1 / 14

Titration

Lab 20- Acids & Bases. Titration. A. Neutralization. Chemical reaction between an acid and a base. Products are a salt (ionic compound) and water. Neutralization. ACID + BASE  SALT + WATER. HCl + NaOH  NaCl + H 2 O. strong. strong. neutral.

thea
Download Presentation

Titration

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript


  1. Lab 20- Acids & Bases Titration

  2. A. Neutralization • Chemical reaction between an acid and a base. • Products are a salt (ionic compound) and water.

  3. Neutralization ACID + BASE  SALT + WATER HCl + NaOH  NaCl + H2O strong strong neutral HC2H3O2 + NaOH  NaC2H3O2 + H2O weak strong basic • Salts can be neutral, acidic, or basic. • Neutralization does not mean pH = 7.

  4. standard solution unknown solution Titration • Titration • Analytical method in which a standard solution is used to determine the concentration of an unknown solution.

  5. B. Titration • Equivalence point (endpoint) • Point at which equal amounts of H3O+ and OH- have been added. • Determined by… • indicator color change • dramatic change in pH

  6. B. Titration moles H3O+ = moles OH- MVn = MVn M: Molarity V: volume n: # of H+ ions in the acid or OH- ions in the base

  7. B. Titration • 42.5 mL of 1.3MNaOHare required to neutralize 50.0 mL of KHP. Find the molarity of KHP. H3O+ M = ? V = 50.0 mL n = 1 OH- M = 1.3M V = 42.5 mL n = 1 MV = MV M(50.0mL) =(1.3M)(42.5mL) M = 1.11 M H2SO4

  8. Procedures • Data you need for part A • KHP =204.2g/mol Formulas M = mol/liters moles H3O+ = moles OH- MV (H3O+) = MV (OH-) % KHP = mass of KHP/ Mass of mixture

  9. Procedures • A. Standardization of NaOH • Add 2.5 grams of KHP into 3 Erlenmeyer flasks • Use analytical balance to 4 sig figs • Add 100 ml of D.I water into each flask • Add 2 drops of Phenolphthalein soln

  10. A. Fill a Burett with NaOH(aq) • Slowly add NaOH into 1st flask, while swirling flask • See fig 20-2 and read procedures for proper titration Record amount of NaOH used to titrate

  11. calculations • Determine moles of KHp • Determine moles of NaOH • Determine Molarity of NaOH • Determine Standard deviation • (do this at home, see pgs 80 - 82)

  12. Part B • . Standardization of unKnown acid • Add 2.5 grams of unknown acid into 3 Erlenmeyer flasks • Use analytical balance to 4 sig figs • Add 100 ml of D.I water into each flask • Add 2 drops of Phenolphthalein soln

  13. A. Fill a Burett with standarizedNaOH • Slowly add NaOH into 1st flask, while swirling flask • See fig 20-2 and read procedures for proper titration Record amount of NaOH used to titrate

  14. calculations • Determine moles of base used • Determine moles of KHP • Determine mass of KHp • Determine % of KHP in unknown

More Related