Question
calculating the pH of a 0.10 mol/L aqueous solution of NaCl
Answers
GPT-4o mini
Sodium chloride (NaCl) is a neutral salt formed from the reaction of a strong acid (HCl) and a strong base (NaOH). It dissociates completely in water into sodium ions (Na\(^+\)) and chloride ions (Cl\(^-\)). Neither of these ions reacts with water to produce H\(^+\) or OH\(^-\) ions, meaning NaCl does not affect the pH of the solution significantly.
In a 0.10 mol/L solution of NaCl:
1. The NaCl completely dissociates into Na\(^+\) and Cl\(^-\):
\[
\text{NaCl} \rightarrow \text{Na}^+ + \text{Cl}^-
\]
2. Since neither ion hydrolyzes to produce H\(^+\) or OH\(^-\), the solution remains neutral.
The pH of a neutral solution at 25°C is approximately 7. Therefore, the pH of a 0.10 mol/L aqueous solution of NaCl is:
\[
\text{pH} = 7.00
\]
In summary, the pH of a 0.10 mol/L NaCl solution is 7.00.
In a 0.10 mol/L solution of NaCl:
1. The NaCl completely dissociates into Na\(^+\) and Cl\(^-\):
\[
\text{NaCl} \rightarrow \text{Na}^+ + \text{Cl}^-
\]
2. Since neither ion hydrolyzes to produce H\(^+\) or OH\(^-\), the solution remains neutral.
The pH of a neutral solution at 25°C is approximately 7. Therefore, the pH of a 0.10 mol/L aqueous solution of NaCl is:
\[
\text{pH} = 7.00
\]
In summary, the pH of a 0.10 mol/L NaCl solution is 7.00.