CHEM 1A Lecture 26: 11-30 Lecture 26

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browncod58

30 Nov 2016

School

UCSB

Department

Chemistry and Biochemistry

Course

CHEM 1A

Professor

Joseph

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CHEM 1A Full Course Notes

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Adding a strong base allows to find the ph. When you add a strong entity into the buffer system, convert it to a weak. The net ionic equation will be h+ + oh- h2o. The equivalence point is the same amount of acid and base. (7) Calculated the ph before the equivalence point (random amount added as long as it"s before the equivalence point) (5 ml). Titrate 25. 0ml of 1. 0 m ch3cooh with 1. 0 m naoh. Before and at the equivalence point (25. 0 ml of 1. 0 m naoh) Two step problem: 1) stoichiometry 2) equilibrium. Similar type of problem but have some nuances see example 8. 2b for before equivalence point and last problem. Major species during titration: ch3cooh, oh-, na+, h2o. Ch3cooh + oh- ch3coo- + h2o. 0. 025 mol -0. 025 mol + 0. 025 mol. Major species in solution: ch3coo-, na+, h2o. Reaction: ch3coo- + h2o ch3cooh + oh-

Related Questions

a. For the titration of 25.0 mL of 0.1 M HCl (aq) with 0.1 M NaOH (aq), at what volume of NaOH (aq) should the equivalence point be reached and why? If an additional 3.0 mL of 0.1 M NaOH (aq) is then added, what is the expected pH of the final solution?

b. What is the initial pH expected for a 0.1 M solution of acetic acid? For the titration of 25.0 mL of 0.1 M acetic acid with 0.1 M NaOH (aq), at what volume of NaOH (aq) is the equivalence point reached? Is the pH at the equivalence point greater than, less than or the same as in problem #a above? Explain.

c. What is the initial pH expected for a 0.1 M solution of phosphoric acid (H3PO4)? For 25.0 mL of 0.1M H3PO4 (aq), what volume of 0.1 M NaOH (aq) is required to fully titrate all three protons to their end points?

d. In the titration of a weak acid with a strong base, how is the half equivalence point determined and what is its significance? How are the pKa and Ka of the weak acid determined from the half equivalence point?

1. For the titration of 25.0 mL of 0.1 M HCl (aq) with 0.1 M NaOH (aq), at what volume of NaOH (aq) should the equivalence point be reached and why? If an additional 3.0 mL of 0.1 M NaOH (aq) is then added, what is the expected pH of the final solution?

2. What is the initial pH expected for a 0.1 M solution of acetic acid? For the titration of 25.0 mL of 0.1 M acetic acid with 0.1 M NaOH (aq), at what volume of NaOH (aq) is the equivalence point reached? Is the pH at the equivalence point greater than, less than or the same as in problem #1 above? Explain.

3. What is the initial pH expected for a 0.1 M solution of phosphoric acid (H3PO4)? For 25.0 mL of 0.1M H3PO4 (aq), what volume of 0.1 M NaOH (aq) is required to fully titrate all three protons to their end points?

4. In the titration of a weak acid with a strong base, how is the half equivalence point determined and what is its significance? How are the pKa and Ka of the weak acid determined from the half equivalence point?

5. Carefully read and study the lecture text sections related to this experiment. 5. Prepare and set up your lab notebook. Be sure to leave spaces for recording observations.

CHEM 1A Lecture 26: 11-30 Lecture 26

CHEM 1A Full Course Notes

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