# Equivalence Point Lab Report

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Pre-lab:

An endpoint is indicated by some form of indicator at the end of a titration. The equivalence point is when the moles of a standard solution equal the moles of a solution of an unknown concentration. The endpoint of the solution should be a faint pink color. If the color is too dark of a pink that means that it is overly titrated.
The independent variable is the amount of base being added to the solution. The dependant variable is the indicator. The constant variable is the acid which is in the flask.
When the solid acid dissolves to form ions, 1 mole of H+ ions are produced for every mole of acid being used.
Molarity is used to calculate moles per liter of solution.
The most dangerous part of this lab is the risk of getting
We dealt with both acids and bases. An acidic solution contains more hydroxide ions than hydrogen ions. The PH scale was developed as a more convenient way to express H+ ion concentrations. Acids have a PH that ranges from 0-6 and bases have a PH of 8-14. Unlike acids, bases contain more OH- ions than H+ ions. If the PH of a solution is 7, then the solution is neutral. Titration is a method for determining the concentration of a solution by reacting it with another solution of a known concentration. For this lab we used 1 molar hydrochloric acid to find the molarity of an unknown base. The equivalency point was reached when the moles of H+ ions equal the moles of OH-.

Procedure and Observations:

In this lab we used a 50 ml burette, a 250 ml beaker, and a 250 ml flask. The burette was filled with the base solution NaOH to the 0 mark. The beaker was filled with 50 ml of HCL and two drops of phenolphthalein indicator solution. The indicator is used to show when the titration point is. This is observed due to the color change. The beaker was placed underneath the burette. It was also on top of a white sheet of paper. The paper was place in order to easily see the faint pink color change when it was to