Question

1.Calculate the theoretical mass of sodium carbonate that should be produced by heating 1.678 g of sodium bicarbonate.

2.If 1.018 grams of sodium carbonate were produced from the sodium bicarbonate in question 1, calculate the percent yield for the bicarbonate decomposition reaction.

3.A classic high school lab experiment involves combining a solution of barium nitrate, Ba(NO3)2, with a sodium sulfate solution, Na2SO4, forming a precipitate of barium sulfate.

Ba(NO3)2(aq) + Na2SO4(aq) ---> BaSO4(s) + 2NaNO3(aq)

a. Identify the hazards associated with the chemicals in this reaction.

b. The purpose of this lab is to teach the techniques and principles of quantitative gravimetric analysis. use your knowledge of solubility products to devise a greener set of solutions that would meet the purpose of this lab.

Answer 1

1) Answer:

2NaHCO₃ Na₂CO₃ + CO₂ + H₂O

84 g/mole 106 g/mole Molar masses

2NaHCO₃ Na₂CO₃ + CO₂ + H₂O

2 x 84 106 of Na₂CO₃ produces

1.678 g .............. ?

= (1.678 x 106 ) / 2 x 84

= 1.0587 g

Hence the theoretical mass of Na₂CO₃ produced is 1.0587 g.

2) Answer:

Produced Na₂CO₃ weight = 1.018 g

Theoretically produced Na2CO3 =  1.0587 g

Theoretical value is consider as the 100% of the yield.

1.0587 ................... 100

1.018 ...................... ?

= (1.018 x 100) / 1.0587

= 101.8 / 1.0587

= 96.155 %