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

copper sulphate lab

Extracts from this document...

Introduction

Chemistry lab report Mariam abduljabbar 641122 October 9th 2007 * Purpose: Finding the number of water molecules attached to copper sulphate crystals CuSO4.xH2O. * To avoid error: 1. Do not make too much movement around the balance when taking any mass. 2. Wait till the balance's reading is stable then take the reading. 3. Make sure that the crystals are well distributed in the beaker to be evenly exposed to as much heat as possible. * In case the experiment was repeated for more accuracy in the final results, variables should be controlled: 1. Use the same balance. 2. Use same size and shape of the container (Beaker or evaporating dish) 3. Use exactly the same mass of copper sulphate crystals. 4. Apply the same amount of heat at the same time intervals. 5. Control room temperature. * Apparatus: 1. Beaker. 2. Balance. 3. Watching glass. 4. Glass stirring rod. ...read more.

Middle

8. As soon as the entire powder turns white, the beaker is covered with watching glass to prevent copper sulphate from reacting, again, with water vapor in the atmosphere. Also, the hot plate is now turned off. 9. The mass of the dehydrated copper sulphate along with that of the beaker and the watching glass is now taken and found to be 91.60g. * Processing: 1. By subtracting the mass of the empty beaker measured at the beginning of the procedure from its mass along with the copper sulphate, the mass of hydrated copper sulphate used at the beginning is found. 33.86g - 29.92g = 3.94g 2. By subtracting the mass of the empty beaker and watching glass measured at the beginning of the procedure from the final mass of the procedure, the mass of dehydrated copper sulphate is obtained. ...read more.

Conclusion

159 18 Number of moles (mol) 0.172 0.067 Ratio 1 10 0.39 3.9 � 4 * Conclusion: The aim of this was to determine the number of water molecules attached to copper sulphate and that is a 4.03*1022 molecule where the compound has a formula of 10CuSo4.4H2O * Sources of error: 1. Uncertainty of the balance used. 2. Stirring may cause crystals to stick on the stirring glass rod affecting the mass. 3. The beaker has a small surface area, therefore not all particles will be exposed to enough heat and so not all water molecules will evaporate. * Ways of improving: Use a container with a larger surface area such as an evaporating dish to avoid the need of stirring and therefore copper sulphate crystals won't be lost by sticking to the glass rod. Also, this will increase the number of water molecules exposed to heat and so it will increase the chance of dehydrating all of the copper sulphate crystals. ?? ?? ?? ?? ...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. Chemistry Lab Report. AIM: To calculate the number of molecules of water of ...

    - Then carefully fill the crucible with 2.5 grams of hydrated copper sulphate. - Carefully light the Bunsen burner using the spirit lamp and leave the air hole on the barrel halfway open in order to provide a non-luminous flame.

  2. IB chemistry revision notes

    Gas Br2 Liquid I2 Solid o Directly proportional to the number of electrons in the species o The Halogens: as we go down Group VII the atoms have more electrons. So, they can have a greater charge imbalance and induce greater dipoles.

  1. Change of Potential Difference in Voltaic Cells Lab Report

    Zinc Sulfate Hepta hydrate (MSDS) Zinc sulfate hepta- hydrate has the same harmful and poisonous effect. The same precautions of copper sulfate should be applied. Potassium chloride is safe to be used and can be discarded in the sink. Data Collection Qualitative Data The colour of CuSO4 solution is blue.

  2. Aim: To find the molar mass of butane, by finding the number of moles ...

    * We waited a little which after the trail before measuring the air temperature to ensure that the temperature of butane inside the burette was the same. * We used water inside the burette since butane barely dissolves in water.

  1. Effect of Current on The Quantity of Products in Copper Purification Through Electrolysis

    * 2 grands et 1 petit entonnoirs en vitre * 2 tiges m�talliques * 2 bases de support � entonnoir * 2 anneaux m�talliques (supports � entonnoir) *Se r�f�rer aux Annexes 1a et 1b pour photos du mat�riel n�cessaire 5)

  2. Electrolysis of copper sulphate

    - Distance between electrodes. Distance between the electrodes should be kept constant. In theory, the closer the distance between the electrode pairs, the quicker the rate of electrolysis occurs. This is as the current would flow through the electrodes faster, therefore increasing the rate of electrolysis, consequently, increasing the mass of Cu deposited on the cathode.

  1. The chemistry of atmospheric and water pollution.

    Electrical conductivity meter, since TDS mostly contains ionic salts. However it is unable to detect any non ionic salts which also make up TDS. Relatively accurate approximation of TDS. Hardness Hard water refers to water which contains significant amounts of calcium and magnesium ions. Hard water is an issue in water quality as it aids in the formation of scale which are deposits of CaCO3 and MgCO3.

  2. Hydrated Crystals Lab. In the experiment of Hydrated Crystals the formula for the ...

    The ratio of moles of water to the anhydrous compound of MgSO4. is 5 H2O to 1 MgSO4, so the formula for the hydrated MgSO4 is MgSO4. 5 H2O. The ratio of moles of water to the anhydrous compound of CuSO4 is 7 H2O to 1 CuSO4, so the formula for the hydrated CuSO4 is CuSO4.

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