Mr. Chapman Chemistry 30.  Acid-base titrations are lab procedures used to determine the concentration of a solution. We will examine their use in determining.

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Presentation transcript:

Mr. Chapman Chemistry 30

 Acid-base titrations are lab procedures used to determine the concentration of a solution. We will examine their use in determining the concentration of acid and base solutions. Titrations are important analytical tools in chemistry.  During an acid-base titration, an acid with a known concentration (a standard solution) is slowly added to a base with an unknown concentration (or vice versa). A few drops of indicator solution are added to the base (such as phenolphthalein).

 The indicator will signal, by colour change, when the base has been neutralized (when [H + ] = [OH - ]).  At that point - called the equivalence point or end point - the titration is stopped. By knowing the volumes of acid and base used, and the concentration of the standard solution, calculations allow us to determine the concentration of the other solution.



-To use titration information to calculate the concentration of the unknown solution, you must know the following information. Note the abbreviations that will be used in our calculations. -Titration questions are pretty easy to recognize, and generally are not difficult to solve.

Need to Know  The concentration of one of the solutions, the acid for example (M A )  The volume of acid used for the titration (V A )  The volume of base used for the titration (V B ) What you will calculate:  The concentration of the other solution, the base for example (M B )

When an acid or base has been titrated completely (neutralized), the moles of acid = the moles of the base. Therefore, we have: M a V a = M b V b

1.During a titration 75.8 mL of a standard solution of HCl is titrated to end point with mL of a NaOH solution with an unknown concentration. What is the concentration of the NaOH solution? 2.A 20.0 mL solution of strontium hydroxide, Sr(OH) 2, is placed in a flask and a drop of indicator is added. The solution turns colour after 25.0 mL of a standard M HCl solution is added. What was the original concentration of the Sr(OH) 2 solution? Always start with a balanced chemical equation!

1.If mL of a M NaOH solution is required to neutralize mL of a solution of HCl, what is the molarity of the acid? 2.What is the concentration of a calcium hydroxide solution, Ca(OH) 2, if mL of the base is completely neutralized by 10.0 mL of M HCl?