Answer to Question #204127 in General Chemistry for Jasmine Enriquez

Question #204127

Sodium Bicarbonate is sometimes used to neutralize acid spills. If 2.0L of 6.0M H2SO4 is spilled, how many liters of Sodium Bicarbnate, NaHCO3, is required to neutralize H2SO4?


1
Expert's answer
2021-06-07T03:13:25-0400

The amount in moles of spilled sulfuric acid is


According to stoichiometry of the chemical reaction

the amount of sodium bicarbonate is two times of the amount of sulfuric acid. Thus

The mass of sodium bicarbonate can be calculated:


no. of moles of NaHCO3 = mass/molar mass

= 2016/84.007 = 23.99 moles


Volume required :-


Molarity = no. of moles of solute/ volume (L)

6.0M = 23.99/volume(L)

Volume(L) = 23.99/6 = 3.99 L


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