• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

Lab #2 Water Hydration of Copper(II) Sulfate. Purpose- To determine the formula of the hydrate from the anhydrous compound.

Extracts from this document...


Lab #2 Water Hydration of Copper(II) Sulfate Purpose- To determine the formula of the hydrate from the anhydrous compound. Materials- Triple beam balance Gas Burner Crucible and cover Iron ring and stand Spatula Crucible tongs Clay triangle Wire gauze Copper(II) sulfate, hydrated crystals, 5g Distilled water Variables- Independent- Temperature, amount of time heated Dependent- Mass of the crucible with Cu(II) SO4 Control- Crucible Procedure- 1) Set up the iron ring stand with the clay triangle and gas burner below it. 2) Place the crucible with the cover slightly tipped on the clay triangle so that gas can escape. 3) Heat the crucible for about five minutes to fully sanitize it. 4) ...read more.


12) Check the mass and if it is the same as the first time you are done. If not, repeat the heating, cooling, and massing until it is consistent. 13) Add a few drops of water and record any observations. Diagrams- Date- +- .02 Trial One Trial Two Mass of crucible 21.88 grams 21.88 grams Mass of crucible and Cu(II)SO4 26.97 grams 25.23 grams Mass of crucible after heated with Cu(II)SO4 25.23 grams 25.23 grams Observations- Cu(II)SO4 was an aqua blue before being heated and looked like mini crystals Once the Cu(II)SO4 was heated it turned white and had an ashy looking texture Once the Cu(II)SO4 has rehydrated it turned aqua blue and crystal looking again as well as very hot. ...read more.


Abstract- In this lab our goal was to determine the formula of the hydrate. In order to do this we had to heat the hydrate to remove all of the water from it. This required heating and massing the hydrate several times until finally the mass was consistent. Once the mass was consistent we were able to calculate how much water was in the hydrate and thus come up with a formula. Our formula ended up being Cu(II)SO4 + 4.6H2O. This was not correct but the class average was 4.96 which shows that you must experiment several times before accurately coming to any conclusions. Throughout the experiment we were able to observe the hydrate turn from crystal like blue to ash like gray. We also rehydrated the hydrate at the end to observe changes and noted that it turned blue again and grew very hot. Christina Cartagena 8/29/10 ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our International Baccalaureate Chemistry section.

Found what you're looking for?

  • Start learning 29% faster today
  • 150,000+ documents available
  • Just £6.99 a month

Not the one? Search for your essay title...
  • Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

See related essaysSee related essays

Related International Baccalaureate Chemistry essays

  1. Formula of a Hydrate Lab. By performing this lab, we will be able ...

    Crucible, cover, paper clip, and hydrated salt 19.8g. Crucible, cover, paper clip, and hydrated salt after heating 10 minutes and cooling 19.0g. The compound turned into a greenish color Crucible, cover, paper clip, and hydrated salt after heating an additional 5 minutes and cooling 19.0g. Magnesium Sulfate Mass Observations Crucible, cover, and paperclip 17.8g.

  2. Lab 1 - Determining Hydrate Formulas

    This is the reason my 4 variables to determine the hydrate formula was the total mass of the hydrated Zinc(II) Sulfate (ZnSO4) salt in the crucible with the lid, the mass of the Zinc(II) Sulfate (ZnSO4) salt in the crucible with the lid after the fourth time it has been

  1. Determination of water of hydration

    = )18x 160(0.86 ) = 18x(1.44 0.04) x = = = 5.3 � 0.3 Conclusion: The value of x in CuSO4.xH2O is quite similar to the value on the label (literal value) of the hydrated copper sulfate jar (% of difference is 6%)

  2. Determination of the amount of water present in copper sulfate hydrate

    - Mass of the test tube = 19.6 - 19.0 = 0.6 g Mass of anhydrous salt = (Mass of the test tube + anhydrated salt) - Mass of the test tube = 19.4 - 19.0 = 0.4 g Mass of water lost = Mass of hydrated salt - Mass

  1. The purpose of this experiment is to determine the empirical formula of a sample ...

    Weighed a watch glass. 12. Transferred filter paper bearing precipitate onto watch glass and inserted assembly into a 77 ?C drying oven for drying. 13. Removed assembly from drying oven at 5 minute intervals, weighing assembly with each removal.

  2. Electrolysis of copper sulphate

    extraneous variables) and often due to human mistakes resulting from the experimenter's inability to perform a measurement in exactly the setting to obtain the exact the same result. A major error that occurred in this experiment is due to the way the cathodes were dried after being removed from the copper sulphate solution.

  1. The chemistry of atmospheric and water pollution.

    Many of these heat rays come back to the Earth's surface. This raises the temperature of the atmosphere.) In the stratosphere, CFCs (as well as halons) absorb heat rays emitted from the earth?s surface ? preventing them from being released into outer space.

  2. Testing the Suitability of Pool Water. The expected amount of chlorine which is ...

    �1000 50 * Mass of Chlorine in 1 dm3 of H2O = 11.4 � 0.71 mg 2) Amount of Chlorine for 100cm3 of Pool water: Volume of pool water = 100 � 0.5 cm3 = 0.1 � 0.0005 dm3 Average Volume of Na2S2O3 = 3.15 � 0.1 cm3 = 0.00315 � 0.0001 dm3 Concentration of Na2S2O3 = 0.01 M No.

  • Over 160,000 pieces
    of student written work
  • Annotated by
    experienced teachers
  • Ideas and feedback to
    improve your own work