Question

In: Chemistry

An old container of sodium bicarbonate is found in the back of the warehouse. It looks...

An old container of sodium bicarbonate is found in the back of the warehouse. It looks like a good product and there is no worry about contamination, but the plant manager want to know if he can use it to manufacturer a batch of cookies next week. You decide to test it according to the FCCIII: Following the direction in the FCC, your sample of 2.9861g requires 34.48mL of 1.000N sulfuric acid. Does this product meet the specification as required in the FCC? What do you tell the plant manager? Can he go ahead and use it in his cookie dough?

Solutions

Expert Solution

Ans. Balanced reaction: 2 NaHCO3(s) +H2SO4(aq) -----> Na2SO4(aq) + 2H2O(l) + 2CO2(g)

# Molarity of H2SO4 solution = Normality / 2 = 1.000 /2 = 0.500 M

Moles of H2SO4 consumed = Molarity x Volume in liters

                                                = 0.500 M x 0.03448 L

                                                = 0.01724 mol

# According to the stoichiometry of balanced reaction, 1 mol H2SO4 neutralizes 2 mol NaHCO3.

So,

            Moles of NaHCO3 in sample = 2 x moles of H2SO4 consumed

                                                            = 2 x 0.01724 mol

                                                            = 0.03448 mol

Mass of NaHCO3 in sample = Moles x Molar mass

                                                            = 0.03448 mol x (84.006908 g/mol)

                                                            = 2.8966 g

# % NaHCO3 in sample = (Actual mass of NaHCO3 / Mass of sample) x 100

                                                = (2.8966 g / 2.9861 g) x 100

                                                = 97.00 %

# FCC threshold value for NaHCO3 : Not less than 99.0 % , and not greater than 100.5 %.

Since % NaHCO3 (97.0%) in given sample is less than the FCC threshold value, the sample can’t be used in cookies dough.


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