Epsom Salt Lab Report
Epsom salt have many uses, including use as bath salts, as a laxative and as a plant nutrient. Epsom salt contains hydrated magnesium sulphate which has the formula MgSO4.xH2O.
Experiment to find the value of x in a pure sample of hydrated magnesium sulphate.
The method i will use is heating a known mass of magnesium sulphate to remove the water of crystallisation. x is found by weighing before and after heating to find the mass of the water then using the moles calculations to find x.
The source I have used is: http://www.rsc.org/learn-chemistry/resource/res00000436/finding-the-formula-of-hydrated-copper-ii-sulfate?cmpid=CMP00006780
1. Weigh the empty crucible, recording the weight, then add one spatula of them magnesium sulphate.
Weigh again and record the result. 2. Set us your bunsen burner as the diagram shows. Then place the crucible securely in the pipe clay triangle on the tripod over the bunsen burner. 3. Heat the crucible gently over the flame for five minutes then carefully remove the crucible from the flame and weigh it again 4. Begin to heat the crucible again for a further 5 minutes and weigh if the weight remained the same all of the water of crystallisation has been driven off. If not continue to heat for a further five minutes and weigh again until the same result is achieved twice and record this result. 5. Now the value of x must be calculated from the results recorded. a. calculate the molar masses of both H2O and MgSO4 b. from the results calculate the mass of water of crystallisation driven off and the mass of the anhydrous salt. c. calculate the number of moles of anhydrous magnesium sulphate formed d. calculate the amount of moles of water of crystallisation have been driven off if one mole of the anhydrous salt had been formed e. write down the formula for hydrated magnesium sulphate.
Experiment to find the value of x in a pure sample of hydrated magnesium sulphate.
The method i will use is heating a known mass of magnesium sulphate to remove the water of crystallisation. x is found by weighing before and after heating to find the mass of the water then using the moles calculations to find x.
The source I have used is: http://www.rsc.org/learn-chemistry/resource/res00000436/finding-the-formula-of-hydrated-copper-ii-sulfate?cmpid=CMP00006780
1. Weigh the empty crucible, recording the weight, then add one spatula of them magnesium sulphate.
Weigh again and record the result. 2. Set us your bunsen burner as the diagram shows. Then place the crucible securely in the pipe clay triangle on the tripod over the bunsen burner. 3. Heat the crucible gently over the flame for five minutes then carefully remove the crucible from the flame and weigh it again 4. Begin to heat the crucible again for a further 5 minutes and weigh if the weight remained the same all of the water of crystallisation has been driven off. If not continue to heat for a further five minutes and weigh again until the same result is achieved twice and record this result. 5. Now the value of x must be calculated from the results recorded. a. calculate the molar masses of both H2O and MgSO4 b. from the results calculate the mass of water of crystallisation driven off and the mass of the anhydrous salt. c. calculate the number of moles of anhydrous magnesium sulphate formed d. calculate the amount of moles of water of crystallisation have been driven off if one mole of the anhydrous salt had been formed e. write down the formula for hydrated magnesium sulphate.