In the titration of 100 mL of 0.1 M NaOH with 0.1 M HCl, what is the expected resultant solution at the equivalence point?
Understand the Problem
The question is asking about the nature of the resultant solution at the equivalence point during the titration of NaOH with HCl. The equivalence point occurs when the amount of NaOH completely neutralizes the amount of HCl, and we're interested in determining if the resultant solution is basic, acidic, neutral, or dependent on initial conditions.
Answer
Neutral solution with pH 7.
The expected resultant solution at the equivalence point is neutral, with a pH of 7.
Answer for screen readers
The expected resultant solution at the equivalence point is neutral, with a pH of 7.
More Information
In the titration between a strong acid (HCl) and a strong base (NaOH), at the equivalence point, the concentrations of H+ and OH- ions are equal, resulting in a neutral pH of 7.
Tips
A common mistake is assuming the pH will not be 7 due to other conditions, but with strong acids and bases, it is neutral.
Sources
- Titration of a Strong Acid With A Strong Base - Chemistry LibreTexts - chem.libretexts.org
- Consider the titration of 100 ml of 0.1 M HCl with 0.1 M NaOH - Socratic - socratic.org
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