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Why do Titration Curves Look Like THAT ????

Why do Titration Curves Look Like THAT ????. Calculate the pH when the following quantities of 0.100 M NaOH solution have been added to 50.0 mL of 0.100 M HCl solution: A. 30.0 mL B, 49.0 mL C. 49.5 mL D. 50.0 mL E. 50.5 mL F. 60.0 mL. Solution for 30.0 mL NaOH.

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Why do Titration Curves Look Like THAT ????

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  1. Why do Titration Curves Look Like THAT ????

  2. Calculate the pH when the following quantities of 0.100 M NaOH solution have been added to 50.0 mL of 0.100 M HCl solution: A. 30.0 mL B, 49.0 mL C. 49.5 mL D. 50.0 mL E. 50.5 mL F. 60.0 mL

  3. Solution for 30.0 mL NaOH • Both Na+ and Cl- are spectator ions. • Find how many moles H+ and moles OH- present, then calculate how many mole of each ion remain after neutralization.

  4. New pH now… • Remaining H+ mole / new soln volume

  5. Solution for 49.0 mL NaOH

  6. New pH now… • Remaining H+ mole / new soln volume

  7. Solution for 49.5 mL NaOH

  8. New pH now… • Remaining H+ mole / new soln volume

  9. Solution for 50.0 mL NaOH

  10. New pH now… • [H+] = [OH-] = 0 M • Neutral • pH = 7

  11. Solution for 50.5 mL NaOH

  12. New pH now… • Remaining OH- mole / new soln volume

  13. Solution for 60.0 mL NaOH

  14. New pH now… • Remaining OH- mole / new soln volume

  15. Titration curve for a strong acid by a strong base Any indicator that changes color along the steep portion of the titration curve is suitable for the titration. Methyl violet changes color too soon, and alizarin yellow R too late.

  16. Subtle vocabulary point • Equivalence point: where equal moles of acid and base are present. • End Point: where an indicator chemical changes color. It may not be exactly at the equivalence point, but generally very close.

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