10.00 g of hydrated sodium sulfate decompose to form 4.40 g of anhydrous sodium sulfate on heating. Calculate the formula mass of hydrated sodium sulfate and the value of x. Na2SO4.XH2O → Na2SO4 + xH₂O
Question
10.00 g of hydrated sodium sulfate decompose to form 4.40 g of anhydrous sodium sulfate on heating. Calculate the formula mass of hydrated sodium sulfate and the value of x. Na2SO4.XH2O → Na2SO4 + xH₂O
Solution
Sure, here is the step by step solution:
Step 1: Calculate the molar mass of anhydrous sodium sulfate (Na2SO4) The molar mass of Na2SO4 = (223) + 32 + (416) = 142 g/mol
Step 2: Calculate the moles of anhydrous sodium sulfate Moles of Na2SO4 = mass/molar mass = 4.40 g / 142 g/mol = 0.031 moles
Step 3: Calculate the mass of water in the hydrated sodium sulfate Mass of water = mass of hydrated sodium sulfate - mass of anhydrous sodium sulfate = 10.00 g - 4.40 g = 5.60 g
Step 4: Calculate the molar mass of water (H2O) The molar mass of H2O = (2*1) + 16 = 18 g/mol
Step 5: Calculate the moles of water Moles of H2O = mass/molar mass = 5.60 g / 18 g/mol = 0.311 moles
Step 6: Calculate the value of x in the formula Na2SO4.xH2O x = moles of H2O / moles of Na2SO4 = 0.311 moles / 0.031 moles = 10
So, the formula of the hydrated sodium sulfate is Na2SO4.10H2O and the formula mass is 142 g/mol + 10*18 g/mol = 322 g/mol.
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