When titrating a solution of potassium hydroxide against nitric acid, a student ran in too much acid from the buret. which ions would not be present in the erlenmeyer flask at this point, ignoring the ionization of water?
Question: When titrating a solution of potassium hydroxide against nitric acid, a student ran in too much acid from the buret. which ions would not be present in the erlenmeyer flask at this point, ignoring the ionization of water?
When titrating a solution of potassium hydroxide (KOH) against nitric acid (HNO3), the reaction between the two would produce potassium nitrate (KNO3) and water (H2O). However, if the student adds too much nitric acid, some of the ions that would not be present in the Erlenmeyer flask at this point are the hydroxide ions (OH-) from potassium hydroxide (KOH).
The reaction between KOH and HNO3 is as follows:
KOH + HNO3 → KNO3 + H2O
If there is excess nitric acid, it means that all the hydroxide ions from KOH have reacted with nitric acid to form water, and no hydroxide ions would be left in the solution. The only remaining ions in the flask would be potassium ions (K+) and nitrate ions (NO3-) from potassium nitrate (KNO3).
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