2Ff16ea2b1-23b3-4825-a97b-66f954a3bb11%2Fq9djvsc_processed.png&w=3840&q=75)
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