Titration Lab Abstract.
The molarity of HCl was determined by titrating the acid, HCl, with a banner base dissolver, NaOH. It was determined that there was a 1.356 M engrossment of HCl, with a very minimal percentage of error of 3.14%.
Introduction.
In order to determine the concentration of an acid in a firmness of purpose, a neutralization reaction will need to be preformed. In this case the concentration of HCl needs to be determined. This is through with(p) by completing a titration of HCl with a NaOH antecedent. A solution of known concentration added to a measured amount of the solution of an dark concentration until an exponent signals the end signify. The end point is point in a titration where the color changes and neutralization is achieved.
The solution of known concentration is called the standard solution, it this case, NaOH. The standard solution is added to the unknown solution (HCl) using a buret, which is set in a buret stand. This titration will continue until the solution has reached its end point, where the phenolphthalein indicator causes the solution to change from a clear solution to a shade of red, indicating the end point.
Procedure.
        The procedure used in this try is located on the ¡¥Titration Lab¡¦ handout. There were no variations to this procedure.
Data.
        running 1         Trial 2 mess of acid (HCl)         25.0mL         25.0mL Volume of NaOH         33.8mL         33.9mL Analysis and Questions.
1.
) The balanced equation for the neutralization reaction that occurred was; HCl(aq) + NaOH(aq) ¡÷ NaCl(aq) + H2O(l) 2.) The pattern of moles of base used in examination one was 0.0338 mol.
NaOH moles ?± 1.00 mol NaOH x 0.0338L = 0.0338 mol.
The number of moles of base used in trial two was; NaOH moles ?±1.00 mol NaOH x 0.0339L = 0.0339 mol.
3.) The number of moles of acid neutralize in trial...
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