Lab Report Chemical Reactions

Analysis of an Acid by Titration with Sodium Hydroxide

Introduction
Titration is the method used to determine the amount or concentration of an unknown substance. One solution is added toanother one until the two solutions react completely.
An indicator is used to determine whether an acid has neutralized a base or vice versa, it is neutralized when the number of moles of acid is equal tothe number of moles of base. When an acid is titrated with a base while using the indicator, it should change its color.
On one hand a strong acid or base solution is the one where the ionizationis 100% complete. This means that an acid with a certain molarity dissociates completely into ions of the same molarity. On the other hand a weak acid or base incompletely ionizes in aqueos solution.An example of these neutralizations is
HCl (aq) + NaOH(aq) NaCl(aq) + H2O(l)
Hydrochloric acid sodium Hydroxide Sodium chloride water
where a strong acid is titrated with a stringbase.
A dilution equation is used to solve the concentration of the solutions.
Equation: M NaOH V NaOH = MHCl V HCl
Where M NaOH is the concentration of the sodium hydroxide
V NaOH is the volumeof sodium hydroxide used to reach the end point
MHCl is the concentration of the hydrochloric acid
V HCl is the volume of hydrochloric acid taken

Procedure
Part I
For the preparation ofthe indicator approximately 30 grams of red cabbage were weighted and the leaves were finely shred into small pieces. Approximately 50 mL of DI water were poured in a large beaker and then brought to aboil. The shredded leaves were added to the beaker and it was covered with a watch glass. When the solution turned into dark purple it was set apart to cool off and then separated for the four peoplein our group.
In a separate Erlenmeyer flask approximately 10.00mL of acid (HCl) were added, as well as ~20 mL of DI water and a few drops of the anthocyanin indicator.
A buret was filled with...