Titrations

The process of adding measured volumes of an acid or base of known concentrations to an acid or base of unknown concentration until neutralization occurs

Performed to determine the concentration of an unknown solution The solution of known concentration is called the standard solution

Titration Equation Found on Table T of reference table M A V A = M B V B M A= molarity of the acid V A= volume of the acid M B = molarity of the base V B = volume of the base

Titrations In titration (neutralization) there must be a 1:1 ratio between H+ and OH- Example: What is the concentration of HCl solution if 50.0ml of a M KOH are needed to neutralize 20.0 ml of HCl?

Solve M A= unknown V A= 20.0 ml M B = M V B = 50.0ml (x) (20 ml) = (.250 M) (50.0) M A= M

Example 2 What if the ratio is not 1:1? Example What is the concentration of H 2 SO 4 if 50.0ml of a 0.25 M KOH are needed to neutralize 20.0 ml of H 2 SO 4 ? Ratio is 2:1

Solve M A= unknown V A= 20.0 ml M B = M V B = 50.0ml (2) (x) (20 ml) = (.250 M) (50.0) M A= 0.31M