Difference between revisions of "Titration of an Acid Final Project Lab"
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*Filled up both burettes to 0mL | *Filled up both burettes to 0mL | ||
| − | '''Titrated with 10.20mL of Acid "B" | + | '''Titrated with 10.20mL of Acid "B" and 10.11mL Base''' |
*'''V<sub>A</sub>*C<sub>A</sub>=V<sub>B</sub>*C<sub>B</sub>''' | *'''V<sub>A</sub>*C<sub>A</sub>=V<sub>B</sub>*C<sub>B</sub>''' | ||
Latest revision as of 12:12, 5 June 2007
Titration of an Unknown Acid Final Project Lab for Chemistry
Contents |
Purpose
To use the concentration of a known base to determine the concentration of an unknown acid
Directions
Titrate to endpoint a sodium hydroxide solution with a acetic acid solution of an unknown concentration. Use phenolphthalein as an indicator. Start with 10mL of acid.
Results
- Using Acid "B" at .1012M concentration
- Filled up both burettes to 0mL
Titrated with 10.20mL of Acid "B" and 10.11mL Base
- VA*CA=VB*CB
- 10.20ml Acid * ?M Acid = 10.11mL base * .1012M Base
- 10.20mL * ?M Acid = 1.023132 mlM base
- (divide both side by 10.20ml)
- .1003M = CA
Formula
NaOH(aq)+CH3COOH(aq) -> Na(aq) + H2O(l)+CH3COO(aq)
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