-5 M Review: 50 mL of 0.1 M carbonic acid, H2CO3, with an initial pH of 3.5, is titrated with 0.2 M lithium hydroxide, LiOH. What volume of.

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Presentation transcript:

-5 M

Review: 50 mL of 0.1 M carbonic acid, H2CO3, with an initial pH of 3.5, is titrated with 0.2 M lithium hydroxide, LiOH. What volume of LiOH would be required to reach the first equivalence point? What additional volume would be required to reach the second equivalence point?

Objectives: Learn how to properly choose an indicator for a given titration Differentiate between the equivalence point and the end-point of a titration Analyze titration curves for reverse titrations

Choosing the correct indicator: Remember the role of an indicator? It must change the color of the solution as close to the equivalence point as possible!!!

Choosing the correct indicator: 1. What indicator should be used for the titration of phenol with sodium hydroxide? (pH at equivalence point is 11.2) 2. What indicator should be used for the titration of a strong acid with a strong base?

Choosing the correct indicator: Remember the role of an indicator? It must change the color of the solution as close to the equivalence point as possible!!! The point in a titration when the indicator changes color is known as the end-point The end-point is close to the equivalence point, but only an approximation

Reverse Titrations Normally, base is added to acid … NaOH and if the pH in the flask is monitored, titration curves look like this … HCl

Reverse Titrations Acid can also be added to a base … HCl and if the pH in the flask is monitored, titration curves look like this … NaOH

Reverse Polyprotic Titrations: A chemical reaction occurs when 0.150 M HCl is added dropwise to 30. mL of 0.100 M Na3PO4. The sodium phosphate solution has an initial pH of 9.30, which decreases as HCl is added. a. Write the 3 net ionic equations for the formation of the major species.

Reverse Polyprotic Titrations: A chemical reaction occurs when 0.150 M HCl is added dropwise to 30. mL of 0.100 M Na3PO4. The sodium phosphate solution has an initial pH of 9.30, which decreases as HCl is added. b. Sketch a graph using the axis provided, showing the shape of the titration curve that results when HCl is added from a burette to the Na3PO4. Exact pH values DO NOT need to be calculated, but volumes of titrant added should be calculated and represented accurately.