Question

5. Sodium bicarbonate (baking soda) will neutralize sulfuric acid according to the following reaction: 2 H200) + 2 CO2()+ Na2SOs(aq) 2 NAHCO3(aq)+H2SO4(aq) If a student spills 250.0 mL of sulfuric acid, how many grams of sodium bicarbonate should they use in order to completely neutralize it? Assume the density of sulfuric acid is 1.84 g/m L.

Answer 1

Mass of H2SO4 = density * volume

= 1.84 g/mL * 250.0 ml

= 460 g

Molar mass of H2SO4,

MM = 2*MM(H) + 1*MM(S) + 4*MM(O)

= 2*1.008 + 1*32.07 + 4*16.0

= 98.086 g/mol

mass of H2SO4 = 4.6*10^2 g

mol of H2SO4 = (mass)/(molar mass)

= 4.6*10^2/98.09

= 4.69 mol

According to balanced equation

mol of NaHCO3 formed = (2/1)* moles of H2SO4

= (2/1)*4.69

= 9.38 mol

Molar mass of NaHCO3,

MM = 1*MM(Na) + 1*MM(H) + 1*MM(C) + 3*MM(O)

= 1*22.99 + 1*1.008 + 1*12.01 + 3*16.0

= 84.008 g/mol

mass of NaHCO3 = number of mol * molar mass

= 9.38*84.01

= 7.88*10^2 g

Answer: 788 g