In a titration, 20.0 mL of sodium hydroxide solution needs 15.0 mL of 0.100 M hydrochloric acid to…
Contributed by StemPy LabTry it on paper first. A hint, the key idea and the worked solution are here when you need them.
In a titration, of sodium hydroxide solution needs of hydrochloric acid to reach the end point. Find the concentration of the sodium hydroxide. What happens to the pH near the end point?
Need a reminder? The key ideaShow
Moles = concentration (M) × volume (L); millimoles = M × mL. At neutralisation the moles of equal the moles of . For a one to one reaction, ; otherwise use the ratio from the equation.
The worked solution
Have you tried it?
Work it out on paper first. It is fine to get stuck or make a mistake: that is how we learn. When you are ready, go through the solution one step at a time, and check each step against your own.
Step 1. Acid. .
Step 2. Base. .
Step 3. pH. It jumps sharply, by several units, for one drop near the end point.
Answer: .
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