1 / 15

Determining the Formula of a Hydrate: Experimental Procedure and Calculations

This experiment focuses on determining the number of moles of water associated with an unknown hydrate. Through careful measurements and calculations, participants will analyze an inorganic salt hydrate, such as CuSO4•xH2O, to establish its formula. Key steps involve measuring the mass of the sample before and after heating to remove water, calculating the moles of water lost and the remaining anhydrous salt, and determining the ratio of water to the anhydrous compound. Precise techniques and safety measures are emphasized for accurate results.

lilka
Télécharger la présentation

Determining the Formula of a Hydrate: Experimental Procedure and Calculations

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. CHEM 1031 DETERMINATION OF THE FORMULA OF A HYDRATE

  2. PURPOSE AND GOALS • DETERMINE THE NUMBER OF MOLES OF WATER IN AN UNKNOWN HYDRATE.

  3. PRINCIPLES INORGANIC SALTS • ANHYDROUS CONDITIONS • HYDRATE-WATER MOLECULES BOUND

  4. WATER • MECHANICALLY TRAPPED • CHEMICALLY BOUND

  5. FORMULA FOR THE HYDRATED SALT EXAMPLE: MgCl2•6H2O HYDRATE = ANHYDROUS SALT + WATER

  6. IN THIS EXPERIMENT • DETERMINE THE NUMBER OF WATERS OF HYDRATION PRESENT IN A SAMPLE EXAMPLE: CuSO4•xH2O

  7. CALCULATIONS • MASS OF SAMPLE= MASS OF CRUCIBLE/COVER/SAMPLE(C/C/S) - MASS OF CRUCIBLE/COVER(C/C) • SHOULD BE ~1 g.

  8. MASS OF WATER IN ORIGINAL SAMPLE= WEIGHT OF C/C/S BEFORE HEATING - WEIGHT OF C/C/S AFTER HEATING

  9. MOLES OF WATER IN ORIGINAL SAMPLE= MASS OF WATER (g) MOLECULAR WEIGHT OF WATER (grams/mole)

  10. MASS OF ANHYDROUS SALT IN ORIGINAL SAMPLE= WEIGHT OF C/C/S AFTER HEATING - WEIGHT OF C/C

  11. MOLES OF ANHYDROUS SALT IN ORIGINAL SAMPLE= MASS OF ANHYDROUS SALT (g) MOLECULAR WEIGHT OF ANHYDROUS SALT (grams/mole)

  12. RATIO OF THE NUMBER OF MOLES OF WATER TO MOLES OF ANHYDROUS SALT = # MOLES WATER # MOLES ANHYDROUS SALT

  13. FORMULA OF HYDRATE: CuSO4•xH2O *WHERE “x” EQUALS THE NUMBER OF MOLES OF WATER PER MOLE OF ANHYDROUS SALT

  14. PERCENT (%) OF WATER IN SAMPLE= MASS OF H2O_LOSS MASS OF SAMPLE X 100

  15. REMINDERS • HEAT GENTLY FIRST THEN STRONGLY • USE TONGS AND WIRE GAUZE • RECORD UNKNOWN SAMPLE CODE

More Related