2.00g of baking powder is used to bake a cake. Using the chemical equation between sodium bicarbonate and citric acid what is the ideal mass composition of these compounds in the baking powder to produce the best cake, assuming that the best cake contains baking powder has risen the most.
Question
2.00g of baking powder is used to bake a cake. Using the chemical equation between sodium bicarbonate and citric acid what is the ideal mass composition of these compounds in the baking powder to produce the best cake, assuming that the best cake contains baking powder has risen the most.
Solution
The chemical reaction between sodium bicarbonate (NaHCO3) and citric acid (C6H8O7) in baking powder is as follows:
3 NaHCO3 + C6H8O7 -> 3 CO2 + 3 H2O + Na3C6H5O7
The molar mass of NaHCO3 is approximately 84 g/mol and the molar mass of C6H8O7 is approximately 192 g/mol.
The stoichiometry of the reaction tells us that 3 moles of NaHCO3 react with 1 mole of C6H8O7. Therefore, the mass ratio of NaHCO3 to C6H8O7 in the baking powder should be 3:1 in terms of moles.
To convert this to a mass ratio, we multiply the molar ratio by the molar mass of each compound:
(3 moles NaHCO3 * 84 g/mol NaHCO3) : (1 mole C6H8O7 * 192 g/mol C6H8O7) = 252 g : 192 g
This simplifies to a mass ratio of approximately 1.31:1 of NaHCO3 to C6H8O7.
Therefore, in a 2.00 g sample of baking powder, there should ideally be:
(2.00 g / (1.31 + 1)) * 1.31 = 1.18 g of NaHCO3 and (2.00 g / (1.31 + 1)) * 1 = 0.82 g of C6H8O7
This will produce the most CO2 and therefore the best rise in the cake.
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