Strong acid and base titration

Strong acid and base titration - 1 Titrations 1 The point...

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1 Titrations: 1. The point in a titration at which chemically equivalent amounts of acid and base have reacted is called the equivalence point. 2. The point in a titration at which a chemical indicator changes color is called the end point. 3. Indicators are very useful in determining the endpoint of a titration. For example: You titrate an unknown concentration of 50.0 mL HCl with a standardized solution of 1.00 M NaOH. 1. A few drops of the indicator, phenolphthalein, is added to the HCl solution. a. In acidic solution the indicator is colorless, and in basic solution the indicator turns pink. 2. After adding 25.0 mL of NaOH, the solution changes color (indicating that the acid had been neutralized). What is the molarity of the HCl when at the endpoint of the titration? HCl + NaOH b H 2 O + NaCl If you add more than 25 mL of NaOH to the above problem, you have “over titrated” the acid solution and the molarity of the HCl solution will be too high! 1.
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This note was uploaded on 03/17/2010 for the course CH 204 taught by Professor Leytner during the Spring '08 term at University of Texas.

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Strong acid and base titration - 1 Titrations 1 The point...

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