How will this affect the final calculation of the molarity of HC2H3O2
A small amount of vinegar adhering to the side of the flaks was left unreacted when the end point was thought to have been reached.
After rinsing any drops of vinegar adhering to the side of the flask, another 20ml of deionized water was added to the vinegar in the flask.
Titration is a type of experiment in which the concentration of an unknown solution is determined by using a solution of a known concentration (known as titrant).
The concentration of an unknown solution is determined on the basis of the end point at which the whole acid present in the reaction gets neutralized by a base. The indicator is added in the titration to detect the end-point of the titration. At the end point, the color of the solution becomes drastically changed.
A small amount of vinegar adhered to the side of the flask remains unreacted at the end point of the titration, this means that, a small amount of acetic acid present in vinegar remains unreacted. In such situation, the calculated value of the molarity of vinegar will correspond to the lesser volume of the solution that the actual volume added in the titration flask. Therefore, the calculated value of the molarity of the vinegar solution will be greater than the actual one.
On adding 20 mL of deionized water to the titration flask that contains vinegar solution, the concent...
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