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Titrations MATH!!!!

Titrations MATH!!!!. weak base. indicator. K a. strong acid. K b. [H + ]. equivalence point. To Find the Equivalence Point. (ex) When titrating 50.0mL of 0.48M HCN with 0.75M NaOH , what volume of base must be added to reach the equivalence point?. Strong Acid with Strong Base.

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Titrations MATH!!!!

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  1. Titrations MATH!!!! weak base indicator Ka strong acid Kb [H+] equivalence point

  2. To Find the Equivalence Point (ex) When titrating 50.0mL of 0.48M HCN with 0.75M NaOH, what volume of base must be added to reach the equivalence point?

  3. Strong Acid with Strong Base

  4. 25.0 mL of 0.20M HCl titrated with 0.20M NaOH initially: after 15mL of NaOH added:

  5. 25.0 mL of 0.20M HCl titrated with 0.20M NaOH at equivpt: after 40.0 mL of NaOH added:

  6. See summary: middle of p.772 in textbook

  7. Notice the differences between a strong acid titration shown in red and a weak acid titration shown in blue (both titrated with a strong base).

  8. Visual differences between SA-SB and WA-SB titration curves: • Initial pH higher when starting with weak acid • The pH of a weak acid rises faster at the start and slower at the equivalence point. Recognize that a buffer solution forms during this portion. 3. pH at the equivalence point >7 with a weak acid

  9. 50.0mL of 0.25M HC2H3O2 titrated with 0.20M NaOH First, where is the equivalence point?

  10. 50.0mL of 0.25M HC2H3O2 titrated with 0.20M NaOH initially: after 15mL of NaOH added:

  11. 50.0mL of 0.25M HC2H3O2 titrated with 0.20M NaOH at equivpt:

  12. 50.0mL of 0.25M HC2H3O2 titrated with 0.20M NaOH after 85.0mL of NaOH added:

  13. See summary: top of p.778 in textbook

  14. Half-Equivalence Point • Volume of titrant added is half the volume of the equivalence point • Moles of strong base added is half that of original weak acid HA + OH- A- + H2O .50 .25 -.25 -.25 +.25 .25 .25 .25 pH = pKa + log .25 pH = pKa @ half-equivalence point

  15. Base Titrated with Strong Acid

  16. Acid-Base Titrations • Add solution (either the acid or the base) from buret to solution in flask • The concentration of one solution is known. One concentration is unknown. • Often, the goal is to find the unknown concentration.

  17. What is the concentration of NaOH when 30.0mL of the base neutralizes 26mL of 0.50M HCl? • When 25 mL of HCl is titrated with 6.00 M Ba(OH)2, it takes 39.3 mL of base to reach the end point. What is the pH of the acid solution?

  18. What is the concentration of NaOH when 30.0mL of the base neutralizes 26mL of 0.50M HCl?

  19. When 25 mL of HCl is titrated with 6.00 M Ba(OH)2, it takes 39.3 mL of base to reach the end point. What is the pH of the acid solution?

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