-Mass of Epson Salt Used (g) -Mass of Salt After Heating (g) -Moles of MgSO4 -Mo

Question

-Mass of Epson Salt Used (g) -Mass of Salt After Heating (g) -Moles of MgSO4 -Moles of H20 Lost (mol) -Ratio of Moles H20 to Moles MgSO4 (Unitless) -Average Number of Moles H20 present in Epson salt Sample (mol) DATA: Trial 2 (g) Mass of Beaker Mass of Beaker w/ Epsom Salt Mass of Beaker and Salt after Heating Mass Lost During Heating Mass of Residue Remaining in Beaker Initial Mass of Epsom Salt Used OBSERVATIONS: (anything you observed, condensation, steam, smoke, spilled compound, etc) Trial 1 Trial 2 Mass of Epsom Salt Used (g) Mass of Salt After Heating (g) Moles of Mgso. Moles of H,0 Lost (mol) Ratio of Moles of H,0 to moles of Mgso, (Unitless) Average number of moles of H o present in Epsom salt sample (mol)

Explanation / Answer

-Mass of Epson Salt Used (g) = mass of beaker + salt - mass of beaker

Trial 1: 56.52 - 54.57 = 1.95 g

Trial 2: 56.20 - 54.40 = 1.80 g

-Mass of Salt After Heating (g) = Mass after heating - mass of beaker

Trial 1: 55.57 - 54.57 = 1.0 g

Trial 2: 55.55 - 54.40 = 1.15 g

Moles of MgSO4 = mass/ molar mass

Trial 1: Moles = 1.0 g/ 120.4 g/mol = 0.00831 moles

Trial 2: Moles = 1.15 g / 120.4 g/mol = 0.00955 moles

-Moles of H20 Lost (mol) = mass of salt - mass after heating / molar mass of H2O

Trial 1: Moles = (1.95 g - 1.0 g) / 18.02 g/mol = 0.0526 moles

Trial 2: Moles = (1.80 g - 1.15 g) / 18.02 g/mol = 0.0361 moles

-Ratio of Moles H20 to Moles MgSO4 (Unitless)

Trial 1: Ratio: 0.0526 :0.00831 = 6.32 : 1

Trial 2: 0.0361 :0.00955 = 3.78: 1

-Average Number of Moles H20 present in Epson salt Sample (mol)

The average is around 6 moles H2O. There is an error in the values for trial 2.

Hope this helps

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