Acids And Base Titration Lab

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Introduction

The objectives in this laboratory were to explore the titrations of several known acids and bases as well as observing the mole reactions of the chemical reactions that each compound undertook. The four following acids and bases were used to predict when a set amount of reactant would reach equilibrium: Hydrochloric Acid (HCl), H2SO4 (Sulfuric Acid), NaOH (Sodium Hydroxide), and Ba(OH)2 (Barium hydroxide). An unbalanced equation of each reaction was given so the balanced equation was then able to be calculated. These are as follows including the theoretical ratio between the acid and base:

HCl + NaOH → H2O + NaCl 1:1 H2SO4 + 2NaOH → 2H2O + Na2SO4 1:2 H2SO4 + Ba(OH)2 → 2H2O +BaSO4 1:2 2HCl + Ba(OH)2 → 2H2O +BaCl2 1:1
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HCl was added to the phenolphthalein indicator and deionized water as in the first trial. 4 mL was added quickly and a singular drop was added slowly from there. A reaction took place at exactly 6 mL which was what was predicted. A light pink solution was produced. The second trial went similarly at 6.1 mL. The HCl solution was dumped into the waste bin and rinsed to prepare for the H2SO4 that would follow in the next trial. The final experiment included the titration of H2SO4 with Ba(OH)2. The same procedure was repeated for obtaining the H2SO4 mixture and the titration process. The estimated 12-13 mL addition was very accurate as it took 12.9 mL and 13 mL both trials to produce a reaction. The leftover H2SO4 and Ba(OH)2 were then discarded into the waste bin, rinsed, and the remainder of the lab materials were cleaned and put away.

Data Table 1.1 gives the exact molarity of the acids and bases used during this lab, which was very important when calculating the experimental ratio between the two. Tables 1.2-1.5 show the calculations for each trial and how a experimental ratio was found. The equipment used is listed in table 1.6 as they are referenced quite frequently.

Concentration of Solution: Table 1.1

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