Experiment 2-Lecture

Experiment 2-Lecture - Experiment No. 2 pH Titrations of...

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Experiment No. 2 pH Titrations of Weak and Strong Acids
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Strong Acids in Solution HX + H 2 O H 3 O + + X - 100% dissociated in water. 2200 [H 3 O + ] = Analytical Concentration of HX pH = -log[H 3 O + ] Examples of Strong Acids HCl, HBr, HI, HNO 3 , H 2 SO 4 , HClO 4 , HBrO 3 , etc.
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pH Calculations for Strong Acids Calculate the pH for a solution containing 0.1M. HCl. O.01M. HCl. O.1M. HNO 3 . 0.01M. HNO 3 .
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Weak Acids in Solution HX + H 2 O H 3 O + + X - Less than 100% dissociated in water. 2200 [H 3 O + ] << Analytical Concentration of HX Remember, pH = -log[H 3 O + ] Examples of Weak Acids H 2 CO 3 , H 3 BO 3 , H 3 PO 4 , H 2 S, H 2 SO 3 , Organic Acids (e.g., HOAc)
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pH Calculations for Weak Acids You are provided with 0.050 M acetic acid solution. Calculate the equilibrium concentration and the pH of the solution given that the K a of acetic acid is 1.75 x 10 -5 .
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Dissociation Constants for Weak Acids HA + H 2 O H 3 O + + A - ] HA [ ] A ][ O H [ K 3 a - + = Approximate Solution HA a 3 c K ] O H [ = + K a ’s can be found in Appendix G
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pH Calculation of a Weak Acid Calculate the pH of a 0.1M. solution of acetic acid. Of a 0.01M. solution. The K a for acetic acid is 1.75 x 10 -5 .
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Acid/Base or Neutralization HCl( aq ) + NaOH( aq ) → NaCl( aq ) + H 2 O( l ) HOAc( aq ) + NaOH( aq ) NaOAc( aq ) + H 2 O( l ) Reactions, that when completed, yield a salt and water. What is the reaction??
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Some Terms Titration -- An analysis performed by adding a standard solution from a buret (or other liquid-dispensing device) to a solution of the analyte until the reaction between the two is judged complete. Equivalence Point -- The point in a titration when the amount of added titrant is chemically equivalent to the amount of analyte in the sample. End Point
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Experiment 2-Lecture - Experiment No. 2 pH Titrations of...

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