The sulfate in a 0.2345 g sample of a mixture containing only K2SO4 (fm = 174.26) and Na2SO4 (fm = 142.04) is to beanalyzed by precipitating all the sulfate as barium sulfate, BaSO4 (fm = 233.39) by the addition of excess BaCl2.
Na2SO4 + BaCl2 image from custom entry toolBaSO4
K2SO4 + BaCl2image from custom entry toolBaSO4
The weight of barium sulfate formed is 0.3456 g. Calculate the % potassium sulfate and sodium sulfate in the mixture.
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To calculate the percentage of potassium sulfate (K2SO4) and sodium sulfate (Na2SO4) in the mixture, we can first determine the moles of barium sulfate (BaSO4) formed, and then use stoichiometry to find the moles of K2SO4 and Na2SO4.
1. Calculate the moles of BaSO4 formed:
The molar mass of BaSO4 is 233.39 g/mol.
Moles of BaSO4 = mass of BaSO4 formed / molar mass of BaSO4
Moles of BaSO4 = 0.3456 g / 233.39 g/mol
2. Use stoichiometry to find the moles of K2SO4 and Na2SO4:
From the balanced chemical equations given, we know that:
1 mole of BaSO4 is formed from 1 mole of Na2SO4, and
1 mole of BaSO4 is formed from 1 mole of K2SO4.
Moles of Na2SO4 = Moles of BaSO4
Moles of K2SO4 = Moles of BaSO4
3. Calculate the mass of Na2SO4 and K2SO4:
Mass of Na2SO4 = Moles of Na2SO4 * molar mass of Na2SO4
Mass of K2SO4 = Moles of K2SO4 * molar mass of K2SO4
4. Calculate the percentage of each sulfate:
Percentage of Na2SO4 = (Mass of Na2SO4 / Total mass of mixture) * 100
Percentage of K2SO4 = (Mass of K2SO4 / Total mass of mixture) * 100
Now, plug in the values obtained from the above calculations to find the percentages of potassium sulfate and sodium sulfate in the mixture.