Some sulfuric acid is spilled on a lab bench. You can neutralize the acid by spr

Question

Some sulfuric acid is spilled on a lab bench. You can neutralize the acid by sprinkling sodium bicarbonate on it and then mopping up the resultant solution. The sodium bicarbonate reacts with sulfuric acid according to: 2NaHCO_3(s) + H_2SO_4(aq) rightarrow Na_2SO_4(aq) + 2H_2O(l) + 2CO_2(g) Sodium bicarbonate is added until the fizzing due to the formation of CO_2(g) stops. If 27 mL of 6.0 M H_2SO_4 was spilled, what is the minimum mass of NaHCO_3 that must be added to the spill to neutralize the acid?

Explanation / Answer

2 NaHCO3 + H2SO4 ------------> Na2SO4 + 2CO2 + H2O

2 mole            1 mole

no of moles of H2So4 = molarity * volume in L

                                     = 6*0.027   = 0.162moles

1 mole of H2SO4 react with 2 moles of NaHCO3

0.162 moles of H2So4 react with = 2*0.162/1   = 0.324 moles of NaHCO3

mass of NaHCO3 = no of moles * gram molar mass

                              = 0.324*84   = 27.22g of NaHCO3

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